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Chapter 2: Problem 22

Hydrogen fluoride, HF, is a liquid at \(15^{\circ} \mathrm{C}\) . All other hydrogen halides (represented by HX, where \(\mathrm{X}\) is any other halogen) are gases at the same temperature. Why? (A) Fluorine has a very high electronegativity; therefore, the H–F bond is stronger than any other H–X bond. (B) HF is smaller than any other H–X molecule; therefore, it exhibits stronger London dispersion forces. (C) The dipoles in a HF molecule exhibit a particularly strong attraction force to the dipoles in other HF molecules. (D) The H–F bond is the most ionic in character compared to all other hydrogen halides.

Short Answer

Expert verified
The most reasonable explanation for hydrogen fluoride, HF, being a liquid at \(15^{\circ} \mathrm{C}\) while other hydrogen halides are gases is because the dipoles in an HF molecule exhibit a particularly strong attraction force to the dipoles in other HF molecules, this allows it to stay in the liquid state (C).

Step by step solution

01

Analyze Answer (A)

Fluorine indeed has a high electronegativity which results in a strong H-F bond. But the strength of the bond doesn't influence the state of the substance, rather it'll impact the bond dissociation energy. Hence, option (A) does not correctly answer the question.
02

Analyze Answer (B)

London dispersion forces are induced instantaneous dipole-induced dipole attractions. These increase as the size and shape of the molecule increases not the other way around. Therefore, since HF is smaller than other HX molecules it would not have stronger London dispersion forces. Option (B) is hence incorrect.
03

Analyze Answer (C)

HF molecule is indeed polar which contributes to the dipole-dipole interactions between HF molecules. These intermolecular forces have a significant impact on the state of the substance. Given HF's high polarity, it's plausible that such forces could contribute to it being a liquid at the given temperature. This makes option (C) a likely answer.
04

Analyze Answer (D)

While the H-F bond does have a high ionic character, this trait does not explain HF's liquid state at 15 degrees Celsius since bond ionicity influences bond strength, not the state of the substance. So, option (D) is not correct.

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