Oxidation state: Difference between revisions

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","dsr":[0,32,null,null]}' about="#mwt1" typeof="mw:Transclusion" data-mw='{"target":{"wt":"distinguish","href":"./Template:Distinguish"},"params":{"1":{"wt":"Oxidation number"}}}'>Not to be confused with <a rel="mw:WikiLink" href="./Oxidation_number" data-parsoid='{"a":{"href":"./Oxidation_number"},"sa":{"href":":Oxidation number"},"stx":"simple"}'>Oxidation number</a>. <table class="metadata plainlinks ambox ambox-move" style="" about="#mwt2" data-parsoid='{"src":"

","dsr":[33,77,null,null]}' typeof="mw:Transclusion" data-mw='{"target":{"wt":"mergefrom","href":"./Template:Mergefrom"},"params":{"1":{"wt":"Oxidation number"},"date":{"wt":"May 2013"}}}'> <tbody data-parsoid="{}">

It has been suggested that <a rel="mw:WikiLink" href="./Oxidation_number" data-parsoid='{"a":{"href":"./Oxidation_number"},"sa":{"href":"::Oxidation number"},"stx":"piped"}'>Oxidation number</a> be <a rel="mw:WikiLink" href="./Wikipedia:Merging" data-parsoid='{"a":{"href":"./Wikipedia:Merging"},"sa":{"href":"Wikipedia:Merging"},"stx":"piped"}'>merged</a> into this article. (<a rel="mw:WikiLink" href="./Talk:Oxidation_state" data-parsoid='{"a":{"href":"./Talk:Oxidation_state"},"sa":{"href":"Talk:Oxidation state"},"stx":"piped"}'>Discuss</a>) Proposed since May 2013. </tbody><link rel="mw:WikiLink/Category" href="./Category:Articles_to_be_merged_from_May_2013" data-parsoid='{"a":{"href":"./Category:Articles_to_be_merged_from_May_2013"},"sa":{"href":"Category:Articles to be merged from May 2013"},"stx":"simple"}' about="#mwt2"><link rel="mw:WikiLink/Category" href="./Category:All_articles_to_be_merged" data-parsoid='{"a":{"href":"./Category:All_articles_to_be_merged"},"sa":{"href":"Category:All articles to be merged"},"stx":"simple"}' about="#mwt2">

The oxidation state is an indicator of the degree of <a rel="mw:WikiLink" href="./Oxidation" data-parsoid='{"a":{"href":"./Oxidation"},"sa":{"href":"oxidation"},"stx":"simple","dsr":[138,151,2,2]}'>oxidation</a> of an <a rel="mw:WikiLink" href="./Atom" data-parsoid='{"a":{"href":"./Atom"},"sa":{"href":"atom"},"stx":"simple","dsr":[158,166,2,2]}'>atom</a> in a <a rel="mw:WikiLink" href="./Chemical_compound" data-parsoid='{"a":{"href":"./Chemical_compound"},"sa":{"href":"chemical compound"},"stx":"simple","dsr":[172,193,2,2]}'>chemical compound</a>. The formal oxidation state is the hypothetical <a rel="mw:WikiLink" href="./Electrical_charge" data-parsoid='{"a":{"href":"./Electrical_charge"},"sa":{"href":"Electrical charge"},"stx":"piped","dsr":[247,275,20,2]}'>charge</a> that an atom would have if all bonds to atoms of different elements were 100% <a rel="mw:WikiLink" href="./Ionic_bond" data-parsoid='{"a":{"href":"./Ionic_bond"},"sa":{"href":"Ionic bond"},"stx":"piped","dsr":[354,374,13,2]}'>ionic</a>. Oxidation states are typically represented by <a rel="mw:WikiLink" href="./Integer" data-parsoid='{"a":{"href":"./Integer"},"sa":{"href":"integer"},"stx":"simple","dsr":[422,434,2,3],"tail":"s"}'>integers</a>, which can be positive, negative, or zero. In some cases, the average oxidation state of an element is a fraction, such as 8/3 for iron in <a rel="mw:WikiLink" href="./Magnetite" data-parsoid='{"a":{"href":"./Magnetite"},"sa":{"href":"magnetite"},"stx":"simple","dsr":[574,587,2,2]}'>magnetite</a> (<span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"Fe
₃O
₄","dsr":[589,606,null,null]}' about="#mwt3" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"Fe"},"2":{"wt":"3"},"3":{"wt":"O"},"4":{"wt":"4"}}}'>Fe
3O
4). The highest known oxidation state is +8 in the tetroxides of <a rel="mw:WikiLink" href="./Ruthenium_tetroxide" data-parsoid='{"a":{"href":"./Ruthenium_tetroxide"},"sa":{"href":"ruthenium tetroxide"},"stx":"piped","dsr":[670,703,22,2]}'>ruthenium</a>, <a rel="mw:WikiLink" href="./Xenon_tetroxide" data-parsoid='{"a":{"href":"./Xenon_tetroxide"},"sa":{"href":"xenon tetroxide"},"stx":"piped","dsr":[705,730,18,2]}'>xenon</a>, <a rel="mw:WikiLink" href="./Osmium_tetroxide" data-parsoid='{"a":{"href":"./Osmium_tetroxide"},"sa":{"href":"osmium tetroxide"},"stx":"piped","dsr":[732,759,19,2]}'>osmium</a>, <a rel="mw:WikiLink" href="./Iridium" data-parsoid='{"a":{"href":"./Iridium"},"sa":{"href":"iridium"},"stx":"simple","dsr":[761,772,2,2]}'>iridium</a>, and <a rel="mw:WikiLink" href="./Hassium" data-parsoid='{"a":{"href":"./Hassium"},"sa":{"href":"hassium"},"stx":"simple","dsr":[778,789,2,2]}'>hassium</a>, and some complexes involving <a rel="mw:WikiLink" href="./Plutonium" data-parsoid='{"a":{"href":"./Plutonium"},"sa":{"href":"plutonium"},"stx":"simple","dsr":[820,833,2,2]}'>plutonium</a>, while the lowest known oxidation state is −4 for some elements in the <a rel="mw:WikiLink" href="./Carbon_group" data-parsoid='{"a":{"href":"./Carbon_group"},"sa":{"href":"carbon group"},"stx":"simple","dsr":[911,927,2,2]}'>carbon group</a>.

The increase in oxidation state of an atom through a chemical reaction is known as an oxidation; a decrease in oxidation state is known as a <a rel="mw:WikiLink" href="./Redox" data-parsoid='{"a":{"href":"./Redox"},"sa":{"href":"redox"},"stx":"piped","dsr":[1071,1090,8,2]}'>reduction</a>. Such reactions involve the formal transfer of electrons, a net gain in electrons being a reduction and a net loss of electrons being an oxidation. For pure elements, the oxidation state is zero.

The definition of the oxidation state listed by <a rel="mw:WikiLink" href="./IUPAC" data-parsoid='{"a":{"href":"./IUPAC"},"sa":{"href":"IUPAC"},"stx":"simple","dsr":[1336,1345,2,2]}'>IUPAC</a> is as follows:<span about="#mwt5" class="reference" data-mw='{"name":"ref","body":{"html":"<a rel=\"mw:WikiLink\" href=\"./IUPAC\" data-parsoid=\"{"a":{"href":"./IUPAC"},"sa":{"href":"IUPAC"},"stx":"simple","dsr":[1379,1388,2,2]}\">IUPAC</a> <a rel=\"mw:WikiLink\" href=\"./Gold_Book\" data-parsoid=\"{"a":{"href":"./Gold_Book"},"sa":{"href":"Gold Book"},"stx":"simple","dsr":[1391,1404,2,2]}\">Gold Book</a> definition: <a rel=\"mw:ExtLink\" href=\"http://goldbook.iupac.org/O04365.html\" data-parsoid=\"{"targetOff":1458,"dsr":[1419,1478,39,1]}\">oxidation state</a>  <a rel=\"mw:ExtLink\" href=\"http://www.iupac.org/goldbook/O04365.pdf\" data-parsoid=\"{"targetOff":1527,"dsr":[1485,1531,42,1]}\">PDF</a>"},"attrs":{"name":"goldbook"}}' id="cite_ref-goldbook-1-0" rel="dc:references" typeof="mw:Extension/ref" data-parsoid="{"src":"^[1]","dsr":[1360,1537,19,6]}"><a href="#cite_note-goldbook-1">[1]</a>

<blockquote class="toccolours" style="float:none; padding: 10px 15px 10px 15px; display:table;" data-parsoid='{"src":"

[Oxidation state] is defined as the charge an atom might be imagined to have when electrons are counted according to an agreed-upon set of rules:\n# the oxidation state of a free element (uncombined element) is zero\n# for a simple (monoatomic) ion, the oxidation state is equal to the net charge on the ion \n# hydrogen has an oxidation state of 1 and oxygen has an oxidation state of −2 when they are present in most compounds. (Exceptions to this are that hydrogen has an oxidation state of −1 in hydrides of active metals, e.g. LiH, and oxygen has an oxidation state of −1 in peroxides, e.g. H₂O₂\n# the algebraic sum of oxidation states of all atoms in a neutral molecule must be zero, while in ions the algebraic sum of the oxidation states of the constituent atoms must be equal to the charge on the ion.

","dsr":[1538,2453,null,null]}' about="#mwt6" typeof="mw:Transclusion" data-mw='{"target":{"wt":"quotation","href":"./Template:Quotation"},"params":{"1":{"wt":"[Oxidation state] is defined as the charge an atom might be imagined to have when electrons are counted according to an agreed-upon set of rules:\n# the oxidation state of a free element (uncombined element) is zero\n# for a simple (monoatomic) ion, the oxidation state is equal to the net charge on the ion \n# hydrogen has an oxidation state of 1 and oxygen has an oxidation state of −2 when they are present in most compounds. (Exceptions to this are that hydrogen has an oxidation state of −1 in hydrides of active metals, e.g. LiH, and oxygen has an oxidation state of −1 in peroxides, e.g. H₂O₂\n# the algebraic sum of oxidation states of all atoms in a neutral molecule must be zero, while in ions the algebraic sum of the oxidation states of the constituent atoms must be equal to the charge on the ion."}}}'> [Oxidation state] is defined as the charge an atom might be imagined to have when electrons are counted according to an agreed-upon set of rules:

the oxidation state of a <a rel="mw:WikiLink" href="./Free_element" data-parsoid='{"a":{"href":"./Free_element"},"sa":{"href":"free element"},"stx":"simple"}'>free element</a> (uncombined element) is zero
for a simple (monoatomic) ion, the oxidation state is equal to the net charge on the ion
hydrogen has an oxidation state of 1 and oxygen has an oxidation state of −2 when they are present in most compounds. (Exceptions to this are that hydrogen has an oxidation state of −1 in <a rel="mw:WikiLink" href="./Hydride" data-parsoid='{"a":{"href":"./Hydride"},"sa":{"href":"hydride"},"stx":"simple","tail":"s"}'>hydrides</a> of active metals, e.g. <a rel="mw:WikiLink" href="./Lithium_hydride" data-parsoid='{"a":{"href":"./Lithium_hydride"},"sa":{"href":"Lithium hydride"},"stx":"piped"}'>LiH</a>, and oxygen has an oxidation state of −1 in <a rel="mw:WikiLink" href="./Peroxide" data-parsoid='{"a":{"href":"./Peroxide"},"sa":{"href":"peroxide"},"stx":"simple","tail":"s"}'>peroxides</a>, e.g. <a rel="mw:WikiLink" href="./Hydrogen_peroxide" data-parsoid='{"a":{"href":"./Hydrogen_peroxide"},"sa":{"href":"hydrogen peroxide"},"stx":"piped"}'>H₂O₂</a>
the algebraic sum of oxidation states of all atoms in a neutral molecule must be zero, while in ions the algebraic sum of the oxidation states of the constituent atoms must be equal to the charge on the ion.

Some general rules for determining oxidation states without use of Lewis structures

Here are general rules for simple compounds without structural formulae:<a href="#cite_note-goldbook-1">[1]</a>

Any pure element (even if it forms diatomic molecules like chlorine, Cl₂) has an oxidation state (OS) of zero. Examples of this are Cu or O₂.
For monatomic ions, the OS is the same as the charge of the ion. For example, S²⁻ has an OS of −2, whereas Li⁺ has an OS of +1.
The sum of OSs for all atoms in a molecule or polyatomic ion is equal to the charge of the molecule or ion, so that the OS of one element can be calculated from the OS of the other elements. For example, in <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"SO²⁻
₃","dsr":[3178,3194,null,null]}' about="#mwt9" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"SO"},"2":{"wt":"3"},"3":{"wt":"2-"}}}'>SO2−
3 (<a rel="mw:WikiLink" href="./Sulfite" data-parsoid='{"a":{"href":"./Sulfite"},"sa":{"href":"sulfite"},"stx":"simple","dsr":[3196,3207,2,2]}'>sulfite</a> ion), the total charge of the ion is −2, and each oxygen is assumed to have its usual oxidation state of −2. The sum of OSs is then OS(S) + 3(−2) = OS(S) − 6 = −2, so that OS(S) = +4.

This means that the <a rel="mw:WikiLink" href="./Sum" data-parsoid='{"a":{"href":"./Sum"},"sa":{"href":"sum"},"stx":"simple","dsr":[3413,3420,2,2]}'>sum</a> of oxidation states of all atoms in a neutral <a rel="mw:WikiLink" href="./Molecule" data-parsoid='{"a":{"href":"./Molecule"},"sa":{"href":"molecule"},"stx":"simple","dsr":[3467,3479,2,2]}'>molecule</a> must be zero. Likewise, in polyatomic ions, the sum of the oxidation states of the constituent atoms must be equal to the charge on the ion. This fact, combined with the fact that some elements almost always have certain oxidation states (due to their very high electropositivity or electronegativity), allows one to compute the oxidation states for the remaining atoms (such as transition metals) in simple compounds.

The following rules can be used for initially assigning oxidation states for certain elements, in simple compounds:

<a rel="mw:WikiLink" href="./Fluorine" data-parsoid='{"a":{"href":"./Fluorine"},"sa":{"href":"Fluorine"},"stx":"simple","dsr":[4019,4031,2,2]}'>Fluorine</a> has an oxidation state of −1 when bonded to any other element, since it has the highest <a rel="mw:WikiLink" href="./Electronegativity" data-parsoid='{"a":{"href":"./Electronegativity"},"sa":{"href":"electronegativity"},"stx":"simple","dsr":[4126,4147,2,2]}'>electronegativity</a> of all reactive elements.
<a rel="mw:WikiLink" href="./Halogen" data-parsoid='{"a":{"href":"./Halogen"},"sa":{"href":"Halogen"},"stx":"simple","dsr":[4175,4187,2,3],"tail":"s"}'>Halogens</a> other than fluorine have an oxidation state of −1 except when they are bonded to oxygen, nitrogen, or another (more electronegative) halogen. For example, the oxidation state of chlorine in <a rel="mw:WikiLink" href="./Chlorine_monofluoride" data-parsoid='{"a":{"href":"./Chlorine_monofluoride"},"sa":{"href":"chlorine monofluoride"},"stx":"simple","dsr":[4378,4403,2,2]}'>chlorine monofluoride</a> (ClF) is +1. However, in <a rel="mw:WikiLink" href="./Bromine_chloride" data-parsoid='{"a":{"href":"./Bromine_chloride"},"sa":{"href":"bromine chloride"},"stx":"simple","dsr":[4429,4449,2,2]}'>bromine chloride</a> (BrCl), the oxidation state of Cl is −1.
<a rel="mw:WikiLink" href="./Hydrogen" data-parsoid='{"a":{"href":"./Hydrogen"},"sa":{"href":"Hydrogen"},"stx":"simple","dsr":[4492,4504,2,2]}'>Hydrogen</a> has an <a rel="mw:WikiLink" href="./Oxidation" data-parsoid='{"a":{"href":"./Oxidation"},"sa":{"href":"oxidation"},"stx":"simple","dsr":[4512,4525,2,2]}'>oxidation</a> state of +1 except when bonded to more electropositive elements such as <a rel="mw:WikiLink" href="./Sodium" data-parsoid='{"a":{"href":"./Sodium"},"sa":{"href":"sodium"},"stx":"simple","dsr":[4598,4608,2,2]}'>sodium</a>, <a rel="mw:WikiLink" href="./Aluminium" data-parsoid='{"a":{"href":"./Aluminium"},"sa":{"href":"aluminium"},"stx":"simple","dsr":[4610,4623,2,2]}'>aluminium</a>, and <a rel="mw:WikiLink" href="./Boron" data-parsoid='{"a":{"href":"./Boron"},"sa":{"href":"boron"},"stx":"simple","dsr":[4629,4638,2,2]}'>boron</a>, as in <a rel="mw:WikiLink" href="./Sodium_hydride" data-parsoid='{"a":{"href":"./Sodium_hydride"},"sa":{"href":"sodium hydride"},"stx":"piped","dsr":[4646,4668,17,2]}'>NaH</a>, <a rel="mw:WikiLink" href="./Sodium_borohydride" data-parsoid='{"a":{"href":"./Sodium_borohydride"},"sa":{"href":"sodium borohydride"},"stx":"piped","dsr":[4670,4708,21,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"NaBH
₄","dsr":[4691,4706,null,null]}' about="#mwt10" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"NaBH"},"2":{"wt":"4"}}}'>NaBH
4</a>, <a rel="mw:WikiLink" href="./Lithium_aluminium_hydride" data-parsoid='{"a":{"href":"./Lithium_aluminium_hydride"},"sa":{"href":"lithium aluminium hydride"},"stx":"piped","dsr":[4710,4756,28,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"LiAlH
₄","dsr":[4738,4754,null,null]}' about="#mwt11" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"LiAlH"},"2":{"wt":"4"}}}'>LiAlH
4</a>, where each H has an oxidation state of −1.
In compounds, <a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"oxygen"},"stx":"simple","dsr":[4816,4826,2,2]}'>oxygen</a> typically has an oxidation state of −2, though there are exceptions that are listed <a rel="mw:WikiLink" href="./Oxidation_state#Elements_with_multiple_oxidation_states" data-parsoid='{"a":{"href":"./Oxidation_state#Elements_with_multiple_oxidation_states"},"sa":{"href":"Oxidation state#Elements with multiple oxidation states"},"stx":"piped","dsr":[4911,4976,58,2]}'>below</a>, such as <a rel="mw:WikiLink" href="./Peroxide" data-parsoid='{"a":{"href":"./Peroxide"},"sa":{"href":"peroxide"},"stx":"simple","dsr":[4986,4999,2,3],"tail":"s"}'>peroxides</a> (e.g. hydrogen peroxide H₂O₂), where oxygen has an OS of −1.
<a rel="mw:WikiLink" href="./Alkali_metal" data-parsoid='{"a":{"href":"./Alkali_metal"},"sa":{"href":"Alkali metal"},"stx":"simple","dsr":[5084,5101,2,3],"tail":"s"}'>Alkali metals</a> have an oxidation state of +1 in virtually all of their compounds (exception, see <a rel="mw:WikiLink" href="./Alkalide" data-parsoid='{"a":{"href":"./Alkalide"},"sa":{"href":"alkalide"},"stx":"simple","dsr":[5184,5196,2,2]}'>alkalide</a>).
<a rel="mw:WikiLink" href="./Alkaline_earth_metal" data-parsoid='{"a":{"href":"./Alkaline_earth_metal"},"sa":{"href":"Alkaline earth metal"},"stx":"simple","dsr":[5200,5225,2,3],"tail":"s"}'>Alkaline earth metals</a> have an oxidation state of +2 in virtually all of their compounds.

Example for a complex salt: In <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"Cr(OH)
₃","dsr":[5331,5348,null,null]}' about="#mwt12" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"Cr(OH)"},"2":{"wt":"3"}}}'>Cr(OH)
3, oxygen has an oxidation state of −2 (no fluorine or O–O bonds present), and hydrogen has a state of +1 (bonded to oxygen). So, each of the three <a rel="mw:WikiLink" href="./Hydroxide" data-parsoid='{"a":{"href":"./Hydroxide"},"sa":{"href":"hydroxide"},"stx":"simple","dsr":[5495,5508,2,2]}'>hydroxide</a> groups has an oxidation state of −2 + 1 = −1. As the compound is neutral, <a rel="mw:WikiLink" href="./Chromium" data-parsoid='{"a":{"href":"./Chromium"},"sa":{"href":"chromium"},"stx":"simple","dsr":[5583,5595,2,2]}'>chromium</a> has an oxidation state of +3.

Oxidation state and formal charge

<div class="rellink relarticle mainarticle" data-parsoid='{"src":"

","dsr":[5667,5731,null,null]}' about="#mwt13" typeof="mw:Transclusion" data-mw='{"target":{"wt":"Main","href":"./Template:Main"},"params":{"1":{"wt":"Formal charge#Formal charge compared to oxidation state"}}}'>Main article: <a rel="mw:WikiLink" href="./Formal_charge#Formal_charge_compared_to_oxidation_state" data-parsoid='{"a":{"href":"./Formal_charge#Formal_charge_compared_to_oxidation_state"},"sa":{"href":"Formal charge#Formal charge compared to oxidation state"},"stx":"piped"}'>Formal charge#Formal charge compared to oxidation state</a>

The oxidation state of an atom is often different from the <a rel="mw:WikiLink" href="./Formal_charge" data-parsoid='{"a":{"href":"./Formal_charge"},"sa":{"href":"formal charge"},"stx":"simple","dsr":[5791,5808,2,2]}'>formal charge</a> often included in Lewis structures (when it is non-zero). The oxidation state is calculated by assuming that each chemical bond (except between identical atoms) is ionic so that both electrons are assigned to the more electronegative bonded atom. In contrast, the formal charge is calculated by assuming that each bonds is covalent so that one electron is assigned to each bonded atom. For example, in ammonium ion (NH₄⁺) the oxidation state of nitrogen is -3, as all eight valence electrons are assigned to the nitrogen atom which is more electronegative than hydrogen. However the formal charge is +1, calculated by assigning only four valence electrons (one per bond) to nitrogen. For comparison, the nitrogen in ammonia (NH₃) has oxidation state -3 also but a formal charge of zero. On <a rel="mw:WikiLink" href="./Protonation" data-parsoid='{"a":{"href":"./Protonation"},"sa":{"href":"protonation"},"stx":"simple","dsr":[6632,6647,2,2]}'>protonation</a> of ammonia the formal charge on nitrogen changes, but its oxidation state does not.

Calculation of formal oxidation states with a Lewis structure

There are two common ways of computing the oxidation state of an atom in a compound. The first is the simple algebraic sum technique above, used in compounds that do not require a <a rel="mw:WikiLink" href="./Lewis_structure" data-parsoid='{"a":{"href":"./Lewis_structure"},"sa":{"href":"Lewis structure"},"stx":"simple","dsr":[6980,6999,2,2]}'>Lewis structure</a>. The second is used for molecules when one has a <a rel="mw:WikiLink" href="./Lewis_structure" data-parsoid='{"a":{"href":"./Lewis_structure"},"sa":{"href":"Lewis structure"},"stx":"simple","dsr":[7049,7068,2,2]}'>Lewis structure</a>.

It should be remembered that the oxidation state of an atom does not represent the "real" charge on that atom: This is particularly true of high oxidation states, where the <a rel="mw:WikiLink" href="./Ionization_energy" data-parsoid='{"a":{"href":"./Ionization_energy"},"sa":{"href":"ionization energy"},"stx":"simple","dsr":[7244,7265,2,2]}'>ionization energy</a> required to produce a multiply positive ion are far greater than the energies available in chemical reactions. The assignment of electrons between atoms in calculating an oxidation state is purely a formalism, but is a useful one for the understanding of many chemical reactions.

For more about issues with calculating atomic charges, see <a rel="mw:WikiLink" href="./Partial_charge" data-parsoid='{"a":{"href":"./Partial_charge"},"sa":{"href":"partial charge"},"stx":"simple","dsr":[7606,7624,2,2]}'>partial charge</a>.

The Lewis structure

When a <a rel="mw:WikiLink" href="./Lewis_structure" data-parsoid='{"a":{"href":"./Lewis_structure"},"sa":{"href":"Lewis structure"},"stx":"simple","dsr":[7661,7680,2,2]}'>Lewis structure</a> of a molecule is available, the oxidation states may be assigned by computing the difference between the number of <a rel="mw:WikiLink" href="./Valence_electron" data-parsoid='{"a":{"href":"./Valence_electron"},"sa":{"href":"valence electron"},"stx":"simple","dsr":[7796,7817,2,3],"tail":"s"}'>valence electrons</a> that a neutral atom of that element would have and the number of electrons that "belong" to it in the Lewis structure. For purposes of computing oxidation states, electrons in a bond between atoms of different elements belong to the more <a rel="mw:WikiLink" href="./Electronegative" data-parsoid='{"a":{"href":"./Electronegative"},"sa":{"href":"electronegative"},"stx":"simple","dsr":[8056,8075,2,2]}'>electronegative</a> atom; electrons in a bond between atoms of the same element are split equally, and electrons in a <a rel="mw:WikiLink" href="./Lone_pair" data-parsoid='{"a":{"href":"./Lone_pair"},"sa":{"href":"lone pair"},"stx":"simple","dsr":[8174,8187,2,2]}'>lone pair</a> belong only to the atom with the lone pair.

For example, consider <a rel="mw:WikiLink" href="./Acetic_acid" data-parsoid='{"a":{"href":"./Acetic_acid"},"sa":{"href":"acetic acid"},"stx":"simple","dsr":[8255,8270,2,2]}'>acetic acid</a>:

The <a rel="mw:WikiLink" href="./Methyl" data-parsoid='{"a":{"href":"./Methyl"},"sa":{"href":"methyl"},"stx":"simple","dsr":[8322,8332,2,2]}'>methyl</a> group carbon atom has 6 valence electrons from its bonds to the hydrogen atoms because carbon is more electronegative than hydrogen. Also, 1 electron is gained from its bond with the other carbon atom because the electron pair in the <a rel="mw:WikiLink" href="./Carbon-carbon_bond" data-parsoid='{"a":{"href":"./Carbon-carbon_bond"},"sa":{"href":"carbon-carbon bond"},"stx":"piped","dsr":[8567,8598,21,2]}'>C–C bond</a> is split equally, giving a total of 7 electrons. A neutral carbon atom would have 4 valence electrons, because carbon is in <a rel="mw:WikiLink" href="./Group_14" data-parsoid='{"a":{"href":"./Group_14"},"sa":{"href":"group 14"},"stx":"simple","dsr":[8723,8735,2,2]}'>group 14</a> of the periodic table. The difference, 4 – 7 = –3, is the oxidation state of that carbon atom. That is, if it is assumed that all the bonds were 100% ionic (which in fact they are not), the carbon would be described as C^3-.

Following the same rules, the <a rel="mw:WikiLink" href="./Carboxylic_acid" data-parsoid='{"a":{"href":"./Carboxylic_acid"},"sa":{"href":"carboxylic acid"},"stx":"simple","dsr":[9003,9022,2,2]}'>carboxylic acid</a> carbon atom has an oxidation state of +3 (it only gets one valence electron from the C–C bond; the oxygen atoms get all the other electrons because oxygen is more electronegative than carbon). The oxygen atoms both have an oxidation state of –2; they get 8 electrons each (4 from the lone pairs and 4 from the bonds), while a neutral oxygen atom would have 6. The hydrogen atoms all have oxidation state +1, because they surrender their electron to the more electronegative atoms to which they are bonded.

Inequivalent atoms of an element

<figure class="mw-halign-right" typeof="mw:Image/Thumb" data-parsoid='{"optList":[{"ck":"thumbnail","ak":"thumb"},{"ck":"right","ak":"right"},{"ck":"width","ak":"150px"},{"ck":"caption","ak":"Structure of the thiosulfate anion"}],"cacheKey":"

","img":{"h":894,"w":1100,"wdset":true},"dsr":[9569,9665,2,2]}'><a href="./File:Thiosulfate-ion-2D-dimensions.png" data-parsoid='{"a":{"href":"./File:Thiosulfate-ion-2D-dimensions.png"},"dsr":[9571,null,null,null]}'><img resource="./File:Thiosulfate-ion-2D-dimensions.png" src="http://upload.wikimedia.org/wikipedia/commons/thumb/e/e7/Thiosulfate-ion-2D-dimensions.png/150px-Thiosulfate-ion-2D-dimensions.png" height="122" width="150" data-parsoid='{"a":{"resource":"./File:Thiosulfate-ion-2D-dimensions.png"},"sa":{"resource":"Image:Thiosulfate-ion-2D-dimensions.png"}}'></a><figcaption class="mw-figcaption" data-parsoid='{"dsr":[null,9663,null,null]}'>Structure of the thiosulfate anion</figcaption></figure> An example of a molecule with inequivalent atoms of the same element is the <a rel="mw:WikiLink" href="./Thiosulfate" data-parsoid='{"a":{"href":"./Thiosulfate"},"sa":{"href":"thiosulfate"},"stx":"simple","dsr":[9742,9757,2,2]}'>thiosulfate</a> ion (S₂O₃²⁻), for which the algebraic sum rule yields the average value +2 for sulfur, where the two ionizing electrons are assigned to the terminal sulfur atom. However, the use of a Lewis structure and electron counting shows that the two sulfur atoms are different. The central sulfur is assigned only one valence electron from the S-S bond and no valence electrons from the S-O bonds, compared to six valence electrons for a free sulfur atom, so the oxidation state of the central sulfur is +5. The terminal sulfur atom is assigned the other electron from the S-S bond plus three lone pairs for a total of seven valence electrons, so its oxidation state is −1.

Redox reactions

Oxidation states can be useful for balancing chemical equations for oxidation-reduction (or <a rel="mw:WikiLink" href="./Redox" data-parsoid='{"a":{"href":"./Redox"},"sa":{"href":"redox"},"stx":"simple","dsr":[10577,10586,2,2]}'>redox</a>) reactions, because the changes in the oxidized atoms have to be balanced by the changes in the reduced atoms. For example, in the reaction of <a rel="mw:WikiLink" href="./Acetaldehyde" data-parsoid='{"a":{"href":"./Acetaldehyde"},"sa":{"href":"acetaldehyde"},"stx":"simple","dsr":[10730,10746,2,2]}'>acetaldehyde</a> with the <a rel="mw:WikiLink" href="./Tollens'_reagent" data-parsoid='{"a":{"href":"./Tollens'_reagent"},"sa":{"href":"Tollens' reagent"},"stx":"simple","dsr":[10756,10776,2,2]}'>Tollens' reagent</a> to acetic acid (shown below), the carbonyl carbon atom changes its oxidation state from +1 to +3 (oxidation). This oxidation is balanced by reducing two equivalents of <a rel="mw:WikiLink" href="./Silver" data-parsoid='{"a":{"href":"./Silver"},"sa":{"href":"silver"},"stx":"simple","dsr":[10945,10955,2,2]}'>silver</a> from Ag⁺ to Ag⁰.

In such structural diagrams for organic chemistry, oxidation states are represented by Roman numerals to distinguish them from <a rel="mw:WikiLink" href="./Formal_charge" data-parsoid='{"a":{"href":"./Formal_charge"},"sa":{"href":"formal charge"},"stx":"simple","dsr":[11223,11241,2,3],"tail":"s"}'>formal charges</a> (calculated with all bonds covalent).

Elements with multiple oxidation states

Most elements have more than one possible oxidation state.

Carbon has nine integer oxidation states:

Integer oxidation states of carbon
Oxidation state	Example compound
–4	<a rel="mw:WikiLink" href="./Methane" data-parsoid='{"a":{"href":"./Methane"},"sa":{"href":"methane"},"stx":"piped","dsr":[11539,11564,10,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CH ₄","dsr":[11549,11562,null,null]}' about="#mwt14" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CH"},"2":{"wt":"4"}}}'>CH 4</a>
–3	<a rel="mw:WikiLink" href="./Ethane" data-parsoid='{"a":{"href":"./Ethane"},"sa":{"href":"ethane"},"stx":"piped","dsr":[11576,11603,9,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₂H ₆","dsr":[11585,11601,null,null]}' about="#mwt15" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"2"},"3":{"wt":"H"},"4":{"wt":"6"}}}'>C 2H 6</a>
–2	<a rel="mw:WikiLink" href="./Chloromethane" data-parsoid='{"a":{"href":"./Chloromethane"},"sa":{"href":"chloromethane"},"stx":"piped","dsr":[11615,11649,16,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CH ₃Cl","dsr":[11631,11647,null,null]}' about="#mwt16" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CH"},"2":{"wt":"3"},"3":{"wt":"Cl"}}}'>CH 3Cl</a>
–1	<a rel="mw:WikiLink" href="./Acetylene" data-parsoid='{"a":{"href":"./Acetylene"},"sa":{"href":"acetylene"},"stx":"piped","dsr":[11661,11691,12,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₂H ₂","dsr":[11673,11689,null,null]}' about="#mwt17" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"2"},"3":{"wt":"H"},"4":{"wt":"2"}}}'>C 2H 2</a>
0	<a rel="mw:WikiLink" href="./Dichloromethane" data-parsoid='{"a":{"href":"./Dichloromethane"},"sa":{"href":"dichloromethane"},"stx":"piped","dsr":[11702,11740,18,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CH ₂Cl ₂","dsr":[11720,11738,null,null]}' about="#mwt18" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CH"},"2":{"wt":"2"},"3":{"wt":"Cl"},"4":{"wt":"2"}}}'>CH 2Cl 2</a>
+1	<a rel="mw:WikiLink" href="./1,1,2,2-Tetrachloroethane" data-parsoid='{"a":{"href":"./1,1,2,2-Tetrachloroethane"},"sa":{"href":"1,1,2,2-Tetrachloroethane"},"stx":"piped","dsr":[11752,11815,28,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CHCl ₂","dsr":[11780,11796,null,null]}' about="#mwt19" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CHCl"},"2":{"wt":"2"},"3":{"wt":""}}}'>CHCl 2—<span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CHCl ₂","dsr":[11797,11813,null,null]}' about="#mwt20" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CHCl"},"2":{"wt":"2"},"3":{"wt":""}}}'>CHCl 2</a>
+2	<a rel="mw:WikiLink" href="./Chloroform" data-parsoid='{"a":{"href":"./Chloroform"},"sa":{"href":"chloroform"},"stx":"piped","dsr":[11827,11857,13,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CHCl ₃","dsr":[11840,11855,null,null]}' about="#mwt21" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CHCl"},"2":{"wt":"3"}}}'>CHCl 3</a>
+3	<a rel="mw:WikiLink" href="./Hexachloroethane" data-parsoid='{"a":{"href":"./Hexachloroethane"},"sa":{"href":"hexachloroethane"},"stx":"piped","dsr":[11869,11907,19,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₂Cl ₆","dsr":[11888,11905,null,null]}' about="#mwt22" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"2"},"3":{"wt":"Cl"},"4":{"wt":"6"}}}'>C 2Cl 6</a>
+4	<a rel="mw:WikiLink" href="./Carbon_tetrachloride" data-parsoid='{"a":{"href":"./Carbon_tetrachloride"},"sa":{"href":"carbon tetrachloride"},"stx":"piped","dsr":[11919,11958,23,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CCl ₄","dsr":[11942,11956,null,null]}' about="#mwt23" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CCl"},"2":{"wt":"4"}}}'>CCl 4</a>

Fractional oxidation states

Fractional oxidation states are often used to represent the average oxidation states of several atoms in a structure. For example, in <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"KO
₂","dsr":[12132,12145,null,null]}' about="#mwt24" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"KO"},"2":{"wt":"2"}}}'>KO
2, the diatomic <a rel="mw:WikiLink" href="./Superoxide" data-parsoid='{"a":{"href":"./Superoxide"},"sa":{"href":"superoxide"},"stx":"simple","dsr":[12160,12174,2,2]}'>superoxide</a> ion has an overall charge of −1, so each of its two oxygen atoms is assigned an oxidation state of −½, This ion is described as a <a rel="mw:WikiLink" href="./Resonance_(chemistry)" data-parsoid='{"a":{"href":"./Resonance_(chemistry)"},"sa":{"href":"resonance (chemistry)"},"stx":"piped","dsr":[12317,12352,24,2]}'>resonance</a> hybrid of two Lewis structures, where each oxygen has oxidation state 0 in one structure and −1 in the other.

For the <a rel="mw:WikiLink" href="./Cyclopentadienyl" data-parsoid='{"a":{"href":"./Cyclopentadienyl"},"sa":{"href":"cyclopentadienyl"},"stx":"simple","dsr":[12479,12499,2,2]}'>cyclopentadienyl</a> ion <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C
₅H
₅","dsr":[12504,12520,null,null]}' about="#mwt25" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"5"},"3":{"wt":"H"},"4":{"wt":"5"}}}'>C
5H
5⁻, the oxidation state of C is (−1) + (−<span class="frac nowrap" data-parsoid='{"src":"1⁄5","dsr":[12583,12595,null,null]}' about="#mwt26" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"5"}}}'>¹⁄₅) = −<span class="frac nowrap" data-parsoid='{"src":"6⁄5","dsr":[12606,12618,null,null]}' about="#mwt27" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"6"},"2":{"wt":"5"}}}'>⁶⁄₅. The −1 occurs because each C is bonded to one hydrogen (a less electronegative element), and the −<span class="frac nowrap" data-parsoid='{"src":"1⁄5","dsr":[12730,12742,null,null]}' about="#mwt28" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"5"}}}'>¹⁄₅ because the total ionic charge is divided among five equivalent C.

If the average refers to atoms that are not equivalent, the average oxidation state may not be representative of each of the atoms. This is true in <a rel="mw:WikiLink" href="./Magnetite" data-parsoid='{"a":{"href":"./Magnetite"},"sa":{"href":"magnetite"},"stx":"simple","dsr":[12959,12972,2,2]}'>magnetite</a> <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"Fe
₃O
₄","dsr":[12973,12990,null,null]}' about="#mwt29" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"Fe"},"2":{"wt":"3"},"3":{"wt":"O"},"4":{"wt":"4"}}}'>Fe
3O
4, whose formula leads to an average oxidation state of +<span class="frac nowrap" data-parsoid='{"src":"8⁄3","dsr":[13046,13058,null,null]}' about="#mwt30" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"8"},"2":{"wt":"3"}}}'>⁸⁄₃. In fact, two-thirds of the iron ions are Fe³⁺, and one-third Fe²⁺.

Likewise, the <a rel="mw:WikiLink" href="./Ozonide" data-parsoid='{"a":{"href":"./Ozonide"},"sa":{"href":"ozonide"},"stx":"simple","dsr":[13164,13175,2,2]}'>ozonide</a> ion O₃⁻ has an average oxidation state of −<span class="frac nowrap" data-parsoid='{"src":"1⁄3","dsr":[13253,13265,null,null]}' about="#mwt31" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"3"}}}'>¹⁄₃. However, this ion is V-shaped, meaning that the central oxygen is not equivalent to the two others and cannot be assumed to have the same oxidation state.

As an example, some species contain carbon in more than one oxidation state, giving a fractional oxidation state overall:

Examples of fractional oxidation states for carbon
Oxidation state	Example species
–<span class="frac nowrap" data-parsoid='{"src":"6⁄5","dsr":[13666,13678,null,null]}' about="#mwt32" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"6"},"2":{"wt":"5"}}}'>⁶⁄₅	<a rel="mw:WikiLink" href="./Cyclopentadienyl_complex" data-parsoid='{"a":{"href":"./Cyclopentadienyl_complex"},"sa":{"href":"Cyclopentadienyl complex"},"stx":"piped","dsr":[13682,13739,27,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₅H ₅","dsr":[13709,13725,null,null]}' about="#mwt33" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"5"},"3":{"wt":"H"},"4":{"wt":"5"}}}'>C 5H 5⁻</a>
–<span class="frac nowrap" data-parsoid='{"src":"6⁄7","dsr":[13746,13758,null,null]}' about="#mwt34" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"6"},"2":{"wt":"7"}}}'>⁶⁄₇	<a rel="mw:WikiLink" href="./Tropylium" data-parsoid='{"a":{"href":"./Tropylium"},"sa":{"href":"tropylium"},"stx":"piped","dsr":[13762,13792,12,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₇H ₇","dsr":[13774,13790,null,null]}' about="#mwt35" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"7"},"3":{"wt":"H"},"4":{"wt":"7"}}}'>C 7H 7</a>⁺
–<span class="frac nowrap" data-parsoid='{"src":"5⁄4","dsr":[13811,13823,null,null]}' about="#mwt36" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"5"},"2":{"wt":"4"}}}'>⁵⁄₄	<a rel="mw:WikiLink" href="./Uranocene" data-parsoid='{"a":{"href":"./Uranocene"},"sa":{"href":"uranocene"},"stx":"piped","dsr":[13827,13870,12,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"C ₈H ₈","dsr":[13839,13855,null,null]}' about="#mwt37" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"C"},"2":{"wt":"8"},"3":{"wt":"H"},"4":{"wt":"8"}}}'>C 8H 8²⁻</a>

Oxygen

As another example, oxygen has eight distinct oxidation states:

Oxidation states of oxygen
Oxidation state	Example compounds
–2	<a rel="mw:WikiLink" href="./Oxide" data-parsoid='{"a":{"href":"./Oxide"},"sa":{"href":"oxide"},"stx":"simple","dsr":[14059,14069,2,3],"tail":"s"}'>oxides</a>, e.g. <a rel="mw:WikiLink" href="./Zinc_oxide" data-parsoid='{"a":{"href":"./Zinc_oxide"},"sa":{"href":"zinc oxide"},"stx":"piped","dsr":[14076,14094,13,2]}'>ZnO</a>, <a rel="mw:WikiLink" href="./Carbon_dioxide" data-parsoid='{"a":{"href":"./Carbon_dioxide"},"sa":{"href":"carbon dioxide"},"stx":"piped","dsr":[14096,14128,17,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"CO ₂","dsr":[14113,14126,null,null]}' about="#mwt38" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"CO"},"2":{"wt":"2"}}}'>CO 2</a>, <a rel="mw:WikiLink" href="./Water" data-parsoid='{"a":{"href":"./Water"},"sa":{"href":"water"},"stx":"piped","dsr":[14130,14154,8,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"H ₂O","dsr":[14138,14152,null,null]}' about="#mwt39" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"H"},"2":{"wt":"2"},"3":{"wt":"O"}}}'>H 2O</a>
–1	<a rel="mw:WikiLink" href="./Peroxide" data-parsoid='{"a":{"href":"./Peroxide"},"sa":{"href":"peroxide"},"stx":"simple","dsr":[14166,14179,2,3],"tail":"s"}'>peroxides</a>, e.g. <a rel="mw:WikiLink" href="./Hydrogen_peroxide" data-parsoid='{"a":{"href":"./Hydrogen_peroxide"},"sa":{"href":"hydrogen peroxide"},"stx":"piped","dsr":[14186,14224,20,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"H ₂O ₂","dsr":[14206,14222,null,null]}' about="#mwt40" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"H"},"2":{"wt":"2"},"3":{"wt":"O"},"4":{"wt":"2"}}}'>H 2O 2</a>
–<span class="frac nowrap" data-parsoid='{"src":"1⁄2","dsr":[14231,14243,null,null]}' about="#mwt41" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"2"}}}'>¹⁄₂	<a rel="mw:WikiLink" href="./Superoxide" data-parsoid='{"a":{"href":"./Superoxide"},"sa":{"href":"superoxide"},"stx":"simple","dsr":[14247,14262,2,3],"tail":"s"}'>superoxides</a>, e.g. <a rel="mw:WikiLink" href="./Potassium_superoxide" data-parsoid='{"a":{"href":"./Potassium_superoxide"},"sa":{"href":"potassium superoxide"},"stx":"piped","dsr":[14269,14307,23,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"KO ₂","dsr":[14292,14305,null,null]}' about="#mwt42" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"KO"},"2":{"wt":"2"}}}'>KO 2</a>
–<span class="frac nowrap" data-parsoid='{"src":"1⁄3","dsr":[14314,14326,null,null]}' about="#mwt43" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"3"}}}'>¹⁄₃	inorganic <a rel="mw:WikiLink" href="./Ozonide" data-parsoid='{"a":{"href":"./Ozonide"},"sa":{"href":"ozonide"},"stx":"simple","dsr":[14340,14352,2,3],"tail":"s"}'>ozonides</a>, e.g. <a rel="mw:WikiLink" href="./Rubidium_ozonide" data-parsoid='{"a":{"href":"./Rubidium_ozonide"},"sa":{"href":"rubidium ozonide"},"stx":"piped","dsr":[14359,14394,19,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"RbO ₃","dsr":[14378,14392,null,null]}' about="#mwt44" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"RbO"},"2":{"wt":"3"}}}'>RbO 3</a>
0	<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"oxygen"},"stx":"piped","dsr":[14405,14428,9,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"O ₂","dsr":[14414,14426,null,null]}' about="#mwt45" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"O"},"2":{"wt":"2"}}}'>O 2</a>
+<span class="frac nowrap" data-parsoid='{"src":"1⁄2","dsr":[14435,14447,null,null]}' about="#mwt46" typeof="mw:Transclusion" data-mw='{"target":{"wt":"frac","href":"./Template:Frac"},"params":{"1":{"wt":"1"},"2":{"wt":"2"}}}'>¹⁄₂	<a rel="mw:WikiLink" href="./Dioxygenyl" data-parsoid='{"a":{"href":"./Dioxygenyl"},"sa":{"href":"dioxygenyl"},"stx":"simple","dsr":[14451,14465,2,2]}'>dioxygenyl</a> ion, e.g. dioxygenyl hexafluoroarsenate <span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"O ₂","dsr":[14506,14518,null,null]}' about="#mwt47" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"O"},"2":{"wt":"2"}}}'>O 2⁺ <meta property="mw:objectAttrVal#href" about="#mwt57" data-parsoid='{"src":"AsF ₆","dsr":[14531,14531,null,null]}'>[<span typeof="mw:Placeholder" data-parsoid='{"src":"AsF ₆","dsr":[14532,14546,null,null]}'>AsF 6]⁻
+1	<a rel="mw:WikiLink" href="./Dioxygen_difluoride" data-parsoid='{"a":{"href":"./Dioxygen_difluoride"},"sa":{"href":"dioxygen difluoride"},"stx":"piped","dsr":[14571,14611,22,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"O ₂F ₂","dsr":[14593,14609,null,null]}' about="#mwt49" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"O"},"2":{"wt":"2"},"3":{"wt":"F"},"4":{"wt":"2"}}}'>O 2F 2</a>
+2	<a rel="mw:WikiLink" href="./Oxygen_difluoride" data-parsoid='{"a":{"href":"./Oxygen_difluoride"},"sa":{"href":"oxygen difluoride"},"stx":"piped","dsr":[14623,14658,20,2]}'><span class="chemf" style="white-space:nowrap;" data-parsoid='{"src":"OF ₂","dsr":[14643,14656,null,null]}' about="#mwt50" typeof="mw:Transclusion" data-mw='{"target":{"wt":"chem","href":"./Template:Chem"},"params":{"1":{"wt":"OF"},"2":{"wt":"2"}}}'>OF 2</a>

Oxidation number

<div class="rellink relarticle mainarticle" data-parsoid='{"src":"

","dsr":[14684,14709,null,null]}' about="#mwt51" typeof="mw:Transclusion" data-mw='{"target":{"wt":"Main","href":"./Template:Main"},"params":{"1":{"wt":"Oxidation number"}}}'>Main article: <a rel="mw:WikiLink" href="./Oxidation_number" data-parsoid='{"a":{"href":"./Oxidation_number"},"sa":{"href":"Oxidation number"},"stx":"piped"}'>Oxidation number</a>

The terms oxidation state and oxidation number are often used interchangeably. However, <a rel="mw:WikiLink" href="./Oxidation_number" data-parsoid='{"a":{"href":"./Oxidation_number"},"sa":{"href":"oxidation number"},"stx":"simple","dsr":[14809,14829,2,2]}'>oxidation number</a> is used in <a rel="mw:WikiLink" href="./Coordination_chemistry" data-parsoid='{"a":{"href":"./Coordination_chemistry"},"sa":{"href":"coordination chemistry"},"stx":"simple","dsr":[14843,14869,2,2]}'>coordination chemistry</a> with a slightly different meaning. In coordination chemistry, the rules used for counting electrons are different: Every electron in a metal-ligand bond belongs to the <a rel="mw:WikiLink" href="./Ligand" data-parsoid='{"a":{"href":"./Ligand"},"sa":{"href":"ligand"},"stx":"simple","dsr":[15038,15048,2,2]}'>ligand</a>, regardless of electronegativity. Also, oxidation numbers are conventionally represented with Roman numerals, while oxidation states use Indo-Arabic numerals.

History

The current concept of "oxidation state" was introduced by <a rel="mw:WikiLink" href="./W._M._Latimer" data-parsoid='{"a":{"href":"./W._M._Latimer"},"sa":{"href":"W. M. Latimer"},"stx":"simple","dsr":[15280,15297,2,2]}'>W. M. Latimer</a> in 1938. Oxidation itself was first studied by <a rel="mw:WikiLink" href="./Antoine_Lavoisier" data-parsoid='{"a":{"href":"./Antoine_Lavoisier"},"sa":{"href":"Antoine Lavoisier"},"stx":"simple","dsr":[15345,15366,2,2]}'>Antoine Lavoisier</a>, who believed that oxidation was always the result of reactions with <a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"oxygen"},"stx":"simple","dsr":[15436,15446,2,2]}'>oxygen</a>,<span about="#mwt53" class="reference" data-mw='{"name":"ref","body":{"html":"The Origin of the Oxidation-State Concept William B. Jensen <a rel=\"mw:WikiLink\" href=\"./J._Chem._Educ.\" data-parsoid=\"{"a":{"href":"./J._Chem._Educ."},"sa":{"href":"J. Chem. Educ."},"stx":"simple","dsr":[15516,15534,2,2]}\">J. Chem. Educ.</a> 2007, 84, 1418"},"attrs":{}}' id="cite_ref-2-0" rel="dc:references" typeof="mw:Extension/ref" data-parsoid="{"src":"^[2]","dsr":[15447,15561,5,6]}"><a href="#cite_note-2">[2]</a> thus the name. Although Lavoisier's idea has been shown to be incorrect, the name he proposed is still used, albeit more generally.

Oxidation states were one of the intellectual "stepping stones" Mendeleev used to derive the modern periodic table.

Unusual formal oxidation states

<div class="rellink relarticle mainarticle" data-parsoid='{"src":"

","dsr":[15848,15873,null,null]}' about="#mwt54" typeof="mw:Transclusion" data-mw='{"target":{"wt":"Main","href":"./Template:Main"},"params":{"1":{"wt":"High-valent iron"}}}'>Main article: <a rel="mw:WikiLink" href="./High-valent_iron" data-parsoid='{"a":{"href":"./High-valent_iron"},"sa":{"href":"High-valent iron"},"stx":"piped"}'>High-valent iron</a>

Unusual formal oxidation states of metals are important in biochemical processes, the notable ones being Fe(IV) and Fe(V) in <a rel="mw:WikiLink" href="./Cytochrome_P450" data-parsoid='{"a":{"href":"./Cytochrome_P450"},"sa":{"href":"Cytochrome P450"},"stx":"simple","dsr":[16001,16020,2,2]}'>Cytochrome P450</a>-containing systems.

References

<div class="reflist " style=" list-style-type: decimal;" data-parsoid='{"src":"

^ ^a ^b IUPAC Gold Book definition: oxidation state  PDF
^ The Origin of the Oxidation-State Concept William B. Jensen J. Chem. Educ. 2007, 84, 1418

","dsr":[16188,16199,null,null]}' about="#mwt55" typeof="mw:Transclusion" data-mw='{"target":{"wt":"Reflist","href":"./Template:Reflist"},"params":{}}'>

↑ <a href="#cite_ref-goldbook-1-0">1.0</a> <a href="#cite_ref-goldbook-1-1">1.1</a> <a rel="mw:WikiLink" href="./IUPAC" data-parsoid='{"a":{"href":"./IUPAC"},"sa":{"href":"IUPAC"},"stx":"simple","dsr":[1379,1388,2,2]}'>IUPAC</a> <a rel="mw:WikiLink" href="./Gold_Book" data-parsoid='{"a":{"href":"./Gold_Book"},"sa":{"href":"Gold Book"},"stx":"simple","dsr":[1391,1404,2,2]}'>Gold Book</a> definition: <a rel="mw:ExtLink" href="http://goldbook.iupac.org/O04365.html" data-parsoid='{"targetOff":1458,"dsr":[1419,1478,39,1]}'>oxidation state</a> <a rel="mw:ExtLink" href="http://www.iupac.org/goldbook/O04365.pdf" data-parsoid='{"targetOff":1527,"dsr":[1485,1531,42,1]}'>PDF</a>
<a href="#cite_ref-2-0">↑</a> The Origin of the Oxidation-State Concept William B. Jensen <a rel="mw:WikiLink" href="./J._Chem._Educ." data-parsoid='{"a":{"href":"./J._Chem._Educ."},"sa":{"href":"J. Chem. Educ."},"stx":"simple","dsr":[15516,15534,2,2]}'>J. Chem. Educ.</a> 2007, 84, 1418

<table cellspacing="0" class="navbox" style="border-spacing:0;" about="#mwt56" data-parsoid='{"src":"

","dsr":[16201,16210,null,null]}' typeof="mw:Transclusion" data-mw='{"target":{"wt":"Oxide","href":"./Template:Oxide"},"params":{}}'><tbody data-parsoid="{}">

</tbody>

[goldbook-1] IUPAC Gold Book definition: oxidation state PDF

[2] The Origin of the Oxidation-State Concept William B. Jensen J. Chem. Educ. 2007, 84, 1418

[goldbook-1] <a href="#cite_ref-goldbook-1-0">1.0</a> <a href="#cite_ref-goldbook-1-1">1.1</a> <a rel="mw:WikiLink" href="./IUPAC" data-parsoid='{"a":{"href":"./IUPAC"},"sa":{"href":"IUPAC"},"stx":"simple","dsr":[1379,1388,2,2]}'>IUPAC</a> <a rel="mw:WikiLink" href="./Gold_Book" data-parsoid='{"a":{"href":"./Gold_Book"},"sa":{"href":"Gold Book"},"stx":"simple","dsr":[1391,1404,2,2]}'>Gold Book</a> definition: <a rel="mw:ExtLink" href="http://goldbook.iupac.org/O04365.html" data-parsoid='{"targetOff":1458,"dsr":[1419,1478,39,1]}'>oxidation state</a> <a rel="mw:ExtLink" href="http://www.iupac.org/goldbook/O04365.pdf" data-parsoid='{"targetOff":1527,"dsr":[1485,1531,42,1]}'>PDF</a>

[2] <a href="#cite_ref-2-0">↑</a> The Origin of the Oxidation-State Concept William B. Jensen <a rel="mw:WikiLink" href="./J._Chem._Educ." data-parsoid='{"a":{"href":"./J._Chem._Educ."},"sa":{"href":"J. Chem. Educ."},"stx":"simple","dsr":[15516,15534,2,2]}'>J. Chem. Educ.</a> 2007, 84, 1418

[1]

[2]

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Boron suboxide (B₁₂O₂) Carbon suboxide (C₃O₂) Chlorine perchlorate (Cl₂O₄) Chloryl perchlorate (Cl₂O₆) Cobalt(II,III) oxide (Co₃O₄) Dichlorine pentoxide (Cl₂O₅) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Mellitic anhydride (C₁₂O₉) Praseodymium(III,IV) oxide (Pr₆O₁₁) Silver(I,III) oxide (Ag₂O₂) Terbium(III,IV) oxide (Tb₄O₇) Tribromine octoxide (Br₃O₈) Triuranium octoxide (U₃O₈)
+1 oxidation state	Aluminium(I) oxide (Al₂O) Copper(I) oxide (Cu₂O) Caesium monoxide (Cs₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Gallium(I) oxide (Ga₂O) Iodine(I) oxide (I₂O) Lithium oxide (Li₂O) Mercury(I) oxide (Hg₂O) Nitrous oxide (N₂O) Potassium oxide (K₂O) Rubidium oxide (Rb₂O) Silver oxide (Ag₂O) Thallium(I) oxide (Tl₂O) Sodium oxide (Na₂O) Water (hydrogen oxide) (H₂O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Berkelium monoxide (BkO) Beryllium oxide (BeO) Bromine monoxide (BrO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chlorine monoxide (ClO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N₂O₂) Europium(II) oxide (EuO) Germanium monoxide (GeO) Iron(II) oxide (FeO) Iodine monoxide (IO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Phosphorus monoxide (PO) Polonium monoxide (PoO) Protactinium monoxide (PaO) Radium oxide (RaO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S₂O₂) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Yttrium(II) oxide (YO) Zinc oxide (ZnO)
+3 oxidation state	Actinium(III) oxide (Ac₂O₃) Aluminium oxide (Al₂O₃) Americium(III) oxide (Am₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Berkelium(III) oxide (Bk₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Caesium sesquioxide (Cs₂O₃) Californium(III) oxide (Cf₂O₃) Cerium(III) oxide (Ce₂O₃) Chromium(III) oxide (Cr₂O₃) Cobalt(III) oxide (Co₂O₃) Dinitrogen trioxide (N₂O₃) Dysprosium(III) oxide (Dy₂O₃) Einsteinium(III) oxide (Es₂O₃) Erbium(III) oxide (Er₂O₃) Europium(III) oxide (Eu₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Gold(III) oxide (Au₂O₃) Holmium(III) oxide (Ho₂O₃) Indium(III) oxide (In₂O₃) Iron(III) oxide (Fe₂O₃) Lanthanum oxide (La₂O₃) Lutetium(III) oxide (Lu₂O₃) Manganese(III) oxide (Mn₂O₃) Neodymium(III) oxide (Nd₂O₃) Nickel(III) oxide (Ni₂O₃) Phosphorus trioxide (P₄O₆) Praseodymium(III) oxide (Pr₂O₃) Promethium(III) oxide (Pm₂O₃) Rhodium(III) oxide (Rh₂O₃) Samarium(III) oxide (Sm₂O₃) Scandium oxide (Sc₂O₃) Terbium(III) oxide (Tb₂O₃) Thallium(III) oxide (Tl₂O₃) Thulium(III) oxide (Tm₂O₃) Titanium(III) oxide (Ti₂O₃) Tungsten(III) oxide (W₂O₃) Vanadium(III) oxide (V₂O₃) Ytterbium(III) oxide (Yb₂O₃) Yttrium(III) oxide (Y₂O₃)
+4 oxidation state	Americium dioxide (AmO₂) Berkelium(IV) oxide (BkO₂) Bromine dioxide (BrO₂) Californium dioxide (CfO₂) Carbon dioxide (CO₂) Carbon trioxide (CO₃) Cerium(IV) oxide (CeO₂) Chlorine dioxide (ClO₂) Chromium(IV) oxide (CrO₂) Curium(IV) oxide (CmO₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (GeO₂) Iodine dioxide (IO₂) Iridium dioxide (IrO₂) Hafnium(IV) oxide (HfO₂) Lead dioxide (PbO₂) Manganese dioxide (MnO₂) Neptunium(IV) oxide (NpO₂) Nitrogen dioxide (NO₂) Osmium dioxide (OsO₂) Platinum dioxide (PtO₂) Plutonium(IV) oxide (PuO₂) Polonium dioxide (PoO₂) Praseodymium(IV) oxide (PrO₂) Protactinium(IV) oxide (PaO₂) Rhodium(IV) oxide (RhO₂) Ruthenium(IV) oxide (RuO₂) Selenium dioxide (SeO₂) Silicon dioxide (SiO₂) Sulfur dioxide (SO₂) Technetium(IV) oxide (TcO₂) Tellurium dioxide (TeO₂) Terbium(IV) oxide (TbO₂) Thorium dioxide (ThO₂) Tin dioxide (SnO₂) Titanium dioxide (TiO₂) Tungsten(IV) oxide (WO₂) Uranium dioxide (UO₂) Vanadium(IV) oxide (VO₂) Zirconium dioxide (ZrO₂)
+5 oxidation state	Antimony pentoxide (Sb₂O₅) Arsenic pentoxide (As₂O₅) Bismuth pentoxide (Bi₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Protactinium(V) oxide (Pa₂O₅) Tantalum pentoxide (Ta₂O₅) Vanadium(V) oxide (V₂O₅)
+6 oxidation state	Chromium trioxide (CrO₃) Molybdenum trioxide (MoO₃) Polonium trioxide (PoO₃) Rhenium trioxide (ReO₃) Selenium trioxide (SeO₃) Sulfur trioxide (SO₃) Tellurium trioxide (TeO₃) Tungsten trioxide (WO₃) Uranium trioxide (UO₃) Xenon trioxide (XeO₃)
+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)
+8 oxidation state	Iridium tetroxide (IrO₄) Osmium tetroxide (OsO₄) Ruthenium tetroxide (RuO₄) Xenon tetroxide (XeO₄) Hassium tetroxide (HsO₄)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxypnictide
Oxides are sorted by oxidation state. Category:Oxides

<a rel="mw:WikiLink" href="./Template:Oxide" data-parsoid='{"a":{"href":"./Template:Oxide"},"sa":{"href":"Template:Oxide"},"stx":"piped"}'>v</a> <a rel="mw:WikiLink" href="./Template%20talk:Oxide" data-parsoid='{"a":{"href":"./Template%20talk:Oxide"},"sa":{"href":"Template_talk:Oxide"},"stx":"piped"}'>t</a> <a rel="mw:ExtLink" href="//en.wikipedia.org/w/index.php?title=Template:Oxide&action=edit" data-parsoid='{"targetOff":715,"a":{"href":"//en.wikipedia.org/w/index.php?title=Template:Oxide&action=edit"},"sa":{"href":" the tetroxides of ruthenium, [[xenon t"}}'>e</a> <a rel="mw:WikiLink" href="./Oxide" data-parsoid='{"a":{"href":"./Oxide"},"sa":{"href":"Oxide"},"stx":"simple","tail":"s"}'>Oxides</a>

Various States	<a rel="mw:WikiLink" href="./Antimony_tetroxide" data-parsoid='{"a":{"href":"./Antimony_tetroxide"},"sa":{"href":"Antimony tetroxide"},"stx":"simple"}'>Antimony tetroxide</a> (<a rel="mw:WikiLink" href="./Antimony" data-parsoid='{"a":{"href":"./Antimony"},"sa":{"href":"Antimony"},"stx":"piped"}'>Sb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Cobalt(II,III)_oxide" data-parsoid='{"a":{"href":"./Cobalt(II,III)_oxide"},"sa":{"href":"Cobalt(II,III) oxide"},"stx":"simple"}'>Cobalt(II,III) oxide</a> (<a rel="mw:WikiLink" href="./Cobalt" data-parsoid='{"a":{"href":"./Cobalt"},"sa":{"href":"Cobalt"},"stx":"piped"}'>Co</a>₃<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Iron(II,III)_oxide" data-parsoid='{"a":{"href":"./Iron(II,III)_oxide"},"sa":{"href":"Iron(II,III) oxide"},"stx":"simple"}'>Iron(II,III) oxide</a> (<a rel="mw:WikiLink" href="./Iron" data-parsoid='{"a":{"href":"./Iron"},"sa":{"href":"Iron"},"stx":"piped"}'>Fe</a>₃<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Lead(II,IV)_oxide" data-parsoid='{"a":{"href":"./Lead(II,IV)_oxide"},"sa":{"href":"Lead(II,IV) oxide"},"stx":"simple"}'>Lead(II,IV) oxide</a> (<a rel="mw:WikiLink" href="./Lead" data-parsoid='{"a":{"href":"./Lead"},"sa":{"href":"Lead"},"stx":"piped"}'>Pb</a>₃<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Manganese(II,III)_oxide" data-parsoid='{"a":{"href":"./Manganese(II,III)_oxide"},"sa":{"href":"Manganese(II,III) oxide"},"stx":"simple"}'>Manganese(II,III) oxide</a> (<a rel="mw:WikiLink" href="./Manganese" data-parsoid='{"a":{"href":"./Manganese"},"sa":{"href":"Manganese"},"stx":"piped"}'>Mn</a>₃<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Silver(I,III)_oxide" data-parsoid='{"a":{"href":"./Silver(I,III)_oxide"},"sa":{"href":"Silver(I,III) oxide"},"stx":"simple"}'>Silver(I,III) oxide</a> (<a rel="mw:WikiLink" href="./Silver" data-parsoid='{"a":{"href":"./Silver"},"sa":{"href":"Silver"},"stx":"piped"}'>Ag</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>)

+1 Oxidation State	<a rel="mw:WikiLink" href="./Copper(I)_oxide" data-parsoid='{"a":{"href":"./Copper(I)_oxide"},"sa":{"href":"Copper(I) oxide"},"stx":"simple"}'>Copper(I) oxide</a> (<a rel="mw:WikiLink" href="./Copper" data-parsoid='{"a":{"href":"./Copper"},"sa":{"href":"Copper"},"stx":"piped"}'>Cu</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Dicarbon_monoxide" data-parsoid='{"a":{"href":"./Dicarbon_monoxide"},"sa":{"href":"Dicarbon monoxide"},"stx":"simple"}'>Dicarbon monoxide</a> (<a rel="mw:WikiLink" href="./Carbon" data-parsoid='{"a":{"href":"./Carbon"},"sa":{"href":"Carbon"},"stx":"piped"}'>C</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Dichlorine_monoxide" data-parsoid='{"a":{"href":"./Dichlorine_monoxide"},"sa":{"href":"Dichlorine monoxide"},"stx":"simple"}'>Dichlorine monoxide</a> (<a rel="mw:WikiLink" href="./Chlorine" data-parsoid='{"a":{"href":"./Chlorine"},"sa":{"href":"Chlorine"},"stx":"piped"}'>Cl</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Lithium_oxide" data-parsoid='{"a":{"href":"./Lithium_oxide"},"sa":{"href":"Lithium oxide"},"stx":"simple"}'>Lithium oxide</a> (<a rel="mw:WikiLink" href="./Lithium" data-parsoid='{"a":{"href":"./Lithium"},"sa":{"href":"Lithium"},"stx":"piped"}'>Li</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Potassium_oxide" data-parsoid='{"a":{"href":"./Potassium_oxide"},"sa":{"href":"Potassium oxide"},"stx":"simple"}'>Potassium oxide</a> (<a rel="mw:WikiLink" href="./Potassium" data-parsoid='{"a":{"href":"./Potassium"},"sa":{"href":"Potassium"},"stx":"piped"}'>K</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Rubidium_oxide" data-parsoid='{"a":{"href":"./Rubidium_oxide"},"sa":{"href":"Rubidium oxide"},"stx":"simple"}'>Rubidium oxide</a> (<a rel="mw:WikiLink" href="./Rubidium" data-parsoid='{"a":{"href":"./Rubidium"},"sa":{"href":"Rubidium"},"stx":"piped"}'>Rb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Silver(I)_oxide" data-parsoid='{"a":{"href":"./Silver(I)_oxide"},"sa":{"href":"Silver(I) oxide"},"stx":"simple"}'>Silver(I) oxide</a> (<a rel="mw:WikiLink" href="./Silver" data-parsoid='{"a":{"href":"./Silver"},"sa":{"href":"Silver"},"stx":"piped"}'>Ag</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Thallium(I)_oxide" data-parsoid='{"a":{"href":"./Thallium(I)_oxide"},"sa":{"href":"Thallium(I) oxide"},"stx":"simple"}'>Thallium(I) oxide</a> (<a rel="mw:WikiLink" href="./Thallium" data-parsoid='{"a":{"href":"./Thallium"},"sa":{"href":"Thallium"},"stx":"piped"}'>Tl</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Sodium_oxide" data-parsoid='{"a":{"href":"./Sodium_oxide"},"sa":{"href":"Sodium oxide"},"stx":"simple"}'>Sodium oxide</a> (<a rel="mw:WikiLink" href="./Sodium" data-parsoid='{"a":{"href":"./Sodium"},"sa":{"href":"Sodium"},"stx":"piped"}'>Na</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Properties_of_water" data-parsoid='{"a":{"href":"./Properties_of_water"},"sa":{"href":"Properties of water"},"stx":"piped"}'>Water (hydrogen oxide)</a> (<a rel="mw:WikiLink" href="./Hydrogen" data-parsoid='{"a":{"href":"./Hydrogen"},"sa":{"href":"Hydrogen"},"stx":"piped"}'>H</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>)

+2 Oxidation State	<a rel="mw:WikiLink" href="./Aluminium(II)_oxide" data-parsoid='{"a":{"href":"./Aluminium(II)_oxide"},"sa":{"href":"Aluminium(II) oxide"},"stx":"simple"}'>Aluminium(II) oxide</a> (<a rel="mw:WikiLink" href="./Aluminium" data-parsoid='{"a":{"href":"./Aluminium"},"sa":{"href":"Aluminium"},"stx":"piped"}'>Al</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Barium_oxide" data-parsoid='{"a":{"href":"./Barium_oxide"},"sa":{"href":"Barium oxide"},"stx":"simple"}'>Barium oxide</a> (<a rel="mw:WikiLink" href="./Barium" data-parsoid='{"a":{"href":"./Barium"},"sa":{"href":"Barium"},"stx":"piped"}'>Ba</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Beryllium_oxide" data-parsoid='{"a":{"href":"./Beryllium_oxide"},"sa":{"href":"Beryllium oxide"},"stx":"simple"}'>Beryllium oxide</a> (<a rel="mw:WikiLink" href="./Beryllium" data-parsoid='{"a":{"href":"./Beryllium"},"sa":{"href":"Beryllium"},"stx":"piped"}'>Be</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Cadmium_oxide" data-parsoid='{"a":{"href":"./Cadmium_oxide"},"sa":{"href":"Cadmium oxide"},"stx":"simple"}'>Cadmium oxide</a> (<a rel="mw:WikiLink" href="./Cadmium" data-parsoid='{"a":{"href":"./Cadmium"},"sa":{"href":"Cadmium"},"stx":"piped"}'>Cd</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Calcium_oxide" data-parsoid='{"a":{"href":"./Calcium_oxide"},"sa":{"href":"Calcium oxide"},"stx":"simple"}'>Calcium oxide</a> (<a rel="mw:WikiLink" href="./Calcium" data-parsoid='{"a":{"href":"./Calcium"},"sa":{"href":"Calcium"},"stx":"piped"}'>Ca</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Carbon_monoxide" data-parsoid='{"a":{"href":"./Carbon_monoxide"},"sa":{"href":"Carbon monoxide"},"stx":"simple"}'>Carbon monoxide</a> (<a rel="mw:WikiLink" href="./Carbon" data-parsoid='{"a":{"href":"./Carbon"},"sa":{"href":"Carbon"},"stx":"piped"}'>C</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Cobalt(II)_oxide" data-parsoid='{"a":{"href":"./Cobalt(II)_oxide"},"sa":{"href":"Cobalt(II) oxide"},"stx":"simple"}'>Cobalt(II) oxide</a> (<a rel="mw:WikiLink" href="./Cobalt" data-parsoid='{"a":{"href":"./Cobalt"},"sa":{"href":"Cobalt"},"stx":"piped"}'>Co</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Copper(II)_oxide" data-parsoid='{"a":{"href":"./Copper(II)_oxide"},"sa":{"href":"Copper(II) oxide"},"stx":"simple"}'>Copper(II) oxide</a> (<a rel="mw:WikiLink" href="./Copper" data-parsoid='{"a":{"href":"./Copper"},"sa":{"href":"Copper"},"stx":"piped"}'>Cu</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Iron(II)_oxide" data-parsoid='{"a":{"href":"./Iron(II)_oxide"},"sa":{"href":"Iron(II) oxide"},"stx":"simple"}'>Iron(II) oxide</a> (<a rel="mw:WikiLink" href="./Iron" data-parsoid='{"a":{"href":"./Iron"},"sa":{"href":"Iron"},"stx":"piped"}'>Fe</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Lead(II)_oxide" data-parsoid='{"a":{"href":"./Lead(II)_oxide"},"sa":{"href":"Lead(II) oxide"},"stx":"simple"}'>Lead(II) oxide</a> (<a rel="mw:WikiLink" href="./Lead" data-parsoid='{"a":{"href":"./Lead"},"sa":{"href":"Lead"},"stx":"piped"}'>Pb</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Magnesium_oxide" data-parsoid='{"a":{"href":"./Magnesium_oxide"},"sa":{"href":"Magnesium oxide"},"stx":"simple"}'>Magnesium oxide</a> (<a rel="mw:WikiLink" href="./Magnesium" data-parsoid='{"a":{"href":"./Magnesium"},"sa":{"href":"Magnesium"},"stx":"piped"}'>Mg</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Mercury(II)_oxide" data-parsoid='{"a":{"href":"./Mercury(II)_oxide"},"sa":{"href":"Mercury(II) oxide"},"stx":"simple"}'>Mercury(II) oxide</a> (<a rel="mw:WikiLink" href="./Mercury_(element)" data-parsoid='{"a":{"href":"./Mercury_(element)"},"sa":{"href":"Mercury (element)"},"stx":"piped"}'>Hg</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Nickel(II)_oxide" data-parsoid='{"a":{"href":"./Nickel(II)_oxide"},"sa":{"href":"Nickel(II) oxide"},"stx":"simple"}'>Nickel(II) oxide</a> (<a rel="mw:WikiLink" href="./Nickel" data-parsoid='{"a":{"href":"./Nickel"},"sa":{"href":"Nickel"},"stx":"piped"}'>Ni</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Nitric_oxide" data-parsoid='{"a":{"href":"./Nitric_oxide"},"sa":{"href":"Nitric oxide"},"stx":"simple"}'>Nitric oxide</a> (<a rel="mw:WikiLink" href="./Nitrogen" data-parsoid='{"a":{"href":"./Nitrogen"},"sa":{"href":"Nitrogen"},"stx":"piped"}'>N</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Palladium(II)_oxide" data-parsoid='{"a":{"href":"./Palladium(II)_oxide"},"sa":{"href":"Palladium(II) oxide"},"stx":"simple"}'>Palladium(II) oxide</a> (<a rel="mw:WikiLink" href="./Paladium" data-parsoid='{"a":{"href":"./Paladium"},"sa":{"href":"Paladium"},"stx":"piped"}'>Pd</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Strontium_oxide" data-parsoid='{"a":{"href":"./Strontium_oxide"},"sa":{"href":"Strontium oxide"},"stx":"simple"}'>Strontium oxide</a> (<a rel="mw:WikiLink" href="./Strontium" data-parsoid='{"a":{"href":"./Strontium"},"sa":{"href":"Strontium"},"stx":"piped"}'>Sr</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Sulfur_monoxide" data-parsoid='{"a":{"href":"./Sulfur_monoxide"},"sa":{"href":"Sulfur monoxide"},"stx":"simple"}'>Sulfur monoxide</a> (<a rel="mw:WikiLink" href="./Sulfur" data-parsoid='{"a":{"href":"./Sulfur"},"sa":{"href":"Sulfur"},"stx":"piped"}'>S</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Disulfur_dioxide" data-parsoid='{"a":{"href":"./Disulfur_dioxide"},"sa":{"href":"Disulfur dioxide"},"stx":"simple"}'>Disulfur dioxide</a> (<a rel="mw:WikiLink" href="./Sulfur" data-parsoid='{"a":{"href":"./Sulfur"},"sa":{"href":"Sulfur"},"stx":"piped"}'>S</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Tin(II)_oxide" data-parsoid='{"a":{"href":"./Tin(II)_oxide"},"sa":{"href":"Tin(II) oxide"},"stx":"simple"}'>Tin(II) oxide</a> (<a rel="mw:WikiLink" href="./Tin" data-parsoid='{"a":{"href":"./Tin"},"sa":{"href":"Tin"},"stx":"piped"}'>Sn</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Titanium(II)_oxide" data-parsoid='{"a":{"href":"./Titanium(II)_oxide"},"sa":{"href":"Titanium(II) oxide"},"stx":"simple"}'>Titanium(II) oxide</a> (<a rel="mw:WikiLink" href="./Titanium" data-parsoid='{"a":{"href":"./Titanium"},"sa":{"href":"Titanium"},"stx":"piped"}'>Ti</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Vanadium(II)_oxide" data-parsoid='{"a":{"href":"./Vanadium(II)_oxide"},"sa":{"href":"Vanadium(II) oxide"},"stx":"simple"}'>Vanadium(II) oxide</a> (<a rel="mw:WikiLink" href="./Vanadium" data-parsoid='{"a":{"href":"./Vanadium"},"sa":{"href":"Vanadium"},"stx":"piped"}'>V</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>) <a rel="mw:WikiLink" href="./Zinc_oxide" data-parsoid='{"a":{"href":"./Zinc_oxide"},"sa":{"href":"Zinc oxide"},"stx":"simple"}'>Zinc oxide</a> (<a rel="mw:WikiLink" href="./Zinc" data-parsoid='{"a":{"href":"./Zinc"},"sa":{"href":"Zinc"},"stx":"piped"}'>Zn</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>)

+3 Oxidation State	<a rel="mw:WikiLink" href="./Aluminium_oxide" data-parsoid='{"a":{"href":"./Aluminium_oxide"},"sa":{"href":"Aluminium oxide"},"stx":"simple"}'>Aluminium oxide</a> (<a rel="mw:WikiLink" href="./Aluminium" data-parsoid='{"a":{"href":"./Aluminium"},"sa":{"href":"Aluminium"},"stx":"piped"}'>Al</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Antimony_trioxide" data-parsoid='{"a":{"href":"./Antimony_trioxide"},"sa":{"href":"Antimony trioxide"},"stx":"simple"}'>Antimony trioxide</a> (<a rel="mw:WikiLink" href="./Antimony" data-parsoid='{"a":{"href":"./Antimony"},"sa":{"href":"Antimony"},"stx":"piped"}'>Sb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Arsenic_trioxide" data-parsoid='{"a":{"href":"./Arsenic_trioxide"},"sa":{"href":"Arsenic trioxide"},"stx":"simple"}'>Arsenic trioxide</a> (<a rel="mw:WikiLink" href="./Arsenic" data-parsoid='{"a":{"href":"./Arsenic"},"sa":{"href":"Arsenic"},"stx":"piped"}'>As</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Bismuth_trioxide" data-parsoid='{"a":{"href":"./Bismuth_trioxide"},"sa":{"href":"Bismuth trioxide"},"stx":"simple"}'>Bismuth trioxide</a> (<a rel="mw:WikiLink" href="./Bismuth" data-parsoid='{"a":{"href":"./Bismuth"},"sa":{"href":"Bismuth"},"stx":"piped"}'>Bi</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Boron_oxide" data-parsoid='{"a":{"href":"./Boron_oxide"},"sa":{"href":"Boron oxide"},"stx":"simple"}'>Boron oxide</a> (<a rel="mw:WikiLink" href="./Boron" data-parsoid='{"a":{"href":"./Boron"},"sa":{"href":"Boron"},"stx":"piped"}'>B</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Chromium(III)_oxide" data-parsoid='{"a":{"href":"./Chromium(III)_oxide"},"sa":{"href":"Chromium(III) oxide"},"stx":"simple"}'>Chromium(III) oxide</a> (<a rel="mw:WikiLink" href="./Chromium" data-parsoid='{"a":{"href":"./Chromium"},"sa":{"href":"Chromium"},"stx":"piped"}'>Cr</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Dinitrogen_trioxide" data-parsoid='{"a":{"href":"./Dinitrogen_trioxide"},"sa":{"href":"Dinitrogen trioxide"},"stx":"simple"}'>Dinitrogen trioxide</a> (<a rel="mw:WikiLink" href="./Nitrogen" data-parsoid='{"a":{"href":"./Nitrogen"},"sa":{"href":"Nitrogen"},"stx":"piped"}'>N</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Erbium(III)_oxide" data-parsoid='{"a":{"href":"./Erbium(III)_oxide"},"sa":{"href":"Erbium(III) oxide"},"stx":"simple"}'>Erbium(III) oxide</a> (<a rel="mw:WikiLink" href="./Erbium" data-parsoid='{"a":{"href":"./Erbium"},"sa":{"href":"Erbium"},"stx":"piped"}'>Er</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Gadolinium(III)_oxide" data-parsoid='{"a":{"href":"./Gadolinium(III)_oxide"},"sa":{"href":"Gadolinium(III) oxide"},"stx":"simple"}'>Gadolinium(III) oxide</a> (<a rel="mw:WikiLink" href="./Gadolinium" data-parsoid='{"a":{"href":"./Gadolinium"},"sa":{"href":"Gadolinium"},"stx":"piped"}'>Gd</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Gallium(III)_oxide" data-parsoid='{"a":{"href":"./Gallium(III)_oxide"},"sa":{"href":"Gallium(III) oxide"},"stx":"simple"}'>Gallium(III) oxide</a> (<a rel="mw:WikiLink" href="./Gallium" data-parsoid='{"a":{"href":"./Gallium"},"sa":{"href":"Gallium"},"stx":"piped"}'>Ga</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Holmium(III)_oxide" data-parsoid='{"a":{"href":"./Holmium(III)_oxide"},"sa":{"href":"Holmium(III) oxide"},"stx":"simple"}'>Holmium(III) oxide</a> (<a rel="mw:WikiLink" href="./Holmium" data-parsoid='{"a":{"href":"./Holmium"},"sa":{"href":"Holmium"},"stx":"piped"}'>Ho</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Indium(III)_oxide" data-parsoid='{"a":{"href":"./Indium(III)_oxide"},"sa":{"href":"Indium(III) oxide"},"stx":"simple"}'>Indium(III) oxide</a> (<a rel="mw:WikiLink" href="./Indium" data-parsoid='{"a":{"href":"./Indium"},"sa":{"href":"Indium"},"stx":"piped"}'>In</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Iron(III)_oxide" data-parsoid='{"a":{"href":"./Iron(III)_oxide"},"sa":{"href":"Iron(III) oxide"},"stx":"simple"}'>Iron(III) oxide</a> (<a rel="mw:WikiLink" href="./Iron" data-parsoid='{"a":{"href":"./Iron"},"sa":{"href":"Iron"},"stx":"piped"}'>Fe</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Lanthanum(III)_oxide" data-parsoid='{"a":{"href":"./Lanthanum(III)_oxide"},"sa":{"href":"Lanthanum(III) oxide"},"stx":"simple"}'>Lanthanum(III) oxide</a> (<a rel="mw:WikiLink" href="./Lanthanum" data-parsoid='{"a":{"href":"./Lanthanum"},"sa":{"href":"Lanthanum"},"stx":"piped"}'>La</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Lutetium(III)_oxide" data-parsoid='{"a":{"href":"./Lutetium(III)_oxide"},"sa":{"href":"Lutetium(III) oxide"},"stx":"simple"}'>Lutetium(III) oxide</a> (<a rel="mw:WikiLink" href="./Lutetium" data-parsoid='{"a":{"href":"./Lutetium"},"sa":{"href":"Lutetium"},"stx":"piped"}'>Lu</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Nickel(III)_oxide" data-parsoid='{"a":{"href":"./Nickel(III)_oxide"},"sa":{"href":"Nickel(III) oxide"},"stx":"simple"}'>Nickel(III) oxide</a> (<a rel="mw:WikiLink" href="./Nickel" data-parsoid='{"a":{"href":"./Nickel"},"sa":{"href":"Nickel"},"stx":"piped"}'>Ni</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Phosphorus_trioxide" data-parsoid='{"a":{"href":"./Phosphorus_trioxide"},"sa":{"href":"Phosphorus trioxide"},"stx":"simple"}'>Phosphorus trioxide</a> (<a rel="mw:WikiLink" href="./Phosphorus" data-parsoid='{"a":{"href":"./Phosphorus"},"sa":{"href":"Phosphorus"},"stx":"piped"}'>P</a>₄<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₆) <a rel="mw:WikiLink" href="./Promethium(III)_oxide" data-parsoid='{"a":{"href":"./Promethium(III)_oxide"},"sa":{"href":"Promethium(III) oxide"},"stx":"simple"}'>Promethium(III) oxide</a> (<a rel="mw:WikiLink" href="./Promethium" data-parsoid='{"a":{"href":"./Promethium"},"sa":{"href":"Promethium"},"stx":"piped"}'>Pm</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Rhodium(III)_oxide" data-parsoid='{"a":{"href":"./Rhodium(III)_oxide"},"sa":{"href":"Rhodium(III) oxide"},"stx":"simple"}'>Rhodium(III) oxide</a> (<a rel="mw:WikiLink" href="./Rhodium" data-parsoid='{"a":{"href":"./Rhodium"},"sa":{"href":"Rhodium"},"stx":"piped"}'>Rh</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Samarium(III)_oxide" data-parsoid='{"a":{"href":"./Samarium(III)_oxide"},"sa":{"href":"Samarium(III) oxide"},"stx":"simple"}'>Samarium(III) oxide</a> (<a rel="mw:WikiLink" href="./Samarium" data-parsoid='{"a":{"href":"./Samarium"},"sa":{"href":"Samarium"},"stx":"piped"}'>Sm</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Scandium(III)_oxide" data-parsoid='{"a":{"href":"./Scandium(III)_oxide"},"sa":{"href":"Scandium(III) oxide"},"stx":"simple"}'>Scandium(III) oxide</a> (<a rel="mw:WikiLink" href="./Scandium" data-parsoid='{"a":{"href":"./Scandium"},"sa":{"href":"Scandium"},"stx":"piped"}'>Sc</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Terbium(III)_oxide" data-parsoid='{"a":{"href":"./Terbium(III)_oxide"},"sa":{"href":"Terbium(III) oxide"},"stx":"simple"}'>Terbium(III) oxide</a> (<a rel="mw:WikiLink" href="./Terbium" data-parsoid='{"a":{"href":"./Terbium"},"sa":{"href":"Terbium"},"stx":"piped"}'>Tb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Thallium(III)_oxide" data-parsoid='{"a":{"href":"./Thallium(III)_oxide"},"sa":{"href":"Thallium(III) oxide"},"stx":"simple"}'>Thallium(III) oxide</a> (<a rel="mw:WikiLink" href="./Thallium" data-parsoid='{"a":{"href":"./Thallium"},"sa":{"href":"Thallium"},"stx":"piped"}'>Tl</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Thulium(III)_oxide" data-parsoid='{"a":{"href":"./Thulium(III)_oxide"},"sa":{"href":"Thulium(III) oxide"},"stx":"simple"}'>Thulium(III) oxide</a> (<a rel="mw:WikiLink" href="./Thulium" data-parsoid='{"a":{"href":"./Thulium"},"sa":{"href":"Thulium"},"stx":"piped"}'>Tm</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Titanium(III)_oxide" data-parsoid='{"a":{"href":"./Titanium(III)_oxide"},"sa":{"href":"Titanium(III) oxide"},"stx":"simple"}'>Titanium(III) oxide</a> (<a rel="mw:WikiLink" href="./Titanium" data-parsoid='{"a":{"href":"./Titanium"},"sa":{"href":"Titanium"},"stx":"piped"}'>Ti</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Tungsten(III)_oxide" data-parsoid='{"a":{"href":"./Tungsten(III)_oxide"},"sa":{"href":"Tungsten(III) oxide"},"stx":"simple"}'>Tungsten(III) oxide</a> (<a rel="mw:WikiLink" href="./Tungsten" data-parsoid='{"a":{"href":"./Tungsten"},"sa":{"href":"Tungsten"},"stx":"piped"}'>W</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Vanadium(III)_oxide" data-parsoid='{"a":{"href":"./Vanadium(III)_oxide"},"sa":{"href":"Vanadium(III) oxide"},"stx":"simple"}'>Vanadium(III) oxide</a> (<a rel="mw:WikiLink" href="./Vanadium" data-parsoid='{"a":{"href":"./Vanadium"},"sa":{"href":"Vanadium"},"stx":"piped"}'>V</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Ytterbium(III)_oxide" data-parsoid='{"a":{"href":"./Ytterbium(III)_oxide"},"sa":{"href":"Ytterbium(III) oxide"},"stx":"simple"}'>Ytterbium(III) oxide</a> (<a rel="mw:WikiLink" href="./Ytterbium" data-parsoid='{"a":{"href":"./Ytterbium"},"sa":{"href":"Ytterbium"},"stx":"piped"}'>Yb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Yttrium(III)_oxide" data-parsoid='{"a":{"href":"./Yttrium(III)_oxide"},"sa":{"href":"Yttrium(III) oxide"},"stx":"simple"}'>Yttrium(III) oxide</a> (<a rel="mw:WikiLink" href="./Yttrium" data-parsoid='{"a":{"href":"./Yttrium"},"sa":{"href":"Yttrium"},"stx":"piped"}'>Y</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃)

+4 Oxidation State	<a rel="mw:WikiLink" href="./Carbon_dioxide" data-parsoid='{"a":{"href":"./Carbon_dioxide"},"sa":{"href":"Carbon dioxide"},"stx":"simple"}'>Carbon dioxide</a> (<a rel="mw:WikiLink" href="./Carbon" data-parsoid='{"a":{"href":"./Carbon"},"sa":{"href":"Carbon"},"stx":"piped"}'>C</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Carbon_trioxide" data-parsoid='{"a":{"href":"./Carbon_trioxide"},"sa":{"href":"Carbon trioxide"},"stx":"simple"}'>Carbon trioxide</a> (<a rel="mw:WikiLink" href="./Carbon" data-parsoid='{"a":{"href":"./Carbon"},"sa":{"href":"Carbon"},"stx":"piped"}'>C</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Cerium(IV)_oxide" data-parsoid='{"a":{"href":"./Cerium(IV)_oxide"},"sa":{"href":"Cerium(IV) oxide"},"stx":"simple"}'>Cerium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Cerium" data-parsoid='{"a":{"href":"./Cerium"},"sa":{"href":"Cerium"},"stx":"piped"}'>Ce</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Chlorine_dioxide" data-parsoid='{"a":{"href":"./Chlorine_dioxide"},"sa":{"href":"Chlorine dioxide"},"stx":"simple"}'>Chlorine dioxide</a> (<a rel="mw:WikiLink" href="./Chlorine" data-parsoid='{"a":{"href":"./Chlorine"},"sa":{"href":"Chlorine"},"stx":"piped"}'>Cl</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Chromium(IV)_oxide" data-parsoid='{"a":{"href":"./Chromium(IV)_oxide"},"sa":{"href":"Chromium(IV) oxide"},"stx":"simple"}'>Chromium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Chromium" data-parsoid='{"a":{"href":"./Chromium"},"sa":{"href":"Chromium"},"stx":"piped"}'>Cr</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Dinitrogen_tetroxide" data-parsoid='{"a":{"href":"./Dinitrogen_tetroxide"},"sa":{"href":"Dinitrogen tetroxide"},"stx":"simple"}'>Dinitrogen tetroxide</a> (<a rel="mw:WikiLink" href="./Nitrogen" data-parsoid='{"a":{"href":"./Nitrogen"},"sa":{"href":"Nitrogen"},"stx":"piped"}'>N</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Germanium_dioxide" data-parsoid='{"a":{"href":"./Germanium_dioxide"},"sa":{"href":"Germanium dioxide"},"stx":"simple"}'>Germanium dioxide</a> (<a rel="mw:WikiLink" href="./Germanium" data-parsoid='{"a":{"href":"./Germanium"},"sa":{"href":"Germanium"},"stx":"piped"}'>Ge</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Hafnium(IV)_oxide" data-parsoid='{"a":{"href":"./Hafnium(IV)_oxide"},"sa":{"href":"Hafnium(IV) oxide"},"stx":"simple"}'>Hafnium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Hafnium" data-parsoid='{"a":{"href":"./Hafnium"},"sa":{"href":"Hafnium"},"stx":"piped"}'>Hf</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Lead(IV)_oxide" data-parsoid='{"a":{"href":"./Lead(IV)_oxide"},"sa":{"href":"Lead(IV) oxide"},"stx":"simple"}'>Lead(IV) oxide</a> (<a rel="mw:WikiLink" href="./Lead" data-parsoid='{"a":{"href":"./Lead"},"sa":{"href":"Lead"},"stx":"piped"}'>Pb</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Manganese(IV)_oxide" data-parsoid='{"a":{"href":"./Manganese(IV)_oxide"},"sa":{"href":"Manganese(IV) oxide"},"stx":"simple"}'>Manganese(IV) oxide</a> (<a rel="mw:WikiLink" href="./Manganese" data-parsoid='{"a":{"href":"./Manganese"},"sa":{"href":"Manganese"},"stx":"piped"}'>Mn</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Nitrogen_dioxide" data-parsoid='{"a":{"href":"./Nitrogen_dioxide"},"sa":{"href":"Nitrogen dioxide"},"stx":"simple"}'>Nitrogen dioxide</a> (<a rel="mw:WikiLink" href="./Nitrogen" data-parsoid='{"a":{"href":"./Nitrogen"},"sa":{"href":"Nitrogen"},"stx":"piped"}'>N</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Plutonium_dioxide" data-parsoid='{"a":{"href":"./Plutonium_dioxide"},"sa":{"href":"Plutonium dioxide"},"stx":"simple"}'>Plutonium dioxide</a> (<a rel="mw:WikiLink" href="./Plutonium" data-parsoid='{"a":{"href":"./Plutonium"},"sa":{"href":"Plutonium"},"stx":"piped"}'>Pu</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Rhodium(IV)_oxide" data-parsoid='{"a":{"href":"./Rhodium(IV)_oxide"},"sa":{"href":"Rhodium(IV) oxide"},"stx":"simple"}'>Rhodium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Rhodium" data-parsoid='{"a":{"href":"./Rhodium"},"sa":{"href":"Rhodium"},"stx":"piped"}'>Rh</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Ruthenium(IV)_oxide" data-parsoid='{"a":{"href":"./Ruthenium(IV)_oxide"},"sa":{"href":"Ruthenium(IV) oxide"},"stx":"simple"}'>Ruthenium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Ruthenium" data-parsoid='{"a":{"href":"./Ruthenium"},"sa":{"href":"Ruthenium"},"stx":"piped"}'>Ru</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Selenium_dioxide" data-parsoid='{"a":{"href":"./Selenium_dioxide"},"sa":{"href":"Selenium dioxide"},"stx":"simple"}'>Selenium dioxide</a> (<a rel="mw:WikiLink" href="./Selenium" data-parsoid='{"a":{"href":"./Selenium"},"sa":{"href":"Selenium"},"stx":"piped"}'>Se</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Silicon_dioxide" data-parsoid='{"a":{"href":"./Silicon_dioxide"},"sa":{"href":"Silicon dioxide"},"stx":"simple"}'>Silicon dioxide</a> (<a rel="mw:WikiLink" href="./Silicon" data-parsoid='{"a":{"href":"./Silicon"},"sa":{"href":"Silicon"},"stx":"piped"}'>Si</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Sulfur_dioxide" data-parsoid='{"a":{"href":"./Sulfur_dioxide"},"sa":{"href":"Sulfur dioxide"},"stx":"simple"}'>Sulfur dioxide</a> (<a rel="mw:WikiLink" href="./Sulfur" data-parsoid='{"a":{"href":"./Sulfur"},"sa":{"href":"Sulfur"},"stx":"piped"}'>S</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Tellurium_dioxide" data-parsoid='{"a":{"href":"./Tellurium_dioxide"},"sa":{"href":"Tellurium dioxide"},"stx":"simple"}'>Tellurium dioxide</a> (<a rel="mw:WikiLink" href="./Tellurium" data-parsoid='{"a":{"href":"./Tellurium"},"sa":{"href":"Tellurium"},"stx":"piped"}'>Te</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Thorium_dioxide" data-parsoid='{"a":{"href":"./Thorium_dioxide"},"sa":{"href":"Thorium dioxide"},"stx":"simple"}'>Thorium dioxide</a> (<a rel="mw:WikiLink" href="./Thorium" data-parsoid='{"a":{"href":"./Thorium"},"sa":{"href":"Thorium"},"stx":"piped"}'>Th</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Tin_dioxide" data-parsoid='{"a":{"href":"./Tin_dioxide"},"sa":{"href":"Tin dioxide"},"stx":"simple"}'>Tin dioxide</a> (<a rel="mw:WikiLink" href="./Tin" data-parsoid='{"a":{"href":"./Tin"},"sa":{"href":"Tin"},"stx":"piped"}'>Sn</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Titanium_dioxide" data-parsoid='{"a":{"href":"./Titanium_dioxide"},"sa":{"href":"Titanium dioxide"},"stx":"simple"}'>Titanium dioxide</a> (<a rel="mw:WikiLink" href="./Titanium" data-parsoid='{"a":{"href":"./Titanium"},"sa":{"href":"Titanium"},"stx":"piped"}'>Ti</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Tungsten(IV)_oxide" data-parsoid='{"a":{"href":"./Tungsten(IV)_oxide"},"sa":{"href":"Tungsten(IV) oxide"},"stx":"simple"}'>Tungsten(IV) oxide</a> (<a rel="mw:WikiLink" href="./Tungsten" data-parsoid='{"a":{"href":"./Tungsten"},"sa":{"href":"Tungsten"},"stx":"piped"}'>W</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Uranium_dioxide" data-parsoid='{"a":{"href":"./Uranium_dioxide"},"sa":{"href":"Uranium dioxide"},"stx":"simple"}'>Uranium dioxide</a> (<a rel="mw:WikiLink" href="./Uranium" data-parsoid='{"a":{"href":"./Uranium"},"sa":{"href":"Uranium"},"stx":"piped"}'>U</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Vanadium(IV)_oxide" data-parsoid='{"a":{"href":"./Vanadium(IV)_oxide"},"sa":{"href":"Vanadium(IV) oxide"},"stx":"simple"}'>Vanadium(IV) oxide</a> (<a rel="mw:WikiLink" href="./Vanadium" data-parsoid='{"a":{"href":"./Vanadium"},"sa":{"href":"Vanadium"},"stx":"piped"}'>V</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂) <a rel="mw:WikiLink" href="./Zirconium_dioxide" data-parsoid='{"a":{"href":"./Zirconium_dioxide"},"sa":{"href":"Zirconium dioxide"},"stx":"simple"}'>Zirconium dioxide</a> (<a rel="mw:WikiLink" href="./Zirconium" data-parsoid='{"a":{"href":"./Zirconium"},"sa":{"href":"Zirconium"},"stx":"piped"}'>Zr</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₂)

+5 Oxidation State	<a rel="mw:WikiLink" href="./Antimony_pentoxide" data-parsoid='{"a":{"href":"./Antimony_pentoxide"},"sa":{"href":"Antimony pentoxide"},"stx":"simple"}'>Antimony pentoxide</a> (<a rel="mw:WikiLink" href="./Antimony" data-parsoid='{"a":{"href":"./Antimony"},"sa":{"href":"Antimony"},"stx":"piped"}'>Sb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Arsenic_pentoxide" data-parsoid='{"a":{"href":"./Arsenic_pentoxide"},"sa":{"href":"Arsenic pentoxide"},"stx":"simple"}'>Arsenic pentoxide</a> (<a rel="mw:WikiLink" href="./Arsenic" data-parsoid='{"a":{"href":"./Arsenic"},"sa":{"href":"Arsenic"},"stx":"piped"}'>As</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Dinitrogen_pentoxide" data-parsoid='{"a":{"href":"./Dinitrogen_pentoxide"},"sa":{"href":"Dinitrogen pentoxide"},"stx":"simple"}'>Dinitrogen pentoxide</a> (<a rel="mw:WikiLink" href="./Nitrogen" data-parsoid='{"a":{"href":"./Nitrogen"},"sa":{"href":"Nitrogen"},"stx":"piped"}'>N</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Niobium_pentoxide" data-parsoid='{"a":{"href":"./Niobium_pentoxide"},"sa":{"href":"Niobium pentoxide"},"stx":"simple"}'>Niobium pentoxide</a> (<a rel="mw:WikiLink" href="./Niobium" data-parsoid='{"a":{"href":"./Niobium"},"sa":{"href":"Niobium"},"stx":"piped"}'>Nb</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Phosphorus_pentoxide" data-parsoid='{"a":{"href":"./Phosphorus_pentoxide"},"sa":{"href":"Phosphorus pentoxide"},"stx":"simple"}'>Phosphorus pentoxide</a> (<a rel="mw:WikiLink" href="./Phosphorus" data-parsoid='{"a":{"href":"./Phosphorus"},"sa":{"href":"Phosphorus"},"stx":"piped"}'>P</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Tantalum_pentoxide" data-parsoid='{"a":{"href":"./Tantalum_pentoxide"},"sa":{"href":"Tantalum pentoxide"},"stx":"simple"}'>Tantalum pentoxide</a> (<a rel="mw:WikiLink" href="./Tantalum" data-parsoid='{"a":{"href":"./Tantalum"},"sa":{"href":"Tantalum"},"stx":"piped"}'>Ta</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅) <a rel="mw:WikiLink" href="./Vanadium(V)_oxide" data-parsoid='{"a":{"href":"./Vanadium(V)_oxide"},"sa":{"href":"Vanadium(V) oxide"},"stx":"simple"}'>Vanadium(V) oxide</a> (<a rel="mw:WikiLink" href="./Vanadium" data-parsoid='{"a":{"href":"./Vanadium"},"sa":{"href":"Vanadium"},"stx":"piped"}'>V</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₅)

+6 Oxidation State	<a rel="mw:WikiLink" href="./Chromium_trioxide" data-parsoid='{"a":{"href":"./Chromium_trioxide"},"sa":{"href":"Chromium trioxide"},"stx":"simple"}'>Chromium trioxide</a> (<a rel="mw:WikiLink" href="./Chromium" data-parsoid='{"a":{"href":"./Chromium"},"sa":{"href":"Chromium"},"stx":"piped"}'>Cr</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Molybdenum(VI)_oxide" data-parsoid='{"a":{"href":"./Molybdenum(VI)_oxide"},"sa":{"href":"Molybdenum(VI) oxide"},"stx":"simple"}'>Molybdenum(VI) oxide</a> (<a rel="mw:WikiLink" href="./Molybdenum" data-parsoid='{"a":{"href":"./Molybdenum"},"sa":{"href":"Molybdenum"},"stx":"piped"}'>Mo</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Rhenium_trioxide" data-parsoid='{"a":{"href":"./Rhenium_trioxide"},"sa":{"href":"Rhenium trioxide"},"stx":"simple"}'>Rhenium trioxide</a> (<a rel="mw:WikiLink" href="./Rhenium" data-parsoid='{"a":{"href":"./Rhenium"},"sa":{"href":"Rhenium"},"stx":"piped"}'>Re</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Selenium_trioxide" data-parsoid='{"a":{"href":"./Selenium_trioxide"},"sa":{"href":"Selenium trioxide"},"stx":"simple"}'>Selenium trioxide</a> (<a rel="mw:WikiLink" href="./Selenium" data-parsoid='{"a":{"href":"./Selenium"},"sa":{"href":"Selenium"},"stx":"piped"}'>Se</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Sulfur_trioxide" data-parsoid='{"a":{"href":"./Sulfur_trioxide"},"sa":{"href":"Sulfur trioxide"},"stx":"simple"}'>Sulfur trioxide</a> (<a rel="mw:WikiLink" href="./Sulfur" data-parsoid='{"a":{"href":"./Sulfur"},"sa":{"href":"Sulfur"},"stx":"piped"}'>S</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Tellurium_trioxide" data-parsoid='{"a":{"href":"./Tellurium_trioxide"},"sa":{"href":"Tellurium trioxide"},"stx":"simple"}'>Tellurium trioxide</a> (<a rel="mw:WikiLink" href="./Tellurium" data-parsoid='{"a":{"href":"./Tellurium"},"sa":{"href":"Tellurium"},"stx":"piped"}'>Te</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Tungsten_trioxide" data-parsoid='{"a":{"href":"./Tungsten_trioxide"},"sa":{"href":"Tungsten trioxide"},"stx":"simple"}'>Tungsten trioxide</a> (<a rel="mw:WikiLink" href="./Tungsten" data-parsoid='{"a":{"href":"./Tungsten"},"sa":{"href":"Tungsten"},"stx":"piped"}'>W</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Uranium_trioxide" data-parsoid='{"a":{"href":"./Uranium_trioxide"},"sa":{"href":"Uranium trioxide"},"stx":"simple"}'>Uranium trioxide</a> (<a rel="mw:WikiLink" href="./Uranium" data-parsoid='{"a":{"href":"./Uranium"},"sa":{"href":"Uranium"},"stx":"piped"}'>U</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃) <a rel="mw:WikiLink" href="./Xenon_trioxide" data-parsoid='{"a":{"href":"./Xenon_trioxide"},"sa":{"href":"Xenon trioxide"},"stx":"simple"}'>Xenon trioxide</a> (<a rel="mw:WikiLink" href="./Xenon" data-parsoid='{"a":{"href":"./Xenon"},"sa":{"href":"Xenon"},"stx":"piped"}'>Xe</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₃)

+7 Oxidation State	<a rel="mw:WikiLink" href="./Dichlorine_heptoxide" data-parsoid='{"a":{"href":"./Dichlorine_heptoxide"},"sa":{"href":"Dichlorine heptoxide"},"stx":"simple"}'>Dichlorine heptoxide</a> (<a rel="mw:WikiLink" href="./Chlorine" data-parsoid='{"a":{"href":"./Chlorine"},"sa":{"href":"Chlorine"},"stx":"piped"}'>Cl</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₇) <a rel="mw:WikiLink" href="./Manganese(VII)_oxide" data-parsoid='{"a":{"href":"./Manganese(VII)_oxide"},"sa":{"href":"Manganese(VII) oxide"},"stx":"simple"}'>Manganese(VII) oxide</a> (<a rel="mw:WikiLink" href="./Manganese" data-parsoid='{"a":{"href":"./Manganese"},"sa":{"href":"Manganese"},"stx":"piped"}'>Mn</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₇) <a rel="mw:WikiLink" href="./Rhenium(VII)_oxide" data-parsoid='{"a":{"href":"./Rhenium(VII)_oxide"},"sa":{"href":"Rhenium(VII) oxide"},"stx":"simple"}'>Rhenium(VII) oxide</a> (<a rel="mw:WikiLink" href="./Rhenium" data-parsoid='{"a":{"href":"./Rhenium"},"sa":{"href":"Rhenium"},"stx":"piped"}'>Re</a>₂<a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₇) <a rel="mw:WikiLink" href="./Technetium(VII)_oxide" data-parsoid='{"a":{"href":"./Technetium(VII)_oxide"},"sa":{"href":"Technetium(VII) oxide"},"stx":"simple"}'>Technetium(VII) oxide</a>

+8 Oxidation State	<a rel="mw:WikiLink" href="./Osmium_tetroxide" data-parsoid='{"a":{"href":"./Osmium_tetroxide"},"sa":{"href":"Osmium tetroxide"},"stx":"simple"}'>Osmium tetroxide</a> (<a rel="mw:WikiLink" href="./Osmium" data-parsoid='{"a":{"href":"./Osmium"},"sa":{"href":"Osmium"},"stx":"piped"}'>Os</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Ruthenium_tetroxide" data-parsoid='{"a":{"href":"./Ruthenium_tetroxide"},"sa":{"href":"Ruthenium tetroxide"},"stx":"simple"}'>Ruthenium tetroxide</a> (<a rel="mw:WikiLink" href="./Ruthenium" data-parsoid='{"a":{"href":"./Ruthenium"},"sa":{"href":"Ruthenium"},"stx":"piped"}'>Ru</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Xenon_tetroxide" data-parsoid='{"a":{"href":"./Xenon_tetroxide"},"sa":{"href":"Xenon tetroxide"},"stx":"simple"}'>Xenon tetroxide</a> (<a rel="mw:WikiLink" href="./Xenon" data-parsoid='{"a":{"href":"./Xenon"},"sa":{"href":"Xenon"},"stx":"piped"}'>Xe</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Iridium_tetroxide" data-parsoid='{"a":{"href":"./Iridium_tetroxide"},"sa":{"href":"Iridium tetroxide"},"stx":"simple"}'>Iridium tetroxide</a> (<a rel="mw:WikiLink" href="./Iridium" data-parsoid='{"a":{"href":"./Iridium"},"sa":{"href":"Iridium"},"stx":"piped"}'>Ir</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄) <a rel="mw:WikiLink" href="./Hassium_tetroxide" data-parsoid='{"a":{"href":"./Hassium_tetroxide"},"sa":{"href":"Hassium tetroxide"},"stx":"simple"}'>Hassium tetroxide</a> (<a rel="mw:WikiLink" href="./Hassium" data-parsoid='{"a":{"href":"./Hassium"},"sa":{"href":"Hassium"},"stx":"piped"}'>Hs</a><a rel="mw:WikiLink" href="./Oxygen" data-parsoid='{"a":{"href":"./Oxygen"},"sa":{"href":"Oxygen"},"stx":"piped"}'>O</a>₄)

Related	<a rel="mw:WikiLink" href="./Oxocarbon" data-parsoid='{"a":{"href":"./Oxocarbon"},"sa":{"href":"Oxocarbon"},"stx":"simple"}'>Oxocarbon</a> <a rel="mw:WikiLink" href="./Suboxide" data-parsoid='{"a":{"href":"./Suboxide"},"sa":{"href":"Suboxide"},"stx":"simple"}'>Suboxide</a> <a rel="mw:WikiLink" href="./Oxyanion" data-parsoid='{"a":{"href":"./Oxyanion"},"sa":{"href":"Oxyanion"},"stx":"simple"}'>Oxyanion</a> <a rel="mw:WikiLink" href="./Ozonide" data-parsoid='{"a":{"href":"./Ozonide"},"sa":{"href":"Ozonide"},"stx":"simple"}'>Ozonide</a>

Oxides are sorted by <a rel="mw:WikiLink" href="./Oxidation_state" data-parsoid='{"a":{"href":"./Oxidation_state"},"sa":{"href":"oxidation state"},"stx":"simple"}'>oxidation state</a>. <a rel="mw:WikiLink" href="./Category:Oxides" data-parsoid='{"a":{"href":"./Category:Oxides"},"sa":{"href":":Category:Oxides"},"stx":"simple"}'>Category:Oxides</a>

Revision as of 12:08, 14 June 2013

Some general rules for determining oxidation states without use of Lewis structures

Oxidation state and formal charge

Calculation of formal oxidation states with a Lewis structure

The Lewis structure

Inequivalent atoms of an element

Redox reactions

Elements with multiple oxidation states

Fractional oxidation states

Oxygen

Oxidation number

History

Unusual formal oxidation states

See also

References