the structure of matter matter – anything that has mass and takes up space mass – the amount of...

The Structure of Matter

Matter – Anything that has mass and takes up space

Mass – The amount of matter in

an object

Molecule – The smallest particle of a substance (such as water) that can still be identified as that substance (Latin = little mass)

Ex. – 60 million H2O – diameter of a

penny

Ex. All water molecules are the same

-Once a molecule is divided it is no longer that substance

Ex. H2O H2 Not water

O Not water

OH H

Physical & Chemical Properties of Matter

Physical Properties – A characteristic of matter that can be observed by using any of your senses

Ex. Hardness, density, melting pt. /

boiling pt., State (solid, liquid, gas)

Size, shape, color, odor, taste

Physical & Chemical Properties of Matter

Chemical Properties – A description of how one kind of matter behaves in the presence of another kind of matter.

Ex. Vinegar & baking soda

- When vinegar is added to baking soda, CO2 is produced

States of Matter

State Definite Shape Definite Volume

Solid

Liquid

Gas NoYes

Yes YesNo

NoSolid Liquid Gas

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Solid

Liquid

Gas

PlasmaPlasma- State of matter where gas

molecules have separated into electrically charged particles

Ex. STARS (fusion)

Physical & Chemical ChangesPhysical Change- a change in which

the form or appearance of matter changes but not its composition

Ex. Shape – crumpled paper

Dissolving – Koolaid

Change in State

Physical Changes

Solid Liquid GasFreezing

Melting

Condensation

Vaporization

Deposition

Sublimation

- Only the MOTION of the molecules has changed!

Chemical ChangesChemical Change – a change in which the composition of a substance changes

Ex. Fireworks, Rust

- causes a new substance to form.

Chemical ChangesSigns of Chemical Changes

- Color Changes Ex. Trees, apples, toast

- EnergyReleased – fire – heat, light

Gained – cooking/cake

Chemical ChangesSigns of Chemical Changes

- Odor Ex. Rotten food

- Bubbles formedEx. Vinegar + Baking soda

Antacid

Chemical ChangesSigns of Chemical Changes

- Solid formed - PrecipitateEx. Sodium iodide = lead nitrate

- Not easily reversed Ex. Ice melting vs.

Wood burning

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Physical Chemical

EASY HARD

VS.

Anton Lavoisier – 18th CenturyThe LAW of Conservation of Mass-- States that mass is neither created nor destroyed

(and as a result, the mass of the substance before a physical or chemical change is equal to the mass of the substances present after the change)

Ex. Apple cut up, candle burning

GasesThe Kinetic Theory of Matter-

- The scientific principal that says that all matter is made of particles whose MOTION determines if the matter is solid, liquid, or gas

-Each of the 3 states of matter is called a phase

State Definite Shape Definite Volume

Solid

Liquid

Gas NoYes

Yes YesNo

No

4 Properties of Gases- explained by the Kinetic theory of matter

1. Gas molecules move VERY FAST-A gas is mostly empty space

(large distance between gas molecules)-Particles collide MANY times per second

(particles are NOT affected by collisions)

- No definite shape, they expand to fill all available space

2.Moving gas molecules cause pressure

Ex. Balloon

(All that moving and colliding into things causes a force to be applied)

Pressure- The amount of force applied to a unit of area

3.Gases have NO definite volume

-can be crowded together

-This the pressure (more collisions)

-can be allowed to expand

-This the pressure (fewer collisions)

4.The temperature of a gas measures how fast molecules move

- Heat = in particle movement

(particles tend to move further apart)

- volume or the pressure

Ex. Bicycle tire on a hot day

- Heat = in particle movement

Absolute Zero - -The Temperature at which particles of matter stop moving -273 oC-No Kinetic Energy at absolute zero-Kelvin (K) Temperature scale - -A temperature scale on which zero is equal to absolute zero

GAS LAWS!

Boyle’s Law

Pressure = Volume

Pressure = Volume

No Temperature change

V1 . P1 = V2 . P2 Ex. The air in a balloon occupies a space of 1000mL and has a pressure of 5 N/cm2. When Gary grabs the balloon the pressure increases to 10 N/cm2. What is the new volume of the balloon?

V1= V2=

P2= P2=

V1= 1000mL V2= ? mL

P1= 5 N/cm2 P2=10N/cm2

1000 . 5 = V2 . 10

V1 . P1 = V2 . P2

5000 = V2 . 10 5000 = V2 . 10 10 = 10 500 = V2V2 = 500 mL

GAS LAWS!

Charle’s Law

Temperature = Volume

Temperature= Volume

V1 . T2 = V2 . T1

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V1 . T2 = V2 . T1 Charle’s Law

10o C

V1= V2=

T2= T1=

30o C

30mL ? mL

30mL

30oC

? mL10oC

V1 . T2 = V2 . T1

Charle’s Law

10o C

V1= V2=

T2= T1=

30o C30mL ? mL

30mL

30oC

? mL

10oC 30 . 30 = V2 . 10 900 = V2 . 10

10 10 90 = V2

V2 = 90mL

Solids & Liquids

(the molecules stay in a fixed patteren)

Solids- A piece of solid matter cannot change shape by itself

Ex. crystal

Crystal- A solid whose orderly arrangement of particles gives it a

regular shape

- The shape (of the crystal) is determined by the way the particles are arranged

-Almost all solids are made of crystals

Ex. salt(different crystals break in different ways)

Super cooled liquids- Solids that have been cooled soooooo quickly that they

have NO crystal pattern-Almost all solids are made of crystals

Ex. Volcanic glass

Liquids- molecules (can move from one place to another) have NO fixed

pattern.

-Can flow (change shape)- when not moving it will have a level surface

Change to a Liquid

-Heat is added (to a solid)- Motion / Temp

- particles can’t stay in crystal pattern

Change to a Liquid

Melting point- the temperature at which a solid becomes a liquid

- each crystalline solid has its own melting point Mercury = -39 oC

Salt = 801 oC

Sugar = 186 oC

Water = 0 oC

Change to a Liquid

Heat of fusion- the amount of heat required to change 1 gram of solid to a liquid

- the energy used to break the crystalline structure

(at the same temp

no temp change)

Sublimation

- Changing from a Solid Gas

Ex. Dry ice

Change to a Gas- In most liquids (at ordinary Temps.) Some molecules have enough energy to (escape and) become a gas

Ex. Water evaporation

Heat = evaporation

Boiling point –The Temp (at ordinary pressure) at which the molecules of a liquid have enough energy to become a gas

Exact boiling point depends on:

1. Energy needed to make particles separate

2. Pressure of the air pressure = boiling point pressure = boiling point

- Water (at normal pressure) will never be hotter than 100oC

Heat of Vaporization-The amount of heat required to change 1 gram of liquid to a gas (No temperature change)

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