1. Chapter 1 review

2. Matter States of Matter: solid, liquid, gas How do we classify matter?
Physical Properties of Matter
Physical Change vs Chemical Change
Measurements

4. Measurements Dimensional Analysis Density Temperature: K, ºF, ºC
ºC = (ºF – 32)/1.8
K = ºC + 273
ºC = K – 273

5. Common Units and Their Equivalents
Length
1 kilometer (km) =
mile (mi)
1 meter (m)
39.37 inches (in.)
1.094 yards (yd)
1 foot (ft)
30.48 centimeters (cm)
1 inch (in.)
2.54 centimeters (cm) exactly

6. Common Units and Their Equivalents
Mass
1 kilogram (km) =
2.205 pounds (lb)
1 pound (lb)
grams (g)
1 ounce (oz)
28.35 grams (g)
Volume
1 liter (L) =
1000 milliliters (mL)
1000 cubic centimeters (cm3)
1.057 quarts (qt)
1 U.S. gallon (gal)
3.785 liters (L)

7. Scientific Notation Locate the decimal point
Move the decimal so that there is only one number to the left of it
Write “x 10” behind you new number
Count the number of places you’ve moved your decimal point and make this number the exponent on your 10
Assign a + or – sign to your exponent
If your original # is larger than your SN #, the exponent is +
If your original # is smaller than your SN #, the exponent is –

8. Significant Figures
Numbers up to and including the “uncertain” number are significant
All non-zero numbers are significant
Zeros may or may not be significant
Zeros are significant if
They are between two non-zero digits
They are at the end of a decimal number

9. Zeros are not significant if
They are used as place holders in large numbers without a decimal point
They are at the beginning of decimal numbers
All numbers displayed in a number written in scientific notation are significant

10. Calculation With Significant Digits
Multiplication and Division
The final answer has the same number of sig figs as the measurement with the fewest sig figs
Addition and Subtraction
The final answer is written so that it has the same number of decimal places as the measurement having the fewest decimal places

11. Write these numbers using standard scientific notation. 0.0468
0.0468
6,600,000 (two significant figures)
Round off these numbers to the number of significant figures indicated.
(two significant figures)
(three significant figures)

12. Write how many significant figures the answer should contain for each of these calculations.
_________
_________
1.2
– _________

13. How many centimeters are in 2.00 ft?
For the following numbers, tell whether the zeros are significant or are not significant.
0.007
8.00 x 102
100.00
4200
3.0030

14. Calculate the following. (Show all work for full credit. Answers should show the correct number of significant figures.)
At 35 cents per liter how much will it cost to fill a 15.8 gal tank with gasoline?
How much would 1.0 kg of potatoes cost if the price is $1.78 for 10 pounds?
Normal body temperature for humans is 98.6 oF. What is this temperature on the Celsius scale?

15. Make the following conversions showing mathematical setups
0.606 cm to km
35.6 m to ft.
35 km to mm
1000. m to km
0.64 mi to inches
3.5 quarts to ml

16. Convert 78oF to degrees Celsius
An object weighs 8.22 lbs. What is the mass in grams?
A graduated cylinder was filled to 25.0 mL with liquid. A solid object weighing 73.5 grams was immersed in the liquid, raising the liquid level to 43.9 mL. Calculate the density of the solid object.
The density of carbon tetrachloride, CCl4, is 1.59 grams/mL. Calculate the volume of grams of CCl4.