What do you call the metal oxide having both acidic and basic properties. Give two examples. Give chemical equations to support your answer
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Amphoteric oxide. Example: Zinc oxide and aluminium oxide.
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In chemistry, an amphoteric compound is a molecule or ion that can react both as an acidas well as a base. Many metals (such as copper, zinc, tin, lead, aluminium, and beryllium) form amphoteric oxides or hydroxides. Amphoterism depends on the oxidation states of the oxide. Al2O3 is an example of an amphoteric oxide.
Metal oxides which react with both acids as well as bases to produce salts and water are known as amphoteric oxides. Amphoteric oxides include lead oxide and zinc oxide, among many others
AMPHOTERIC OXIDES:
Zinc oxide (ZnO) reacts with both acids and with bases:
In acid: ZnO + H2SO4 → ZnSO4 + H2OIn base: ZnO + 2 NaOH + H2O → Na2[Zn(OH)4]
This reactivity can be used to separate different cations, such as zinc(II), which dissolves in base, from manganese(II), which does not dissolve in base.
Lead oxide (PbO):
In acid: PbO + 2 HCl → PbCl2 + H2OIn base: PbO + 2 NaOH + H2O → Na2[Pb(OH)4]
Aluminium oxide (Al2O3)
In acid: Al2O3 + 6 HCl→ 2 AlCl3 + 3 H2OIn base: Al2O3 + 2 NaOH + 3 H2O → 2 Na[Al(OH)4] (hydrated sodium aluminate)
Stannous oxide (SnO)
In acid : SnO +2 HCl ⇌ SnCl2 + H2OIn base : SnO +4 NaOH + H2O ⇌ Na4[Sn(OH)6]
Some other elements which form amphoteric oxides are gallium, indium, scandium, titanium, zirconium, vanadium, chromium, iron, cobalt, copper, silver, gold, germanium, antimony, bismuth, and tellurium.
Amphoteric Hydroxides:
Aluminium hydroxide is also amphoteric:
As a base (neutralizing an acid): Al(OH)3 + 3 HCl → AlCl3 + 3 H2OAs an acid (neutralizing a base): Al(OH)3 + NaOH → Na[Al(OH)4]
Beryllium hydroxide
with acid: Be(OH)2 + 2 HCl → BeCl2 + 2 H2Owith base: Be(OH)2 + 2 NaOH → Na2[Be(OH)4]
In chemistry, an amphoteric compound is a molecule or ion that can react both as an acidas well as a base. Many metals (such as copper, zinc, tin, lead, aluminium, and beryllium) form amphoteric oxides or hydroxides. Amphoterism depends on the oxidation states of the oxide. Al2O3 is an example of an amphoteric oxide.
Metal oxides which react with both acids as well as bases to produce salts and water are known as amphoteric oxides. Amphoteric oxides include lead oxide and zinc oxide, among many others
AMPHOTERIC OXIDES:
Zinc oxide (ZnO) reacts with both acids and with bases:
In acid: ZnO + H2SO4 → ZnSO4 + H2OIn base: ZnO + 2 NaOH + H2O → Na2[Zn(OH)4]
This reactivity can be used to separate different cations, such as zinc(II), which dissolves in base, from manganese(II), which does not dissolve in base.
Lead oxide (PbO):
In acid: PbO + 2 HCl → PbCl2 + H2OIn base: PbO + 2 NaOH + H2O → Na2[Pb(OH)4]
Aluminium oxide (Al2O3)
In acid: Al2O3 + 6 HCl→ 2 AlCl3 + 3 H2OIn base: Al2O3 + 2 NaOH + 3 H2O → 2 Na[Al(OH)4] (hydrated sodium aluminate)
Stannous oxide (SnO)
In acid : SnO +2 HCl ⇌ SnCl2 + H2OIn base : SnO +4 NaOH + H2O ⇌ Na4[Sn(OH)6]
Some other elements which form amphoteric oxides are gallium, indium, scandium, titanium, zirconium, vanadium, chromium, iron, cobalt, copper, silver, gold, germanium, antimony, bismuth, and tellurium.
Amphoteric Hydroxides:
Aluminium hydroxide is also amphoteric:
As a base (neutralizing an acid): Al(OH)3 + 3 HCl → AlCl3 + 3 H2OAs an acid (neutralizing a base): Al(OH)3 + NaOH → Na[Al(OH)4]
Beryllium hydroxide
with acid: Be(OH)2 + 2 HCl → BeCl2 + 2 H2Owith base: Be(OH)2 + 2 NaOH → Na2[Be(OH)4]
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