CLASSIFICATION of MATTER - Typepad€¦ · Matter Anything that has both mass AND volume –MASS A measure of the amount of matter contained in an object –VOLUME A measure of the

CLASSIFICATION

of

MATTER

What is matter?

Matter is anything that has mass

and takes up space.

Matter Anything that has both mass AND volume

– MASS

A measure of the amount of matter contained in an object

– VOLUME

A measure of the amount of space an object takes up

Substances

– Matter that has a uniform and unchanging chemical

composition

– EX. Water (H2O); Table salt (NaCl)

Properties of Matter

How It Looks (Shiny ,Dull, Color, etc.)

How It Feels (Hard, Soft, Rough , Smooth, etc.)

How It Smells (Sweet, Sharp, Terrible, No Smell, etc.)

How It Sounds (Loud, Soft, Echo, No Sound, etc.)

What It Does (Bounce, Stretch, Tear, Break, Magnetism etc.)

Physical Properties of Matter

A characteristic that can be observed or measured without changing the sample’s composition – Also used to describe pure substances

There are two types of physical properties – EXTENSIVE PROPERTIES

dependent on the amount of the substance present

– INTENSIVE PROPERTIES

NOT dependent on the amount of the substance present

Chemical Properties of Matter

Ability OR inability of a substance to

combine with or change into one or more

other substances

Identify Properties Classify each of the properties below into

either PHYSICAL or CHEMICAL

5 States of Matter

Solids

Liquids

Gases

Plasma

Bose-Einstein Condensate (This one only

happens within a few billionths of a degree

above absolute zero…so, yeah. You won’t

see this unless you are in a lab.)

SOLIDS

SOLID

A solid is matter that has that has definite size

and shape.

Example: Put a sneaker in a box. It stays the

same.

States of Matter Solid

– Form of matter that has its own

definite shape and volume

– Particles within a solid are

tightly packed

When heated, it will expand only

slightly

Cannot be compressed

Low Kinetic Energy (KE)

Liquids

LIQUID

A liquid takes the shape of any container.

Example: Pour juice into a glass. The juice

will take on the shape of the glass.

States of Matter Liquid

– Form of matter that flows,

has a constant volume, and

takes the shape of its

container

Less tightly packed

– When heated, it will expand

– Is virtually incompressible

– Moderate Kinetic Energy (KE)

GAS

Gas

Gas is matter that has no definite shape.

Gases take the shape of whatever container

they are in .

Example: The air all around us is a gas.

States of Matter Gas – Form of matter that flows to conform to the

shape of its container and fills the entire volume of its container Very loosely packed

– When heated, it will expand and sometimes escape

– Easily compressed

– High Kinetic Energy (KE)

Gas vs. Vapor – Gas = the state of matter

– Vapor = gaseous state of a substance that is either a liquid or gas at room temperature

BOTH liquids and gases are “fluids” because they flow

Plasma Doesn’t happen regularly on Earth

EX:

The Northern Lights Ball lightning

– It takes a very special environment to keep

plasmas going. They are different and unique from

the other states of matter.

Physical changes in matter

A Physical change is a change in how matter looks, but not the kind of matter is it is.

Tear

Cut

Folded

Written

Liquid

Solid

Gas

Mixture

Solution

Physical Changes

Changes that DO NOT alter the composition

of a substance

– Physical changes are those that are causing a

change in a physical property

– Examples:

Cutting paper

Breaking a crystal

PHYSICAL CHANGES

Changes in States of Matter

Changes in the state of matter are all

PHYSICAL CHANGES as they do NOT alter

the arrangement of the substance

Deposition

Chemical changes in matter

New Matter is formed.

– Burning

– Rusting

– Cooking

Chemical Changes

Process that involves one or more substances

changing into new substances

a.k.a. Chemical reaction

– Reactants – Starting substances

– Products – Resulting substances

Newly formed substances will have different

compositions and properties than the original

substances Fe + O FeO

Iron reacts with Oxygen to produce Iron Oxide

CHEMICAL CHANGES

Four Indications of a

Chemical Change

1. release of a gas

2. release of heat, light or sparks

3. formation of a precipitate

4. color change

Law of Conservation of Mass Mass is neither created nor destroyed, it is only rearranged.

– The total mass you have in the beginning of a reaction must be present at the end of the reaction

Mercury + Oxygen Mercury Oxide

If there are 200g of mercury and 16g of oxygen, what mass of mercury oxide is produced.

Mercury + Oxygen Mercury Oxide

200g 16g ?

216g

Is this a solid, a liquid, or a gas? Can you find more than one type of matter in any of the pictures?

Is this a physical change or a chemical change? Can you find more than one physical or chemical change in the pictures?

Let’s watch a video clip about

matter!

States of Matter

Click to go to the next

slide.

Mixtures

A combination of two or more pure

substances in which each pure substance

retains its own individual chemical

properties

– physical combination

– can be separated physically

– has no definite ratio

Mixtures versus Compounds

S

Fe

Physically mixed, can be

separated by physical means.

Chemically reacted, cannot be

separated by physical means.

Elements

A pure substance that cannot be separated into

simpler substances by physical or chemical

means.

– 91 occur naturally

– Allotropes- element is found in more than one form.

Ex. Carbon- diamond & graphite, Oxygen- O2 & O3.

– Diatomic elements- found as a pair with itself

Ex. O2, N2, F2, Cl2, H2, I2, Br2

– Expressed with a chemical symbol

-one, two or three letters

-only the first letter is capitalized

-organized on the Periodic Table

Periodic Table Horizontal

rows-periods

Vertical row-

groups/family

– Elements in a

group/family

together have

similar

properties

Compounds

Chemical combination of two or more elements – definite ratio

– can only be separated by chemical changes

– Compounds that occur naturally are more stable than the individual component elements.

– properties of a compound are different from the properties of the elements that make it

Water

aspirin

sugar NaCl (salt)

NH3 (ammonia)

HCl (hydrochloric acid)

Fe2O3 (Iron III Oxide)