1. Chemistry…
The Study of MATTER

2. MATTER Matter is anything that has MASS OR VOLUME
Mass: Amount of MATTER in an object
Volume: Amount of SPACE occupied by an object

3. There are TWO types of Matter…
PURE SUBSTANCES
MIXTURES
Contain one type of particle
Examples:
- copper
- water
- hydrogen gas
- NaCl (sodium chloride)
Contain 2 or more pure substances
Examples:
- salt mixed in water
- granola

4. 1. Pure Substances ELEMENTS COMPOUNDS
Contain only 1 kind of particle. It’s as simple as you can get!
Examples:
- Zinc (Zn)
- Magnesium (Mg)
Contain 2 or more elements
Examples:
- water (hydrogen + oxygen)
- copper chloride (copper
+ chlorine)

7. Element or Compound?
Grab the selection of pure substances I have provided for your group… Let’s see if you can figure out if they are elements or compounds. Record an “E” (element) or “C” (compound) AND explain your reasoning. 1.Element 4.Element 2.Compound 5.Compound 3.Compound 6.Element

8. 2. Mixtures HETEROGENOUS HOMOGENOUS Not uniform in composition
Have big clumps you can see
Examples:
- oil with water
- sulfur mixed with iron
Substances are evenly mixed together
Solutions such as pop or air are a great example

10. PROPERTIES OF MATTER
Properties are how we describe something. Another term for this would be “Characteristics of Matter” Physical Properties: -State -Solubility -Melting/Boiling Point -Conductivity -Malleability -Density -Ductility

11. 1.States of Matter There are 3 Kinds!
Solids- these DON’T need to be in a special container in order to be carried.
An example is rocks
Liquids- these take the shape of the container they are in
An example is water
Gas- these take the volume and shape of the container they are in
An example is oxygen

12. 2.Melting and Boiling Point
A substance’s MELTING point is when it turns from a solid to a liquid
A substances BOILING point is when it turns from a liquid to a gas.

13. 3.Malleability **
Malleable means a material can be beaten into sheets (ex. metal foil)

14. 4.Ductility
Ductile means a material can be pulled into wires (ex. copper or aluminum)

15. 5.Solubility
How well a substance will dissolve into a given amount of another substance.
Example. Salt is soluble in water. This means it dissolves in water!

16. 6.Conductivity
The ability for something to conduct electricity or heat.

17. 7.Density How heavy something is
Remember the math equation for density?
Density = Mass
Volume
Density is expressed in these units: g/cm3 or g/mL

18. Chemical Properties
Chemical Properties describe the behaviour of a substance as it changes into a NEW substance
Flammability:
Rapid reaction of substance with oxygen  release ENERGY
Also called burning or combustion
Example… burning gas in car engines; burning paper

19. Corrosion:
Slow reaction of metal with oxygen to form metal oxides
Example… Rusting of iron into iron oxide
Reactions with Acids:
Reaction of some metals (often produces gases like H2 or CO2)
Example… Limestone broken down by weak acid

20. Let’s Remind ourselves- Chemical Changes…
Are irreversible (can’t “go back” to the original reactants)
Produce new substances
Create new properties (ex. colours, solids from 2 liquids, etc)
Give off heat or light or sometimes absorb heat!

21. Some More info on Density
Density: The amount of matter in a certain volume of a substance
Density is a quantitative property
We measure density using this formula:
Density = Mass (measured in grams “g”)
Volume (measure in mL or cm3)
When you compare densities, you are comparing heaviness

22. Densities of Different Substances
Water… 1.00 g/mL
Silver… 10.5 g/cm3
Ethanol… 0.79 g/mL
If you put silver in water it will sink. This is because silver is more dense than water.
If you put ethanol in water it will float. This is because ethanol is less dense than water.