Question

Match the LIST-I with LIST-II.

Choose the correct answer from the options given below :

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

Hint:

In molecular structures, use the VSEPR theory to determine the number of bonding and lone pairs on the central atom, which helps in predicting the molecular geometry and bond pair to lone pair ratios.

Answer 1

The Correct Option is B

To match LIST-I with LIST-II, we need to determine the bond pair and lone pair on the central atom for each molecule/ion.

1. ICl₂^-: Iodine (I) is the central atom with 7 valence electrons. It has 2 additional electrons due to the two chlorine atoms, making 9 electrons, or 4.5 pairs. After forming two bonds with Cl atoms, 3 lone pairs remain. Thus, the bond pair: lone pair ratio is 2:3 (III).
2. H₂O: Oxygen (O) is the central atom with 6 valence electrons. It forms 2 bonds with hydrogen atoms, making 2 bond pairs, and has 2 lone pairs remaining. This results in a 2:2 ratio (IV).
3. SO₂: Sulfur (S) is the central atom with 6 valence electrons. It forms 2 bonds with oxygen atoms and typically has 1 lone pair. Thus, the ratio is 4:1 (II).
4. XeF₄: Xenon (Xe) is the central atom with 8 valence electrons. It forms 4 bonds with fluorine atoms, leaving 2 lone pairs. The ratio here is 4:2 (I).

Based on the above calculations, the correct pairings are:

• A-III
• B-IV
• C-II
• D-I

The correct answer is A-III, B-IV, C-II, D-I.

Answer 2

To solve the given matching problem, we need to determine the number of bond pairs and lone pairs on the central atom for each molecule or ion in LIST-I, and match it with the correct pair in LIST-II. The details are as follows:

1. ICl₂^-: The central iodine atom has 7 valence electrons. With two chlorine atoms, it forms two bonds, and there is an additional electron due to the negative charge, totaling 8 electrons. Thus, it has 3 lone pairs (6 electrons) and 2 bond pairs.
   • Bond pairs: 2
   • Lone pairs: 3
2. H₂O: The central oxygen atom has 6 valence electrons. It forms 2 bonds with hydrogen atoms, leaving 4 electrons as 2 lone pairs.
   • Bond pairs: 2
   • Lone pairs: 2
3. SO₂: The central sulfur atom forms double bonds with two oxygen atoms, utilizing all 4 valence electrons for bonding. It also has a lone pair.
   • Bond pairs: 4
   • Lone pairs: 1
4. XeF₄: The central xenon atom has 8 valence electrons. With four fluorine atoms, it forms 4 bonds and has 2 lone pairs of electrons.
   • Bond pairs: 4
   • Lone pairs: 2

Based on the analysis above, let's match LIST-I with LIST-II:

• A (ICl₂^-): 2 bond pairs, 3 lone pairs → Matches with III.
• B (H₂O): 2 bond pairs, 2 lone pairs → Matches with IV.
• C (SO₂): 4 bond pairs, 1 lone pair → Matches with II.
• D (XeF₄): 4 bond pairs, 2 lone pairs → Matches with I.

Thus, the correct matching is A-III, B-IV, C-II, D-I.