Here are some examples:
* Aluminum oxide (Al₂O₃):
* With acid: Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
* With alkali: Al₂O₃ + 2NaOH + 3H₂O → 2Na[Al(OH)₄]
* Zinc oxide (ZnO):
* With acid: ZnO + 2HCl → ZnCl₂ + H₂O
* With alkali: ZnO + 2NaOH + H₂O → Na₂[Zn(OH)₄]
* Beryllium oxide (BeO):
* With acid: BeO + 2HCl → BeCl₂ + H₂O
* With alkali: BeO + 2NaOH + H₂O → Na₂[Be(OH)₄]
* Tin(II) oxide (SnO):
* With acid: SnO + 2HCl → SnCl₂ + H₂O
* With alkali: SnO + 2NaOH + H₂O → Na₂[Sn(OH)₄]
Why do amphoteric oxides behave this way?
Amphoteric oxides have the ability to act as both acids and bases. This is because the metal cation in these oxides can either accept an electron pair (acting as a Lewis acid) or donate a proton (acting as a Brønsted-Lowry acid).
Important note: The exact products formed may vary depending on the specific acid or alkali used. The above reactions are just examples.
