Question

Match List - I with List - II.List - I	List - II
(A) ICl	(IV) Linear
(B) ICl3	(I) T-Shape
(C) ClF5	(II) Square pyramidal
(D) IF7	(III) Pentagonal bipyramidal
Choose the correct answer from the options given below:

• A. (A)–(I), (B)–(IV), C–(III), D–(II)
• B. (A)–(I), (B)–(III), C–(II), D–(IV)
• C. (A)–(IV), (B)–(I), C–(II), D–(III)
• D. (A)–(IV), (B)–(III), C–(II), D–(I)

Answer 1

Answer: (C)

(A)–(IV), (B)–(I), C–(II), D–(III)

Answer 2

To determine the correct matches, we analyze the molecular geometry of each compound based on the number of bond pairs and lone pairs of electrons around the central atom.
Step 1: Molecular geometry of $\text{ICl}$
$\text{ICl}$ consists of only two atoms (iodine and chlorine), forming a diatomic molecule. Its molecular geometry is linear. Thus:
$(A) \, \text{ICl} \rightarrow \text{(IV) Linear}.$
Step 2: Molecular geometry of $\text{ICl}_3$
$\text{ICl}_3$ has 3 bond pairs and 2 lone pairs around the iodine atom. According to the VSEPR theory, this results in a T-shaped molecular geometry. Thus:
$(B) \, \text{ICl}_3 \rightarrow \text{(I) T-Shape}.$
Step 3: Molecular geometry of $\text{ClF}_5$
$\text{ClF}_5$ has 5 bond pairs and 1 lone pair around the central chlorine atom. According to the VSEPR theory, this configuration forms a square pyramidal geometry. Thus:
$(C) \, \text{ClF}_5 \rightarrow \text{(II) Square pyramidal}.$
Step 4: Molecular geometry of $\text{IF}_7$
$\text{IF}_7$ has 7 bond pairs and no lone pairs around the iodine atom. This configuration corresponds to a pentagonal bipyramidal geometry.
Thus:
$(D) \, \text{IF}_7 \rightarrow \text{(III) Pentagonal bipyramidal}.$
Final Matches:
$(A) \rightarrow \text{(IV)}, \, (B) \rightarrow \text{(I)}, \, (C) \rightarrow \text{(II)}, \, (D) \rightarrow \text{(III)}.$
Correct Answer: (3).