Question

Identify the correct statements with reference to VSEPR theory:
(A) Lone pairs cause more repulsion than double bonds,
(B) Double bonds cause more repulsion than a single bond,
(C) Single bonds cause more repulsion than a lone pair

• A. (A), (B), and (C) only
• B. (B) and (C) only
• C. (A), (C), and (D) only
• D. (A), (B), and (D) only

Hint:

Lone pair repulsion is higher than bond pair repulsion. Triple bonds being electron dense regions have higher repulsion than double and single bonds. Thus, lone pairs are the most effective at disrupting the regular geometric shape of the molecule, by increasing the bond angles.

Answer 1

The Correct Option is B

VSEPR (Valence Shell Electron Pair Repulsion) theory describes molecular geometries, positing that electron pairs in a central atom's valence shell repel each other, thus orienting themselves to minimize these repulsions.
• A hierarchy of repulsive forces exists among lone pairs, triple bonds, double bonds, and single bonds.
• Lone pairs exert the strongest repulsion, being held by only one nucleus and occupying a significant volume around the central atom.
• Multiple bonds (triple and double) exhibit greater repulsion than single bonds due to their increased electron density.
• Consequently, the repulsive force order is: Lone pair>Triple Bond>Double Bond>Single bond. This implies statements B and C are accurate, while A and D are inaccurate.