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Chapter 10: Problem 26

Use valence bond theory to explain the bonding in \(\mathrm{Cl}_{2}\) and \(\mathrm{HCl}\). Show how the atomic orbitals overlap when a bond is formed.

Short Answer

Expert verified
Valence Bond Theory explains that a bond is formed due to overlapping of atomic orbitals. In \(\mathrm{Cl}_{2}\), the \(\mathrm{Cl}\)-\(\mathrm{Cl}\) bond results from the overlap of the atomic orbitals of two Chlorine atoms, each contributing one electron. In \(\mathrm{HCl}\), the \(\mathrm{H}\)-\(\mathrm{Cl}\) bond forms through the overlapping of s orbital of Hydrogen and a p orbital of Chlorine, with each atom contributing one electron to form a sigma bond.

Step by step solution

01

Understanding VBT and Overlapping of Atomic Orbitals in \(\mathrm{Cl}_{2}\)

According to Valence Bond Theory, a chemical bond is formed by the overlapping of atomic orbitals, with each creating a strong attractive force between the electron pair in the bond and the atomic nuclei. In \(\mathrm{Cl}_{2}\), each Chlorine atom has 7 electrons in its outer shell. These Chlorine atoms can contribute one electron each for the bond formation, and thus the atomic orbitals of the two Chlorine atoms overlap with each other. The overlapping atomic orbitals result in a shared electron pair, forming a covalent bond. Thus, \(\mathrm{Cl}_{2}\) molecule forms a single covalent bond.
02

Understanding VBT and Overlapping of Atomic Orbitals in \(\mathrm{HCl}\)

The process of bond formation in \(\mathrm{HCl}\) is similar to \(\mathrm{Cl}_{2}\). However, it involves different atoms, i.e., Hydrogen (H) and Chlorine (Cl). Both of these atoms contribute one electron each for the bond formation. The s orbital in Hydrogen overlaps with one of the p orbitals in Chlorine to form a sigma bond. The overlapping of orbitals results in a shared electron pair, forming a covalent bond in \(\mathrm{HCl}\).

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Most popular questions from this chapter

Predict the geometries of the following species: (a) \(\mathrm{AlCl}_{3},\) (b) \(\mathrm{ZnCl}_{2}\), (c) \(\mathrm{ZnCl}_{4}^{2-}\).

In the trigonal bipyramidal arrangement, why does a lone pair occupy an equatorial position rather than an axial position?

What is the relationship between the dipole moment and the bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?

Aluminum trichloride \(\left(\mathrm{AlCl}_{3}\right)\) is an electrondeficient molecule. It has a tendency to form a dimer (a molecule made of two \(\mathrm{AlCl}_{3}\) units): $$ \mathrm{AlCl}_{3}+\mathrm{AlCl}_{3} \longrightarrow \mathrm{Al}_{2} \mathrm{Cl}_{6} $$ (a) Draw a Lewis structure for the dimer. (b) Describe the hybridization state of \(\mathrm{Al}\) in \(\mathrm{AlCl}_{3}\) and \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\). (c) Sketch the geometry of the dimer. (d) Do these molecules possess a dipole moment?

What hybrid orbitals are used by nitrogen atoms in the following species? (a) \(\mathrm{NH}_{3}\), (b) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{NH}_{2}\) (c) \(\mathrm{NO}_{3}^{-}\)
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