Intermolecular Forces

Front

What are intermolecular forces?

Back

Intermolecular forces are the forces of attraction or repulsion between neighboring particles (molecules, atoms, or ions). They play a crucial role in determining the physical properties of substances.

Front

What is the strongest type of intermolecular force?

Back

Hydrogen bonding is the strongest type of intermolecular force, occurring when hydrogen is bonded to highly electronegative atoms like nitrogen, oxygen, or fluorine.

Front

What is the boiling point of a substance?

Back

The boiling point is the temperature at which a substance changes from a liquid to a gas, occurring when the vapor pressure of the liquid equals the atmospheric pressure.

Front

How do London dispersion forces arise?

Back

London dispersion forces arise from temporary fluctuations in electron distribution within molecules, leading to temporary dipoles that induce attraction between molecules.

Front

What is the role of dipole-dipole interactions?

Back

Dipole-dipole interactions occur between polar molecules, where the positive end of one molecule is attracted to the negative end of another, influencing boiling and melting points.

Front

What phase change occurs when a solid turns into a liquid?

Back

Melting is the phase change that occurs when a solid absorbs heat and turns into a liquid.

Front

What is condensation?

Back

Condensation is the phase change in which a gas turns into a liquid, typically occurring when the gas is cooled or compressed.

Front

What is evaporation?

Back

Evaporation is the process by which molecules at the surface of a liquid gain enough energy to enter the gas phase, requiring energy input.

Front

How do intermolecular forces affect boiling points?

Back

Stronger intermolecular forces result in higher boiling points, as more energy is required to overcome these forces during the phase change from liquid to gas.

Front

What is kinetic molecular theory?

Back

Kinetic molecular theory explains the behavior of gases, stating that gas particles are in constant, random motion and that they do not attract or repel each other.