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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 are stronger in \(H_{2}O(l)\) (liquid water) than in \(H_{2}O(g)\) (gaseous water). This is because in its liquid form, water displays significant hydrogen bonding, which is a strong type of intermolecular force. In its gas form, these hydrogen bonds are mostly broken due to increased molecular movement, making the intermolecular forces weaker.

Step by step solution

01

Understand Intermolecular Forces

Intermolecular forces are forces of attraction between molecules. These forces play a key role in determining the physical and chemical properties of substances. Types of intermolecular forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Hydrogen bonding is the strongest type among these.
02

Determine Intermolecular Forces in \(H_{2}O(l)\)

In the liquid phase, \(H_2O\), or water, has strong hydrogen bonding due to the polarity of the molecule. This means that the oxygen atom of one water molecule is attracted to the hydrogen atoms of other water molecules, resulting in a 'network' of water molecules held together by these strong hydrogen bonds.
03

Determine Intermolecular Forces in \(H_{2}O(g)\)

In the gas phase, however, these hydrogen bonds are mostly broken due to increased kinetic energy of the individual molecules in the gaseous state. While some hydrogen bonding may still be present between gas molecules, it is significantly less compared to that in the liquid phase.
04

Compare Intermolecular Forces

Comparing these two states, it can be concluded that intermolecular forces in \(H_2O(l)\) are stronger than in \(H_2O(g)\). In the gaseous state, the intermolecular forces are weakened because the molecules are spread out and move more freely, reducing the chances for hydrogen bonds to form.

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Most popular questions from this chapter

Find an alkane, a ketone, and an alcohol with roughly the same MW (within 5 \(\mathrm{g} / \mathrm{mole}\) ). Rank these compounds in terms of relative boiling points.

What is the difference between intramolecular bonds and intermolecular forces?

Is the strength of intermolecular forces determined by the bond strengths within the individual molecules? Explain your reasoning.

When water evaporates, are any bonds between \(\mathrm{H}\) atoms and \(\mathrm{O}\) atoms within \(\mathrm{a}\) molecule broken?

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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