1. Physical & Chemical Properties & Changes

2. Matter Anything that has mass and takes up space
Mass – a measurement that reflects the amount of matter
Weight – a measure of the amount of matter and the effect of Earth;s gravitational pull on that matter.
Air is matter!

3. States of Matter Solid – matter with its own definite shape and volume
Ex: wood, iron, paper, sugar
Liquid – matter that flows
Ex: water, blood, mercury
Gas – matter that flows to conform to the shape of its container and fills the entire volume
Neon, methane, air

4. States of Matter State Shape Volume Compressible? Solid Liquid Gas
Definite No
Liquid
Indefinite
Gas
Yes

5. Physical Properties
A characteristic that can be observed or measured without changing the samples composition.
Density
Color
Odor
Taste
Hardness
Melting point
Boiling point
Solubility

6. Extensive Properties Intensive Properties
Depends of how much (the extent) matter there is
Ex: mass, length, volume
Intensive Properties
Independent (does NOT depend) of how much matter
Substance can often be identified by intensive property
Ex: density, temperature
Pour two quantities of same-temperature water together and take temp. again. No change.
Put a cork in a small beaker of water. It floats. Repeat with a large beaker of water. It still floats.

7. Chemical Properties
The ability of a substance to combine with or change into one or more other substances
Combustibility
Sodium reacts with water, may combust
Reactivity with other substances
Iron rusts when exposed to oxygen

8. Types of Matter Substance (Pure Substance) Element Compound Mixture
Matter that has uniform and unchanging composition
Only 1 type of matter present
Element
A pure substance that cannot be separated into simpler substances by physical or chemical means
Compound
Combination of two or more different elements chemically combined
Mixture
Combination of two or more pure substances in which each pure substances retains its chemical properties

9. Classes of Matter Matter Pure substance mixture element homogeneous
compound
heterogeneous
Pure substances- on periodic table
Compounds- water, salt, sugar, carbon dioxide
Solutions- salt water, air, brass

10. Mixtures Homogeneous Mixture- Heterogeneous Mixture-
Has a constant composition throughout
Single phase
Looks the same throughout
Also referred to as solutions
Heterogeneous Mixture-
Does not blend smoothly throughout
Individual substances remain distinct

11. Examples Element Compound Heterogenous Mix. Homogenous Mix. Carbon
Iron
Gold
Mercury
Compound
Water
Carbon Dioxide
Table Salt
Aspirin
Heterogenous Mix.
Concrete
Milk
Wood
Sand
Homogenous Mix.
Air
Salt water
White gold
Brass
Brass is a mixture of copper and zinc
Mixture- contains more than 1 substance. Can be separated into pure components.
Homogeneous- uniform in composition (solutions) i.e. salt water, air
Heterogeneous- not uniform throughout i.e. clay in water, soup, concrete
Separation methods- filtration, evaporation, centrifuge (blood), magnets

12. General Classes of Elements
Metals –
Have luster (shine)
Malleable (not brittle)
Ductile (can be drawn into wires)
Conduct heat and electricity
Nonmetals –
Brittle
Poor conductors of heat and electricity
Metalloids –
Have characteristics of both metals and nonmetals

13. Solutions A homogeneous mixture Composed of 2 parts
Solvent – substance there is more of
Dissolving substance
Solute – substance that is added to solvent
Dissolved substance
Concentrated solutions have a lot of solute in the solvent.

16. Physical Changes Alter a substance without changing its composition
Identifying properties remain unchanged
Phase change
Breaking or cutting
Dissolving
Bend
Crumple
Split
Crush
distillation

17. Chemical Changes One or more substances changing into new substances
Different substances formed
Burning
Rusting
Decaying or spoiling
Fermentation
Acid reacting with metal

18. Signs of a Chemical Change
Heat gained or lost
Production of a gas
Formation of a precipitate
Color change
Sulfuric acid and sugar- heat, gas, and color change.

20. Water breaking down into hydrogen and oxygen gases
Ice changing to liquid water
Physical change
Chemical change

21. Law of Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction, it is always conserved.
Mass of reactants always equals mass of reactants.
Massreactants = Massproducts

22. Law of Definite Proportions
Regardless of amount, a compound is always composed of the same elements in the same proportion by mass.
Water, H2O
Always made of 2:H’s and 1:O no matter how much water you have

23. Percent by Mass
% by mass = Mass of Element X 100 Mass of Comound

24. Law of Multiple Proportions
When different compounds are formed by a combination of the same elements, different masses of one element combine with the same relative mass of the other element in a ratio of small whole numbers.
H2O vs. H2O2
Water has 2 H’s for every 1 O
Hydrogen peroxide has 2 H’s for every 2 O’s

25. Methods of Separating Mixtures
Use different properties of substances to separate them
Sand and iron filings
Sand and salt
Sand and water
Water and salt water
Oil in water (immiscible liquids)
Mixture of pigments
Remove iron with magnet
Dissolve salt, evaporate water
filter
Distill the water
Settle and extract less dense liquid
Paper chromatography

26. Chromatography
Distillation

27. Chemical Symbols First letter is ALWAYS capitalized
Second letter, if there is one, is NEVER capitalized
Co and CO are very different!
Some elements use their Latin name
2 O means 2 oxygen atoms
O2 means 2 oxygen atoms are chemically bonded together