The correct statement about ` ICI _ 5 and ICI _ 4 ^ - ` is :

Options

A. `ICl _5 ` is trigonal bipyramidal and `ICl _ 4 ^( - ) ` is tetrahedral
B. ` ICl _ 5 ` is sqare pyramidal and ` ICl _ 4 ^ - ` is square planar.
C. both are isostructural
D. ` ICl _ 5 ` is square pyramidal and `ICl _ 4^( -) ` is tetrahedral

Explanation

To solve the question regarding the correct statement about ICl5 and ICl4^-, we need to determine the molecular geometries of both compounds.

### Step 1: Determine the molecular geometry of ICl5
1. **Count the valence electrons**: Iodine (I) has 7 valence electrons, and each chlorine (Cl) has 7 valence electrons. For ICl5, the total number of valence electrons is:
\[ 7 + 5 \times 7 = 7 + 35 = 42 \text{ electrons} \]
2. **Draw the Lewis structure**: Iodine is the central atom with 5 chlorine atoms bonded to it. This results in 5 bond pairs and 1 lone pair on the iodine atom.
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