Question

The

bond angle in \(\mathrm{H}_2\mathrm{O}\) is \(104.5^{\circ}\). This fact can be explained with the help of

• A. valence shell electron pair repulsion theory (VSEPR)
• B. molecular orbital theory
• C. presence of hydrogen bond
• D. electronegativity difference between hydrogen and oxygen atoms

Hint:

Lone pairs occupy more space than bond pairs, causing bond angles to decrease.

Answer 1

The Correct Option is A

Step 1: Underlying Concept:
VSEPR theory explains molecular shapes based on electron pair repulsion.
Step 2: Explanation:
O in H\(_2\)O has 2 bond pairs and 2 lone pairs. Lone pair-lone pair repulsion>lone pair-bond pair repulsion, reducing the ideal tetrahedral angle (\(109.5^\circ\)) to \(104.5^\circ\).
Step 3: Conclusion:
Valence shell electron pair repulsion theory (VSEPR).