A) Fe (II)
B) \[Mn\](II)
C) Co (III)
D) Ni (IV)
Correct Answer: B
Solution :
[a] \[Fe=[Ar]3{{d}^{6}},4{{s}^{2}}\] \[F{{e}^{2+}}=[Ar]3{{d}^{6}}\] [b] \[Mn=[Ar]3{{d}^{5}},4{{s}^{2}}\] \[M{{n}^{2+}}=[Ar]3{{d}^{5}}\] [c] \[Co=[Ar]3{{d}^{7}},4{{s}^{2}}\] \[C{{o}^{3+}}=[Ar]3{{d}^{6}}\] [b] \[Ni=[Ar]3{{d}^{8}},4{{s}^{2}}\] \[N{{i}^{4+}}=[Ar]3{{d}^{6}}\] Therefore, the valence shell electronic configuration of\[Mn\](II) is not\[{{d}^{6}}\].You need to login to perform this action.
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