Oxygen when combines with other elements or atoms or molecules, it called as oxides. Here we are discussing about amphoteric oxide example and some facts about it. Amphoteric means ‘both’ and the word amphoteric are derived from ‘Amphoteroi’ which is an Greek word it means both. Amphoteric oxides are consists of metal elements.
- Al2O3(s)+6H3O+(aq)+3H2O(l)→2Al(OH2)3+6(aq)
- Al2O3(s)+2OH-(aq)+3H2O(l)→2Al(OH)-4(aq)
- ZnO(s) + 2HNO3(aq) → Zn(NO3)2(aq) + H2O(l)
- ZnO + H2SO4 → ZnSO4 + H2O
- ZnO(s) + 2NaOH(aq) → Na2ZnO2(aq) + H2O(l)
- Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(l)
- Al2O3(s) + 2NaOH(aq) → 2NaAlO2(aq) + H2O(l)
- PbO + 2HCl → PbCl2 + H2O
- PbO + 2NaOH + H2O → Na2[Pb(OH)4]
- SnO + 2HCl ⇌ SnCl2 + H2O
- SnO + 4NaOH + H2O ⇌ Na4[Sn(OH)6]
- VO2 + 2HCl → VOCl2 + H2O
- 4VO2 + 2NaOH → Na2V4O9 + H2O
- As2O3(s) + 6HCl(aq) → 2AsCl(aq) + 3H2O(l)
- Ga2O3 + 6HCl → 2GaCl3 + 3H2O
- NaOH + Ga2O3 = H2O + NaGaO2
- Ge2O3 + 2NaOH = Na2Ge2O4 + H2O
- Ge2O3 + HCl = GeCl3 + H2O
- Bi2O3 + 6HCl → 2BiCl3 + 3H2O
- Bi2O3 + NaOH + NaOCl = NaBiO3 + NaCl + H2O
- Sb2O3 + 2NaOH = 2NaSbO2 + H2O
- Sb2O3 + HCl = SbCl3 + H2O
Amphoteric oxides examples
Amphoteric oxide example includes amino acids and proteins, which comes under carboxylic acids and amine molecules which are auto ionized like water. Oxygen compounds and amphoteric oxides both can show the acidic and basic nature. Hence, this oxides can undergoes the neutralization reaction and form salt and water when they get reacts with acid compounds.
Likewise, alkali metals also react to form salt and water to show its acidic character. All kind of oxides can be produced with heating the metals or any elements with oxygen. When aqueous metal trihalides gets reacts with hydrogen oxides, hydrated oxides get formed. When we go down in the group of periodic table, there is the transition of oxides i.e. acidic oxide then amphoteric oxide and then basic oxides.
Al2O3(s)+6H3O + (aq)+3H2O(l)→2Al(OH2)3+6(aq)
When aluminium oxide reacts with hydronium ion and water aluminium hydroxide oxides are formed. Aluminium oxide (Al2O3) which is amphoteric in nature and shows both behaviour of acidic and basic oxide.
Al2O3(s)+2OH-(aq)+3H2O(l)→2Al(OH)-4(aq)
When aluminium oxide (Al2O3) get reacts with hydroxide ions and water aluminium hydroxide is formed. Here, Al2O3 (aluminium oxide is an amphoteric oxide.
ZnO(s) + 2HNO3(aq) → Zn(NO3)2(aq) + H2O(l)
When zinc oxide get reacts with nitric acid aqueous zinc nitrate is formed with the removal of water. Zinc oxide (ZnO) is an amphoteric oxide example.
ZnO + H2SO4 → ZnSO4 + H2O
When ZnO reacts with sulphuric acid, zinc sulphate is formed with water removal. ZnO is amphoteric in nature.
ZnO(s) + 2NaOH(aq) → Na2ZnO2(aq) + H2O(l)
When Zinc oxide (ZnO) is reacts with sodium hydroxide which is a base, sodium zinc oxide get formed with the removal of water as by- product. Here ZnO is amphoteric oxide example.
Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(l)
Aluminium oxide (Al2O3) when reacts with strong acid like hydrochloric acid (HCl) there is the formation of aluminium chloride with the removal of water. Here, Al2O3 is an amphoteric oxide example.
Al2O3(s) + 2NaOH(aq) → 2NaAlO2(aq) + H2O(l)
When aluminium oxide (Al2O3) get reacts with a strong base like sodium hydroxide (NaOH), aqueous sodium aluminium oxide get formed with the removal of water molecules. Here, Al2O3 aluminium oxide is the amphoteric oxide example.
PbO + 2HCl → PbCl2 + H2O
When lead oxide get react hydrochloric acid, lead chloride is formed with removal of water. Here PbO is amphoteric oxide example.
PbO + 2NaOH + H2O → Na2[Pb(OH)4]
When lead oxide get reacts with basic sodium hydroxide and water, sodium lead hydroxide is obtained. PbO is amphoteric oxide.
SnO + 2HCl ⇌ SnCl2 + H2O
When stannous oxide (tin (ii) oxide) reacts with hydrochloric acid, stannous chloride get formed with removal of water. SnO is amphoteric in nature.
SnO + 4NaOH + H2O ⇌ Na4[Sn(OH)6]
When stannous oxide reacts with base like sodium hydroxide and water, sodium stannous hydroxide is formed. SnO is amphoteric oxide example.
VO2 + 2HCl → VOCl2 + H2O
When vanadium oxide reacts with hydrochloric acid, vanadium chloride is formed with removal of water. Here, VO2 is amphoteric oxide example.
4VO2 + 2NaOH → Na2V4O9 + H2O
When vanadium oxide reacts with sodium hydroxide, Na2V4O9 is formed with water removal. Here, VO2 vanadium oxide is amphoteric in nature.
As2O3(s) + 6HCl(aq) → 2AsCl(aq) + 3H2O(l)
When arsenic oxide reacts with hydrochloric acid, arsenic chloride is formed with water removal. As2O3 is amphoteric oxide example.
Ga2O3 + 6HCl → 2GaCl3 + 3H2O
When gallium oxide reacts with hydrochloric acid, gallium chloride (salt) is formed with water. Here, gallium oxide is an amphoteric oxide example.
NaOH + Ga2O3 = H2O + NaGaO2
When gallium oxide reacts with base like sodium hydroxide, sodium gallium oxide is formed with the removal of water. Here, gallium oxide is the amphoteric oxide example.
Ge2O3 + 2NaOH = Na2Ge2O4 + H2O
When germanium oxide get reacts with sodium hydroxide which is a base, sodium germanium oxide is formed with the removal of water. Germanium oxide (Ge2O3) is an amphoteric oxide example.
Ge2O3 + HCl = GeCl3 + H2O
When germanium oxide reacts with hydrochloric acid, germanium chloride is formed with the removal of water. Here germanium oxide (Ge2O3) is the amphoteric oxide example.
Bi2O3 + 6HCl → 2BiCl3 + 3H2O
When bismuth oxide get reacts with hydrochloric oxide, bismuth chloride is formed with removal of water. Here, Bi2O3 is an amphoteric oxide example.
Bi2O3 + NaOH + NaOCl = NaBiO3 + NaCl + H2O
When bismuth oxide reacts with sodium hydroxide and sodium oxo-chloride, sodium bismuth oxide is formed with sodium chloride and water. Here, bismuth oxide is amphoteric oxide example.
Sb2O3 + 2NaOH = 2NaSbO2 + H2O
When antimony oxide get reacts with sodium hydroxide, sodium antimony oxides get produced with the removal of water. Here, Sb2O3 is amphoteric oxide example.
Sb2O3 + HCl = SbCl3 + H2O
When antimony oxide get reacts with hydrochloric acid, antimony chloride is formed with the removal of water molecule. Here, antimony oxide is the amphoteric oxide example.
The oxides acts both as acids and base are the amphoteric oxides. The 2nd and 13th group elements which are lighter elements and some d- block elements and the 14th and 15th group elements which are heavier in nature can have amphoteric oxides when reacts with oxygen. The very basic oxides are present at lower left side of periodic table and the very acidic oxides are present at the upper right side of periodic table.
The elements Berellium (Be), Aluminium (Al), Gallium (Ga), Germanium (Ge), Arsenic (As), Tin (Sn), Lead (Pb), Antimony (Sb) and Bismuth (Bi) are the elements which can form amphoteric oxides when reacts with oxygen. These elements are placed diagonally between the acidic and basic oxides.Thus the border line between acidic oxides and basic oxides happens beside a diagonal.
Some important facts about amphoteric oxides
Amphoteric nature of any metal oxides depends upon the oxidation state of that metal. The amphoteric nature of any oxide possibly reflects the metal ability to polarize the neighbouring oxide ions (cations or anions) i.e. to host the important covalent character in metal oxygen (M-O) bonds. Amphoteric oxides can show both the characteristics of acidic oxides and basic oxides.
Also it has the ability to neutralize both the acidic oxides and basic oxides. This ability of amphoteric oxides increases with the oxidation state as the positive charge on the central metal atom increased. Therefore, the oxides of group 15th of periodic table having lower oxidation state is amphoteric, while oxides having higher oxidation state are more acidic to show amphoteric nature.
Oxygen when reacts with the metals or non- metal elements the compound formed are the oxides. Basically amphoteric oxides are categorized as metal oxide, which can reacts both with acids and bases and also creates salts and water. Zinc oxides and lead oxide are comes under amphoteric oxides and both can reacts with acids and bases.
Conclusion:
Amphoteric oxides are consists of metal elements and this metals are present diagonally between the acidic and basic oxides. Oxides are the compounds formed with the reaction of metals and oxygen. Amphoteric oxides can behave both as an acid or a base. Some metals of group 2nd, 13th, 14th and 15th of periodic table can show the amphoteric oxide characteristics. Berellium (Be), Aluminium (Al), Gallium (Ga), Germanium (Ge), Arsenic (As), Tin (Sn), Lead (Pb), Antimony (Sb) and Bismuth (Bi) are some amphoterix oxide forming metals.
Hello everyone, I am Dr. Shruti M Ramteke, I did my Ph.D. in chemistry. I am passionate about writing and like to share my knowledge with others . Feel free to contact me on linkedin
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