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Chapter 11: Problem 4

Describe the molecular geometry of \(\mathrm{CCl}_{4}\) suggested by each of the following methods: (a) Lewis theory; (b) valence-bond method using simple atomic orbitals; (c) VSEPR theory; (d) valence-bond method using hybridized atomic orbitals.

Short Answer

Expert verified
The molecular geometry of \(\mathrm{CCl}_{4}\) is tetrahedral according to all four methods: Lewis theory, valence-bond method using simple atomic orbitals, VSEPR theory, and valence-bond method using hybridized atomic orbitals.

Step by step solution

01

Lewis Theory Analysis

According to the Lewis theory, all atoms achieve a noble gas configuration. The central carbon atom shares its 4 electrons with 4 chlorine atoms, each contributing one electron leading to formation of 4 single covalent bonds. This results in the tetrahedral geometric shape.
02

Valence-Bond Method Using Simple Atomic Orbitals

In this method, atomic orbitals of the carbon atom overlap with atomic orbitals of the chlorine atom to form covalent bonds. The four 2p orbitals of the carbon overlap individually with the 3p orbitals of the four chlorine atoms. This creates 4 individual bonds resulting in a tetrahedral geometry.
03

VSEPR Theory Analysis

The Valence Shell Electron Pair Repulsion (VSEPR) theory suggests that electron pairs arranged around the central atom will orient themselves as far apart as possible to minimize repulsion. Carbon has 4 bonding pairs and no lone pairs, so according to VSEPR theory, this leads to a tetrahedral geometry.
04

Valence-Bond Method Using Hybridized Atomic Orbitals

In this method, carbon's 2s and three 2p orbitals blend together to form four new sp3 hybrid orbitals which are oriented toward the corners of a regular tetrahedron. In CCl4, these hybridized orbitals overlap with chlorine's 3p orbitals, forming the bonds and giving the molecule a tetrahedral geometry.

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