1. Matter is anything that has
Properties of Matter
What is matter?
Matter is anything that has
mass and volume.

2. Classification of Matter
Matter can be divided into 2 categories:
SUBSTANCES & MIXTURES
Substances can NOT be separated into
different kinds of matter by physical means.
Mixtures can be separated into different
kinds of matter by physical means.

3. Classification of Matter
What are substances?
In science, substances are limited to elements and compounds.
Elements
Any substance in which all the atoms in a sample are alike, one kind of matter
Examples: Carbon, Sodium and Oxygen
Compounds
2 or more elements chemically
combined in a fixed ratio
Usually has different appearance from
elements that make it up
Examples: Water – H2O and Salt - NaCl

4. Classification of Matter
Atom-smallest possible particle of an element
Molecule- smallest possible particle of a compound

5. Classification of Matter
What are mixtures?
2 or more substances that can be separated by physical means
Do not always contain the same amounts of the different substances that make them up
Homogeneous
same throughout, particles so tiny that cannot be seen, don’t settle out or scatter light
Examples: milk, salt water and cola
Heterogeneous
a mixture in which different materials can be easily distinguished
Suspension-visible particles settle-muddy water
Examples: Sand/water, Italian salad dressing, pizza and dry soups

6. Classification of Matter

7. Measuring Matter Volume of a liquid Volume of solid
Graduated cylinder- read from bottom of meniscus
Volume of solid
Length X Width X Height
Volume of Irregular Shaped Objects
Water Displacement
Indirect Measuring
Large objects-take a core sample and use a formula
Small objects-weigh 100 and then divide weight by 100 to get one small objects weight

8. Phases & Properties of Matter
What is the matter?

9. Phases of Matter Solids - definite shape and volume
Atoms are held close together by strong bonds
Movement is slow
Crystalline Solids (crystals) - atoms are
arranged in regular fashion
Ex. - ice, salt, diamonds
Amorphous Solids - atoms LACK a regular
arrangement
Ex. - rock, glass, wax

10. Phases of Matter - Continued
Liquids - definite volume, but NO definite shape
Bonds are weaker and atoms are spaced
farther apart
They take the shape of container they
are in

11. Phases of Matter - Continued
Gases - NO definite volume OR shape
Bonds are weakest and atoms far apart
Expand to fill the container they are in
Examples - air, oxygen, smoke

12. Phases of Matter - Continued
Plasma
Gas like mixture of + and – charged particles
Movement very rapid
99% of mass of our solar system
Examples: Sun, Stars and Lightning

13. Physical Properties of Matter
Viscosity –
Measure of the material’s resistance to flow
High-viscosity liquids take longer to flow
Example: Ketchup when comparing to water
Low-viscosity liquids flow easier
Example: Tomato Juice flows
easier than ketchup
Temperature raising-viscosity decreases except in gases.
·         

14. Physical Properties of Matter – Cont.
Elasticity –
Measure of ability to be stretched and
then return to its original size.
Example:Rubber Bands, Elastic, and
Playground Balls
Question: Which ball would you rather play
basketball?

15. Physical Properties of Matter – Cont.
Malleability –
Ability to be hammered into sheets
Example: Gold &Silver Coins, Aluminum
Foil and Soda Cans

16. Physical Properties of Matter – Cont.
Brittleness –
measures a material’s tendency to shatter upon impact
Example: Sulfur, Calcium and Glass
Hardness –
Resistance to breaking or scratching
Example: diamonds

17. Physical Properties of Matter – Cont.
Luster –
shininess
Example: Gold, Silver, Mercury
Ductility –
ability to be pulled into wires
Example: Most metals (Copper, Silver)

18. Physical Properties of Matter – Cont.
Tensile Strength-
Measure of how much pulling, or tension, a material can withstand before breaking
Property of fibers, ropes, cables, girders
DuPont Kevlar-5 times tensile strength of steel

19. Physical Properties of Matter – Cont.
Density –
The amount of mass in a given volume
How tightly packed the atoms or molecules are in a substance
Formula to calculate density is:
Density = Mass
Volume
Units are expressed as:
g/mL or g/L for liquids (remember the graduated cylinder)
g/cm3 for solids

20. Density of a Fluid Fluid- Any matter that is able to flow
Liquids and gases
Density of a liquid might be different from the density of the same solid
Most materials are denser in solid phase than their liquid phase
Exception- Water-freezes with air spaces so it is less dense and floats.
Density of water is 1 g/cm3

21. Physical Properties of Matter – Cont.
Buoyancy –
Upward force a fluid exerts on an object
Determines whether the object will sink or float
Example: Buoyancy of water keeping
you afloat while swimming

22. Buoyancy Buoyancy force is LESS then object’s weight, object will SINK
Buoyancy force is equal to the object’s weight, object will FLOAT
Buoyancy force is MORE then object’s weight, object will FLOAT IN AIR

23. Archimedes's Principle
Greek mathematician, 3rd century BC
Principle states-The buoyancy force on an object in a fluid is equal to the weight of the fluid displaced by the object
Buoyancy of Gasses
Balloon floats because it displaces a very large volume of air
Volume of air displaced weighs more than the balloon

24. Charles’ Law Jacques Charles, French scientist (1742-1823)
Law states-volume of a gas increases when temperature increases and reverse, volume of gas decreases when temperature decreases.
Pascal-unit for pressure (Pa) (kPa)
V1 / T1 = V2 / T2
Temperature must be in Kelvin degrees

25. Boyle’s Law Robert Boyle-British scientist (1627-1691)
Law states-as pressure of a gas increases, its volume decreases proportionately and reverse pressure of gas decreases, its volume increases proportionately.
P1 V1 = P2 V2