Solids, Liquids, & Gases

I. States of MatterKinetic Molecular Theory

Four States of Matter

Thermal Expansion

MATTER

A. Kinetic Molecular Theory

KMT

All matter is composed of small particles (atoms, molecules, ions).

These particles are in constant, random motion.

Motion is dependent on temperature. Higher temp. = higher KE.

Thermal energy Total energy of a material’s particles KE – vibration and movement between

particles PE – results from forces acting within

or between particles Thermal Energy (Heat) = KE + PE

A. Kinetic Molecular Theory

B. Four States of Matter

Solids low KE - particles vibrate but

can’t move around definite shape & volume crystalline - repeating

geometric pattern amorphous - no pattern (e.g.

glass, wax)

B. Four States of Matter

Liquids higher KE - particles can

move around but are still close together

indefinite shape definite volume

B. Four States of Matter

Gases high KE - particles can

separate and move throughout container

indefinite shape & volume

B. Four States of Matter

Plasma very high KE - particles collide with

enough energy to break into charged particles (+/-)

gas-like, indefiniteshape & volume

stars, fluorescentlight bulbs, TV tubes

C. Thermal Expansion

Most matter expands when heated & contracts when cooled.

Temp causes KE. Particles collide with more force & spread out.

EX: thermostats (bimetallic strip), sidewalks

Solids, Liquids, & Gases

II. Changes in StatePhase Changes

Heating Curves

MATTER

A. Phase Changes

Melting solid to liquid

Freezing liquid to solid

melting point = freezing point

A. Phase Changes

Vaporization (boiling) liquid to gas at the boiling point

Evaporation liquid to gas below the boiling point

Condensation gas to liquid

A. Phase Changes

Sublimation solid to gas EX: dry ice,

freeze drying, iodine

A. Phase Changes

B. Heating Curves

Kinetic Energy motion of particles related to temperature

Potential Energy space between particles related to phase changes

B. Heating Curves

Solid - KE

Melting - PE

Liquid - KE Boiling - PE

Gas - KE

B. Heating Curves

Heat of Fusion energy required to change from solid

to liquid some attractive forces are broken

B. Heating Curves

Heat of Vaporization energy required to change from liquid

to gas all attractive forces are broken EX: steam burns, sweating, and… the

drinking bird

HEATING CURVE

Solids, Liquids, & Gases

III. Properties of FluidsArchimedes Principle

Pascal’s Principle

Bernoulli’s Principle

Fluid Flow

MATTER

A. Archemides Principle

Buoyant force of an object in a fluid is equal to the weight of the fluid displaced

A. Pascal’s Principle

Pressure applied to a fluid is transmitted unchanged throughout the fluid.

A. Bernoulli’s Principle

Pressure exerted by a fluid decreases as its velocity increases.

Solids, Liquids, & Gases

IV. Behavior of Gases Pressure

Boyle’s Law

Charles’ Law

Gay-Lussac’s Law

MATTER

A. Pressure

area

forcepressure

Which shoes create the most pressure?

A. Pressure

Key Units at Sea Level

101.325 kPa (kilopascal)

1 atm

760 mm Hg

14.7 psi 2m

NkPa

A. Pressure

Barometer

Atm

osph

eric

Pre

ssur

e

Manometer

Con

tain

ed P

ress

ure

A. Pressure

Effect on Boiling Point When atmospheric pressure

increases, the boiling point of a liquid increases.

EX: high altitude cooking, boiling cold water

B. Boyle’s Law

When the volume of a gas decreases, its pressure increases (at constant temp).

P

V

PV = k

INVERSE

kT

VV

T

C. Charles’ Law

When the temperature of a gas increases, its volume also increases (at constant pressure).

DIRECT

C. Charles’ Law

Absolute Zero - Temp at which... the volume of a gas would equal zero. all particle motion would stop.

-273°Cor

0 K

kT

PP

T

C. Gay-Lussac’s Law

The pressure and absolute temperature (K) of a gas are directly related at constant mass & volume