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Chapter 12: Problem 1

For each of the following substances describe the importance of dispersion (London) forces, dipoledipole interactions, and hydrogen bonding: (a) \(HCl;\) (b) \(\mathrm{Br}_{2} ;\) (c) ICl; (d) \(\mathrm{HF} ;\)\ (e) \(\mathrm{CH}_{4}\)

Short Answer

Expert verified
HCl exhibits dispersion forces and dipole-dipole interactions. Br2 and CH4 only exhibit dispersion forces. ICl exhibits dispersion forces and dipole-dipole interactions. HF exhibits all three forces: dispersion, dipole-dipole, and hydrogen bonding.

Step by step solution

01

Identify the Type of Substance in HCl

HCl is a polar covalent compound and hence, it exhibits dipole-dipole forces and dispersion forces. Hydrogen bonding is not observed in HCl, as it does not contain a hydrogen atom bonded to F, O, or N.
02

Identify the Type of Substance in Br2

Br2 is a nonpolar covalent compound. In nonpolar compounds, only dispersion forces exist. Thus, Br2 exhibits dispersion (London) forces.
03

Identify the Type of Substance in ICl

ICl is a polar covalent compound, thus it exhibits dipole-dipole forces and dispersion forces. Just like HCl, ICl does not present hydrogen bonding since it lacks a hydrogen atom that is directly bonded to F, O or N.
04

Identify the Type of Substance in HF

HF is a polar covalent compound that contains a hydrogen atom bonded to F. Thus, apart from dispersion forces and dipole-dipole forces, HF also exhibits hydrogen bonding.
05

Identify the Type of Substance in CH4

Finally, CH4 is a nonpolar covalent compound, just as Br2. Therefore, it only exhibits dispersion (London) forces.

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