According to Valence Shell Electron Pair Repulsion (VSEPR) Theory, how does electron pair repulsion influence the geometry of a molecule?

• A. Electron pairs attract each other, causing the molecule to adopt a linear geometry regardless of the number of pairs.
• B. Electron pair repulsion only affects the bond angles but not the overall molecular geometry.
• C. Electron pairs around a central atom arrange themselves as far apart as possible to minimize repulsion, determining the molecular shape.
• D. Electron pair repulsion is responsible for breaking chemical bonds, which changes the molecular shape.

Answer: (C)

Verified step by step guidance

1. Understand that Valence Shell Electron Pair Repulsion (VSEPR) theory is based on the idea that electron pairs around a central atom repel each other because they have the same negative charge.
2. Recognize that to minimize this repulsion, electron pairs will arrange themselves as far apart as possible in three-dimensional space.
3. Know that this arrangement of electron pairs determines the geometry of the molecule, including bond angles and overall shape.
4. Differentiate between bonding electron pairs (shared between atoms) and lone pairs (non-bonding), as lone pairs tend to repel more strongly and can influence the molecular geometry differently.
5. Conclude that the molecular shape is a direct result of electron pair repulsions seeking to minimize their interactions, which is why molecules adopt specific geometries predicted by VSEPR theory.