The option(s) with only amphoteric oxides is (are):

C r_{2} O_{3}, B e O, S n O, S n O_{2}

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C r_{2} O_{3}, C r O, S n O, P b O

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Z n O, A l_{2} O_{3}, P b O, P b O_{2}

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N O, B_{2} O_{3}, P b O, S n O_{2}

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Solution

The correct options are
A $C r_{2} O_{3}, B e O, S n O, S n O_{2}$
C $Z n O, A l_{2} O_{3}, P b O, P b O_{2}$
The options with only amphoteric oxides are
$C r_{2} O_{3}, B e O, S n O, S n O_{2}$
$Z n O, A l_{2} O_{3}, P b O, P b O_{2}$

However, $B_{2} O_{3}$ is acidic oxides, $C r O$ is basic oxide and $N O$ is neutral.

Note: Amphoteric oxides react with acids as well as bases.

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Similar questions

P b O_{2}

P b O Δ G_{298} < 0

S n O_{2}

S n O

Δ G_{298}

P b O_{2} \to P b O

Δ G_{298} < 0

S n O_{2} \to S n O

Δ G_{298} > 0

P b

S n

C O, C O_{2}, N a_{2} O, P b O_{2}, P b O, S n O, G e O_{2}, G e O

P b O_{2} \to P b O

Δ G_{298} < 0

S n O_{2} \to S n O

Δ G_{298} > 0

Consider the reactions;

P b O_{2} \to P b O, Δ G_{298} < 0;

$S n O_{2} \to S n O, Δ G_{298} < 0$

The most probable oxidation state of $P b$ and $S n$ will be :

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