Chemistry Vocab Unit 5

Surfactant

A compound that reduces the repulsion (tension between two liquid, a liquid and a solid, or a liquid and air

Barometer

A device for measuring pressure

Plasma

A high energy state of matter characterized by ionized particles

Solid

A low energy state of condensed matter characterized by structural rigidity and resistance to changes of shape or volume

Lattice

A regular arrangement of particles (atoms, ions, molecules)

Crystal

A solid in which the particles are arranged in a regular, repeating pattern

Amorphous solid

A solid matter whose particles are arranged in a nonuniform pattern

Thermal equilibrium

A term describing a temperature equal to that of the surroundings

Long-Range order

A term for arrangement of particles characterized by structural rigidity and resistance to changes of shape or volume

Ideal Gas

A theoretical gas composed of random non-interacting point particles

Sublimation

A transition directly from solid to vapor phase

Deposition

A transition directly from vapor to solid phase

Freezing

A transition from liquid to solid phase

Boiling

A transition from liquid to vapor phase

Melting

A transition from solid to liquid phase

Condensing

A transition from vapor to liquid phase

Ideal gas law

An equation that relates volume, pressure, absolute temperature, and number of moles of a gas under ideal conditions

Partial pressure

An individual gas's contribution to the total pressure exerted by a mix of gases

Immiscible

Referring to a solid, liquid, or gas into a host liquid (solvent)

Ideal gas constant

The constant that is used to relate volume, pressure, absolute temperature, and number of miles of a gas in the ideal gas law equation

Kinetic energy

The energy associated with movement

Pressure

The force exerted by the particles of a gas colliding with the walls of a container

Combined gas law

The law that combined Boyle's, Charle's, and Gay-Lusaac's law, and states that for a fixed quantity of a gas, the pressure varies inversely with volume, while the temperature varies directly with pressure and volume

Gay-Lussac's Law

The law that states that the pressure and absolute temperature of a fixed quantity of a gas are directly proportional under constant volume conditions

Boyle's Law

The law that states that the pressure and volume of a fixed quantity of a gas are inversely proportional under constant temperature conditions

Dalton's Law

The law that states that the total pressure exerted by a mixture of gases is the sum of the individual partial pressures of the gases in the mixture

Charle's Law

The law that states that the volume and absolute temperature of a fixed quantity of a gas are directly proportional under constant pressure conditions

Avogrado's Law

The law that states that the volume of a gas is proportional to the number of moles of the gas when pressure and temperature are kept constant

Effusion

The movement of gas from a small opening into a larger volume

Vapor pressure

The pressure exerted by the gas in equilibrium with a pure liquid at a given temperature

Surface tension

The property of the surface of a liquid that allows it to resist and external force

Diffusion

The spread of particles through random motion from regions of high concentration to regions of low concentration

Standard temperature and pressure

The standard conditions used to compare gas measurements, defined as an absolute temperature of 273.15 K and a pressure 100 kPa

Kinetic-Molecular theory

The theory that describes gases as a large number of constantly randomly moving particles (atom/molecules) that collide with one another and with the walls of the container

Viscosity

The thickness of resistance to flow of a liquid

Molar volume

The volume of one mole of any ideal gas STP=22.4 L

Dissolve

To integrate a solid, liquid, or gas into a host liquid (solvent)