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Simple Oxides
Mixed Oxides
Classification of Simple oxides
Acidic Oxide
Basic Oxide
Amphoteric Oxide
Neutral Oxide
Oxides of nonmetals have a tendency to be acidic, oxides of metals have a tendency to be basic, and oxides of elements in or close to the corner to corner band of semimetals are by and large amphoteric.
An oxide is a binary compound obtained when oxygen reacts with another element. On the premise of their oxygen content, oxides can be extensively arranged into mixed oxides and simple oxides.
Simple oxides are oxides that carry only that number of oxygen atoms as is allowed by the normal valency of its metal.
Example: H2O, MgO& Al2O3.
Two simple oxides combine to form mixed oxides.
Example: Lead dioxide (PbO2) and lead monoxide (PbO) together form the mixed oxide Red lead (Pb3O4).
Ferric oxide (Fe2O3) and ferrous oxide (FeO) together form the mixed oxide Ferro-ferric oxide (Fe3O4).
Simple Oxides on the basis of their chemical behaviour can further be classified into acidic oxides, basic oxides, amphoteric oxides and neutral oxides.
An oxide that reacts with water to give an acid is called as Acidic Oxide. Example: Oxides of non-metals, such as SO2, CO2, SO3, Cl2O7, P2O5, & N2O5, or oxides of metals with high oxidation states, such as CrO3, Mn2O7, &V2O5 are acidic in nature.
SO2 + H2O → H2SO3 Sulphur dioxide Water Sulphurous acid
Cr2O3 + H2O → H2Cr2O4 Chromic anhydride Water Chromic acid
An oxide that reacts with water to give a base is called as a basic oxide.
Example: Oxides of most metals, such asNa2O, CaO, BaO, are basic in nature.
CaO + H2O → Ca(OH)2 Calcium oxide Water Calcium hydroxide
Some metallic oxides display dual behavior that is they show both the characteristics of acid as well as base. These metal oxides are known as Amphoteric Oxides. They can react with both alkalis as well as acids.
Example: Zinc oxide when reacts with concentrated sodium hydroxide behaves as an acidic oxide but when reacts with hydrochloric acid acts as a basic oxide.
ZnO + 2H2O + 2NaOH → Na3Zn[OH]4 + H2 Zinc oxide Water NaOH(conc) Sodium Zincate Hydrogen
ZnO + 2HCl → ZnCl2 + H2O Zinc oxide Hydrochloric acid Zinc chloride Water
Aluminium oxide is another example that reacts with alkalis as well as acids.
Al2O3 (s) + 6NaOH (aq) + 3H2O (l) → 2Na3[Al(OH)6] (aq)
Al2O3 (s) + 6HCl (aq) + 9H2O (l) → 2[Al(H2O)6]3+ (aq) + 6Cl- (aq)
Neutral Oxides, as name suggests do not exhibit any tendency to form salts either with acids or bases.
Example: Nitrous oxide and Carbon monoxide are neutral oxides.
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