1. Scientific Notation Write 17,500 in scientific notation. 1.75 x 104
(3.0 x 105)(5.0 x 10-2)= (3.0 x 5.0) x 105+(-2)

2. Addition and subtraction: all numbers must be changed to the same exponent. Then add or subtract the numbers, attaching the common exponent.
ex.: 8.3 x x 103
0.83 x 103
+5.7 x 103
6.53 x x 103

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

4. SI Prefixes Giga 109 Mega 106 kilo 103 basic unit deci 10-1 centi 10-2
milli 10-3
micro 10-6
nano 10-9
pico
Bobby measures a stick and says it is 5. Billy measures the same stick and says it is 15. They are both right. How can that be? UNITS!!!

5. From DOE

6. Indicate the uncertainty of a measurement
Significant Figures
Indicate the uncertainty of a measurement
If the earth is 4 billion years old, will it be 4 billion and one next year?
If I ask you how tall you are and you say between 5-6 feet, that isn’t very interesting. You left out the interesting information.

7. 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

8. 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

9. Beginning zeros are not significant.
Ending zeros are only significant when there is a decimal.

10. 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.

11. Operations with significant figures
Multiplication and division
Sample 1: 24 cm x 31.8 cm = cm2
answer: 760 cm2
Sample 2: 8.40 g ÷ 4.2 ml = 2 g/ml
answer: 2.0 g/ml

12. Addition and Subtraction
Sample 1: 49.1 g g = g
answer: 57.1 g
Sample 2: m – 7.35 m = 74 m
answer: m

13. 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 precise, nor accurate
Precise, not accurate
Precise and accurate

14. 
5.8 
These thermometers have different levels of precision. The increments on the left one are .2 but on the right one they are 1 . How should their temperatures be recorded?

16. 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?
80-68 x 100% = 15% 80

17. Derived Units Measurements derived from basic units. Area= L x W (m2)
Volume = L x W x H (cm3)
Density = m/V (g/cm3)

18. Calculations
1. What is the density of a substance whose mass is 3.0 grams and its volume is 15cm3?
3.0 grams = .20 g/cm3
15 cm3
2. Cobalt has a density of 8.90 g/cm3. What volume would 17.8 g of cobalt have?
D=m/V so V=m/D
V = 17.8 g = 2.00 cm3
8.90 g/cm3

20. 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

21. In Switzerland, gas prices are listed in Swiss Francs per liter
In Switzerland, gas prices are listed in Swiss Francs per liter. Convert the Swiss prices below to dollars per gallon.

22. Conversion factors needed:
Dollars to Francs: 1 SF = $.83
Liters to gallons: 1 quart = L
1 gallon = 4 quarts
1.71 SF x $.83 x .946L x 4 qt = $5.37
1 L SF 1 qt gal gal