Name:______________________________________________________Pd:_______Date:_________________
*Do not forget about the extra resources available to help you study and prepare for this test!

Textbook pages 41- 55 (answers to odd questions in the back of the book)

Mastering Chemistry Study Area: http://www.pearsonmylabandmastering.com/northamerica/

Miss Marnik’s Website: http://www.northallegheny.org/Page/16665
(text pages 16-24)
Need to be able to:

Determine which digits in a number are significant.

Round to the correct number of significant figures.

Distinguish between exact numbers and measurements.

Determine the correct number of significant figures in multiplication and division problems.

Determine the correct number of significant figures in addition and subtraction problems.

Determine the correct number of significant figures in problems with both addition/subtraction and multiplication/division.
Practice Problems:
1.
Describe the following targets as precise/imprecise and accurate/inaccurate.
2.
Which of the following is most likely to produce data that are not precise? a.
a balance that is not set to zero b.
not reading a graduated cylinder at eye level c.
altering the procedure the same way during each experiment d.
making the same error with each trial
3.
Determine how many significant figures are in each number. a.
58.31 e.
0.500 b.
c.
2.7 x 10 3 d.
0.00250
1 cm = 0.01 m f.
2100 g.
4.8070 h.
3.10 x 10 -4
Honors Chemistry 1

4.
Perform each calculation to the correct number of significant figures. a.
4.562 × 3.99870 ÷ 89.5 c.
3.46 m

1.82 s b.
16 m × 2.82 m × 0.05 m d.
65.2 × 0.0015 × 12.02
5.
Perform each calculation to the correct number of significant figures. a.
2.18 + 5.621 + 1.5870 – 1.8 c.
6.435 cm

2.18 cm b.
51.2 kg + 64.44 kg d.
7.2 + 4.8 + 9 – 1.45
6.
Perform each calculation to the correct number of significant figures. a.
(4.58 ÷ 1.239) – 0.578 c.
(8.9 × 10 5 ÷ 2.948 × 10 2 ) + 121 b.
(238.5 + 456.18) × 0.810 d.
(5.2 × 10 3 – 1.53 × 10 3 ) ÷ 34.5
(text pages 13-15)
Need to be able to:

Express very large and very small numbers using scientific notation.

Convert a number between decimal and scientific notation.
Practice Problems
1.
Write the following measurements in scientific notation: a.
802,347,894 s c.
0.000421 g b.
5,000,000 km d.
0.03 cm
Honors Chemistry 2

2.
Write the following measurements in decimal notation: a.
1.61 x 10 2 b.
3.145 x 10 -6 c.
4.46 x 10 3 d.
2.0 x 10 -4
(text pages 24-26)
Need to be able to:

Report measured quantities to the correct number of digits.

Recognize and work with the SI base units of measurement, prefix multipliers, and derived units.
Practice Problems:
1.
Complete the following table:
Quantity
SI Base Units
Base Unit Unit Symbol a.) s b.) Mass c.) Kelvin d.) Length
2.
Arrange the following prefixes in order from the largest to smallest: centi- mega- nano- kilo- milli- deka- deci- micro-
3.
True or false: a.
The mass of an object is the measure of the quantity of matter within it. b.
The SI unit of mass is the gram. c.
The SI prefix multiplier milli- means 1000. d.
The SI prefix multiplier for 10 6 is micro. e.
Cubic centimeter (cm 3 ) is a unit of volume?
Honors Chemistry 3

4.
Record the following measurements: a.
b. c.
(text pages 27-36)
Need to be able to:

Convert between units using dimensional analysis.

Convert between units raised to a power.
Practice Problems:
1.
Perform the following conversions: a.
5678 m to km d. d.
4.60 x 10 8 µL to kL b.
0.032 kg to g c.
3.009 cm to nm e.
0.03 m 3 to cm 3 f.
7.69 x 10 -4 L to mL
2.
Perform the following conversions: a.
6.8 mm to in b.
8.44 ft 3 to L c.
182.5 lbs. to kg
Honors Chemistry d.
140 gal to kL e.
55 km/hr to m/s f.
1.303 kg/cL to g/mL
4

(text pages 36-41)
Need to be able to:

Calculate the density of a substance.

Use density as a conversion factor to solve for mass or volume.
Practice Problems:
1.
What are the two units for density and when is each one used?
2.
A block of aluminum has the following dimensions:
Length = 0.50 cm Width = 2.50 cm Height = 2.00 cm Mass = 6.75 g a.
What is the density of aluminum? b.
Would aluminum sink or float in water? Explain.
3.
Iron has a density of 7.86 g/cm 3 . A piece of iron is placed in 7.0 mL of water. The water rises to 9.0 mL.
What is the mass of this piece of iron?
4.
Glycerin has a density of 1.26 g/mL. What would be the volume of glycerin that would have a mass of
1.10 g?
5.
A 147 g piece of metal has a density of 7.00 g/mL. A graduated cylinder contains 20.0 mL of water.
What is the final volume of water after the metal is added to the graduated cylinder?
6.
Which of the following samples have the same density?
SAMPLE A:
Mass = 8.0 x 10 4 mg
Volume = 2.0 cL
SAMPLE B:
Mass = 1.2 dag
Volume = 30.0 cm 3
SAMPLE C:
Mass = 44 g
Volume = 1.10 x 10 -5 kL
Honors Chemistry 5