MATTER

MATTER IS ANYTHING THAT TAKES UP SPACE AND HAS MASS.

THREE FORMS OF MATTER

I. PURE SUBSTANCE

1. Elements (Found on periodic chart)

Made of Atoms

Example: Hydrogen

2. Compounds

Made of two or more different Atoms

combined to form a molecule

Example: H₂0

II. MIXTURE (when put together the parts stay the same)

1. Heterogeneous

Has unlike parts

Example: Fruit Cocktail Jello

Concrete

Cereal

2. Homogeneous

Has like parts

Example: Solutions

a. pop

b. Kool Aid

STATES OF MATTER

1. Solid

2. Liquid

3. Gas

4. Plasma

State Molecular Definition Make-up

Solid : : : : Molecules held tightly. Definite shape and volume

Add Goes through melting point (bonds broken)

Heat Liquid · . · . Molecules less tight. Only definite volume

Add Goes through boiling point or evaporation below boiling point

Heat Gas . ·

. · Molecules little or no attraction. No definite shape or volume

. ·

Plasma High energy only found in stars

Solid

remove

heat Goes through freezing point

Liquid

remove

heat Goes through condensation point

Gas

EVAPORATION – when a liquid turns to a gas below its boiling point. Surface molecules only.

CONDENSTATION – when gas molecules lose energy, slow down and form a liquid.

SUBLIMATION - when a solid goes to a gas without becoming a liquid.

PHYSICAL AND CHEMICAL CHANGE

PHYSICAL CHANGE is a change in size, shape, or state.

THE SUBSTANCE STAYS THE SAME

Example: Tree to sawdust – size and shape

Ice to steam - state

CHEMICAL CHANGE – when reaction creates a different substance. Can recognize by something happening. Heat, smoke, bubbles etc. You cannot change it back to what it was.

PHYSICAL PROPERTIES are related to physical characteristics

Example: Boiling point

Freezing point

CHEMICAL PROPERTIES are related to chemical characteristics

Example: Zinc added to an acid will form

hydrogen gas

SEPARATION OF MIXTURES

1. MIXTURES ARE NOT CHEMICALLY COMBINED. SINCE THE PARTS OF A MIXTURE HAVE JUST BEEN PHYSICALLY PLACE TOGETHER, THEY CAN BE PHYSICALLY SEPARATED.

EXAMPLES:

For Heterogeneous Mixtures

1. Filtration

2. Centrifuge

3. Magnetic

For Homogeneous Mixtures

1. Distillation

2. Crystallization

3. Chromatography

CONSERVATION OF MATTER

Antoine Lavoister, after carefully and accurate measurement, over threw much old thinking and established the science of chemistry, when he stated the Law of Conservation of Matter. Matter like energy, as stated by Joule, can neither be created or destroyed.

ENERGY

1. ENERGY IS THE ABILITY TO DO WORK.

2. THERE ARE MANY FORMS OF ENERGY (ELECTRICAL, MECHANICAL, ETC.) BUT ALL THE DIFFERENT FORMS CAN BE CLASSIFIED INTO BASIC FORMS – RADIANT, KINETIC, POTENTIAL.

A. RADIANT ENERGY

1. SUNLIGHT

2. X-RAYS

3. RADIOWAVES

B. KINETIC ENERGY

1. MOLECULES OF HOT SUBSTANCE

2. WATER IN A RIVER

3. MOVING PARTS OF AN ENGINE

C. POTENTIAL ENERGY – DUE TO POSITION OR ARRANGEMENT

1. BATTERIES

2. GASOLINE

3. FOOD

3. ENERGY IS MEASURED BY SPECIFIC UNITS.

A. A CALORIE IS THE ENERGY IT TAKES TO RAISE 1GAL. OF WATER 1 DEGREE CENTIGRADE.

B. A FOOD CALORIE WRITTEN Calorie IS 1000 TIMES CALORIES.

C. THE JOULE CREATED BY JAMES JOYLE IS THE SI UNIT. IT RELATES MECHANICAL ENERGY UNITS TO HEAT. 1 cal = 4.184J

4. A. BEING ABLE TO CREATE ENERGY BY MECHANICAL MEANS AND BEING ABLE TO RELATE IT TO UNITS OF HEAT ENERGY IMPLIES THAT ENERGY CAN BE CHANGED FROM ONE FORM TO ANOTHER. FOR EXAMPLE SUNLIGHT (RADIANT) CAN HEAT WATER (KINETIC) OR CREATE ELECTRICITY (KINETIC). THE POTENTIAL ENERGY IN GASOLINE CAN CONVERTED INTO MECHANICAL ENERGY (KINETIC) FOR AN ENGINE.

B. THIS LED TO LAW OF CONSERVATION OF ENERGY BY JAMES JOULE. THIS LAW STATES THAT: IN ANY PROCESS ENERGY CAN CHANGE FORMS BUT IT CAN NEITHER BE CREATED OR DESTROYED.

C. IF ENERGY CAN’T BE CREATED OR DESTROYED, WHY IS THERE A POTENTIAL ENERGY SHORTAGE?

a. OUR SOURCE OF ENERGY IS PRIMARILY FOSSIL FUELS. WHEN THESE POTENTIAL ENERGY SOURCES HAVE BEEN CONVERTED TO KINETIC FORMS OF ENERGY, THEY BECOME DEPLETED.

D. EXAMPLE PROBLEM: A STUDENT USED 30J OF ENERGY TO PUT BOOKS ON THE SHELF. HOW MANY CALORIES DID HE USE?

1cal = 4.184J conversion factors equal 4.154J/1cal or

E = 30J x 1cal/4.184J = 7.3 cal

BY DEFINITION IF YOU HAVE WATER AND KNOW HOW MANY GRAMS YOU HAVE AND HOW MUCH TEMPERATURE CHANGE YOU HAVE YOU CAN CALCULATE CALORIES.

Calories = grams of water x T

WHERE = CHANGE

WHERE T =

TEMPERATURE CHANGE

TO SOLVE THE PROBLEMS SUBSTITUTE TWO OF THE KNOWNS GIVEN YOU AND SOLVE FOR THE THIRD ALGEBRAICALLY.

TEMPERATURE

1. TEMPERATURE IS A MEASUREMENT OF THE AVERAGE MOTION OF MOLECULES.

2. SCALES FOR THERMOMETERS COULD BE ANYTHING.

A. ONE OF THE MOST COMMON WAS CREATED BY GABRIEL FAHRENHEIT – THIS IS THE FAHRENHEIT SCALE.

B. A SCALE THAT IS DIVISIBLE INTO 10THS IS BETTER SUITED FOR SCIENCE. THIS IS THE CELSIUS SCALE CREATED BY ANDRUS CELSIUS. THIS PLACES THE FREEZING POINT OF WATER AT 0 DEGREES AND THE BOILING POINT AT 100 DEGREES.

C. THE KELVIN SCALE IS THE SI SCALE CREATED BY LORD KELVIN. THE GELVIN AND CELSIUS SCALE HAVE THE SAME UNIT SIZE. THE ONLY DIFFERENCE IS THAT KELVIN’S SCALE IS 273 DEGREES HIGHER THAN CELSIUS. THIS PLACES 0 DEGREES KELVIN AT ABSOLUTE ZERO. AT THIS POINT ALL MOTION CEASES. TO CONVERT BETWEEN THE TWO SCALES THE FOLLOWING EQUATION IS USED:

K = C + 273

C = K – 273