Download EOC review I

Name: ______________________
Class: _________________
Date: _________
EOC review questions I
Matching
Match each item with the correct statement below.
a. mixture
d. reactant
b. product
e. heterogeneous mixture
c. phase
f. vapor
____
1. gaseous state of substance that is a liquid or solid at room temperature
____
2. a physical blend of two or more components
____
3. part of a sample having uniform composition and properties
____
4. not uniform in composition
____
5. a substance formed in a chemical reaction
____
6. starting substance in a chemical reaction
Match each item with the correct statement below.
a. distillation
d. compound
b. mass
e. element
c. chemical reaction
f. homogeneous
____
7. amount of matter an object contains
____
8. describes mixture with a uniform composition
____
9. a process in which a liquid is boiled to produce a vapor that is condensed again into a liquid
____ 10. substance that cannot be changed into simpler substances by chemical means
____ 11. composed of two or more substances chemically combined in a fixed proportion
____ 12. process in which substances are changed into different substances
Match each item with the correct statement below.
a. proton
d. electron
b. nucleus
e. neutron
c. atom
____ 13. the smallest particle of an element that retains the properties of that element
____ 14. a positively charged subatomic particle
____ 15. a negatively charged subatomic particle
____ 16. a subatomic particle with no charge
____ 17. the central part of an atom, containing protons and neutrons
1
ID: A
Name: ______________________
ID: A
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 18. A horizontal row of the periodic table is usually referred to as a
a. family.
b. period.
c. group.
d. property.
____ 19. Which of the following is a physical property?
a. explosive
b. combustible
c. melting point
d. ability to rust
____ 20. Which state of matter has a definite volume and takes the shape of its container?
a. solid
b. liquid only
c. gas only
d. both b and c
____ 21. Which state of matter expands when heated and is easy to compress?
a. gas
b. liquid only
c. solid only
d. both b and c
____ 22. Which of the following is a physical change?
a. corrosion
b. explosion
c. evaporation
d. rotting of food
____ 23. Which of the following can be classified as a mixture?
a. pure water
b. pure air
c. pure nitrogen
d. pure gold
____ 24. Which of the following is a heterogeneous mixture?
a. air
b. salt water
c. steel
d. soil
____ 25. A substance that can be separated into two or more substances only by a chemical change is a(n) ____.
a. solution
b. element
c. mixture
d. compound
2
Name: ______________________
____ 26. The
a.
b.
c.
d.
ID: A
chemical symbol for iron is _____.
fe
FE
Fe
Ir
____ 27. Which of the following is a chemical change?
a. grating cheese
b. melting cheese
c. fermenting of cheese
d. mixing two cheeses in a bowl
____ 28. What must be done to be certain that a chemical change has taken place?
a. Check for the production of bubbles before and after the change.
b. Demonstrate that a release of energy occurred after the change.
c. Check the composition of the sample before and after the change.
d. Demonstrate that energy was absorbed by the reactants after the change.
____ 29. What happens to matter during a chemical reaction?
a. Matter is neither destroyed or created.
b. Some matter is destroyed.
c. Some matter is created.
d. Some matter is destroyed and some is created.
____ 30. The diameter of a carbon atom is 0.000 000 000 154 m. What is this number expressed in scientific
notation?
a.
1.54 × 10
12
b.
1.54 × 10
−12
1.54 × 10
10
1.54 × 10
−10
c.
d.
m
m
m
m
____ 31. The expression of 5008 km in scientific notation is ____.
3
a.
5.008 × 10 km
b.
50.08× 10
−4
−3
km
c.
5.008 × 10
d.
5.008 × 10 km
____ 32. The
a.
b.
c.
d.
km
4
closeness of a measurement to its true value is a measure of its ____.
precision
accuracy
reproducibility
usefulness
3
Name: ______________________
ID: A
____ 33. Which of the following measurements contains two significant figures?
a. 0.004 00 L
b. 0.004 04 L
c. 0.000 44 L
d. 0.004 40 L
____ 34. In the measurement 0.503 L, which digit is the estimated digit?
a. 5
b. the 0 immediately to the left of the 3
c. 3
d. the 0 to the left of the decimal point
____ 35. How many significant figures are in the measurement 0.003 4 kg?
a. two
b. four
c. five
d. This cannot be determined.
____ 36. How many significant figures are in the measurement 811.40 grams?
a. two
b. three
c. four
d. five
____ 37. What is the measurement 111.009 mm rounded off to four significant digits?
a. 111 mm
b. 111.0 mm
c. 111.01 mm
d. 110 mm
____ 38. A conversion factor that shows the relationship between grams and kilograms is
a.
b.
c.
÷ 1000
× 1000
d.
____ 39. What quantity is represented by the metric system prefix deci-?
a. 1000
b. 100
c. 0.1
d. 0.01
____ 40. What is the temperature –34°C expressed in kelvins?
a. 139 K
b. 207 K
c. 239 K
d. 339 K
4
Name: ______________________
ID: A
____ 41. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?
a. 93°C
b. 34°C
c. –61°C
d. –34°C
____ 42. What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
a. 0.23 mL
b. 4.34 mL
c. 479 mL
d. none of the above
____ 43. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.
____ 44. Which discovery did J. J. Thomson make that improved upon Dalton's atomic theory?
a. Atoms contain tiny, negatively charged electrons.
b. Atoms are always in motion.
c. Atoms contain a tiny, positively charged nucleus.
d. Atoms that combine do so in simple whole-number ratios.
____ 45. All
a.
b.
c.
d.
atoms are
positively charged, with the number of protons exceeding the number of electrons.
negatively charged, with the number of electrons exceeding the number of protons.
neutral, with the number of protons equaling the number of electrons.
neutral, with the number of protons equaling the number of electrons, which is equal
to the number of neutrons.
____ 46. The
a.
b.
c.
d.
particles that are found in the nucleus of an atom are ____.
neutrons and electrons
electrons only
protons and neutrons
protons and electrons
____ 47. Which model of the atom is thought to be true?
a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the
atom.
b. The nucleus is made of protons, electrons, and neutrons.
c. Electrons are distributed around the nucleus and occupy almost all the volume of the
atom.
d. The nucleus is made of electrons and protons.
____ 48. The
a.
b.
c.
d.
atomic number of an element is the total number of which particles in the nucleus?
neutrons
protons
electrons
protons and electrons
5
Name: ______________________
____ 49. The
a.
b.
c.
d.
ID: A
sum of the protons and neutrons in an atom equals the ____.
atomic number
nucleus number
atomic mass
mass number
____ 50. What does the number 84 in the name krypton-84 represent?
a. the atomic number
b. the mass number
c. the sum of the protons and electrons
d. twice the number of protons
____ 51. All
a.
b.
c.
d.
atoms of the same element have the same ____.
number of neutrons
number of protons
mass numbers
mass
____ 52. Isotopes of the same element have different
a. numbers of neutrons.
b. numbers of protons.
c. numbers of electrons.
d. atomic numbers.
____ 53. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
b. Zn, 30 protons, 60 electrons
c. Cs, 55 protons, 132.9 electrons
d. F, 19 protons, 19 electrons
____ 54. Using the periodic table, determine the number of neutrons in
a. 4
b. 8
c. 16
d. 24
16
O.
____ 55. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125
contain?
a. 50 protons, 50 electrons, 75 neutrons
b. 75 electrons, 50 protons, 50 neutrons
c. 120 neutrons, 50 protons, 75 electrons
d. 70 neutrons, 75 protons, 50 electrons
6
Name: ______________________
ID: A
____ 56. Which of the following sets of symbols represents isotopes of the same element?
91
92
93
a. 42 J 42 J 40 J
b.
50
L
19
50
L
20
50
L
21
c.
84
M
38
86
M
38
87
M
38
d.
138
59
133
55
133
54
Q
Q
Q
____ 57. How is the number of neutrons in the nucleus of an atom calculated?
a. Add the number of electrons and protons together.
b. Subtract the number of electrons from the number of protons.
c. Subtract the number of protons from the mass number.
d. Add the mass number to the number of electrons.
____ 58. What unit is used to measure weighted average atomic mass?
a. amu
b. gram
c. angstrom
d. nanogram
____ 59. The
a.
b.
c.
d.
atomic mass of an element is the ____.
total number of subatomic particles in its nucleus
weighted average of the masses of the isotopes of the element
total mass of the isotopes of the element
average of the mass number and the atomic number for the element
Short Answer
60. The following length measurements were taken by students using several different measuring devices.
Find the average of the measurements. Make sure that your answer has the correct number of significant
figures.
10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm
61. Round off the measurement 0.003 095 5 m to three significant figures.
7
ID: A
EOC review questions I
Answer Section
MATCHING
1. ANS:
OBJ:
2. ANS:
OBJ:
3. ANS:
OBJ:
4. ANS:
OBJ:
5. ANS:
OBJ:
BLM:
6. ANS:
OBJ:
BLM:
F
PTS: 1
DIF: L1
2.1.3 Classify physical changes.
BLM: knowledge
A
PTS: 1
DIF: L1
2.2.1 Explain how mixtures are classified.
C
PTS: 1
DIF: L1
2.2.1 Explain how mixtures are classified.
E
PTS: 1
DIF: L1
2.2.1 Explain how mixtures are classified.
B
PTS: 1
DIF: L1
2.4.1 Describe what happens during a chemical change.
knowledge
D
PTS: 1
DIF: L1
2.4.1 Describe what happens during a chemical change.
knowledge
REF: p. 37
REF:
BLM:
REF:
BLM:
REF:
BLM:
REF:
p. 38
knowledge
p. 39
knowledge
p. 39
knowledge
p. 48
REF: p. 48
7. ANS:
OBJ:
BLM:
8. ANS:
OBJ:
9. ANS:
OBJ:
10. ANS:
OBJ:
BLM:
11. ANS:
OBJ:
BLM:
12. ANS:
OBJ:
BLM:
B
PTS: 1
DIF: L1
REF: p. 34
2.1.1 Explain why all samples of a substance have the same intensive properties.
knowledge
F
PTS: 1
DIF: L1
REF: p. 39
2.2.1 Explain how mixtures are classified.
BLM: knowledge
A
PTS: 1
DIF: L1
REF: p. 40
2.2.2 Explain how mixtures can be separated.
BLM: knowledge
E
PTS: 1
DIF: L1
REF: p. 42
2.3.1 Explain the difference between an element and a compound.
knowledge
D
PTS: 1
DIF: L1
REF: p. 42
2.3.1 Explain the difference between an element and a compound.
knowledge
C
PTS: 1
DIF: L1
REF: p. 48
2.4.1 Describe what happens during a chemical change.
knowledge
13. ANS:
OBJ:
BLM:
14. ANS:
OBJ:
15. ANS:
OBJ:
16. ANS:
OBJ:
C
PTS: 1
DIF: L1
REF: p. 102
4.1.1 Explain how Democritus and John Dalton described atoms.
knowledge
A
PTS: 1
DIF: L1
REF: p. 107
4.2.1 Identify three types of subatomic particles.
BLM: knowledge
D
PTS: 1
DIF: L1
REF: p. 105
4.2.1 Identify three types of subatomic particles.
BLM: knowledge
E
PTS: 1
DIF: L1
REF: p. 107
4.2.1 Identify three types of subatomic particles.
BLM: knowledge
1
ID: A
17. ANS: B
PTS: 1
DIF: L1
REF: p. 108
OBJ: 4.2.2 Describe the structure of atoms according to the Rutherford model.
BLM: knowledge
MULTIPLE CHOICE
18. ANS: B
PTS: 1
DIF: L1
REF: p. 46
OBJ: 2.3.4 Explain how a periodic table is useful.
BLM: knowledge
19. ANS: C
PTS: 1
DIF: L2
REF: p. 35
OBJ: 2.1.1 Explain why all samples of a substance have the same intensive properties.
BLM: application
20. ANS: B
PTS: 1
DIF: L2
REF: p. 36
OBJ: 2.1.2 Identify the three states of matter.
BLM: comprehension
21. ANS: A
PTS: 1
DIF: L2
REF: p. 36
OBJ: 2.1.2 Identify the three states of matter.
BLM: comprehension
22. ANS: C
PTS: 1
DIF: L2
REF: p. 37
OBJ: 2.1.3 Classify physical changes.
BLM: application
23. ANS: B
PTS: 1
DIF: L2
REF: p. 36 | p. 44
OBJ: 2.3.1 Explain the difference between an element and a compound. | 2.3.2 Distinguish between a
substance and a mixture.
BLM: application
24. ANS: D
PTS: 1
DIF: L2
REF: p. 39
OBJ: 2.2.1 Explain how mixtures are classified.
BLM: application
25. ANS: D
PTS: 1
DIF: L2
REF: p. 42
OBJ: 2.3.1 Explain the difference between an element and a compound.
BLM: comprehension
26. ANS: C
PTS: 1
DIF: L2
REF: p. 46
OBJ: 2.3.3 Describe what chemists use to represent elements and compounds.
BLM: application
27. ANS: C
PTS: 1
DIF: L2
REF: p. 48
OBJ: 2.4.1 Describe what happens during a chemical change.
BLM: application
28. ANS: C
PTS: 1
DIF: L2
REF: p. 48
OBJ: 2.4.1 Describe what happens during a chemical change.
BLM: comprehension
29. ANS: A
PTS: 1
DIF: L1
REF: p. 50
OBJ: 2.4.3 Describe how the mass of the reactants and the mass of the products of a chemical reaction
are related.
BLM: knowledge
30. ANS: D
PTS: 1
DIF: L2
REF: p. 62
OBJ: 3.1.1 Write numbers in scientific notation.
BLM: application
31. ANS: A
PTS: 1
DIF: L2
REF: p. 62
OBJ: 3.1.1 Write numbers in scientific notation.
BLM: application
32. ANS: B
PTS: 1
DIF: L1
REF: p. 64
OBJ: 3.1.2 Evaluate accuracy and precision.
BLM: knowledge
33. ANS: C
PTS: 1
DIF: L2
REF: p. 62
OBJ: 3.1.1 Write numbers in scientific notation.
BLM: application
2
ID: A
34. ANS:
OBJ:
BLM:
35. ANS:
OBJ:
BLM:
36. ANS:
OBJ:
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47. ANS:
OBJ:
BLM:
48. ANS:
OBJ:
BLM:
49. ANS:
OBJ:
BLM:
50. ANS:
OBJ:
C
PTS: 1
DIF: L2
REF: p. 66
3.1.3 Explain why measurements must be reported to the correct number of significant
application
A
PTS: 1
DIF: L2
REF: p. 67
3.1.3 Explain why measurements must be reported to the correct number of significant
comprehension
D
PTS: 1
DIF: L2
REF: p. 67
3.1.3 Explain why measurements must be reported to the correct number of significant
application
B
PTS: 1
DIF: L2
REF: p. 68 | p. 69
3.1.3 Explain why measurements must be reported to the correct number of significant
application
A
PTS: 1
DIF: L2
REF: p. 85
3.3.1 Explain what happens when a measurement is multiplied by a conversion factor.
application
C
PTS: 1
DIF: L2
REF: p. 75
3.2.1 Explain why metric units are easy to use.
BLM: comprehension
C
PTS: 1
DIF: L2
REF: p. 79
3.2.2 Identify the temperature units scientists commonly use.
analysis
D
PTS: 1
DIF: L2
REF: p. 79
3.2.2 Identify the temperature units scientists commonly use.
analysis
B
PTS: 1
DIF: L2
REF: p. 80
3.2.3 Calculate the density of a substance.
BLM: analysis
C
PTS: 1
DIF: L2
REF: p. 102
4.1.1 Explain how Democritus and John Dalton described atoms.
comprehension
A
PTS: 1
DIF: L2
REF: p. 105
4.2.1 Identify three types of subatomic particles.
BLM: comprehension
C
PTS: 1
DIF: L3
REF: p. 107
4.2.1 Identify three types of subatomic particles.
BLM: synthesis
C
PTS: 1
DIF: L2
REF: p. 108 | p. 109
4.2.2 Describe the structure of atoms according to the Rutherford model.
comprehension
C
PTS: 1
DIF: L2
REF: p. 109
4.2.2 Describe the structure of atoms according to the Rutherford model.
comprehension
B
PTS: 1
DIF: L1
REF: p. 112
4.3.1 Explain what makes one element different from another.
knowledge
D
PTS: 1
DIF: L1
REF: p. 113
4.3.1 Explain what makes one element different from another.
knowledge
B
PTS: 1
DIF: L2
REF: p. 115
4.3.2 Explain how isotopes of an element differ.
BLM: application
3
figures.
figures.
figures.
figures.
ID: A
51. ANS:
OBJ:
BLM:
52. ANS:
OBJ:
53. ANS:
OBJ:
54. ANS:
OBJ:
BLM:
55. ANS:
OBJ:
BLM:
56. ANS:
OBJ:
57. ANS:
OBJ:
BLM:
58. ANS:
OBJ:
59. ANS:
OBJ:
B
PTS: 1
DIF: L2
4.3.1 Explain what makes one element different from
comprehension
A
PTS: 1
DIF: L1
4.3.2 Explain how isotopes of an element differ.
A
PTS: 1
DIF: L2
4.2.1 Identify three types of subatomic particles.
B
PTS: 1
DIF: L2
4.3.1 Explain what makes one element different from
analysis
A
PTS: 1
DIF: L2
4.3.1 Explain what makes one element different from
analysis
C
PTS: 1
DIF: L2
4.3.2 Explain how isotopes of an element differ.
C
PTS: 1
DIF: L2
4.3.1 Explain what makes one element different from
comprehension
A
PTS: 1
DIF: L1
4.3.3 Calculate the atomic mass of an element.
B
PTS: 1
DIF: L2
4.3.3 Calculate the atomic mass of an element.
REF: p. 112
another.
REF: p. 114
BLM: knowledge
REF: p. 112
BLM: application
REF: p. 113
another.
REF: p. 113
another.
REF: p. 115
BLM: application
REF: p. 113
another.
REF:
BLM:
REF:
BLM:
p. 116
knowledge
p. 117
comprehension
SHORT ANSWER
60. ANS:
Average = (10.05 + 10.1 + 9.741 + 10.6 + 10.5) / 5 = 10.2 cm
PTS: 1
DIF: L3
REF: p. 67 | p. 70 | p. 71
OBJ: 3.1.3 Explain why measurements must be reported to the correct number of significant figures.
BLM: analysis
61. ANS:
0.003 10 m
PTS: 1
DIF: L2
REF: p. 68 | p. 69
OBJ: 3.1.3 Explain why measurements must be reported to the correct number of significant figures.
BLM: application
4