Based on your knowledge of intermolecular forces and trends, select the statement that is most accurately compares HF and HCl.

(A) The intermolecular attraction between HF molecules are stronger than between HCl molecules mainly to due hydrogen bonding.

(B) The intermolecular attraction between HF molecules are stronger than between HCl molecules mainly to due larger London dispersion forces.

(C) The intermolecular attraction between HCl molecules are stronger than between HF molecules mainly to due larger dipole-dipole forces.

(D) The intermolecular attraction between HCl molecules are stronger than between HF molecules mainly to due larger hydrogen bonding and London dispersion forces.

Question

Chemistry

Emily Welch

14 April, 08:33

Based on your knowledge of intermolecular forces and trends, select the statement that is most accurately compares HF and HCl.

(A) The intermolecular attraction between HF molecules are stronger than between HCl molecules mainly to due hydrogen bonding.

(B) The intermolecular attraction between HF molecules are stronger than between HCl molecules mainly to due larger London dispersion forces.

(C) The intermolecular attraction between HCl molecules are stronger than between HF molecules mainly to due larger dipole-dipole forces.

(D) The intermolecular attraction between HCl molecules are stronger than between HF molecules mainly to due larger hydrogen bonding and London dispersion forces.

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Answers (1)

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Chance · Answer 1

(A) The intermolecular attraction between HF molecules are stronger than between HCl molecules mainly to due hydrogen bonding.

Explanation:

Since Flourine is highly electronegative and as such, when it bonds with Hydrogen it forms a hydrogen bond. Whereas the HCL molecule is a polar molecule whose inter-molecular forces are dipole dipole interactions. Although a Hydrogen bond is a type of dipole dipole interaction it is stronger than the traditional dipole dipole forces and London dispersion forces. HF also has a shorter bond length which makes the bond and inter-molecular forces stronger as compared to HCL.