Chapter 12: Intermolecular Forces and the Liquid State

These flashcards cover important vocabulary and concepts related to intermolecular forces and the states of matter discussed in Chapter 12.

Condensed States

The states of matter comprising solids and liquids.

Kinetic Molecular Theory

A theory that describes gases as being in constant, random motion.

Intermolecular Forces

Forces that are responsible for the attractions between molecules in condensed states.

Thermal Energy

Energy that is associated with the temperature of an object, related to the motion of its molecules.

Molar Volume

The volume occupied by one mole of substance, which is significantly larger in gases than in solids or liquids.

Crystalline Solids

Solids with an ordered three-dimensional arrangement of particles.

Amorphous Solids

Solids that lack a defined structure and do not have long-range order.

Phase Transition

The transformation from one state of matter to another, such as solid to liquid or liquid to gas.

Dipole-Dipole Force

Attraction between polar molecules that occurs when the positive end of one polar molecule is attracted to the negative end of another.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs between molecules containing hydrogen bonded to highly electronegative atoms like F, O, or N.

Ion-Dipole Force

The force of attraction between an ion and a polar molecule, significant in solutions of ionic compounds.

Surface Tension

The tendency of liquid surfaces to shrink into the least surface area possible, due to cohesive forces.

Viscosity

The resistance of a liquid to flow, influenced by intermolecular forces.

Capillary Action

The ability of a liquid to flow in narrow spaces without the assistance of external forces, due to cohesive and adhesive forces.

Vaporization

The phase transition from liquid to gas, which is an endothermic process.

Dynamic Equilibrium

A state in which the rates of condensation and vaporization are equal, leading to a constant concentration of vapor.

Critical Temperature

The temperature above which a gas cannot be liquefied, regardless of the pressure applied.

Sublimation

The transition of a substance from solid to gas without passing through the liquid state.

Fusion

The phase transition from solid to liquid, also known as melting.

Heat of Vaporization (ΔHvap)

The amount of energy required to vaporize one mole of a liquid at its boiling point.

Phase Diagram

A graphical representation of the phases of a substance at different temperatures and pressures.

Specific Heat Capacity

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.

Polarity

The distribution of electrical charge over the atoms joined by the bond, which influences the interactions between molecules.