Summer Review Packet

BASIC CONCEPTS REVIEW PACKET CHEMISTRY I L-H AND L-1 1.

A graduated cylinder contains 31.5 mL of water. A rock is dropped into this graduated cylinder and the water level in the graduated cylinder rises to 43.0 mL. What is the volume of this rock?

2.

How is mass different from weight?

3.

What piece of equipment is used to measure mass?

4.

What piece of equipment is used to measure weight?

5.

Define density. What are the metric units for density?

6.

A block of wood is 23.5 cm long, 17.6 cm wide, and 10.3 cm high. Its mass is 3,795.00 g. Calculate the density of the block of wood.

7.

The density of aluminum is 2.70 g/cm3. A piece of aluminum has a mass of 17.35 g. Calculate its volume. If this piece of aluminum is dropped into a graduated cylinder containing 57.0 mL of water, to what level will the water in the graduated cylinder rise?

8.

A cylinder made out of copper has a diameter of 4.1 cm and a length of 12.5 cm. What is the mass of this cylinder? The density of copper is 8.90 g/cm3.

9.

Graph the following sets of data. For each graph: • Draw a best fit line. • Calculate the slope of the best fit line.

• What does the slope of the best fit line that you drew signify or represent? a. A student masses a series of obtained pennies and obtains the boiling water: following data: Number of pennies 1 2 3 4 5 Laliberte, 8/25/08

Mass of pennies, grams 3.15 6.25 9.87 13.05 15.15

b. The following data is from a sample of Boiling time, minutes 0 2 4 6 8 10

Mass of water, grams 15.00 14.10 13.20 12.00 10.90 10.10

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10. What are the values for the following metric prefixes? a) deci b) centi c) milli d) deka e) hecto

f) kilo

11. a) A book is 31.3 centimeters in length. Convert this measurement to kilometers. b) A cube of sugar has a mass of 0.35 dekagrams. Convert this mass to milligrams. 12. a) A bag of rock salt has a mass of 4,450 grams. Write this mass in scientific notation. b) A sheet of aluminum foil is 0.00075 cm thick. Write this thickness in scientific notation. 13. a) Define the terms “element”, “mixture”, and “compound”. b) Classify each of the following as an element, a mixture, or a compound: 1) methyl alcohol 5) gold 2) salt water 6) oxygen 3) carbon dioxide 7) salt and pepper 4) granite 8) water 14. a) Define “heterogeneous” and “homogeneous”. b) Classify each substance listed in Question 13 as heterogeneous or homogeneous. 15. a) Define “chemical change” and “physical change”. b) Classify each of the following as a chemical change or a physical change: 1) Dissolving sugar into water. 2) Burning gasoline in an automobile engine. 3) Melting ice. 4) Shredding paper. 5) Tarnishing of silverware. 6) Evaporating water. 7) Passing an electric current through water so that it breaks down into hydrogen gas and oxygen gas. 8) Producing light by burning a candle. 9) Producing light by turning on an incandescent light bulb. 10) Baking a cake. 17. What is the difference between an atom and a molecule?

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18. a) What are the three basic subatomic particles that make up an atom? b) Where is each particle located in the atom? c) What is the difference between “atomic number” and “mass number”? d) What is an isotope? 19. The following terms are associated with designing and conducting an experiment. a) What is meant by “hypothesis”? b) What is meant by “independent variable” and “dependent variable”? c) What is meant by “control”? Why is it important to include a control in an experiment? d) What does “replicable” mean? Why is it important to write an experimental procedure that is replicable? e) What does it mean to “control variables” when designing an experiment and why is this important? f) When is it appropriate to draw a bar graph from experimental data? g) When is it appropriate to draw a line graph from experimental data? h) What is meant by “draw a conclusion”? i) What is meant by “validity of the conclusions”? Why is it important to consider the validity of conclusions?

Laliberte, 8/25/08

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