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Chapter 27: Problem 2

On average, are the intermolecular forces stronger in \(\mathrm{H}_{2} \mathrm{O}(\boldsymbol{\ell})\) or in \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) ? Explain.

Short Answer

Expert verified
The intermolecular forces in liquid water (H2O(l)) are stronger than in water vapor (H2O(g)) due to the closer proximity of the water molecules in the liquid phase, which allows for more significant hydrogen bonding.

Step by step solution

01

Identify the Phase and Intermolecular Forces

First, identify the phases being compared - liquid (H2O(l)) and gas (H2O(g)). H2O, or water, is capable of forming relatively strong hydrogen bonds due to its polar nature.
02

Compare Intermolecular Forces

In the liquid phase, the molecules are closer together and therefore the intermolecular forces, specifically hydrogen bonds, will be stronger. In the gaseous phase, the water molecules are more spread out and can move freely, meaning the intermolecular forces will be weaker.
03

Draw Conclusion

So, based on these analyses, we can conclude that H2O(l) would have stronger intermolecular forces than H2O(g).

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Most popular questions from this chapter

In terms of intermolecular forces, why does the boiling point of a particular type of compound (for example, an alkane) increase as the molecular weight increases?

In the ketones: a) what type(s) of intermolecular force is (are) present? b) what is the strongest intermolecular force present?

Rank these intermolecular forces in terms of their typical relative strengths: hydrogen bonding; dipole-dipole; induced dipole-induced dipole.

In the alcohols: a) what type(s) of intermolecular force is (are) present? b) what is the strongest intermolecular force present?

Recall that the electronegativity of \(\mathrm{C}\) and \(\mathrm{H}\) are roughly the same, but that \(\mathrm{O}\) has a significantly higher electronegativity. For each type of compound (alkane, ketone, alcohol) predict whether or not the compound is expected to be polar or nonpolar.
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