1. Matter
I. What is Matter?

2. Matter
Anything that has mass and takes up space

3. A. Kinetic Molecular Theory
KMT
Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.

4. B. Pure Substances Element composed of identical atoms
Atom is the smallest unit of element that maintains the properties of the element
EX: copper wire, aluminum foil

5. B. Pure Substances Compound
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)

6. B. Pure Substances Compound
Every compound is different from the elements it contains
Atoms can join together to make molecules like letters of the alphabet combine to form different words

7. B. Pure Substances Chemical Formulas
Shows how many atoms of each element are in a unit of a substance
The subscripts (little numbers on the bottom) tell you how many atoms of each are present
Sugar has 6 Carbon atoms, 12 Hydrogen atoms, and 6 oxygen atoms

8. B. Pure Substances Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.

9. Two different compounds, each has a definite composition.
B. Pure Substances
For example…
Two different compounds, each has a definite composition.

10. C. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous
Homogeneous

11. C. Mixtures particles don’t settle EX: rubbing alcohol, sugar water
Solution
homogeneous
very small particles
particles don’t settle
EX: rubbing alcohol, sugar water

12. C. Mixtures particles DO settle EX: flour and water Solution
heterogeneous
Substances are not evenly distributed or uniform
particles DO settle
EX: flour and water

13. Can it be physically separated?
A. Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

14. C. Mixtures Examples: element graphite hetero. mixture pepper compound
Homogenous mixture
Examples:
graphite
pepper
sugar (sucrose)
paint
soda

15. C. Mixtures Liquids can either be miscible or immiscible Miscible
Homogenous
Only looks like one liquid when combined
Ex. Gas (really about 100 liquids)
Immiscible
Heterogeneous
Liquids don’t mix and they form layers
Ex. Oil in water; italian salad dressing

16. B. Density
A measure of mass per unit of volume, remains constant for pure substances
How much matter is contained in a certain volume
The higher the object’s density, the higher its mass per volume.
This is what decides if something floats or sink…
If you have to substances, the one with the larger density will sink and the one with the smaller density will float
SI Unit: kg/m3
Common units in problems: g/mL, g/cm3

17. B. Density M
Mass (g) D V
Volume (cm3)

18. Problem-Solving Steps
1. Analyze
2. Plan
3. Compute
4. Evaluate

19. B. Density V = 825 cm3 M = DV D = 13.6 g/cm3 M = (13.6 g/cm3)(825cm3)
An object has a volume of 825 cm3 and a density of 13.6 g/cm3. Find its mass.
GIVEN:
V = 825 cm3
D = 13.6 g/cm3
M = ?
WORK:
M = DV
M = (13.6 g/cm3)(825cm3)
M = 11,200 g

20. B. Density D = 0.87 g/mL V = M V = ? M = 25 g V = 25 g 0.87 g/mL
A liquid has a density of 0.87 g/mL. What volume is occupied by 25 g of the liquid?
GIVEN:
D = 0.87 g/mL
V = ?
M = 25 g
WORK:
V = M D
V = g
0.87 g/mL
V = 29 mL

21. II. Properties & Changes in Matter Physical vs. Chemical

22. A. Physical vs. Chemical Properties
Physical Property
can be observed or measured without changing the identity of the substance
Chemical Property
describes the ability of a substance to undergo changes in identity

23. A. Physical vs. Chemical Examples: physical melting point chemical
flammable
density
magnetic
tarnishes in air
reactivity

24. More examples of chemical and physical properties
Melting pt
Boiling pt
Freezing pt
Density (mass, vol.)
Buoyancy
Color
Texture
Change in Physical State (solid, liquid, gas, plasma)
Reactivity
Fermentation
Flammability
Oxidation pH
Toxicity
electronegativity

25. C. Physical vs. Chemical Changes
Physical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Change
changes the identity of a substance
products have different properties

26. C. Physical vs. Chemical Changes
Signs of a Chemical Change- How you know if a reaction occurred…
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat

27. C. Physical vs. Chemical Changes
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices
chemical
physical

28. Quick Summary of Physical and Chemical Changes
Physical changes are changes in the physical properties of a substance that do not change the identity of a substance
Physical changes are often easily reversed
Chemical Changes form new substances that have new properties. Chemical changes can be reversed ONLY through chemical reactions
Chemical changes often cause changes in color, smell, or produce sound, light, odor, heat