CHAPTER 1, 2 and 3 CUMULATIVE REVIEW
Name: __________________________
Period_________Date: ____________
1. Record the measurements from the following instruments to the correct number of digits with
the correct unit.
a. BALANCE
b. Graduated
Cylinder
___________
____________
c. Graduated
Cylinder
___________
d. Lab
Thermometer
____________
2. Record the number of significant digits in each of the following:
2500 _____
0.157 ____
2500. ____
0.002300 ____
43.07 ____
6.751 ____
3. Convert between regular and scientific notation with correct significant digits:
2.22 x 10-4 ________ 5.47 x 103 ________ 66,000 ______________ .089 _______________
4. Convert between Celsius and Kelvin temperature scales with correct significant digits:
290. K = ______ °C
127 K = _______ °C
392°C = _________ K
-157°C = _________ K
5. Use conversion factors to solve the following. Answer with correct sig digits & unit:
72 feet to inches
350. cm to meters
25 km to centimeters
6. A block of aluminum has a mass of 36.40 g and a volume of 13.5 cm3. What is its density?
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7. What is the volume of 227 g of olive oil if its density is 0.92 g/mL.
8. Define accuracy _____________________________ & precision _______________________________.
9.
MASS OF SAMPLE
Team 1 Team 2 Team 3
Reading 1
41.04 g
31.33 g
42.34 g
Reading 2
39.77 g
31.30 g
41.12 g
Reading 3
43.15 g
31.36 g
41.21 g
Average
41.32 g 31.33 g 41.55 g
Accepted measure from issuing lab: 41.33 g
Percent error
0.02%
24.2%
0.53%
Which team is most accurate? _______ Least accurate? _______
Which team is most precise? _______ Least precise? _______
Which team has the best accuracy and precision? ________
10. Label the phases, phase changes, and freezing/boiling temperatures on the heating/cooling curve for water.
What is happening to kinetic energy during section A? _________ What is happening to kinetic energy
during section E/F? ______________
11. Pure substances are either __________________ or __________________. Mixtures may be either
________________________ or ____________________________. Three types of homogeneous
mixtures are: _________________ (clear & uniform), __________________ (cloudy & uniform) and
_________ (opaque, uniform blend of metals). At first glance a colloid & suspension may look similar.
The difference is ___________________________________________________________________.
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12. Classify the following as element (E), compound (C), solution (S), alloy (A), colloid (CL) or
suspension (SP).
____ gold
____ water
____ brass
____ carbon
____ whipped cream
____ milk
____ salt & water
____ carbon dioxide
____ gold jewelry
____ sand & water
13. ______________ properties can be measured without changing the chemical composition of a substance.
______________ properties describe chemical reactions a substance will/will not undergo.
14. Classify the following as physical (P) or chemical (C) properties:
____color
____ tendency to rust
____ mass
____ boiling point
____ reactivity with oxygen ____ flammability
____ noble gases are inert
____ density
15. Physical changes change the ___________________, but not the chemical composition of a substance.
Chemical changes (chemical reactions) create new _______________________.
16. Classify the following as physical (P) or chemical (C) changes:
____ melting iron
____ burning gasoline
____ breaking test tube
____ wood rotting
____ dissolving NaCl
____ reacting Mg w HCl
____ boiling water
____ iron rusting
17. What are the four signs of a chemical change?
18. A student experimentally determined the density of a piece of aluminum to be 2.95 g/cm3.
The accepted value for aluminum density is 2.70 g/cm3. Calculate the student’s percent error.
19. How many seconds has a teenager been alive by their 17th birthday? Put your answer in scientific notation.
20. If you drive 1.08 x 106 cm from the high school to 309 Cinema, how many miles is it?
(Given: 1 mile = 5280 ft and 2.54 cm = 1 in)
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21.
Isotope Name
Symbol
Atomic
Number
Mass
Number
Protons
Neutrons
Electrons
potassium-38
Charge
0
65
29
Cu +2
20
22
78
51
35
+2
36
123
-3
22. In Thomson’s experiment, the cathode ray was deflected by a magnet, this indicated that the ray had
____________. When the electrically charged plates were turned on, the cathode ray was deflected
toward the positive plate, this indicated that the beam had a ________________ charge.
23. Therefore a cathode ray is made of a beam of ____________________.
24. Rutherford used a radioactive sample and determined that natural radiation has ______ components:
alpha particles which have a _______ charge and a relatively _______________ mass,
________________ particles which have a negative charge and a mass of ______ and
________________ rays which are neutral and have ________ mass.
25. Rutherford used alpha particles in his Gold Foil experiment. Because the alpha particles are relatively
large and positive the fact that most of them proceeded straight through the foil proved that the atom
is mostly _______________ ______________. Some of the positive alpha particles deflected directly
back toward the source which indicated that the nucleus was __________________ charged
Thus, Rutherford is credited with discovering the ________________.
26. Draw a simple sketch of each chemist’s model of the atom. Indicate charge where needed.
Dalton
Thomson
Rutherford
Bohr
Modern Model
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