- Source: Acidic oxide
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. 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.
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.
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
Carbonic 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
= Aluminium oxide
=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
=Silicon dioxide is an acidic oxide. It will react with strong bases to form silicate salts.
Silicon dioxide is the anhydride of silicic acid:
H4SiO4 → 2 H2O + SiO2
= Phosphorus oxides
=Phosphorus(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
=Sulfur 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
=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
=Iron(II) oxide is the anhydride of the aqueous ferrous ion:
[Fe(H2O)6]2+ → FeO + 2 H+ + 5 H2O
= Chromium oxides
=Chromium trioxide is the anhydride of chromic acid:
H2CrO4 → H2O + CrO3
= Vanadium oxides
=Vanadium trioxide is the anhydride of vanadous acid:
2H3VO3 → 3H2O + V2O3
Vanadium pentoxide is the anhydride of vanadic acid:
2H3VO4 → 3H2O + V2O5
See also
Organic acid anhydride, similar compounds in organic chemistry
Base anhydride
References
Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
Kata Kunci Pencarian:
- Asam asetat
- Eniya Listiani
- Metaloid
- Peningkatan keasaman air laut
- Daftar nomor UN 3201 sampai 3300
- Letusan dan tsunami Hunga Tonga 2022
- Acidic oxide
- Basic oxide
- Beta oxidation
- Sulfur dioxide
- Phosphorus pentoxide
- Lead dioxide
- Nitric acid
- NOx
- Nitrous oxide
- Ethylene oxide
