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Not to be confused with keto acids or oxo carboxylic acids, which are sometimes called oxy acids.

An oxo-acid is an acid that contains oxygen. To be more specific, it is a compound that contains hydrogen, oxygen, and at least one other element, with at least one hydrogen atom bound to oxygen that can dissociate to produce the H+ cation and the anion of the acid.[1]


Generally, oxy-acids are simply polyatomic anions attached to a positively polarized hydrogen, which can be split off as a cation(ion).

Under Lavoisier's original theory, all acids contained oxygen, which was named from the Greek ὀξύς (oxys) (acid, sharp) and the root –γενής (–genes) (engender). It was later discovered that some acids, notably hydrochloric acid, did not contain oxygen and so acids were divided into oxoacids and these new hydracids.

All oxy-acids have the acidic hydrogen bound to an oxygen atom, so bond strength (length) is not a factor, as it is with binary nonmetal hydrides. Rather, the electronegativity of the central atom (E) and the number of O atoms determine oxy-acid acidity. With the same "central atom" E to which the O is attached, acid strength increases as the number of oxygen attached to E increases. With the same number of oxygens around E, acid strength increases with the electronegativity of E.

Imidic acids are created by replacing =O with =NR in an oxoacid.[2]


An oxy-acid molecule contains the structure M-O-H, where other atoms or atom groups can be connected to the central atom M. In a solution, such a molecule can be dissociated to ions in two distinct ways:

  • M-O-H <=> (M-O) + H+
  • M-O-H <=> (M)+ + OH[3]

If the central atom M is strongly electronegative, then it attracts strongly the electrons of the oxygen atom. In that case, the bond between the oxygen and hydrogen atom is weak, and the compound ionizes easily in the way of the former of the two chemical equations above. In this case, the compound MOH is thus an acid, because it releases a proton, that is, a hydrogen ion. For example, nitrogen, sulfur and chlorine are strongly electronegative elements, and therefore nitric acid, sulfuric acid, and perchloric acid, are strong acids.

If, however, the electronegativity of M is weak, then the compound is dissociated to ions according to the latter chemical equation, and MOH is an alkaline hydroxide. Examples of such compounds are sodium hydroxide NaOH and calcium hydroxide Ca(OH)2.[3] If the electronegativity of M is somewhere in between, the compound can even be amphoteric, and in that case, it can dissociate to ions in both ways, in the former case when reacting with bases, and in the latter case when reacting with acids.[3]

Inorganic oxy-acids typically have a chemical formula of type HmXOn, where X is some atom functioning as a central atom, whereas parameters m and n depend on the oxidation state of the element X. In most cases, the element X is a nonmetal, but even some metals, for example chromium and manganese, can form oxy-acids when occurring at their highest oxidation state.[3]

When oxy-acids are heated, many of them dissociate to water and the anhydride of the acid. In most cases, such anhydrides are oxides of nonmetals. For example, carbon dioxide, CO2, is the anhydride of carbonic acid, H2CO3, and sulfur trioxide, SO3, is the anhydride of sulfuric acid, H2SO4. These anhydrides react quickly with water and form those oxy-acids again.[4]

Many organic acids, like carboxylic acids and phenols, are oxy-acids.[3] Their molecular structure, however, is much more cumbersome than that of inorganic oxy-acids.

Most acids are oxoacids.[3] Indeed, in the 18th century, Lavoisier assumed that all acids contain oxygen and that oxygen causes their acidity. Because of this, he gave to this element its name, oxygenium, derived from Greek and meaning sharp-maker, which is still, in a more or less modified form, used in most languages.[5] Later, however, Humphry Davy showed that the so-called muriatic acid did not contain oxygen, despite its being a strong acid; instead, it is a solution of hydrogen chloride, HCl.[6] Such acids which do not contain oxygen are nowadays known as hydracids.

Names of inorganic oxoacids[edit]

Many inorganic oxoacids are traditionally called with names ending with the word acid and which also contain, in a somewhat modified form, the name of the element they contain in addition to hydrogen and oxygen. Well-known examples of such acids are sulfuric acid, nitric acid and phosphoric acid.

This practice is fully well-established, and even IUPAC has accepted such names. In light of the current chemical nomenclature, this practice is, however, very exceptional, because systematic names of all other compounds are formed only according to what elements they contain and what is their molecular structure, not according to what other properties (for example, acidity) they have.[7]

IUPAC, however, does not recommend to call future compounds not yet discovered with a name ending with the word acid.[7] Indeed, acids can even be called with names formed by adding the word hydrogen in front of the corresponding anion; for example, sulfuric acid could just as well be called hydrogen sulfate (or dihydrogen sulfate).[8] In fact, the fully systematic name of sulfuric acid, according to IUPAC's rules, would be dihydroxidodioxidosulfur and that of the sulfate ion, tetraoxidosulfate(2-),[9] Such names, however, are almost never used.

However, the same element can form more than one acid when compounded with hydrogen and oxygen. In such cases, the English practice to distinguish such acids is to use the suffix -ic in the name of the element in the name of the acid containing more oxygen atoms, and the suffix -ous in the name of the element in the name of the acid containing fewe oxygen atoms. Thus, for example, sulfuric acid is H2SO4, and sulfurous acid, H2SO3. Analogously, nitric acid is HNO3, and nitrous acid, HNO2. If there are more than two oxoacids having the same element as the central atom, then, in some cases, acids are distinguished by adding the prefix per- or hypo- to their names. The prefix per-, however, is used only when the central atom is a halogen or a group 7 element.[8] For example, chlorine has the four following oxoacids:

The suffix -ite occurs in names of anions and salts derived from acids whose names end to the suffix -ous. On the other hand, the suffix -ate occurs in names of anions and salts derived from acids whose names end to the suffix -ic. Prefixes hypo- and per- occur even in name of anions and salts; for example the ion ClO4 is called perchlorate.[8]

In a few cases, even prefixes ortho- and para- occur in names of some oxoacids and their derivative anions. In such cases, the para acid is what can be thought as remaining of the ortho acid if a water molecule is separated from the ortho acid molecule. For example, phosphoric acid,H3PO4, has sometimes even be called as orthophosphoric acid, in order to distinguish it from metaphosphoric acid, HPO3.[8] However, according to IUPAC' s current rules, the prefix ortho- should only be used in names of orthotelluric acid and orthoperiodic acid, and their corresponding anions and salts.[10]


In the following table, the formula and the name of the anion refer to what remains of the acid when it cedes all hydrogen atoms as protons. Many of these acids, however, are polyprotic, and in such cases, there exists also one or more intermediate anions. In name of such anions, the prefix hydro-, is added if needed, with some numeral prefixes. For example, SO42− is the sulfate anion, and HSO4, the hydrosulfate anion. In a similar way, PO43− is the phosphate, H2PO42−, the dihydrophosphate, and HPO4, the hydrophosphate ion.

Element group Element (central atom) Formula of the acid Name of the acid[8][9] Formula of the corresponding anion Name of the anion
6 Chromium H2CrO4 Chromic acid CrO42− Chromate
H2Cr2O7 Dichromic acid Cr2O72− Dichromate
7 Manganese HMnO4 Permanganic acid MnO4 Permanganate
HMnO3 Manganic acid MnO3 Manganate
Technetium HTcO4 Pertechnetic acid TcO4 Pertechnetate
HTcO3 Technetic acid TcO3 Technetate
Rhenium HReO4 Perrhenic acid ReO4 Perrhenate
HReO3 Rhenic acid ReO3 Rhenate
13 Boron H3BO3 Boric acid
(formerly orthoboric acid)[10]
BO33− Borate
(formerly orthoborate)
(HBO2)n Metaboric acid BO2 Metaborate
14 Carbon H2CO3 Carbonic acid CO32− Carbonate
Silicon H4SiO4 Silicic acid
(formerly. orthosilicic acid)[10]
SiO44− Silicate (formerly orthosilicate)
H2SiO3 Metasilicic acid SiO32− Metasilicate
14, 15 Carbon, nitrogen HOCN Cyanic acid OCN Cyanate
HNCO Isocyanic acid NCO Isocyanate
HONC Fulminic acid ONC Fulminate
15 Nitrogen HNO3 Nitric acid NO3 Nitrate
HNO2 Nitrous acid NO2 Nitrite
HNO4 Peroxynitric acid NO4 Peroxynitrate
HOONO Peroxynitrous acid OONO Peroxynitrite
H2NO2 Nitroxylic acid NO22− Nitroxylate
H2N2O2 Hyponitrous acid N2O22− Hyponitrite
Phosphorus H3PO4 Phosphoric acid
(formerly even orthophosphoric acid)[10]
PO43− Phosphate
HPO3 Metaphosphoric acid PO3 Metaphosphate
H4P2O7 Pyrophosphoric acid
(diphosphoric acid)
P2O74− Pyrophosphate
H3PO5 Peroxomonophosphoric acid PO33− Peroxomonophosphate
(HO)2OP-PO(OH)2 Hypophosphoric acid
(diphosphoric(IV) acid)
O2OP-POO24− Hypophosphate
(HO)2P-O-PO(OH)2 Diphosphoric(III,V) acid O2-P-O-POO22− Diphosphate(III,V)
H2PHO3 Phosphonic acid PHO32− Phosphonate
H2P2H2O5 Diphosphonic acid P2H2O35− Diphosphonate
HPH2O2 Phosphinic acid PH2O2 Phosphinate
Arsenic H3AsO4 Arsenic acid AsO43− Arsenate
H3AsO3 Arsenous acid AsO33− Arsenite
16 Sulfur H2SO4 Sulfuric acid SO42− Sulfate
H2SO3 Sulfurous acid SO32− Sulfite
H2S2O7 Disulfuric acid S2O72− Disulfate
H2SO5 Peroxomonosulfuric acid SO52− Peroxomonosulfate
H2S2O8 Peroxodisulfuric acid S2O82− Peroxodisulfate
H2S2O3 Thiosulfuric acid S2O32− Thiosulfate
H2S2O6 Dithionic acid S2O62− Dithionate
H2S2O5 Disulfurous acid S2O52− Disulfite
H2S2O2 Thiosulfurous acid S2O22− Thiosulfite
H2S2O4 Dithionous acid S2O42− Dithionite
H2SO2 Sulfoxylic acid SO22− Sulfoxylate
H2SxO5 Polythionic acids


See also[edit]


  1. ^ http://goldbook.iupac.org/O04374.html
  2. ^ http://goldbook.iupac.org/I02949.html
  3. ^ a b c d e f Kivinen, Mäkitie: Kemia, p. 202-203, chapter=Happihapot
  4. ^ "Hapot". Otavan iso Fokus, Part 2 (El-Io). Otava. 1973. p. 990. ISBN 951-1-00272-4. 
  5. ^ Otavan suuri Ensyklopedia, s. 1606, art. Happi
  6. ^ Otavan suuri Ensyklopedia, s. 1605, art. Hapot ja emäxet
  7. ^ a b Red Book 2005, s. 124, chapter IR-8: Inorganic Acids and Derivatives
  8. ^ a b c d e Kivinen, Mäkitie: Kemia, p. 459-461, chapter Kemian nimistö: Hapot
  9. ^ a b Red Book 2005, p. 129-132, table IR-8-1
  10. ^ a b c d Red Book 2005, p. 132, note a

External links[edit]