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 explains molecular shapes by stating that electron pairs in the valence shell of a central atom repel each other, therefore arranging themselves to minimize repulsions.
• Lone pairs, triple bonds, double bonds and single bonds create a hierarchy of repulsive forces between electron pairs.
• Lone pairs: Experience the strongest repulsive forces because they are only held by one nucleus and occupy a large space around the central atom.
• Multiple bonds (triple and double bonds): They create more repulsion than single bonds because they have a higher electron density.
• Therefore, the order of repulsion is: Lone pair > Triple Bond > Double Bond > Single bond. Therefore, statements B and C are correct, and A and D are incorrect.