Acidic oxide

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Acidic oxides, or acid anhydrides, are oxides that react with water to form an acid, or with a base to form a salt. They are oxides of either nonmetals or of metals in high oxidation states. Their chemistry can be systematically understood by taking an oxoacid and removing water from it, until only an oxide remains. The resulting oxide belongs to this group of substances. An inorganic anhydride (a somewhat archaic term) is acid anhydride without an organic moiety.

Acidic oxides are not Brønsted–Lowry acids because they do not donate protons; however, they are Arrhenius acids because they increase the hydrogen ion concentration of water. For instance, carbon dioxide increases the hydrogen ion concentration of rain water (pH = 5.6) by a factor of 25 compared to pure water (pH = 7). They are also Lewis acids, because they accept electron pairs from some Lewis bases, most notably base anhydrides.[1]

The oxides of period three elements demonstrate periodicity with respect to acidity. As you move across the period, the oxides become more acidic. Sodium and magnesium oxides are alkaline. Aluminium oxides are amphoteric (reacting both as a base or acid). Silicon, phosphorus, sulfur, and chlorine oxides are acidic.[2] Some non-metal oxides, such as nitrous oxide (N2O) and carbon monoxide (CO), do not display any acid/base characteristics.

Acidic oxides can also react with basic oxides to produce salts of oxoanions:

2 MgO + SiO2 → Mg2SiO4

Acidic oxides are environmentally relevant. Sulfur and nitrogen oxides are considered air pollutants as they react with atmospheric water vapour to produce acid rain.

Reactions of acidic oxides[edit]

Although it is difficult to classify these oxides as acids, the property is manifest in reactions with bases. For example, carbon dioxide reacts with alkali.

CO2 + OH ⇌ HCO3 + OH ⇌ CO32− + H2O

For this reason, alkali is kept in stoppered vessels to inhibit reaction with atmospheric carbon dioxide. In geochemistry complex silicates are often written as though they are the products of an acid-base reaction. For example, the chemical formula of the mineral olivine can be written either as (Mg,Fe)2SiO4 or as (MgO,FeO)2SiO2. This mineral is said to be ultramafic, meaning that it has a very high nominal content of the bases magnesium oxide and iron oxide and hence, a low content of the acid silicon dioxide.

Examples of reactions[edit]

H2CO3 –> H2O + CO2
  • The enzyme carbonic anhydrase, which catalyzes this reaction, is named after this property of carbon dioxide.

Examples[edit]

Aluminium oxide[edit]

Aluminium oxide (Al2O3) is an amphoteric oxide; it can act as a base or acid. For example with base different aluminate salts will be formed:

Al2O3 + 2 NaOH + 3 H2O → 2 NaAl(OH)4

Silicon dioxide[edit]

Silicon dioxide is a weakly acidic oxide. It will react with strong bases to form silicate salts, but not with water:

SiO2 + 2 NaOH → Na2SiO3 + H2O

Silicon dioxide is the anhydride of silicic acid: Si(OH)4 –> 2H2O + SiO2

Phosphorus oxides[edit]

Phosphorus(III) oxide reacts to form phosphorous acid in water:

P4O6 + 6 H2O → 4 H3PO3

Phosphorus(V) oxide reacts with water to give phosphoric (v) acid:

P4O10 + 6 H2O → 4 H3PO4

Phosphorus pentoxide is the anhydride of phosphoric acid: 2H3PO4 –> 3H2O + P2O5.

Sulfur oxides[edit]

Sulfur dioxide reacts with water to form the weak acid, sulfurous acid:

SO2 + H2O → H2SO3

Sulfur trioxide forms the strong sulfuric acid with water (so, sulfur trioxide is the anhydride of sulfuric acid):

SO3 + H2O → H2SO4

This reaction is important in the manufacture of the acid.

Chlorine oxides[edit]

Chlorine(I) oxide reacts with water to form hypochlorous acid, a very weak acid:

Cl2O + H2O ↔ 2 HOCl

Chlorine(VII) oxide reacts with water to form perchloric acid, a strong acid:

Cl2O7 + H2O → 2 HClO4

Iron oxides[edit]

Iron(II) oxide is the anhydride of the aqueous ferrous ion: [Fe(H2O)6]2+ --> FeO + 2H+ + 5H2O

Chromium oxides[edit]

Chromium trioxide is the anhydride of chromic acid: H2CrO4 –> H2O + CrO3

Vanadium oxides[edit]

Vanadium pentoxide is the anhydride of vanadic acid: 2H3VO4 –> 3H2O + V2O5.


See also[edit]

References[edit]

  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  1. ^ David Oxtoby; H. P. Gillis; Alan Campion. Principles of Modern Chemistry (7th ed.). Cengage Learning. pp. 675–676. ISBN 978-0-8400-4931-5.
  2. ^ Chang, Raymond; Overby, Jason (2011). General chemistry: the essential concepts (6th ed.). New York, NY: McGraw-Hill. ISBN 9780073375632. OCLC 435711011.