Question

\(ICl_2^-\) is isostructural with

• A. \(XeF_2\)
• B. \(SbCl_3\)
• C. \(BaCl_2\)
• D. \(TeF_2\)

Hint:

Species with \(AX_2E_3\) arrangement are linear, for example \(XeF_2\) and \(ICl_2^-\).

Answer 1

The Correct Option is A

Concept:
Isostructural species have the same shape or geometry. To find geometry, we use VSEPR theory. According to VSEPR theory, electron pairs around the central atom arrange themselves to minimize repulsion.

Step 1: Find the structure of \(ICl_2^-\).
Central atom is iodine. Iodine has 7 valence electrons. There is one negative charge, so add one more electron: \[ 7+1=8 \] Two chlorine atoms form two bonds with iodine. So iodine has: \[ 2 \text{ bond pairs} \] Remaining electrons form: \[ 3 \text{ lone pairs} \] Thus, \(ICl_2^-\) has: \[ AX_2E_3 \]

Step 2: Determine geometry.
For \(AX_2E_3\), electron pair geometry is trigonal bipyramidal. The three lone pairs occupy equatorial positions. The two bond pairs remain axial. So molecular shape is: \[ \text{linear} \]

Step 3: Compare with \(XeF_2\).
\(XeF_2\) also has: \[ AX_2E_3 \] Therefore, \(XeF_2\) is also linear. So \(ICl_2^-\) and \(XeF_2\) are isostructural.

Step 4: Check the options.
Option (A) \(XeF_2\) is correct.
Option (B) \(SbCl_3\) is not linear.
Option (C) \(BaCl_2\) is ionic and not comparable in the same molecular VSEPR sense.
Option (D) \(TeF_2\) does not match the same \(AX_2E_3\) arrangement. Hence, the correct answer is: \[ \boxed{(A)\ XeF_2} \]