Acidic oxide
From Wikipedia, the free encyclopedia
Acidic oxides are inorganic chemicals that react with water to form an acid; or react with a base to form a salt. Acidic oxides are oxides of either nonmetals or of metals in high oxidation states. They are formed when a nonmetal burns. Their chemistry can be systematically understood by taking an oxoacid and removing water from it, until only the oxide is left. The resulting oxide belongs to this group of substances.
Acidic oxides are not Arrhenius acids, nor are they Brønsted–Lowry acids, since they neither accept protons, nor do they increase the hydrogen ion concentration of water. However, they are Lewis acids, since they accept electron pairs from certain Lewis bases, most notably Base anhydrides.[1]
Examples
- Carbon dioxide which reacts with water to produce carbonic acid.
- Sulfur dioxide, which does not form the non-existent sulfurous acid but does react with bases to form sulfites.
- Silicon dioxide, which does not react with water but will react with bases to form silicates
- Chromium trioxide, which reacts with water to form chromic acid. Chromic acid is a hypothetical acid. The monomer and dimer would respectively have structures similar to sulfuric and disulfuric acids.
- Phosphorus pentoxide (P2O5) reacts with water and forms phosphoric acid (H3PO4)
- Dinitrogen pentoxide, also known as nitronium nitrate, react with water to form nitric acid.
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 0080379419.
- ↑ Principles of Modern Chemistry, 7th Edition. David Oxtoby, H. P. Gillis, Alan Campion. Published by Cengage Learning. Page 675-676. ISBN 978-0840049315
This article is issued from Wikipedia. The text is available under the Creative Commons Attribution/Share Alike; additional terms may apply for the media files.