A) \[Xe{{F}_{2}},IF_{2}^{-}\]
B) \[N{{H}_{3}},\text{ }B{{F}_{3}}\]
C) \[CO_{3}^{2-},SO_{3}^{2-}\]
D) \[PC{{l}_{5}},\text{ I}C{{l}_{5}}\]
Correct Answer: A
Solution :
\[Xe{{F}_{2}}\]is a linear molecule\[(Xe\]is\[s{{p}^{3}}{{d}^{2}}\]hybridised with three equitorial positions occupied by lone pairs). \[IF_{2}^{-}\]is also a linear molecule as explained below. Number of electrons around\[1=7+2+1\](due-recharge) =10 Therefore,\[I\]is\[s{{p}^{3}}{{d}^{2}}\]hybridised. There are 3 lone pairs and 2 bond pairs. Thus, its structure is similar to\[Xe{{F}_{2}}\].
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