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States of Matter
States of Matter
21
Chemistry
10th Grade
03/26/2012

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Cards

Term

 

Properties of Gases

Definition

 

1) they exert pressure

2) they exist at different, measurable temperatures

3) they take up space (have volume)

4) they have low (weak) intermolecular forces between molecules(that's why they are gases)

Term

 

Kinetic Theory

Definition

1) the particles in a gas are assumed to be small, hard spheres with an insignificant volume

2)  the motion of particles in a gas is rapid and random.

3)  the collisions between gas particles are perfectly elastic

Term

 

Gas Pressure

Definition

 

results from the force exerted by a gas per unit surface area of an object

Term

 

Atmospheric Pressure

Definition

 

a result of the collisions of atoms and molecules in the air with objects

Term

 

Absolute Zero

Definition

 

the theoretical temperature at which gas molecules have no kinetic energy and where they  have zero volume and exert zero pressure

Term

 

Intermolecular Forces

Definition

 

the interactions between disruptive motions of particles in a liquid and the attractions among the particles

Term

 

Vaporization

Definition

 

the conversion of a liquid to a gas or a vapor

Term

 

Evaporation

Definition

 

the conversion of a liquid to a gas or vapor at a temperature below the boiling point.  Occurs at the surface of a liquid.

Term

 

Vacuum

Definition

 

an empty space with no particles or matter

Term

 

Barometer

Definition

 

a device used to measure atmospheric pressure

Term

 

Vapor Pressure

Definition

 

a measure of the force exerted by a gas above a liquid

Term

 

Dynamic Equilibrium

Definition

 

when the rate of evaporation of a liquid equals the rate of condensation of a vapor

Term

 

Manometer

Definition

 

a device used to measure vapor pressure

Term

 

Boiling Point

Definition

 

the temperature at which the vapor pressure of the liquid is just equal to the external pressure on the the liquid

Term

 

Normal Boiling Point

Definition

 

the temperature at which a liquid boils at a apressure of 101.3 kPa (or 760 mm Hg or 1 atm)

Term

 

Condensation

Definition

 

transition from the vapor (gas) phase to the liquid phase

Term

 

Melting

Definition

 

transition from the solid phase to the liquid phase

Term

 

Freezing

Definition

 

the transition from the liquid phase to solid phase

Term

 

Sublimation

Definition

 

transition from the solid phase to the gas phase

Term

 

Critical Point

Definition

 

the temperature above which a substance cannot exist as a liquid.  It will be a gas no matter what pressure

Term

 

Triple Point

Definition

 

the only set of conditions at which all three phases can exist in equilibrium with one another

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