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Chapter 13: Problem 8

What is boiling point? How does it depend on intermolecular forces?

Short Answer

Expert verified
Boiling point is the temperature at which a liquid turns into vapor. It depends on the strength of intermolecular forces; stronger forces lead to higher boiling points.

Step by step solution

01

- Define Boiling Point

Boiling point is the temperature at which a liquid's vapor pressure equals the external pressure surrounding the liquid, causing it to turn into vapor.
02

- Understand Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions). Common types include hydrogen bonds, dipole-dipole interactions, and London dispersion forces.
03

- Relationship Between Boiling Point and Intermolecular Forces

The boiling point of a substance is influenced by the strength of its intermolecular forces. Stronger intermolecular forces require more energy (i.e., higher temperature) to break, thus increasing the boiling point. Conversely, weaker intermolecular forces require less energy to break, resulting in a lower boiling point.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

intermolecular forces
Intermolecular forces are the attractive or repulsive interactions between neighboring particles such as atoms, molecules, or ions. They govern many physical properties of substances, including their boiling points.
  • Types of Intermolecular Forces: There are several types of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and London dispersion forces.
  • Strength: The strength of these forces varies. For instance, hydrogen bonds are generally stronger compared to London dispersion forces.
  • Role in Boiling Point: Stronger intermolecular forces mean higher boiling points because more energy is needed to break these forces and convert the liquid into vapor.
Understanding intermolecular forces helps in predicting and explaining the boiling points of different substances.
hydrogen bonds
One of the strongest types of intermolecular forces is the hydrogen bond.
  • Formation: Hydrogen bonds form when a hydrogen atom is covalently bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine and is also attracted to another electronegative atom nearby.
  • Impact on Boiling Point: Substances with hydrogen bonds tend to have higher boiling points because a significant amount of energy is required to break these bonds during the phase change from liquid to vapor.
For example, water has a high boiling point relative to its molecular weight due to the presence of hydrogen bonds.
vapor pressure
Vapor pressure is the pressure exerted by the vapor when a liquid evaporates.
  • Equilibrium Condition: When a liquid's vapor pressure equals the external pressure, it begins to boil.
  • Relation to Boiling Point: At the boiling point, the vapor pressure of a liquid matches the surrounding atmospheric pressure, allowing bubbles to form within the liquid.
  • Influence of Intermolecular Forces: Liquids with strong intermolecular forces have lower vapor pressures at a given temperature, necessitating a higher temperature (higher boiling point) to reach equilibrium vapor pressure.
Understanding vapor pressure is vital for understanding why substances boil at different temperatures under different pressures.
temperature
Temperature is a measure of the average kinetic energy of particles in a substance. It significantly affects boiling points and phase changes.
  • Definition: Boiling point is the temperature at which a liquid鈥檚 vapor pressure equals the external pressure.
  • Energy Absorption: As temperature increases, the kinetic energy of the liquid's particles increases, weakening the intermolecular forces and facilitating the phase transition to vapor.
  • Practical Example: At higher altitudes where atmospheric pressure is lower, water boils at a temperature lower than 100掳C because it needs less energy to match the reduced pressure.
Thus, temperature and intermolecular forces are closely intertwined in determining the boiling point of a substance.

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Most popular questions from this chapter

Rank the following molecules in order of increasing London dispersion forces: \(\mathrm{CCl}_{4}, \mathrm{CI}_{4}\), and \(\mathrm{CBr}_{4}\).

Ether has a higher vapor pressure than water. Which of these two liquids has stronger intermolecular forces? Which liquid would you expect to have the higher boiling point?

The flow rate of a liquid is related to the strength of the cohesive forces between molecules. The stronger the cohesive forces, the harder it is for the molecules to slide past one another. Honey is a very thick liquid that pours slowly at ordinary temperatures. A student tried an experiment. She filled five eyedroppers with honey at different temperatures and then measured the rate of dripping for each sample (see the table below). Graph the rate of dripping versus temperature for the honey and propose a relationship between temperature and flow rate. Propose an explanation for the trend that you observe.

The specific heat of zinc is \(0.096 \mathrm{cal} / \mathrm{g}^{\circ} \mathrm{C}\). Determine the energy required to raise the temperature of 250 . \(g\) of zinc from room temperature \(\left(20.0^{\circ} \mathrm{C}\right)\) to \(150 .^{\circ} \mathrm{C}\).

You work in a hardware store and notice that whenever you spill water on the waxed floors it tends to bead up and stay fairly well confined. When you spill hexane, however, it spreads over the entire floor and is a big mess to clean up. Based on your knowledge of adhesive and cohesive forces, explain this difference in behavior.
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