The correct order of stability of superxides of alkali metals is:

K O_{2} > R b O_{2} > C s O_{2}

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R b O_{2} > C s O_{2} > K O_{2}

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C s O_{2} > R b O_{2} > K O_{2}

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K O_{2} > C s O_{2} > R b O_{2}

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Solution

The correct option is C $C s O_{2} > R b O_{2} > K O_{2}$
Option $(C)$ is correct.
The correct order of stability of superoxides of alkali metals is $C s O_{2} > R b O_{2} > K O_{2}$ . Going down the group, the stability of superoxide increases as the size of the metal ion increases. It is due to the stabilization of larger anions by larger cation through higher lattice energies.

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Similar questions

Q. Assertion :The oxidation state of superoxide ion in

{K O}_{2}, {C s O}_{2}

and

{R b O}_{2}

- \frac{1}{2}

. Reason: Since the oxidation state of an alkali metal in any compound is always

+ 1

, the oxidation state of oxygen is

\frac{1}{2}

in the

O_{2}^{-}

ion.

Read the above assertion and reason and choose the correct option regarding it.

Q. The oxidation state of Na, K, Rb respectively in

N a_{2} O_{2}, K O_{2}, R b O_{2}

is :

The stability of $K_{2} O$ , $K_{2} O_{2}$ and $K O_{2}$ is in order $K_{2} O < K_{2} O_{2} < K O_{2}$ . The increasing stability at the size of metal ion increases is due to stabilization of:

$R b O_{2}$ is

Q. Out of

K O_{2}, N O_{2}, N O

and

K_{2} O_{2}

unpaired electron are present in:

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