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Chapter 9: Problem 22

Use the localized electron model to describe the bonding in \(\mathrm{CCl}_{4}\) .

Short Answer

Expert verified
In the localized electron model (LEM), the bonding in CCl4 is described as covalent, with the central Carbon (C) atom sharing electrons with each of the four Chlorine (Cl) atoms. The central Carbon atom undergoes sp3 hybridization, forming four equivalent hybrid orbitals that overlap with orbitals of Chlorine atoms to create sigma bonds. The molecular geometry of CCl4 is tetrahedral, which is consistent with the electron domain geometry based on the Valence Shell Electron Pair Repulsion (VSEPR) theory.

Step by step solution

01

Determine the number of valence electrons for Carbon and Chlorine atom

Carbon (C) has 4 valence electrons, as it belongs to Group 4 in the periodic table. Chlorine (Cl) has 7 valence electrons, being a member of Group 7. Since there are 4 Chlorine atoms bonded to a single Carbon atom, we have a total of 4 * 7 + 4 = 32 valence electrons.
02

Write the Lewis structure of CCl4

In the Lewis structure, we need to represent the valence electrons of each atom and depict how they are shared between the atoms to form bonds. In CCl4, Carbon forms four single bonds with four Chlorine atoms, as each atom contributes one electron to form a single bond. The Lewis structure of CCl4 is: Cl | C - Cl | Cl
03

Find the electron domain geometry around the central atom

The electron domain geometry around the central Carbon atom can be determined based on the number of electron domains (bonding and non-bonding). In CCl4, there are four bonding domains around the central Carbon atom with no non-bonding pairs of electrons. According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, the electron domain geometry of CCl4 is tetrahedral.
04

Determine the molecular geometry of CCl4

As all electron domains around the central Carbon atom are occupied by bonding electron pairs, the molecular geometry is the same as the electron domain geometry, which is a tetrahedron.
05

Using Localized Electron Model (LEM) to describe the bonding in CCl4

LEM is a model that assumes electrons in a molecule are localized (either shared between two atoms or localized around a single atom). In CCl4, bonding between Carbon and Chlorine is covalent, and electrons are shared between Carbon and each Chlorine atom. Each of the 4 C-Cl bonds can be described as sigma bonds, involving the overlap of sp3 hybrid orbitals from Carbon and Chlorine. The sp3 hybridization of the central Carbon atom leads to the formation of four equivalent hybrid orbitals that form bonds with Chlorine atom orbitals, resulting in a tetrahedral molecular geometry.

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Most popular questions from this chapter

The molecules \(\mathrm{N}_{2}\) and \(\mathrm{CO}\) are isoelectronic but their properties are quite different. Although as a first approximation we often use the same MO diagram for both, suggest how the \(\mathrm{MOs}\) in \(\mathrm{N}_{2}\) and \(\mathrm{CO}\) might be different.

Describe the bonding in the \(\mathrm{O}_{3}\) molecule and the \(\mathrm{NO}_{2}^{-}\) ion using the localized electron model. How would the molecular orbital model describe the \(\pi\) bonding in these two species?

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The three most stable oxides of carbon are carbon monoxide \((\mathrm{CO}),\) carbon dioxide \(\left(\mathrm{CO}_{2}\right),\) and carbon suboxide \(\left(\mathrm{C}_{3} \mathrm{O}_{2}\right) .\) The space-filling models for these three compounds are For each oxide, draw the Lewis structure, predict the molecular structure, and describe the bonding (in terms of the hybrid orbitals for the carbon atoms).
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