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Chapter 6: Problem 32

Consider the molecules \(\mathrm{HCl}\) and \(\mathrm{HBr}\). (a) Which molecule has the larger bond dipole moment? Explain why. (b) Which molecule is more polar? Explain why.

Short Answer

Expert verified
(a) HCl has the larger bond dipole moment due to the larger difference in electronegativity between H and Cl (\(0.96 > 0.76\)). (b) HCl is more polar because it has a larger bond dipole moment compared to HBr.

Step by step solution

01

Understand bond dipole moments

A bond dipole moment is a measure of the polarity of a chemical bond between two atoms. It results from the difference in electronegativity between the two atoms. The greater the difference in electronegativity, the larger the bond dipole moment.
02

Compare electronegativity between HCl and HBr

Firstly, we need to understand the electronegativity values of the individual elements. Hydrogen (H) has an electronegativity of 2.20, while chlorine (Cl) has an electronegativity of 3.16 and bromine (Br) has an electronegativity of 2.96. We can calculate the electronegativity difference for each molecule as follows: HCl: \(|3.16 - 2.20| = 0.96\) HBr: \(|2.96 - 2.20| = 0.76\)
03

Determine bond dipole moments

Since HCl has a larger difference in electronegativity, it has a larger bond dipole moment compared to HBr. Therefore, the answer to part (a) is that HCl has the larger bond dipole moment.
04

Understand molecularity and polarity

Molecularity refers to the number of atoms in a molecule, while polarity refers to the distribution of the molecules' charges. In our case, both HCl and HBr are diatomic molecules, meaning they each have only two atoms.
05

Compare the polarity of HCl and HBr

Since both HCl and HBr are diatomic molecules, the polarity of each molecule is determined by their bond dipole moments. We have already established that HCl has a larger bond dipole moment than HBr. As a result, the HCl molecule is more polar than the HBr molecule. Therefore, the answer to part (b) is that HCl is more polar than HBr. In conclusion: (a) HCl has a larger bond dipole moment due to the larger difference in electronegativity between H and Cl. (b) HCl is more polar because it has a larger bond dipole moment compared to HBr.

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Most popular questions from this chapter

Which, if any, of these molecules do you expect to be polar: \(\mathrm{CO}_{2}, \mathrm{CS}_{2}\), or \(\mathrm{CSO}\) (carbon is the central atom in all three molecules)? Explain your answer.

Why do we use an arrow to represent a bond dipole moment? Why not just use a number?

What is the difference between intermolecular forces and intramolecular forces? Which are stronger?

Shown below are dot diagrams for some simple molecules and polyatomic ions: \(: \ddot{B r}-\dot{S}_{\cdots}^{\prime \prime}-\vec{B}_{r}^{\prime \prime}\) (a) Draw the three-dimensional shape for each molecule. Use lines, solid wedges, and dashed wedges as necessary. Indicate the numeric value of all bond angles. (b) For each species, name both the electrongroup geometry around the central atom and the molecular shape.

Two molecules may both be correctly described as bent, even though one has a bond angle of approximately \(118^{\circ}\) and the other has a bond angle of approximately \(105^{\circ} .\) How is this possible?
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