States of Matter and Kinetic Molecular Theory Vocabulary

Vocabulary flashcards based on lecture notes about states of matter and kinetic molecular theory.

Evaporation

A slow process that occurs at the surface of a liquid.

Boiling

A rapid process that happens throughout the liquid.

Rate of Diffusion

How tightly the particles are packed together.

Crystalline Solid

Particles have orderly, geometric structure, consists of unit cells, and have a defined melting point.

Amorphous Solid

Particles are not orderly, does not contain crystals, and does not have a defined melting point.

Ice

The only solid to be less dense than its liquid counterpart.

Property of Gas

Gas: weak intermolecular forces.

Ionic Solid

Positive and negative ions with strong ionic bonds; hard and brittle with high melting points.

Kinetic Molecular Theory

Describes the behavior of matter in terms of particles of motion, making assumptions about particle size, motion, and energy.

Gas Particle Motion

Small particles separated and in random constant motion.

Kinetic Energy Formula

KE = 1/2mV^2

Temperature

Measure of average kinetic energy of the particles in a sample of matter; as temperature increases, molecular motion increases.

States of Matter Able to Flow

Gas and Liquid

Compressible State of Matter

Gas

Diffusion

Movement of one material through another.

Effusion

When gas escapes through a tiny opening.

Least Common State of Matter

Liquid

Kinetic Molecular Theory (Liquids)

a. no defined shape; b. constant motion; c. particles closer and lower in energy than gas particles; d. attraction forces are stronger than gases; e. Liquids are more orderly

Why Liquids Diffuse Slower Than Gases

There are more collisions with liquid particles because they are packed together.

Viscosity

Measure of resistance to flow.

Covalent Network Crystals

Atoms share electrons with neighbors; covalent bonds are strong; hard and brittle with high melting points.

Metallic Crystals

Element; sea of electrons - force between atoms of same metal; high electrical conductivity; wide range of boiling and melting points.

Covalent Molecular Crystals

Covalently bonded molecules held together by intermolecular forces; IMF's are weaker than ionic and metallic; soft and volatile, low melting points.

Equilibrium

Condition where two opposing charges occur at equal rates in a closed system.

Condensation

Gas to liquid; heat is released.

Freezing

Liquid to solid; heat is released.

Deposition

Gas to solid; heat is released.

Vaporization

Liquid to gas; heat is absorbed.

Melting

Solid to liquid; heat is absorbed.

Sublimation

solid to vapor phase; heat is absorbed.

Exothermic

Heat is released

Endothermic

Heat is absorbed

Temperature During Phase Change

Temperature remains constant until complete.

Boiling Point

Temperature at which the vapor pressure of the liquid is equal to the atmospheric pressure.

Vapor Pressure

Pressure exerted by a vapor at a given temp.

Molar Heat of Vaporization

Amount of heat required to vaporize one mole of a liquid at its boiling point.

Freezing Point

Temperature at which the solid and liquid phases are in equilibrium.

Molar Heat of Fusion

Energy required to melt one mole of a solid at its melting point.

Phase Diagrams Show

The condition where gas, liquid, and solid of a substance exist.

Triple Point

Single temp and pressure condition where all three states are occurring at the same time.