STATES OF STATES OF MATTER MATTER

CHAPTER 3CHAPTER 3KONICHEKKONICHEK

DOES IT REALLY MATTER?DOES IT REALLY MATTER?

I. Classification of matterI. Classification of matter A. solids-definite shape and volumeA. solids-definite shape and volume 1. atoms are in an exact positions—just sit 1. atoms are in an exact positions—just sit

and vibrateand vibrate B. Liquid- no definite shape, but a definite B. Liquid- no definite shape, but a definite

volume.- Takes the shape of its container(fluid)volume.- Takes the shape of its container(fluid) 2. atoms flow around each other2. atoms flow around each other C. Gas(- No definite shape or volume.C. Gas(- No definite shape or volume. 3. atoms move freely- takes shape of its 3. atoms move freely- takes shape of its

container(fluid)container(fluid)

STATES OF MATTERSTATES OF MATTERSOLIDSSOLIDS

•Particles of solids are tightly packed, vibrating about a fixed position.

•Solids have a definite shape and a definite volume. Heat

STATES OF MATTERSTATES OF MATTERLIQUIDLIQUID

Particles of liquids Particles of liquids are tightly packed, are tightly packed, but are far enough but are far enough apart to slide over apart to slide over one another. one another.

Liquids have an Liquids have an indefiniteindefinite shape and shape and a a definitedefinite volume. volume. Heat

STATES OF MATTERSTATES OF MATTERGASGAS

Particles of Particles of gases are very gases are very far apart and far apart and move freely. move freely.

Gases have an Gases have an indefinite shape indefinite shape and an indefinite and an indefinite volume. volume. Heat

II. Other states of matterII. Other states of matter A. Plasma- exist at very high A. Plasma- exist at very high

temperaturestemperatures 1. stars, Lightning1. stars, Lightning 2. Most abundant form of matter in 2. Most abundant form of matter in

the universe( stars)the universe( stars) B. Bose-Einstein condensate- Exist at B. Bose-Einstein condensate- Exist at

very low temperaturesvery low temperatures 1. temperatures near 0 Kelvin1. temperatures near 0 Kelvin 2. All the electrons fall to the 2. All the electrons fall to the

lowest quantum levellowest quantum level

III. Kinetic Theory of matterIII. Kinetic Theory of matter A. Describes how matter behavesA. Describes how matter behaves B. Basic assumptionsB. Basic assumptions 1.matter is made of particles 1.matter is made of particles constantly in motion.constantly in motion. 2.The particles are constantly colliding 2.The particles are constantly colliding with each other without losing with each other without losing energy(perfect elastic collisions)energy(perfect elastic collisions) 3. the temperature depends upon the 3. the temperature depends upon the average Ke of the particlesaverage Ke of the particles

• C. Motion in gases- Very randomC. Motion in gases- Very random• 1.Average velocity is 1.Average velocity is

1600Km/hr.1600Km/hr.• 2. Very little attraction between 2. Very little attraction between

particles.particles.• D. The constant motion of gases D. The constant motion of gases

allow them to fill the container of allow them to fill the container of any shape or volume.any shape or volume.

E. Explaining the Behavior of liquids.E. Explaining the Behavior of liquids. 1. Average velocity is much slower than 1. Average velocity is much slower than

gases.gases. 2. particles are closer together.2. particles are closer together. 3. the forces of attraction, and molecular 3. the forces of attraction, and molecular

motion explain the behavior of liquids.- motion explain the behavior of liquids.- Liquids take the volume of the container, Liquids take the volume of the container, and can flowand can flow

PRESSURE’S ON!!!!

IV. Pressure- Force per unit area A. P=F/A( units: N/m2 = Pascal) 1. Kilopascal(Kpa) = 1000 pa B. Caused by collisions of particles

on the wall of the container.

V. Factors which affect gas pressureV. Factors which affect gas pressure A. Temperature-raises the average ke of A. Temperature-raises the average ke of

the particles.the particles. . 1. Raising temp of a gas will increase . 1. Raising temp of a gas will increase

the pressure if the volume is kept the pressure if the volume is kept constant.constant.

B. Volume-Reducing the volume of a gas B. Volume-Reducing the volume of a gas increases the pressure if the temp and increases the pressure if the temp and number of particles are constant.number of particles are constant.

C. Particles- Increasing the number of C. Particles- Increasing the number of particles will increase pressure if temp and particles will increase pressure if temp and volume are constantvolume are constant

VI. Gas laws: A. Charles Law- the volume of a gas is directly

proportional to the temperature (Kelvin), if Pressure and number of particles is constant.

1. V1/T1=V2/t2

B. Boyles law-The volume is inversely proportional to the pressure of a Gas.

1. P1V1=P2V2

• VII. Phase Changes.- A reversible physical change from one state to another.

• A.Melting,freezing,vaporization, condensation,deposition, sublimation

• B. Temperature always remains constant during a phase change.

VIII. Energy and Phase changes.VIII. Energy and Phase changes. A. Energy is either absorbed or released.A. Energy is either absorbed or released. 1. endothermic- absorbing energy( melting 1. endothermic- absorbing energy( melting

ice to water)ice to water) a. heat of fusion of water- the amount of a. heat of fusion of water- the amount of

heat necessary for 1 g of ice to melt into 1 g of heat necessary for 1 g of ice to melt into 1 g of water at the same tempwater at the same temp

1. 334j/g1. 334j/g 2. Exothermic- Energy is released(freezing of 2. Exothermic- Energy is released(freezing of

water to ice)water to ice)

• IX. Melting and freezing• A. melting- The force of attraction

between particles is diminished because their overall energy content has increased.

• 1.moving farther apart• B. freezing- the force of attraction is

increasing because the overall energy content of the particle is decreasing

• 1. moving closer together

PHASE CHANGESDescription of Phase Change

Term for Phase Change

Heat Movement DuringPhase Change

Solid to liquid

MeltingHeat goes into the solid as it melts.

Liquid to solid

FreezingHeat leaves the liquid as it freezes.

X. Vaporization and condensation A. Vaporization-Endothermic 1. the liquid has absorbed enough heat to

become a gas. 2. heat of vaporization- The amount of heat

necessary to change 1 g of a liquid to 1 g of a solid at the same temperature( water 2260j/g)

3. takes place at the surface of the liquid.

PHASE CHANGESDescription of Phase Change

Term for Phase Change

Heat Movement During Phase Change

Liquid to gas

Vaporization, which includes boiling and evaporation

Heat goes into the liquid as it vaporizes.

Gas to liquid

CondensationHeat leaves the gas as it condenses.

Solid to gas SublimationHeat goes into the solid as it sublimates.

• B. Evaporation- when a gas gains enough energy at temperatures far below boiling to escape from a liquid.

• C. Boiling-Takes place throughout the entire liquid.

• 1. temp doesn’t rise during boiling

• D. Condensation- when a gas becomes a liquid

STATES OF MATTER

SOLID LIQUID GAS PLASMA

Tightly packed, in a regular pattern

Vibrate, but do not move from place

to place

Close together with no regular arrangement.Vibrate, move

about, and slide past each other

Well separated with no regular arrangement.

Vibrate and move freely at high

speeds

Has no definite volume or shape and is composed

of electrical charged particles

XI Sublimation and depositionXI Sublimation and deposition A. Sublimation- The process of going A. Sublimation- The process of going

directly from a solid to a gasdirectly from a solid to a gas 1. Endothermic Rx1. Endothermic Rx 2. dry Ice, ice Cubes in the freezer2. dry Ice, ice Cubes in the freezer B. Deposition- when a gas vapor goes B. Deposition- when a gas vapor goes

directly into a solid state.directly into a solid state. 1. Water vapor on a cold Plate of 1. Water vapor on a cold Plate of

GlassGlass