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Question

If the electronic configuration of a transition metal is [Ar]3d34s2, then its possible oxidation states are:

A
+I,+II,+III
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B
+II,+III
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C
+II,+III,+IV,+V
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D
+I,+II,+III,+IV
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Solution

The correct option is C +II,+III,+IV,+V

Given that the electronic configuration of a transition metal is [Xe]3d34s2. The possible oxidation states shown by the metal are +II,+III,+IV,+V.

+II oxidation state is obtained when 2 electrons from 4s orbital are lost to give an electronic configuration [Xe]3d34s0. +V oxidation state is obtained when all the five electrons are lost to give the electronic configuration [Xe]3d04s0. Similarly, loss of 3 and 4 electrons will give +III and +IV oxidation states with electronic configurations, [Xe]3d24s0 and [Xe]3d14s0 respectively.


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