STATES OF

MATTER

I.   STATES OF MATTERA. Kinetic Theory of

Matter1.Matter exists as a

solid, liquid, gas, or plasma.

2.Tiny particles (atoms) in constant motion make up all matter.

Gas Liquid Solid

I.   STATES OF MATTERB. Solids

1. Mc tightly packed - can’t be compressed

2. Definite shape & volume

3.Least kinetic energy - mc only vibrating

I.   STATES OF MATTERB. Solids

4. most are formed of crystals Crystal:

atoms are arranged in arepeating geometric

pattern.

I.   STATES OF MATTERB. Solids

5. Some solids are amorphous: • They lack an ordered

internal structure. • They appear to be

solids, but are not made of crystals.

• Ex. rubber, plastic, glass, etc.

I.   STATES OF MATTERC. Liquids

1.Mc less tightly packed than solids

(slightly compressible)

2. Indefinite shape (mc flow past each

other)3. Definite volume4. More kinetic energy

than solids

Liquid

Solid

I.   STATES OF MATTERD. Gases

1.Mc spread out. - very compressible

2. Indefinite shape and volume

3. More kinetic energy than solids and liquids Gas Liquid Solid

ALL TOGETHER NOW!

E.   Plasma

1.Hot ionized gas particles

2.Particles are electrically charged

E.   Plasma

3. Exists only at very high temp.

4. Most kinetic energy

I.   STATES OF MATTERE. Plasma

5.The most common state of matter in the universe!– Not found naturally

on earth.– Found on stars, the

sun, inside fluorescent bulbs

II.   Changes in StateA. Thermal Expansion

1.Almost all matter expands as it gets hot and contracts as it cools Name an exception.

2.Different materials expand at different rates.

II.   Changes in StateB. Melting

1.the change from a solid to a liquid

2.Melting pt. – temp. at which a solid becomes a liquid

II.   Changes in StateC. Freezing

the change from a liquid to a solidnote:

freezing pt. = melting pt.

II.   Changes in StateD.

Vaporization1. the

change from a liquid to a gas

II.   Changes in StateD. Vaporization

2. Boiling – rapid; gas bubbles form throughout liquid

– Boiling pt. temp. at which a liquid becomes a gas

II.   Changes in StateD. Vaporization

3. Evaporation• liquid changes

to a gas at temperatures below the boiling point

• Slow• Occurs at the surface

II.   Changes in StateE. Condensation

change from a gas to a liquid Note:Boiling pt. = Condensation pt.

II.   Changes in StateF. Sublimation

• A solid becomes a gas without first becoming a liquid

• Example: Dry Ice

II.   Changes in StateG. Deposition

• A gas becomes a solid without first becoming a liquid

• Example: Frost

THERMAL

ENERGY

B. Motion & Energy

1. Atoms & Mc have KE

a. solids: mc vibrate

slowly in place and are

closely packed

mc vibrate a little faster and move slightly apart

b. liquids:

B. Motion & Energy1. Atoms & Mc have KE

a. solids: b. liquids:

c. gases: mc are in rapid motionand are widely separated

Phase Change Review

Solid to Liquid Melting

Liquid to Solid

Liquid to Gas

Gas to Liquid

Solid to Gas

Gas to Solid

Freezing

Vaporization

Condensation

Sublimation

Deposition

A coupla videos to illustrate…

boiling water to snow

liquid nitrogen in pool

Phase diagram

• http://www.chm.davidson.edu/vce/PhaseChanges/HeatingCurve.html

II. Temperature and Heat

A.Temperature 1. is how hot or cold an object is2. The higher the temp.

the faster the mc move

       

 

Each beaker below contains one molecule of the same gas. Which beaker is at the higher temperature?

Your Turn!

A B

Each beaker below contains one molecule of the same gas. Which beaker is at the higher temperature?

Your Turn!

A B

Answer:

Beaker A

I. Temperature and Heat A.Temperature

3. Thermometerinstrument for

measuring

temperature

4. Temperature ScalesCelsius (C)

metric, used in science

Kelvin (K) 0 K is absolute zero (lowest temp.

possible; where all motion

stops)Fahrenheit (F) English system

A.Temperature

II. Temperature and Heat

A.TemperatureB.Heat - Thermal Energy

1. the amount of energy a substance has

because of the movement of

its particles2. Thus heat is

internal energy

II. Temperature and Heat

B.Heat – Thermal Energy

3. is E transferred between objects at

different tempsThermal Energymoves from an

area of high heat to low heat

A. What is it?3. Examples

Sand vs Ocean Water Which feels hotter?

1 kg sand absorbs 6x more heat than 1 kg

ocean water

III. Specific Heat

A. What is it?1. amount of heat

needed to raise the temp. of 1 kg of a

substance 1oC 2. Units

J/g.Co

III. Specific Heat

A. Formula

Q = m x c x TQ = thermal energym = mass (g)c =specific heatT = change in temp.

= final T – initial TTAKE NOTE: the “c” for

water is 4.18 J/g .Co

IV. Calculating Thermal E Changes

• And now…

The MATH

B. Sample Problem 1. The temperature of a 32.0 g silver spoon increases from 20.0O C to 60.0o C. If silver has a specific heat of 0.057 J/g.oC, what is the change in thermal energy of the spoon?

IV. Calculating Thermal E Changes

B. Sample Problem m = 32.0 g T = 60.0o C – 20.0O C = 40.0 oC C = 0.057 J/oC

Q = m x T x C

Q = 32 g x 40.0 oC x 0.057 J/oC

Q = 72.96J or 73J

IV. Calculating Thermal E Changes

Triple point diagram

solid

liquid

gas