The Cl-C-Cl angle in 1,1,2,2-tetrachloroethene and...

The $\mathrm{Cl}-\mathrm{C}-\mathrm{Cl}$ angle in $1,1,2,2$-tetrachloroethene and tetrachloromethane will be about
(a) $120^{\circ}$ and $109.5^{\circ}$
(b) $90^{\circ}$ and $109.5^{\circ}$
(c) $109.5^{\circ}$ and $90^{\circ}$
(d) $109.5^{\circ}$ and $120^{\circ}$

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Key Concepts

VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a model used to predict the geometry of molecules based on the repulsion between electron pairs in the valence shell of atoms. The theory explains how electron pairs, whether bonding or non-bonding, arrange themselves to minimize repulsion, resulting in specific bond angles and molecular shapes. This principle is crucial for understanding why certain compounds exhibit bond angles like 109.5° or 120°.

Hybridization

Hybridization refers to the mixing of atomic orbitals to create new hybrid orbitals that determine the geometry of a molecule. For example, sp3 hybridization leads to a tetrahedral arrangement with bond angles around 109.5°, while sp2 hybridization results in a trigonal planar geometry with bond angles about 120°. This concept is key to explaining the difference in bond angles observed in various molecular structures.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms within a molecule. It is directly influenced by hybridization and the repulsions among electron pairs as described by VSEPR theory. Differences in molecular geometry, such as tetrahedral versus trigonal planar structures, lead to characteristic bond angles that are essential for understanding the overall shape and reactivity of a compound.

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