Question

Given below are two statements:
Statement I:\(F_2O < H_2O < Cl_2O\) is the correct trend in terms of bond angle.
Statement II:\(SiF_4, SnF_4\) and \(PbF_4\) are ionic in nature. Choose the correct answer.

• A. Both Statement I and Statement II are true
• B. Both Statement I and Statement II are false
• C. Statement I is true but Statement II is false
• D. Statement I is false but Statement II is true

Answer 1

The Correct Option is C

Step 1: Understanding the Question:
We need to evaluate statements about molecular geometry (bond angles) and the nature of chemical bonds (ionic vs. covalent).
Step 2: Key Formula or Approach:
- Bond angle depends on central atom electronegativity and steric crowding (size) of surrounding atoms.
- Fajan's Rule: Smaller, highly charged cations favor covalency. Larger cations favor ionic character.
Step 3: Detailed Explanation:
1. Statement I: Bond angle in \(\text{H}_2\text{O}\) is \(104.5^{\circ}\). In \(\text{F}_2\text{O}\), the more electronegative F pulls electrons away from center, reducing BP-BP repulsion, narrowing angle (\(103^{\circ}\)). In \(\text{Cl}_2\text{O}\), the large Cl atoms cause steric repulsion, widening angle (\(111^{\circ}\)). Trend is Correct.
2. Statement II: \(\text{SiF}_4\) is a gas and purely covalent. \(\text{SnF}_4\) and \(\text{PbF}_4\) have significant ionic character but the group as a whole (especially Si) is not ionic. Statement II is False.
Step 4: Final Answer:
Statement I is true, Statement II is false.