1. Review for Test 1

2. Fields of chemistry Analytical chemistry- Physical chemistry- Organic-
composition of matter
Physical chemistry-
mechanisms of reactions
Organic-
compounds with carbon
Inorganic-
noncarbon compounds
Biochemistry-
processes in living organisms

3. Matter Anything that has Law of Conservation of Mass states that
takes up space
has mass
Law of Conservation of Mass states that
matter is always conserved. The total mass of reactants equals the total mass of products.

4. Classes of matter solutions Pure substances- on periodic table
Compounds- water, salt, sugar, carbon dioxide
Solutions- salt water, air, brass
solutions

5. Ways of separating a mixture
Filtration
Distillation/evaporation
Dissolving
Using a magnet

6. Phases (states) of matter
Solid- retains its size and shape
- incompressible (definite volume)
Liquid- not rigid (takes the shape of its container)
- definite volume
Gas- easily compressed
- indefinite shape and volume

7. States of Matter Solid Definite No Liquid Indefinite Gas yes State
Shape
Volume
Compressible?
Solid
Definite No
Liquid
Indefinite
Gas
yes

8. Physical properties
Can be determined without changing the identity of the material
Freezing point
Boiling point
Color
Odor
Hardness
Density
Solubility

9. Extensive Properties Intensive Properties
Depend on how much (the extent) matter there is
i.e. length, mass, volume
Intensive Properties
Do NOT depend on how much matter there is
i.e. temperature, density (m/V)
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.

10. Chemical Properties
Describe the behavior of a material in reactions that change its identity
Combustibility
Reactivity with acids

11. General classes of elements
Metals – have luster (shine)
- are malleable (not brittle)
- are ductile (can be drawn into wires)
- conduct heat and electricity
Nonmetals- poor conductors of heat and electricity
-brittle
Metalloids- have characteristics of metals and nonmetals

12. Physical Changes
are those in which the identifying properties of a substance are unchanged
Ex. : change of phase
breaking, cutting
dissolving

13. Chemical Changes are those in which different substances are formed
Ex.: burning
rusting
decaying or spoiling
acid reacting with metal
fermenting

14. Signs of a chemical change
Heat gained or lost
Production of a gas
Formation of a precipitate
Color change

15. The significant figures in a measurement are all the digits that are known with certainty, plus the first digit that is uncertain.
Read the bottom of the meniscus (line AB) ml

16. Significant Figures All nonzero digits are significant 43.5
Zeros are significant when. . .
between two nonzero digits
to the right of a decimal point and to the right of a nonzero digit
to the left of an expressed decimal point and to the right of a nonzero digit. 19,000.
Not significant when. . .
the zeros to the right of a decimal and to the left of a nonzero digit
to the right of a nonzero digit but to the left of an understood decimal 109,000

17. Operations with significant figures
Multiplication and division
The answer contains the same number of significant figures as the measurement with the least number of significant figures.
Addition and Subtraction
The answer has the same number of decimal places as the measurement with the least number of decimal places.

18. Precision vs. Accuracy
Precision is the agreement between measurements.
Accuracy is the nearness of a measurement to its actual value.
x x x
x x
x x x
x x x
x x x
Not accurate
Not precise
Not accurate
Is precise
`Accurate
Precise

19. Scientific Notation
Write 17,500 in scientific notation x 104 Write in scientific notation. 5.0 x 10-3 (3.0 x 105)(5.0 x 10-2)= (3.0 x 5.0) x 105+(-2)

20. SI Prefixes
mega 106
kilo 103
basic unit
deci 10-1
centi 10-2
milli 10-3
micro 10-6
nano 10-9
pico

21. Metric (SI) Base Units Length- meter Mass- kilogram
Volume- liter (displacement)
- cm3 (L x W x H)
Temperature- Celsius oC=5/9(F-32)
oF = 9/5C +32
- Kelvin 0◦C = 273 K
to solve for Kelvin:
K = oC + 273
Time- sec
Amount of substance- mole

22. Percent Error
theoretical – experimental x 100% = theoretical Ex.: You analyze a sample of copper sulfate and find that it is 68% copper. The theoretical value is 80%. What is your percent error? x 100% = 15% 80

23. Dimensional Analysis
Multiply your starting point by a conversion factor (equal to 1)
Units should cross out algebraically, leaving you with the unit desired.
Ex.: Convert 2hr to min.
Conversion factor is 1hr = 60min
2hr x 60min = 120 min
1 hr

24. Practice Problems
How many significant digits are in the following numbers? 4 3 2 8 6

25. Using significant figures
Perform the following operations cm x 12.1 cm = 3.45 cm3  cm2 = = – 5.4 = Round to two significant figures
418 cm2
.285 cm
122
192.8
.0049

26. Scientific notation
2.315 x 105
231, x 105 Dimensional analysis Convert 66.5km to ft. Hint: 1 mi = 1.61 km and 1 mi = 5280 ft 66.5km x 1mi x 5280ft = 1.61km 1 mi
2.05 x 10-3
5.5 x 106
218,000 ft

27. Metric units Change 5L to kL Convert 499 kg to mg
How many nm are in 5mm?
Which is larger, a picogram or milligram?
Which is smaller, a Mm or a mm?
What is the freezing point of water in Kelvin?
499,000,000 mg
5 x 106 nm
milligram mm
273K

28. Classify the types of matter
Table salt
Air
Gasoline
Salad dressing
Stainless steel
Sucrose
Nitrogen
compound
Homogeneous mixture
Homogeneous mixture
Heterogeneous mixture
Homogeneous mixture
compound
element