1. Matter

2. What is matter? Has mass Like a rock is an idea matter? Takes up space
Like air or water
is heat matter?

3. Matter Pure substance Can it be physically separated mixture yes no no
Can be chemically separated
Uniform composition?
Homogeneous mixture
Heterogeneous mixture
compound
element

4. Physical separation methods
Filtration – process that separates materials based on size
Distillation – process that separates substances in solution based on their boiling points
Chromatography -

5. Mixtures Homogeneous: evenly mixed cannot see individual parts
solution
example: salt water
Heterogeneous:
can see individual parts
example: granite rock

6. Solution Systems gas-gas: Air Gas-liquid: Soft drink Liquid-gas
Moist air
Liquid –liquid
Vinegar
Solid-solid
Steel (an alloy)

7. Pure Substances Examples: table salt (NaCl) Elements:
Composed of identical atoms
Examples – copper, hydrogen
Compounds:
Composed of 2 or more elements in a fixed ratio
Has different properties than constituent elements
Examples: table salt (NaCl)

8. Changes in state of matter
sublimation
melting
vaporization
solid
liquid
gas
freezing
condensation
deposition

9. Solids have a definite shape and a definite volume.
Liquids have and indefinite shape and a definite volume.
Gases have a indefinite shape and an indefinite volume.

10. Particle movement and phase
solid
liquid
gas

11. Particle movement and phase
Add heat
Add heat
solid
liquid
gas

12. Physical Properties
Can be observed or measured without changing the composition of the matter
Melting point, boiling point
Density
Solubility
Color
Malleable/ductile
Hardness
Conductivity
Viscosity
Odor

13. Physical Changes
Changes of state: melting, freezing, condensation, etc…
Drawing copper into a wire
Desalinization
The substance only changes size, shape or state – it does not become a different substance

14. Chemical Properties
The ability of a substance to combine with or change into another substance
Reactivity
flammability
A new substance is formed

15. Chemical Changes
Combustion
Rusting, tarnishing

16. Evidence of a chemical change
Color change
Production of a gas
Formation of a precipitate (a solid that forms and separates from a liquid)
Temperature change

17. Check for understanding indicate if the change is physical or chemical
Melting ice
Painting wood
Burning wood
baking
Breaking glass
Burning propane
Iron rusting

18. Temperature The average kinetic energy of the particles in an object
Absolute zero – no particle movement; theoretically impossible
Regardless of how cold an object is the particles that make up that object are moving.
The warmer an object is the more the particles move; the cooler – the slower

19. Phase change diagram

20. Phase Change Diagram
Triple point – the point that represents the temperature and pressure at which all three states can coexist
Lines between phases – water can exist in both phases
Critical point – the temperature and pressure above which water cannot exist as a liquid

21. Changes in state of matter
sublimation
melting
vaporization
solid
liquid
gas
freezing
condensation
deposition

22. Vapor pressure is the pressure exerted by a vapor over a liquid
The temperature at which the vapor pressure of a liquid equals the atmospheric pressure is the boiling point of that liquid
Vapor pressure and boiling (11)
vapor pressure and boiling
Boiling on Everest

23. Heating/cooling curve

24. Heating curve
Diagonal lines are temperature ranges at which the substance exist as a solid, liquid or gas.
The horizontal lines are temperatures at which the substance is melting or boiling.
During a phase change the temperature of the substance is not changing.

25. q = mcDT – formula for calculating heat
q – heat absorbed or released
m - mass of substance
c – specific heat (the heat required to raise the temperature on one gram of a substance by one degree Celsius)
DT – change in or difference in heat
The unit for heat is the joule (J)

26. Heat of Fusion/heat of Vaporization
Heat of fusion – q = Hf is used to calculate heat absorbed or released during melting or freezing
Heat of vaporization – Hv is used to calculate heat absorbed or released during vaporization or condensation

27. One joule = calories
In the metric system the amount of heat required to raise the temperature of one gram of pure water by one degree Celsius = one calorie