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Chapter 16

Phases of Matter

Physical Science

What makes up matter?

What is the difference between a solid, a

liquid, and a gas?

What kind of energy do all particles of

matter have?

Kinetic theory Kinetic Theory

3 Parts

1. All matter is made of tiny particles.

2. These tiny particles are always in

motion. The higher the temperature, the faster the

particles move.

3. At the same temperature, more

massive (heavier) particles move slower

Animation

Kinetic Molecular Theory:

This motion is different for the 3 states of matter.

Copyright © 2010 Ryan P. Murphy

6

State the three parts of Kinetic Theory

Kinetic theory

States of Matter

When a substance

changes from one

phase of matter to

another, the identify

of the substance

does NOT change.

• Water freezes to a

solid and melts to

a liquid, but it is

still just water.

States of Matter Microscopic view of matter

• Activity! Describing Solid-Liquid-Gas

– Possible Answers!

Solid Liquid Gas

Volume

Shape

Mass

Copyright © 2010 Ryan P. Murphy

Easy to find –

in ml or cm3

Many different

forms. Easy

to mold.

Generally

Heavy / Weigh

in grams

Easy to find.

Easy to find.

Use graduated

cylinder – ml

Takes shape

of the

container.

Generally

Heavy / Weigh

in grams.

Difficult to find in

a classroom .

No Shape

Lighter in mass /

Harder to weigh

in a classroom

SOLIDS

•Solids have a definite shape and

volume

•The particles are held closely together

by strong attractions

•Packed close together

•Vibrate in place.

•Don’t flow

States of Matter

Characteristics of Solids

_______ have a rigid

structure.

– They do not need

a container to

maintain shape.

But they can still

________ in

place.

Solids

vibrate

Fill in the blanks

Characteristics of Solids

Definite

volume and a

definite shape.

Particles are

packed close

together in

relatively fixed

positions.

Particles are

held by strong

attractive forces

between them.

Particles vibrate

about in a fixed

position.

LIQUIDS

States of Matter

1. Has a definite volume but no definite shape. • Volume remains the same, but shape changes.

2. Take shape of container.

3. Particles are held close together but can

flow freely.

4. The particles in a liquid move much faster

than in a solid. • This allows the particles of a liquid to temporarily

overcome the attractive forces between them.

Characteristics of Liquids

________ can fill the

bottom of their container.

Particles are close

together, but not as close

as particles in a

_________.

Liquids

solid

Characteristics of Liquids

Definite

volume and not

definite shape.

Particles

are close

together

Takes shape

of container

Particles flow

freely and slide

past each other

GASES

States of Matter

Characteristics of Gases

A ______ expands to fill any available

space.

–_______ can exert pressure on their

container.

gas

Gases

•These particles are approximately 10 times farther

apart than those of a liquid or solid.

Characteristics of Gases

Gases

Gases

Gases

Attractive forces

between gas

particles are much

weaker than those in

liquids and solids.

Particles move very

rapidly and are at

great distance from

one another.

No definite

shape nor

definite volume.

PLASMA

States of Matter

Characteristics of Plasma

Ionized gas that emits electrons.

High-energy plasma collides

with gas particles.

• Plasmas are similar to gases but have some properties

that are different. • Example: plasmas conduct electric current, while gases do

NOT!

• The glow of fluorescent light is caused by artificial plasma

which is formed by passing electric currents through gases.

PLASMA

States of Matter

Energy is the ability to change or move

matter, or to do work.

The energy of motion is called kinetic energy

Because atoms and molecules are always in

motion, all particles of matter have kinetic

energy.

Energy’s Role

Energy’s Role

Which is a solid,

which is a liquid,

and which is a gas?

Gas

Solid

Liquid

• Identify as a Solid, Liquid, Gas, Plasma

Copyright © 2010 Ryan P. Murphy

Chapter 16 Changes of State

• What happens when a substance changes

from one state of matter to another?

• What happens to mass and energy during

physical and chemical changes?

Energy and Changes of State

– The identity of a substance does not change

during a change in state

– The ability to change or move matter

• As you add energy to a liquid, the temperature

goes up separating molecules

– Some changes of state require energy

• Melting, evaporation and sublimation

• The change of state from a liquid to a gas

Energy and Changes of State

• Boiling Point- The temperature

at which a liquid boils.

• The temperature of boiling water is

100oC on the celsius scale and 212oF

on the Fahrenheit scale.

• The temp in the room is about 22°C

and 70°F.

• Are the following temperatures hot or

cold?

65°F

• The process in which a solid changes

directly into a gas

Sublimation

Ex. Dry ice (Carbon dioxide in the solid

form) changes directly from a solid to a gas

Video Clip

Melting Point • The temperature at which a substances

changes from solid to liquid.

• Melting point depends on the pressure.

32 degrees F

0 degrees C

• Energy is released in some changes of

state

– Freezing and condensation

Name the physical phase

change

Copyright © 2010 Ryan P. Murphy

Freezing

Melting

Sublimation

Evaporation

Condensation

Solid Liquid Gas

sublimation

Freezing Condensation

Melting Boiling or

evaporation

46

Look at the vertical

lines.

What is the energy

doing if it is not

increasing the

temperature?

Why are the

arrows on each

side of the graph

the same

length?

En

erg

y o

f S

yste

m

• Please sketch the following into your

notes

Copyright © 2010 Ryan P. Murphy

What is the name of the first

electricity detective?

Sherlock Ohms

Joke of the Day

Copyright © 2010 Ryan P. Murphy

Energy

Energy

Sublim

ation

Depositio

n

Copyright © 2010 Ryan P. Murphy

• The temperature of a substance does not

change during a change of state. – For example, if you add energy to ice at 0oC,

the temperature will NOT rise until all of the

ice has melted.

– When energy is added – Move up a step.

– When energy is removed – Go down a step.

Heat added

Tem

pera

ture

(oC

)

0

100

Melting

Ice

Water

Water Vapor Boiling

Copyright © 2010 Ryan P. Murphy

• Latent Heat: The energy absorbed or

released when a substance changes its

physical state.

Heat added

Tem

pera

ture

(oC

)

0

100

Melting

Ice

Water

Water Vapor Boiling

Latent Heat

Latent Heat

Copyright © 2010 Ryan P. Murphy

• Mass cannot be created or destroyed.

• Matter can change form, and turn into different forms, but the TOTAL mass stays the same.

• Gas has mass!

Conservation of Mass and Energy

The Law of conservation of energy

• Energy cannot be created or destroyed.

– Energy can convert from one form to another,

but the TOTAL energy, before and after the

change, is the same.

Conservation of Mass and Energy

• In any physical or chemical change, matter is

neither created nor destroyed

– Matter can be changed from one form to another.

Copyright © 2010 Ryan P. Murphy

Heat

Law Conservation of Matter

Conservation of Mass and Energy

• Law Conservation of Matter

Copyright © 2010 Ryan P. Murphy

Chapter 16 Fluids • How do fluids exert pressure?

• What force makes a rubber duck float in a

bathtub?

• What happens when pressure in a fluid

changes?

• What affects the speed of a fluid in motion?

Fluids • A nonsolid state of matter in which the atoms

or molecules are free to move past each

other.

• Liquids and gases are fluids, because their

particles can move past each other.

• Pressure is the amount of force exerted

on a given area of surface.

• Fluids exert pressure evenly in all

directions. How does the pressure change if you remove

some of the air?

Pressure

• The SI unit of pressure is the pascal.

– One pascal (1 Pa) is the force of one newton exerted over an area of one

square meter (1N/m2).

• The newton is the SI unit of force.

Pressure

Pressure = force

area P = F

A

Blaise Pascal

• Buoyancy is the force with which a more

dense fluid pushes a less dense fluid

substance upward.

• All fluids exert an upward buoyant force on

matter.

• Archimededs’ principle is used to find

buoyant force.

Buoyant Force

How does this relate to me?

–Buoyancy tells me whether or

not an object will float.

Archimedes Principle

• The buoyant force on an object in a fluid

is an upward force that equals the weight

of the fluid that the object displaces.

Buoyant Force

65

Archimedes Principle

• Explains

why a

steel

ship

floats!

Density

• An object will float or sink

based on its density.

• You can determine if a

substance will float or sink by

comparing densities.

Buoyant Force

Pascal’s Principle

• A change in pressure at any point in an enclosed fluid

will be transmitted equally to all parts of the fluid.

P=force/ area

Hydraulic devices are based

on Pascal’s Principle.

How does this relate to me?

Viscosity tells me how

thick a liquid or gas is.

Fluids In Motion

• Fluids move faster through small areas

than through larger areas.

• Rates at which they flow also varies.

• Viscosity is the resistance of a fluid to

flow.

Which has a greater

viscosity? Water or honey

Stronger attraction between particles, the more viscous

69

Chapter 16 Behavior of Gases

• What are some properties of gases?

• How can you predict the effects of

pressure, temperature, and volume

changes on gases?

Think about this…….

The gas in the toy balloon expands outward, as shown below. After this expansion, does the pressure of the gas

a. increase?

b. decrease?

c. remain unchanged? The temperature of the water vapor in the pressure cooker increases. Does the pressure of the gas a. increase? b. decrease? c. remain unchanged?

Volume goes up

Pressure goes down

Temperature increases

Pressure increases

Properties of Gases

• Have low densities and are

compressible.

• Mostly empty space.

• Gases fill containers

uniformly and completely.

• Gases diffuse and mix

rapidly.

• The gas laws will help you understand

and predict the behavior of gases in

specific situations.

• Boyle’s Law (relates pressure to volume)

• Gay-Lussac’s Law (relates pressure to temperature)

• Charles’s Law (relates temperature to volume)

Gases Laws

Boyle’s Law

Robert Boyle

(1627-1691).

Son of Earl of

Cork, Ireland.

• Boyle’s law relates the pressure of a

gas to its volume.

• For a constant temperature, as the

pressure goes up the volume goes

down.

• As the volume goes up the pressure

goes down.

Gases Laws

Pressure Volume

Temperature is constant

• A bicycle pump is an

example.

• As the volume of the

air trapped in the

pump is reduced, its

pressure goes up, and

air is forced into the

tire.

Gases Laws

Boyle’s Law

(pressure1) (volume1) = (pressure2) (volume2)

P1V1 = P2V2

Gases Laws

Boyle’s Law

The gas in a balloon has a volume of 7.5 L at 100.0 kPa. In the atmosphere,

the has expands to a volume of 11 L. Assuming a constant temperature, what

is the final pressure in the balloon?

V1 =

P1=

V2 =

P2 = ?

V1 = 7.5 L

P1= 100.0 kPa

V2 = 11 L

P2 = ?

P1V1 = P2V2

P2= P1V1

V2

P2= (100.0 kPa)(7.5 L)

11 L

P2= 68 kPa

• Relates gas pressure to temperature.

• The pressure of a gas increases as the

temperature increases.

• If the volume of the gas does not change.

The pressure decreases as the

temperature decreases.

Gases Laws

Gay-Lussac’s Law

Volume is constant

Pressure Temperature

P lower in winter than summer

• Charles’s law relates temperature to volume.

• For a fixed amount of gas at a constant

pressure, the volume of the gas increases as the

gas’s temperature increases.

• Likewise, the volume of the gas decreases as

the gas’s temperature decreases.

Gases Laws

Charle’s Law

Pressure is constant

Volume Temperature

Charles’s Law