STATES OF MATTER

FOUR STATES OF MATTER Solid Liquid Gas Plasma

SOLIDS Definite Shape and Volume

Particles are often arranged in repeating geometric patterns to form crystals

Some are composed of particles with no particular order (amorphous solids)

LIQUIDS Definite Volume

Can’t normally be squeezed into a smaller space

Indefinite ShapeFlow and take shape of container

GASES No definite shape or volume

Molecules can be squeezed together or spread out to fill the space available

PLASMA Gas-like mixture of positively and

negatively charged particles Only exists at very high temperatures MOST of the matter in the universe!!

Around 99% Ex’s

natural plasmas- lightning, fireartificial- fluorescent light

WHICH STATE OF MATTER HAS A DEFINITE VOLUME, BUT NOT A DEFINITE SHAPE?

0%

4%

91%

4% 1. Solid2. Liquid3. Gas4. Plasma

TERMS RELATED TO STATES OF

MATTER

KINETIC THEORY OF MATTER

Question #1 on page 781. All matter is made of atoms and molecules

that act like particles 2. These particles are always in motion. The

higher the temperature of the substance, the faster the particles move.

3. At the same temp, more massive (heavier) particles move slower than less massive (lighter) particles

KINETIC THEORY OF MATTER

In other words… All matter is made of tiny particles (atoms)

in constant motionHow MUCH they move depends on how much

energy they have Increased temperature will…

increase kinetic energy= more movement

THERMAL EXPANSION Almost all matter expands as it gets

hotter and contracts when it cools.Temperature is a measure of the average

kinetic energy of the particles in the objectTheoretically, absolute 0, (0 degrees Kelvin)

has no movement of particles Never achieved in a lab

TEMPERATURE IS A MEASURE OF THE _______ OF THE PARTICLES IN AN OBJECT

4%

96%

0% 1. Degrees Celsius2. Average Kinetic Energy3. Average Potential Energy

ENERGY OF PHASE

CHANGES

EXOTHERMIC PHASE CHANGES ENERGY RELEASED Energy is RELEASED from the substance out

to its surroundings Ex’s- each of these products have molecules with

LESS energy than they did before the phase change Freezing (liquid water has more energy than ice) Condensation (gas to liquid) Deposition (gas to solid)

ENDOTHERMIC PHASE CHANGES ENERGY REQUIRED Energy is ABSORBED by the substance from

its surroundings Ex’s- each of these products have molecules with

MORE energy than they did before the phase change Melting (ice has less energy than water) Evaporation (liquid gas) Sublimation (solid gas))

FOR EACH OF THE FOLLOWING…

Name the process described and then determine if it is exothermic or endothermic

LIQUID TO GAS…

0%

9%

83%

9%

0% 1. Sublimation, Exothermic2. Condensation, Exothermic3. Evaporation, Endothermic4. Sublimation, Endothermic5. Condensation, Endothermic

GAS TO LIQUID…

30%

0%

0%

65%

4% 1. Sublimation, Exothermic2. Condensation, Exothermic3. Evaporation, Endothermic4. Sublimation, Endothermic5. Condensation, Endothermic

SOLID TO GAS…

5%

77%

0%

0%

18% 1. Sublimation, Exothermic2. Condensation, Exothermic3. Evaporation, Endothermic4. Sublimation, Endothermic5. Condensation, Endothermic

INTERMOLECULAR FORCES The force between two molecules

Holds them together weaklyStronger in a solid than liquid, etc.

INTERMOLECULAR FORCES

The attractions between molecules are not nearly as strong as the intramolecular attractions that hold compounds together.

INTERMOLECULAR FORCES

They are, however, strong enough to control physical properties such as boiling and melting points, vapor pressures, and viscosities.

INTERMOLECULAR FORCES AFFECT MANY PHYSICAL PROPERTIES

The strength of the attractions between particles can greatly affect the properties of a substance or solution.

VISCOSITY Resistance of a

liquid to flow is called viscosity.

It is related to the ease with which molecules can move past each other.

Viscosity increases with stronger intermolecular forces and decreases with higher temperature.

SURFACE TENSION

Surface tension results from the net inward force experienced by the molecules on the surface of a liquid.

WATER IS SPECIAL

Surface Tension! Density of ice is

special!

Contains H bonds (which are not actually bonds, but strong Intermolecular forces)

Gives water special properties like…

PHASE CHANGES

THE STATES OF MATTER The state a substance is in at a particular

temperature and pressure depends on two antagonistic entities:The kinetic energy of the particlesThe strength of the attractions between the

particles

PHASE CHANGES CANNOT OCCUR WITHOUT BREAKING OR FORMING THE IF FORCES

ENERGY CHANGES ASSOCIATED WITH CHANGES OF STATE

The heat added to the system at the melting and boiling points goes into pulling the molecules farther apart from each other.

The temperature of the substance does not rise during the phase change.

**IN ORDER TO CHANGE STATE, THESE INTERMOLECULAR FORCES MUST BE BROKEN OR FORMED, AND THIS REQUIRES ADDING OR SUBTRACTING __________________ENERGY

THE ENERGY PUT IN TO BREAK BONDS AT A PHASE CHANGE IS __________ ____ THE ENERGY RELEASED WHEN THE BONDS ARE REFORMED TO CHANGE BACK!

Heat of Vaporization: Energy required to change a liquid at its boiling point to a gas is equal to the energy released from the particles when a gas is changed to a liquid!

Heat of Fusion: Energy required to change a solid at its melting point to a liquid is equal to the energy released from the particles when a liquid is changed to a solid!

SO WHAT DOES THIS MEAN ABOUT MELTING AND FREEZING POINT TEMPERATURES?

They are EQUAL!

SPECIAL INFO ABOUT THE HEATING AND COOLING CURVES OF WATER

heating curve of water animation The total energy absorbed in the

heating curve is equal to the total energy released in the cooling curve of waterMelting/freezing pt: occur at same temperatureBoiling/condensation pt: occur at same

temperature

MORE SPECIAL INFO Temperature does not change

during a phase changeSo, the graphs have 2 main plateau areas

where phase changes are occurring

COOLING CURVE OF WATER

USING EVERYTHING WE HAVE LEARNED… Explain what happens when a cold glass

of water “sweats”

Condensation - gas to liquid Water particles in the air have more kinetic energy

(heat) than the glass of water. As water particles get close to the glass, energy is transferred from the particles to the glass. This starts the following process…

a. Particles lose kinetic energy, slow down, and come closer together.

b. IF’s become strong enough to make particles merely rotate around each other.

c. The energy they lose to turn into a liquid is the heat of vaporization.

d. Substance is releasing energy to the surroundings (exothermic)

USING EVERYTHING WE HAVE LEARNED… Explain what happens when liquid water

changes to ice.

Freezing - liquid to solid-.

a. Particles lose kinetic energy

and slow down.

b. Substance releases energy to surroundings

(exothermic)

c. IF’s b/w particles become stronger than the particles’ motion, so the particles begin merely vibrating in place to form a solid.

d. The amount of heat the particles must lose to turn into a solid is called the heat of fusion.

IS THIS A HEATING OR COOLING GRAPH?

0%0%0%0%

Heating Cooling

Both of the above None of the above

1. Heating2. Cooling3. Both of the above4. None of the above

10

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

THERE ARE TWO FLAT SECTIONS IN THE ABOVE GRAPH. WHY?

10

a

b c

d

e

Time (min)

T e m p p

0%

0%

0%

0%1. IF are breaking2. IF are being

created (forming)3. The phase

change is increasing the temp

4. None of the above

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

A COOLING CURVE IS

0%

0%

0%

0% 1. Exothermic and a chemical change2. Endothermic and a physical change3. endothermic and a chemical change4. Exothermic and a physical change

10

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

WHICH OF THE FOLLOWING IS SUBLIMATION?

0%

0%

0%

0%

10

1. Solid to liquid2. Solid to gas3. Liquid to gas4. Gas to liquid

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

WHICH TYPE OF MATTER HAS A DEFINITE SHAPE AND DEFINITE VOLUME?

Gas

Liq

uid

Solid

pla

sma

0% 0%0%0%

10

1. Gas2. Liquid3. Solid4. plasma

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

WHICH TYPE OF MATTER HAS INDEFINITE SHAPE BUT DEFINITE VOLUME AND CAN TAKE THE SHAPE OF THE CONTAINER?

0% 0%0%0%

1. Gas2. Liquid3. Solid4. plasma

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1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

21 22 23 24 25 26 27 28

Why are there 2 portions of the phase change curve in which the temperature is not increasing? (the water is not removed from the heat source during any portion of time)

AT WHICH OF THE FOLLOWING STAGES IN THE EXPERIMENT WOULD THE AVERAGE MOLECULAR SPEED OF THE WATER MOLECULES BE GREATEST?

10

0 of 28

0%

0%

0%

0% 1. Ice stage2. Water + ice stage3. Water stage4. Water vapor stage

WHAT IS THE THEORY THAT SAYS TINY PARTICLES ARE ALWAYS IN MOTION AND THE HIGHER THE TEMP. THE FASTER THE PARTICLES MOVE?

0%

0%

0%

0%

10

0 of 28

1. Thermal energy 2. Kinetic theory3. Law of conservation of mass4. Law of conservation of

motion