Question

Match List I with List II 

Choose the correct answer from the options given below:

• A. A - IV, B - I, C - II, D - III
• B. A - II, B - I, C - IV, D - III
• C. A - II, B - III, C - IV, D - I
• D. A - IV, B - III, C - II, D - I

Answer 1

The Correct Option is D

Step 1: Determine the Lone Pairs for Each Molecule/Ion
The number of lone pairs on the central atom can be determined using the following steps:
Count the total valence electrons of the central atom.
Subtract the electrons used for bonding with surrounding atoms.
Divide the remaining electrons by 2 to get the number of lone pairs.
Step 2: Analyze Each Molecule/Ion
\(\text{IF}_7\): Iodine has 7 valence electrons. All are used for bonding with 7 fluorine atoms. Therefore, 0 lone pairs (IV).
\(\text{ICl}_4^-\): Iodine has 7 valence electrons and gains 1 due to the negative charge. Four are used for bonding with chlorine atoms, leaving 4 electrons (2 lone pairs). Therefore, 2 lone pairs (III).
\(\text{XeF}_6\): Xenon has 8 valence electrons. Six are used for bonding with fluorine atoms, leaving 2 electrons (1 lone pair). Therefore, 1 lone pair (II).
\(\text{XeF}_2\): Xenon has 8 valence electrons. Two are used for bonding with fluorine atoms, leaving 6 electrons (3 lone pairs). Therefore, 3 lone pairs (I)}