Question
Explain different types of oxides.
✓
Answer
Oxides are of four types as follows :
$(1)$ acidic oxides :
The oxide, which on reaction with water forms an acid or reacts with a base to give a salt is called an acidic oxide.
It is formed by the combination of oxygen with non$-$metals. For example $CO_2, SO_3,$ etc.
$CO _{2( g )}+ H _2 O _{( l )} \longrightarrow \underset{\text { Carbonic acid }}{ H _2 CO _{3( aq )}}$
$ SO _{3( g )}+ H _2 O _{( l )} \longrightarrow H _2 SO _{4( aq )}$
$ SO _{3( g )}+2 NaOH _{( aq )} \longrightarrow Na _2 SO _{4( aq )}+ H _2 O $
$(2)$ Basic oxide :
The oxide, which on reaction with water forms a base or reacts with an acid to give a salt is called basic oxide.
It is formed by the reaction of oxygen with highly electropositive metals.
For example, $Na _2 O , CaO$, etc.
$ Na _2 O _{( s )}+ H _2 O _{(1)} \rightarrow 2 NaOH _{( aq )}$
$ CaO _{( s )}+ H _2 O _{(1)} \rightarrow Ca ( OH )_{2( aq )}$
$ BaO _{( s )}+2 HCl _{( aq )} \rightarrow BaCl _2+ H _2 O$
Basic oxides are generally ionic in nature.
$(3)$ Amphoteric oxide :
The oxide, which shows both acidic and basic I characteristics is called an amphoteric oxide.
They are formed by the reaction of oxygen with elements which lie on the border of electroposi$-$five $($metals$)$ and electronegative (non$-$metals) nature.
For example, $Al _2 O _3, ZnO$, etc.
$Al _2 O _{3( s )}+6 HCl _{( aq )}+9 H _2 O _{( l )} \longrightarrow$
$ \text { (Basic) } 2\left[ Al \left( H _2 O \right)_6\right]^{3+}+6 Cl _{\text {(aq) }}^{-}$
$\underset{\text { Acidic }}{ Al _2 O _{3( s )}}+\underset{\text { Base }}{6 NaOH _{( aq )}}+\underset{2 H _2 O _{( l )}}{2 Na _3\left[ Al ( OH )_6\right]_{( aq )}}$
Along the period, from left to right the nature of oxides changes from basic to amphoteric to acidic.
$(4)$ Neutral oxide : The oxide which behaves neither acidic nor basic is called a neutral oxide.
For example, $CO , NO , N _2 O$.
$(1)$ acidic oxides :
The oxide, which on reaction with water forms an acid or reacts with a base to give a salt is called an acidic oxide.
It is formed by the combination of oxygen with non$-$metals. For example $CO_2, SO_3,$ etc.
$CO _{2( g )}+ H _2 O _{( l )} \longrightarrow \underset{\text { Carbonic acid }}{ H _2 CO _{3( aq )}}$
$ SO _{3( g )}+ H _2 O _{( l )} \longrightarrow H _2 SO _{4( aq )}$
$ SO _{3( g )}+2 NaOH _{( aq )} \longrightarrow Na _2 SO _{4( aq )}+ H _2 O $
$(2)$ Basic oxide :
The oxide, which on reaction with water forms a base or reacts with an acid to give a salt is called basic oxide.
It is formed by the reaction of oxygen with highly electropositive metals.
For example, $Na _2 O , CaO$, etc.
$ Na _2 O _{( s )}+ H _2 O _{(1)} \rightarrow 2 NaOH _{( aq )}$
$ CaO _{( s )}+ H _2 O _{(1)} \rightarrow Ca ( OH )_{2( aq )}$
$ BaO _{( s )}+2 HCl _{( aq )} \rightarrow BaCl _2+ H _2 O$
Basic oxides are generally ionic in nature.
$(3)$ Amphoteric oxide :
The oxide, which shows both acidic and basic I characteristics is called an amphoteric oxide.
They are formed by the reaction of oxygen with elements which lie on the border of electroposi$-$five $($metals$)$ and electronegative (non$-$metals) nature.
For example, $Al _2 O _3, ZnO$, etc.
$Al _2 O _{3( s )}+6 HCl _{( aq )}+9 H _2 O _{( l )} \longrightarrow$
$ \text { (Basic) } 2\left[ Al \left( H _2 O \right)_6\right]^{3+}+6 Cl _{\text {(aq) }}^{-}$
$\underset{\text { Acidic }}{ Al _2 O _{3( s )}}+\underset{\text { Base }}{6 NaOH _{( aq )}}+\underset{2 H _2 O _{( l )}}{2 Na _3\left[ Al ( OH )_6\right]_{( aq )}}$
Along the period, from left to right the nature of oxides changes from basic to amphoteric to acidic.
$(4)$ Neutral oxide : The oxide which behaves neither acidic nor basic is called a neutral oxide.
For example, $CO , NO , N _2 O$.
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