Select the correct order of stability of oxidation states:

G a^{+} > G a^{+ 3}

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T l^{+ 3} > G a^{+ 3}

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T l^{+ 3} > T 1^{+}

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T l^{+} > G a^{+}

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Solution

The correct option is D $T l^{+} > G a^{+}$
Both $G a$ and $T l$ are group 13 elements with an electronic configuration $n s^{2} n p^{1}$ . So, they are expected to be trivalent but the heavy elements are more stable in lower oxidation states. $s$ electrons do not participate in bonding and this effect is called the inert pair effect. Due to this, $T l$ has a more stable +1 oxidation state than the +3 oxidation state.
$A l and G a$ are more stable in the +3 oxidation state. So, option (d) is correct.

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Similar questions

The relative stability of the different oxidation states,

$T I^{+} > T I^{3 +}, > G a^{3 +} > G a^{+} T I^{+} > I n^{+} > G a^{+} is because of$

G a^{3 +} > I n^{3 +} > T l^{3 +}

G a^{3 +} < I n^{3 +} < T l^{3 +}

G e^{+ 4} > S n^{+ 4} > P b^{+ 4}

G e^{+ 2} < S n^{2 +} < P b^{2 +}

A s^{3 +} < S b^{3 +} < B i^{3 +}

A l^{+}, G a^{+}, I n^{+}, T l^{+}

+ 1

A l

G a

I n

T l

M^{+ 3}

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