Pre-IB Chemistry Chapter 10

Kinetic-Molecular Theory

Particles of matter are always in motion

Ideal Gas

hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

Gas consists of large numbers of tiny particles that are far apart _____ to their size.

relative

Collisions between gas particles and between particles and container walls are __________.

elastic collision

Gas particles are in ______, _____, ______ motion.

continuous, rapid, random

There are no forces of _____ between gas particles.

attraction

The _____ of the gas depends on the average kinetic energy of the particles of the gas.

temperature

Gas do not have a ______ shape or ______ volume.

definite

Gas has a _____ density.

low

Diffusion

spontaneous mixing of the particles of two substances caused by their random motion

Effusion

process by which gas particles pass through a tiny opening

Real Gas

a gas that does not behave completely according to the assumptions of the kinetic-molecular theory

Fluid

a substance that can flow and therefore take the shape of its container

Liquids have a relative ____ density.

high

Liquids are _____ compressible.

less

Liquids have the ability to ____.

diffuse

Surface Tension

a force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size

Surface tension cause liquid droplets to take on a spherical shape because a sphere has the smallest possible ________.

surface area

Capillary Action

the attraction of the surface of a liquid to the surface of a solid

Vaporization

the process by which a liquid or solid changes to a gas

Evaporation

the process by which particles escape from the surface of a non-boiling liquid and enter the gas state.

Freezing

the physical change of a liquid to a solid by removed of energy as heat

Solids have a _____ shape and volume.

definite

Crystalline Solids

a solid that consists of crystals

Crystal

a substance in which the particles are arranged in an orderly, geometric, repeating pattern.

Amorphous solid

in which the particles are arranged randomly

The volume of a solid changes slightly with a change in temperature or pressure because _______.

their particles are packed closely together

Melting

the physical change of a solid to a liquid by the addition of energy as heat

Melting Point

the temperature at which a solid becomes a liquid

Supercooled Liquids

substances that retain certain liquid properties even at temperatures at which they appear to be solid

Solids have a _____ density.

high

Solids have a low rate of ________.

diffusion

Crystal structure

The total three-dimensional arrangement of particles of a crystal

Unit Cell

The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice.

Ionic Crystals

positive and negative ions arranged in a regular pattern

Covalent Network Crystals

they are hard, brittle, and have high melting points

Metallic crystals

made up on delocalized valence electrons

Covalent Molecular Crystals

consists of covalently bonded molecules held together by intermolecular forces

Phase

any part of a system that has uniform composition and properties

Condensation

the process by which a gas changes to a liquid

Equilibrium

a dynamic condition in which two opposing changes occur at equal rates in a closed system

sublimation

solid to gas

deposition

gas to solid

Equilibrium Vapor Pressure

The pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature

Volatile Liquids

liquids that evaporate easily

boiling

the conversion of a liquid to a vapor within the liquid as well as at its surface

boiling point

the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure

freezing point

the temperature at which the solid and liquid are in equilibrium at 1 ATM pressure

phase diagram

a graph of pressure versus temperature that shows the conditions under which the phases of a substance exist

triple point

a substance indicates the temperature and pressure conditions at which the solid, liquid, and vapor of the substance can coexist at equilibrium

Critical Point

indicates the critical temperature and critical pressure

critical temperature

temperature above which the substance cannot exist in the liquid state

critical pressure

the lowest pressure at which the substance can exist as a liquid at the critical temperature

Intramolecular

within the molecule(stronger)

Intermolecular

between molecules(weaker)

Example of Intermolecular Forces

hydrogen bonding

Example of Intramolecular Forces

covalent, ionic, and metallic bond