According to Valence Shell Electron Pair Repulsion (VSEPR) Theory, how does increasing the number of lone pairs on the central atom affect the arrangement of bonding pairs around it?

• A. It forces bonding pairs to form double bonds.
• B. It has no effect on the arrangement of bonding pairs.
• C. It increases the bond angles between bonding pairs.
• D. It causes bonding pairs to move closer together, reducing bond angles.

Answer: (D)

Verified step by step guidance

1. Recall that VSEPR theory is based on the idea that electron pairs around a central atom repel each other and arrange themselves to minimize this repulsion.
2. Understand that lone pairs (non-bonding electron pairs) occupy more space than bonding pairs because lone pairs are localized closer to the central atom and are not shared between atoms.
3. Recognize that as the number of lone pairs on the central atom increases, these lone pairs push the bonding pairs closer together due to their stronger repulsive effect.
4. This increased repulsion from lone pairs causes the bonding pairs to move closer, which results in a decrease in the bond angles between bonding pairs.
5. Therefore, increasing lone pairs on the central atom reduces bond angles between bonding pairs, altering the molecular geometry accordingly.