Which is correct order of their tendency of the given elements to form $M^{3 -}$ ion $?$

B i > S b > A s > P > N

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B i < S b < A s < P < N

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N < P < S b < B i < A s

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B i > S b \sim N \sim P > A s

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Solution

The correct option is B $B i < S b < A s < P < N$
As we Know, on moving down the group, the stability of $- 3$ oxidation state decreases.
This is due to the following reasons.
(i) On descending a group the size of the atom or ion increases. As a result, attraction of the nucleus per newly added electron decreases.
(ii) A large anion cannot fit easily into lattice of a small cation. (iii) As the negative charge on the ion increases, it becomes more and more susceptible to polarisation.

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