An acidic oxide is an oxide that either produces an acidic solution upon addition to water, or acts as an acceptor of hydroxide ions effectively functioning as a Lewis acid.[1] Acidic oxides will typically have a low pKa and may be inorganic or organic. A commonly encountered acidic oxide, carbon dioxide produces an acidic solution (and the generation of carbonic acid) when dissolved.[2]
The acidity of an oxide can be reasonably assumed by its accompanying constituents. Less electronegative elements tend to form basic oxides such as sodium oxide and magnesium oxide, whereas more electronegative elements tend to produce acidic oxides as seen with carbon dioxide and phosphorus pentoxide. Some oxides like aluminium oxides are amphoteric.[3]
Acidic oxides are of environmental concern. Sulfur and nitrogen oxides are considered air pollutants as they react with atmospheric water vapour to produce acid rain.
Examples
editCarbonic acid is an illustrative example of the Lewis acidity of an acidic oxide.
- CO2 + 2OH− ⇌ HCO3− + OH− ⇌ CO32− + H2O
This property is a key reason for keeping alkali chemicals well sealed from the atmosphere, as long-term exposure to carbon dioxide in the air can degrade the material.
- Carbon dioxide is also the anhydride of carbonic acid:
- H2CO3 → H2O + CO2
- Chromium trioxide, which reacts with water forming chromic acid:
- CrO3 + H2O → H2CrO4
- Dinitrogen pentoxide, which reacts with water forming nitric acid:
- N2O5 + H2O → 2 HNO3
- Manganese heptoxide, which reacts with water forming permanganic acid:
- Mn2O7 + H2O → 2 HMnO4
Further examples
editAluminium oxide
editAluminium 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
editSilicon dioxide is an acidic oxide. It will react with strong bases to form silicate salts.[4]
Silicon dioxide is the anhydride of silicic acid:
- H4SiO4 → 2 H2O + SiO2
Phosphorus oxides
editPhosphorus(III) oxide reacts to form phosphorous acid in water:
- P4O6 + 6 H2O → 4 H3PO3
Phosphorus(V) oxide reacts with water to give phosphoric acid:
- P4O10 + 6 H2O → 4 H3PO4
Sulfur oxides
editSulfur dioxide reacts with water to form the weak acid, sulfurous acid:
- SO2 + H2O → H2SO3
Sulfur trioxide forms the strong acid sulfuric acid with water:
- SO3 + H2O → H2SO4
This reaction is important in the manufacturing of sulfuric acid.
Chlorine oxides
editChlorine(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
editIron(II) oxide is the anhydride of the aqueous ferrous ion:
- [Fe(H2O)6]2+ → FeO + 2 H+ + 5 H2O
Chromium oxides
editChromium trioxide is the anhydride of chromic acid:
- H2CrO4 → H2O + CrO3
Vanadium oxides
editVanadium trioxide is the anhydride of vanadous acid:
- 2H3VO3 → 3H2O + V2O3
Vanadium pentoxide is the anhydride of vanadic acid:
- 2H3VO4 → 3H2O + V2O5
See also
edit- Organic acid anhydride, similar compounds in organic chemistry
- Base anhydride
References
edit- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ John Daintith (February 2008). "acidic". A Dictionary of Chemistry.
3. Describing a compound that forms an acid when dissolved in water. Carbon dioxide, for example, is an acidic oxide.
- ^ David Oxtoby; H. P. Gillis; Alan Campion. Principles of Modern Chemistry (7th ed.). Cengage Learning. pp. 675–676. ISBN 978-0-8400-4931-5.
- ^ Chang, Raymond; Overby, Jason (2011). General chemistry: the essential concepts (6th ed.). New York, NY: McGraw-Hill. ISBN 9780073375632. OCLC 435711011.
- ^ Comprehensive Chemistry Volume 1. New Delhi, India: Laxmi Publications. 2018. p. 6.13. ISBN 978-81-318-0859-7.