Download Midterm Review

Midterm Review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. What distinguishes a substance from a mixture?
a. Substances are compounds, and mixtures are not.
b. Mixtures are groupings of elements, and compounds are not.
c. Samples of the same substance can have different intensive properties.
d. Mixtures can be separated physically, while compounds cannot.
____
2. 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.
____
3. What is the volume of a salt crystal measuring 2.44 10 m by 1.4
a. 2.9 10 m
c. 2.9 10 m
b. 2.9 10 m
d. 2.9 10 m
____
4. The density of mercury is 5,427 kg/(m3). If the density of water is 1.0 g/mL, will mercury float or sink in
water?
a. Mercury will float because the density of mercury is 0.005427 g/mL, which is less than the
1.0 g/mL density of water.
b. Mercury will float because the density of mercury is 0.05427 g/mL, which is less than the
1.0 g/mL density of water.
c. Mercury will sink because the density of mercury is 5.427 g/mL, which is greater than the
1.0 g/mL density of water.
d. Mercury will sink because the density of mercury is 5,427 g/mL, which is greater than the
1.0 g/mL density of water.
____
5. Which of the following equalities is NOT correct? Use the table above to help you.
a. 100 cg = 1 g
c. 1 cm = 1 mL
b. 1000 mm = 1 m
d. 10 kg = 1 g
____
6. What is the quantity 0.0075 meters expressed in centimeters? Use the table above to help you.
a. 0.075 cm
c. 7.5 cm
b. 0.75 cm
d. 70.5 cm
____
7. Which hypothesis led to the discovery of the proton?
a. When a neutral hydrogen atom loses an electron, a positively-charged particle should
remain.
b. A proton should be 1840 times heavier than an electron.
c. Cathode rays should be attracted to a positively-charged plate.
d. The nucleus of an atom should contain neutrons.
____
8. Which of the following is correct concerning subatomic particles?
a. The electron was discovered by Goldstein in 1886.
b. The neutron was discovered by Chadwick in 1932.
c. The proton was discovered by Thomson in 1880.
10
m by 8.4
10
m?
d. Cathode rays were found to be made of protons.
____
9. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. negatively charged, with the number of electrons exceeding the number of protons
c. neutral, with the number of protons equaling the number of electrons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the
number of neutrons
____ 10. Which of the following sets of symbols represents isotopes of the same element?
a.
c.
J
J
J
M
M
M
b.
d.
L
L
L
Q
Q
Q
____ 11. How do the isotopes hydrogen-1 and hydrogen-2 differ?
a. Hydrogen-2 has one more electron than hydrogen-1.
b. Hydrogen-2 has one neutron; hydrogen-1 has none.
c. Hydrogen-2 has two protons; hydrogen-1 has one.
d. Hydrogen-2 has one proton; hydrogen-1 has none.
____ 12. Which of the following isotopes has the same number of neutrons as phosphorus-31?
a.
c.
P
Si
b.
d.
S
Si
____ 13. What is the maximum number of electrons in the second principal energy level?
a. 2
c. 18
b. 8
d. 32
____ 14. When an electron moves from a lower to a higher energy level, the electron ____.
a. always doubles its energy
b. absorbs a continuously variable amount of energy
c. absorbs a quantum of energy
d. moves closer to the nucleus
____ 15. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in
the three orbitals?
a. one electron in each orbital
b. two electrons in one orbital, one in another, none in the third
c. three in one orbital, none in the other two
d. Three electrons cannot fill three empty 2p atomic orbitals.
____ 16. How many unpaired electrons are in a sulfur atom (atomic number 16)?
a. 0
c. 2
b. 1
d. 3
____ 17. How many half-filled orbitals are in a bromine atom?
a. 1
c. 3
b. 2
d. 4
____ 18. Which of the following electron configurations of outer sublevels is the most stable?
a. 4d 5s
c. 4d 5s
b. 4d 5s
d. 4d 5s
____ 19. What is the wavelength of an electromagnetic wave that travels at 3
MHz? (1 MHz = 1,000,000 Hz)
a.
10 m/s and has a frequency of 60
b. 60 MHz  300,000,000 m/s
c.
d. No answer can be determined from the information given.
____ 20. Which variable is directly proportional to frequency?
a. wavelength
c. position
b. velocity
d. energy
____ 21. How do the energy differences between the higher energy levels of an atom compare with the energy
differences between the lower energy levels of the atom?
a. They are greater in magnitude than those between lower energy levels.
b. They are smaller in magnitude than those between lower energy levels.
c. There is no significant difference in the magnitudes of these differences.
d. No answer can be determined from the information given.
____ 22. In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend
on ____.
a. a quantum mechanical model
c. the Schrodinger equation
b. direction with respect to the nucleus
d. the electron energy sublevel
____ 23. Of the elements Fe, Hg, U, and Te, which is a representative element?
a. Fe
c. U
b. Hg
d. Te
____ 24. Which of the following factors contributes to the increase in atomic size within a group in the periodic table
as the atomic number increases?
a. more shielding of the electrons by the highest occupied energy level
b. an increase in size of the nucleus
c. an increase in number of protons
d. fewer electrons in the highest occupied energy level
____ 25. Which of the following elements has the smallest atomic radius?
a. sulfur
c. selenium
b. chlorine
d. bromine
____ 26. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al
c. Rb , Ba , P
b. K , Sr , O
d. N , O , F
____ 27. In which of the following groups of ions are the charges all shown correctly?
a. Li , O , S
c. K , F , Mg
b. Ca , Al , Br
d. Na , I , Rb
____ 28. Which of the following factors contributes to the increase in ionization energy from left to right across a
period?
a. an increase in the shielding effect
b. an increase in the size of the nucleus
c. an increase in the number of protons
d. fewer electrons in the highest occupied energy level
____ 29. As you move from left to right across the second period of the periodic table ____.
a. ionization energy increases
c. electronegativity decreases
b. atomic radii increase
d. atomic mass decreases
____ 30. Of the following elements, which one has the smallest first ionization energy?
a. boron
c. aluminum
b. carbon
d. silicon
____ 31. An unstable nucleus ____.
a. increases its nuclear mass by fission
b. increases its half-life
c. emits energy when it decays
d. expels all of its protons
____ 32. What particle is needed to complete the following nuclear equation?
Mn
____ + e
a.
c.
Co
Fe
b.
Mn
d.
Cr
____ 33. What particle is needed to complete the following equation?
N + ____
C+ H
a.
c.
n
He
b.
e
d.
e
____ 34. To what element does polonium-208 (atomic number 84) decay when it emits an alpha particle?
a.
c.
Pb
Pb
b.
Po
d.
Rn
____ 35. The production of carbon-14 ____.
a. takes place in the upper atmosphere
b. is mostly due to fallout from nuclear explosions
c. occurs to a large extent in nuclear reactors
d. is caused by photosynthesis in plants
____ 36. Which of the following best describes an example of pure chemistry?
a. testing the effects of lower concentrations of a drug on humans
b. studying chemicals containing carbon
c. developing a cure for osteoporosis
d. finding an antidote for a new strain of virus
____ 37. Which of the following statements is false?
a. Knowledge of chemistry allows the public to make informed decisions.
b. Studying chemistry ensures that officials make correct choices in funding technology.
c. Knowledge of chemistry helps prepare people for careers in soil science.
d. Chemistry explains many aspects of nature.
____ 38. Which of the following is NOT an example of chemistry research in the main area of energy?
a.
b.
c.
d.
producing hook-and-loop tape
determining the usefulness of oil from soybean plants
developing rechargeable batteries
studying the effects of insulation
____ 39. Which state of matter expands when heated and is easy to compress?
a. gas
c. solid
b. liquid
d. all of the above
____ 40. Which of the following is a physical change?
a. corrosion
b. explosion
c. evaporation
d. rotting of food
____ 41. Which of the following is a homogeneous mixture?
a. salt water
c. sand and water
b. beef stew
d. soil
____ 42. Which of the following items is NOT a compound?
a. baking soda
c. sucrose
b. salad dressing
d. table salt
____ 43. What is one difference between a mixture and a compound?
a. A compound consists of more than one phase.
b. A compound can only be separated into its components by chemical means.
c. A mixture can only be separated into its components by chemical means.
d. A mixture must be uniform in composition.
____ 44. The chemical formula of a compound does NOT indicate the ____.
a. identity of the elements in the compound
b. how elements are joined in the compound
c. the composition of the compound
d. relative proportions of the elements in the compound
____ 45. All of the following changes to a metal are physical changes EXCEPT ____.
a. bending
c. rusting
b. melting
d. polishing
____ 46. Which of the following is a chemical property of water at 4 C?
a. its color
b. its state
c. its temperature
d. its ability to decompose into hydrogen and oxygen
____ 47. Which of the following does NOT indicate that a chemical change may have taken place?
a. fracture formation
c. precipitate formation
b. gas production
d. energy transfer
____ 48. Which action changes the identity of the substance referenced?
a. melting gold
b. running an electric current through copper
c. corroding iron
d. breaking an ice cube
____ 49. What is the result of adding 2.5
a. 2.9 10
b. 6.0 10
10 and 3.5
10 ?
c. 2.9
d. 6.0
10
10
____ 50. What is the measurement 1042 L rounded off to two significant digits?
a. 1.0 10 L
c. 1050 L
b. 1040 L
d. 1.1 10 L
____ 51. Which of the following mass units is the largest?
a. 1 cg
c. 1 mg
b. 1 dg
d. 1 ng
____ 52. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?
a. 93 C
c. –61 C
b. 34 C
d. –34 C
____ 53. What is the density of an object having a mass of 8.0 g and a volume of 25 cm ?
a. 0.32 g/cm
c. 3.1 g/cm
b. 2.0 g/cm
d. 200 g/cm
____ 54. The comparison of the number of atoms in a copper coin the size of a penny with the number of people on
Earth is made to illustrate which of the following?
a. that atoms are indivisible
b. that atoms are very small
c. that atoms are very large
d. that in a copper penny, there is one atom for every person on Earth
____ 55. The range in size of most atomic radii is approximately ____.
a. 2 to 5 cm
c. 5 10
m to 2
b. 2 to 5 nm
d. 5 10
m to 2
10
10
m
m
____ 56. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
a. Cathode rays are negatively-charged particles.
b. Cathode rays can be deflected by magnets.
c. An electron is 2000 times lighter than a hydrogen atom.
d. Charge-to-mass ratio of electrons was the same, regardless of the gas used.
____ 57. Who conducted experiments to determine the quantity of charge carried by an electron?
a. Rutherford
c. Dalton
b. Millikan
d. Thomson
____ 58. As a consequence of the discovery of the nucleus by Rutherford, 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.
____ 59. The nucleus of an atom is ____.
a. the central core and is composed of protons and neutrons
b. positively charged and has more protons than neutrons
c. negatively charged and has a high density
d. negatively charged and has a low density
____ 60. If E is the symbol for an element, which two of the following symbols represent isotopes of the same
element?
1. E
2. E
3. E
4. E
a. 1 and 2
b. 3 and 4
c. 1 and 4
d. 2 and 3
____ 61. 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.
____ 62. Which of the following statements is NOT true?
a. Protons have a positive charge.
b. Electrons are negatively charged and have a mass of 1 amu.
c. The nucleus of an atom is positively charged.
d. Neutrons are located in the nucleus of an atom.
____ 63. The atomic mass of an element depends upon the ____.
a. mass of each electron in that element
b. mass of each isotope of that element
c. relative abundance of protons in that element
d. mass and relative abundance of each isotope of that element
____ 64. Which of the following is necessary to calculate the atomic mass of an element?
a. the atomic mass of carbon-12
b. the atomic number of the element
c. the relative masses of the element’s protons and neutrons
d. the masses of each isotope of the element
____ 65. How many energy sublevels are in the second principal energy level?
a. 1
c. 3
b. 2
d. 4
____ 66. What is the maximum number of f orbitals in any single energy level in an atom?
a. 1
c. 5
b. 3
d. 7
____ 67. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
c. 3f
b. 3d
d. 4s
____ 68. What is the number of electrons in the outermost energy level of an oxygen atom?
a. 2
c. 6
b. 4
d. 8
____ 69. Which of the following electromagnetic waves have the highest frequencies?
a. ultraviolet light waves
c. microwaves
b. X-rays
d. gamma rays
____ 70. How are the frequency and wavelength of light related?
a. They are inversely proportional to each other.
b. Frequency equals wavelength divided by the speed of light.
c. Wavelength is determined by dividing frequency by the speed of light.
d. They are directly proportional to each other.
____ 71. Which of the following quantum leaps would be associated with the greatest energy of emitted light?
a. n = 5 to n = 1
c. n = 2 to n = 5
b. n = 4 to n = 5
d. n = 5 to n = 4
____ 72. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
____ 73. What causes the shielding effect to remain constant across a period?
a. Electrons are added to the same principal energy level.
b. Electrons are added to different principal energy levels.
c. The charge on the nucleus is constant.
d. The atomic radius increases.
____ 74. Which of the following elements has the smallest ionic radius?
a. Li
c. O
b. K
d. S
____ 75. Which of the following elements has the smallest first ionization energy?
a. sodium
c. potassium
b. calcium
d. magnesium
____ 76. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 77. What is the change in the atomic number when an atom emits an alpha particle?
a. decreases by 2
c. increases by 1
b. decreases by 1
d. increases by 2
____ 78. What is the change in atomic number caused by the emission of gamma radiation?
a. decreases by 2
c. remains the same
b. decreases by 1
d. increases by 1
____ 79. Which symbol is used for an alpha particle?
a.
He
b.
He
c.
He
d.
He
____ 80. Which of the following materials is most effective for stopping gamma radiation?
a. several cm of lead
c. single sheet of aluminum foil
b. one cm of water
d. single sheet of paper
____ 81. How does an atom with too many neutrons relative to protons undergo radioactive decay?
a. by emitting an alpha particle
c. by emitting gamma radiation
b. by emitting a beta particle
d. by emitting X radiation
____ 82. What particle does argon-39 (atomic number 18) emit when it decays to potassium-39 (atomic number 19)?
a. neutron
c. proton
b. electron
d. alpha particle
____ 83. What does neutron absorption accomplish in a nuclear reactor?
a. It slows down the reaction.
b. It speeds up the reaction.
c. It increases the rate of heat absorption.
d. It recycles the fuel.
____ 84. Radioisotopes taken internally for medical reasons ____.
a. must be eliminated from the body slowly
b. should be fissionable isotopes
c. are usually deposited in fat tissue
d. should have a short half-life
____ 85. Which field of science studies the composition and structure of matter?
a. physics
c. chemistry
b. biology
d. geology
____ 86. One characteristic of a scientific theory is that ____.
a. it can never be proved
c. it cannot be modified
b. it can be proved
d. it summarizes a set of observations
____ 87. All of the following are physical properties of matter EXCEPT ____.
a. mass
c. melting point
b. color
d. ability to rust
____ 88. Which state of matter takes both the shape and volume of its container?
a. solid
c. gas
b. liquid
d. both b and c
____ 89. Which of the following is used for chemical symbols today?
a. drawings
c. letters
b. icons
d. numbers
____ 90. When paper turns yellow-brown upon exposure to sunlight, what type of change is likely taking place?
a. a physical change
b. a chemical change
c. neither a physical change nor a chemical change
d. both a physical change and a chemical change
____ 91. 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.
____ 92. Express the product of 2.2 mm and 5.00 mm using the correct number of significant digits.
a. 10 mm
c. 11.0 mm
b. 11 mm
d. 11.00 mm
____ 93. What quantity is represented by the metric system prefix deci-?
a. 1000
c. 0.1
b. 100
d. 0.01
____ 94. Which of the following volumes is the smallest?
a. one microliter
c. one milliliter
b. one liter
d. one deciliter
____ 95. What is the boiling point of water in kelvins?
a. 0 K
b. 100 K
c. 273 K
d. 373 K
____ 96. If a liter of water is heated from 20 C to 50 C, what happens to its volume?
a. The volume decreases.
b. The volume increases.
c. The volume first increases, then decreases.
d. The volume first decreases, then increases.
____ 97. Isotopes of the same element have different ____.
a. numbers of neutrons
c. numbers of electrons
b. numbers of protons
d. atomic numbers
____ 98. Which of the following equals one atomic mass unit?
a. the mass of one electron
b. the mass of one helium-4 atom
c. the mass of one carbon-12 atom
d. one-twelfth the mass of one carbon-12 atom
____ 99. What is another name for the representative elements?
a. Group A elements
c. Group C elements
b. Group B elements
d. transition elements
____ 100. What particle is emitted in alpha radiation?
a. electron
b. photon
c. helium nucleus
d. hydrogen nucleus
Midterm Review
Answer Section
MULTIPLE CHOICE
1. ANS: D
PTS: 1
DIF: L3
REF: p. 50 | p. 51
OBJ: 2.3.2 Distinguish between a substance and a mixture.
STA: 5.6.A.6
2. ANS: C
PTS: 1
DIF: L3
REF: p. 54
OBJ: 2.4.1 Describe what happens during a chemical change. STA: 5.6.A.6
3. ANS: A
PTS: 1
DIF: L3
REF: p. 68
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: 5.3.B.1
4. ANS: C
PTS: 1
DIF: L3
REF: p. 86
OBJ: 3.3.2 Apply the techniques of dimensional analysis to a variety of conversion problems. | 3.3.4
Convert complex units, using dimensional analysis. STA:
5.3.B.1 | 5.3.D.1
5. ANS: D
PTS: 1
DIF: L2
REF: p. 84
OBJ: 3.3.2 Apply the techniques of dimensional analysis to a variety of conversion problems.
STA: 5.3.B.1 | 5.3.D.1
6. ANS: B
PTS: 1
DIF: L1
REF: p. 84
OBJ: 3.3.2 Apply the techniques of dimensional analysis to a variety of conversion problems.
STA: 5.3.B.1 | 5.3.D.1
7. ANS: A
PTS: 1
DIF: L3
REF: p. 106
OBJ: 4.2.1 Identify three types of subatomic particle.
STA: 5.2.B.1
8. ANS: B
PTS: 1
DIF: L3
REF: p. 105 | p. 106
OBJ: 4.2.1 Identify three types of subatomic particle.
STA: 5.2.B.1
9. ANS: C
PTS: 1
DIF: L3
REF: p. 106
OBJ: 4.2.1 Identify three types of subatomic particle.
STA: 5.6.A.1
10. ANS: C
PTS: 1
DIF: L3
REF: p. 112 | p. 113
OBJ: 4.3.1 Explain what makes elements and isotopes different from each other.
11. ANS: B
PTS: 1
DIF: L3
REF: p. 111 | p. 112 | p. 113
OBJ: 4.3.1 Explain what makes elements and isotopes different from each other. | 4.3.2 Calculate the
number of neutrons in an atom.
12. ANS: B
PTS: 1
DIF: L3
REF: p. 111
OBJ: 4.3.2 Calculate the number of neutrons in an atom.
13. ANS: B
PTS: 1
DIF: L3
REF: p. 132
OBJ: 5.1.3 Describe the energies and positions of electrons according to the quantum mechanical model.
STA: 5.6.A.8
14. ANS: C
PTS: 1
DIF: L3
REF: p. 128
OBJ: 5.1.3 Describe the energies and positions of electrons according to the quantum mechanical model.
STA: 5.6.A.8
15. ANS: A
PTS: 1
DIF: L3
REF: p. 134
OBJ: 5.2.1 Describe how to write the electron configuration for an atom.
STA: 5.6.A.3
16. ANS: C
PTS: 1
DIF: L3
REF: p. 133 | p. 134
OBJ: 5.2.1 Describe how to write the electron configuration for an atom.
STA: 5.6.A.3
17. ANS: A
PTS: 1
DIF: L3
REF: p. 133 | p. 134
OBJ: 5.2.1 Describe how to write the electron configuration for an atom.
STA: 5.6.A.3
18. ANS: A
PTS: 1
DIF: L3
REF: p. 133 | p. 134 | p. 135 | p. 136
OBJ: 5.2.2 Explain why the actual electron configurations for some elements differ from those predicted by
the aufbau principle.
STA: 5.6.A.8
19. ANS: C
PTS: 1
DIF: L3
REF: p. 140
OBJ: 5.3.1 Describe the relationship between the wavelength and frequency of light.
20. ANS: D
PTS: 1
DIF: L3
REF: p. 142
OBJ: 5.3.3 Explain how the frequencies of light are related to changes in electron energies.
21. ANS: B
PTS: 1
DIF: L3
REF: p. 143
OBJ: 5.3.3 Explain how the frequencies of light are related to changes in electron energies.
22. ANS: B
PTS: 1
DIF: L3
REF: p. 131
OBJ: 5.1.4 Describe how the shapes of orbitals at different sublevels differ. | 5.3.4 Distinguish between
quantum mechanics and classical mechanics.
STA: 5.6.A.8
23. ANS: D
PTS: 1
DIF: L3
REF: p. 162 | p. 163 | p. 164
OBJ: 6.2.3 Distinguish representative elements and transition metals.
STA: 5.6.A.5
24. ANS: A
PTS: 1
DIF: L3
REF: p. 171
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA: 5.6.A.5
25. ANS: B
PTS: 1
DIF: L3
REF: p. 171 | p. 175
OBJ: 6.3.1 Describe trends among elements for atomic size.
STA: 5.6.A.5
26. ANS: B
PTS: 1
DIF: L3
REF: p. 162 | p. 163 | p. 172
OBJ: 6.3.2 Explain how ions form.
STA: 5.6.A.4
27. ANS: B
PTS: 1
DIF: L3
REF: p. 162 | p. 163 | p. 172
OBJ: 6.3.2 Explain how ions form.
STA: 5.6.A.4
28. ANS: C
PTS: 1
DIF: L3
REF: p. 174
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: 5.6.A.5 | 5.6.A.8
29. ANS: A
PTS: 1
DIF: L3
REF: p. 178
OBJ: 6.2.1 Describe the information in a periodic table. | 6.3.3 Describe periodic trends for first ionization
energy, ionic size, and electronegativity.
STA: 5.6.A.5
30. ANS: C
PTS: 1
DIF: L3
REF: p. 173
OBJ: 6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
STA: 5.6.A.5 | 5.6.A.8
31. ANS: C
PTS: 1
DIF: L3
REF: p. 800
OBJ: 25.1.1 Explain how an unstable nucleus releases energy.
32. ANS: C
PTS: 1
DIF: L3
REF: p. 803 | p. 804
OBJ: 25.2.1 Describe the type of decay a radioisotope undergoes.
33. ANS: A
PTS: 1
DIF: L3
REF: p. 803 | p. 804
OBJ: 25.2.1 Describe the type of decay a radioisotope undergoes.
34. ANS: C
PTS: 1
DIF: L3
REF: p. 800 | p. 804
OBJ: 25.1.2 Describe the three main types of nuclear radiation. | 25.2.1 Describe the type of decay a
radioisotope undergoes.
35. ANS: A
PTS: 1
DIF: L3
REF: p. 806
OBJ: 25.2.3 Identify the two ways transmutations can occur.
36. ANS: B
PTS: 1
DIF: L2
REF: p. 9
OBJ: 1.1.2 Relate pure chemistry to applied chemistry.
STA: 5.6.A.7
37. ANS: B
PTS: 1
DIF: L2
REF: p. 10 | p. 11
OBJ: 1.1.3 Identify reasons to study chemistry.
38. ANS: A
PTS: 1
DIF: L2
REF: p. 12 | p. 13
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
OBJ: 1.2.1 Identify some areas affected by chemistry research.
STA: 5.2.B.2
ANS: A
PTS: 1
DIF: L2
REF: p. 42
OBJ: 2.1.3 Differentiate among the three states of matter.
STA: 5.6.A.7
ANS: C
PTS: 1
DIF: L2
REF: p. 42
OBJ: 2.1.4 Describe a physical change. STA: 5.6.A.6
ANS: A
PTS: 1
DIF: L2
REF: p. 45
OBJ: 2.2.2 Distinguish between homogeneous and heterogeneous samples of matter.
STA: 5.6.A.6
ANS: B
PTS: 1
DIF: L2
REF: p. 50
OBJ: 2.3.1 Explain the difference between an element and a compound.
STA: 5.6.A.6
ANS: B
PTS: 1
DIF: L2
REF: p. 50
OBJ: 2.3.2 Distinguish between a substance and a mixture.
STA: 5.6.A.6
ANS: B
PTS: 1
DIF: L2
REF: p. 52
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given their
symbols.
ANS: C
PTS: 1
DIF: L2
REF: p. 53
OBJ: 2.4.1 Describe what happens during a chemical change. STA: 5.6.A.6
ANS: D
PTS: 1
DIF: L2
REF: p. 53
OBJ: 2.4.1 Describe what happens during a chemical change. STA: 5.6.A.7
ANS: A
PTS: 1
DIF: L2
REF: p. 54
OBJ: 2.1.4 Describe a physical change. | 2.4.2 Identify four possible clues that a chemical change has taken
place. STA:
5.6.A.6
ANS: C
PTS: 1
DIF: L2
REF: p. 53
OBJ: 2.1.4 Describe a physical change. | 2.4.1 Describe what happens during a chemical change.
STA: 5.6.A.6
ANS: A
PTS: 1
DIF: L2
REF: p. 63 | p. 71
OBJ: 3.1.1 Convert measurements to scientific notation.
STA: 5.3.B.1
ANS: A
PTS: 1
DIF: L2
REF: p. 66 | p. 68
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: 5.3.B.1
ANS: B
PTS: 1
DIF: L2
REF: p. 74 | p. 76
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: 5.3.B.1
ANS: D
PTS: 1
DIF: L2
REF: p. 77 | p. 78
OBJ: 3.2.3 Convert between the Celsius and Kelvin temperature scales.
STA: 5.3.B.1
ANS: A
PTS: 1
DIF: L2
REF: p. 90 | p. 91
OBJ: 3.4.1 Calculate the density of a material from experimental data.
ANS: B
PTS: 1
DIF: L2
REF: p. 103
OBJ: 4.1.3 Identify the special instruments necessary to observe individual atoms.
STA: 5.6.A.1
ANS: C
PTS: 1
DIF: L2
REF: p. 103
OBJ: 4.1.3 Identify the special instruments necessary to observe individual atoms.
STA: 5.6.A.1
ANS: D
PTS: 1
DIF: L2
REF: p. 105
OBJ: 4.2.1 Identify three types of subatomic particle.
STA: 5.2.B.1
ANS: B
PTS: 1
DIF: L2
REF: p. 105
OBJ:
58. ANS:
OBJ:
STA:
59. ANS:
OBJ:
STA:
60. ANS:
OBJ:
61. ANS:
OBJ:
62. ANS:
OBJ:
63. ANS:
OBJ:
64. ANS:
OBJ:
65. ANS:
OBJ:
STA:
66. ANS:
OBJ:
STA:
67. ANS:
OBJ:
STA:
68. ANS:
OBJ:
STA:
69. ANS:
OBJ:
70. ANS:
OBJ:
71. ANS:
OBJ:
72. ANS:
OBJ:
73. ANS:
OBJ:
74. ANS:
OBJ:
STA:
75. ANS:
OBJ:
STA:
76. ANS:
OBJ:
STA:
77. ANS:
4.2.1 Identify three types of subatomic particle.
STA: 5.2.B.1
C
PTS: 1
DIF: L2
REF: p. 108
4.2.2 Describe the structure of atoms according to the Rutherford model.
5.2.B.1
A
PTS: 1
DIF: L2
REF: p. 107 | p. 108
4.2.2 Describe the structure of atoms according to the Rutherford model.
5.6.A.1
C
PTS: 1
DIF: L2
REF: p. 112
4.3.1 Explain what makes elements and isotopes different from each other.
C
PTS: 1
DIF: L2
REF: p. 111
4.3.2 Calculate the number of neutrons in an atom.
STA: 5.6.A.1
B
PTS: 1
DIF: L2
REF: p. 114
4.3.3 Calculate the atomic mass of an element.
D
PTS: 1
DIF: L2
REF: p. 115
4.3.3 Calculate the atomic mass of an element.
D
PTS: 1
DIF: L2
REF: p. 116
4.3.3 Calculate the atomic mass of an element.
B
PTS: 1
DIF: L2
REF: p. 131
5.1.3 Describe the energies and positions of electrons according to the quantum mechanical model.
5.6.A.8
D
PTS: 1
DIF: L2
REF: p. 131 | p. 132
5.1.3 Describe the energies and positions of electrons according to the quantum mechanical model.
5.6.A.8
D
PTS: 1
DIF: L2
REF: p. 133
5.2.1 Describe how to write the electron configuration for an atom.
5.6.A.8
C
PTS: 1
DIF: L2
REF: p. 134 | p. 135
5.2.1 Describe how to write the electron configuration for an atom.
5.6.A.3
D
PTS: 1
DIF: L2
REF: p. 139
5.3.1 Describe the relationship between the wavelength and frequency of light.
A
PTS: 1
DIF: L2
REF: p. 139
5.3.1 Describe the relationship between the wavelength and frequency of light.
A
PTS: 1
DIF: L2
REF: p. 143
5.3.3 Explain how the frequencies of light are related to changes in electron energies.
A
PTS: 1
DIF: L2
REF: p. 157
6.2.1 Describe the information in a periodic table.
STA: 5.6.A.1
A
PTS: 1
DIF: L2
REF: p. 171
6.3.1 Describe trends among elements for atomic size.
STA: 5.6.A.5
A
PTS: 1
DIF: L2
REF: p. 175
6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
5.6.A.4 | 5.6.A.5
C
PTS: 1
DIF: L2
REF: p. 173
6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
5.6.A.5 | 5.6.A.8
A
PTS: 1
DIF: L2
REF: p. 172 | p. 176
6.3.3 Describe periodic trends for first ionization energy, ionic size, and electronegativity.
5.6.A.5
A
PTS: 1
DIF: L2
REF: p. 800
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
OBJ: 25.1.1 Explain how an unstable nucleus releases energy. | 25.1.2 Describe the three main types of
nuclear radiation.
ANS: C
PTS: 1
DIF: L2
REF: p. 802
OBJ: 25.1.2 Describe the three main types of nuclear radiation.
ANS: D
PTS: 1
DIF: L2
REF: p. 800
OBJ: 25.1.2 Describe the three main types of nuclear radiation.
ANS: A
PTS: 1
DIF: L2
REF: p. 802
OBJ: 25.1.2 Describe the three main types of nuclear radiation.
ANS: B
PTS: 1
DIF: L2
REF: p. 804
OBJ: 25.2.1 Describe the type of decay a radioisotope undergoes.
ANS: B
PTS: 1
DIF: L2
REF: p. 801
OBJ: 25.2.1 Describe the type of decay a radioisotope undergoes.
ANS: A
PTS: 1
DIF: L2
REF: p. 811
OBJ: 25.3.3 Distinguish fission reactions from fusion reactions.
ANS: D
PTS: 1
DIF: L2
REF: p. 805
OBJ: 25.4.2 Describe how radioisotopes are used in medicine.
ANS: C
PTS: 1
DIF: L1
REF: p. 7
OBJ: 1.1.1 Identify five traditional areas of study in chemistry.
STA: 5.6.A
ANS: A
PTS: 1
DIF: L1
REF: p. 23
OBJ: 1.3.2 Identify three steps in the scientific method.
STA: 5.1.B.2
ANS: D
PTS: 1
DIF: L1
REF: p. 40
OBJ: 2.1.2 Define physical property and list several common physical properties of substances.
STA: 5.6.A.7
ANS: C
PTS: 1
DIF: L1
REF: p. 42
OBJ: 2.1.3 Differentiate among the three states of matter.
STA: 5.6.A.7
ANS: C
PTS: 1
DIF: L1
REF: p. 51
OBJ: 2.3.3 Identify the chemical symbols of common elements, and name common elements, given their
symbols.
ANS: B
PTS: 1
DIF: L1
REF: p. 54
OBJ: 2.4.2 Identify four possible clues that a chemical change has taken place.
STA: 5.6.A.6
ANS: A
PTS: 1
DIF: L1
REF: p. 55
OBJ: 2.4.3 Apply the law of conservation of mass to chemical reactions.
STA: 5.6.B.1
ANS: B
PTS: 1
DIF: L1
REF: p. 68 | p. 71
OBJ: 3.1.3 Identify the number of significant figures in a measurement and in a calculated answer.
STA: 5.3.B.1
ANS: C
PTS: 1
DIF: L1
REF: p. 74
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: 5.3.B.1
ANS: A
PTS: 1
DIF: L1
REF: p. 74 | p. 75
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: 5.3.B.1
ANS: D
PTS: 1
DIF: L1
REF: p. 77
OBJ: 3.2.1 List SI units of measurement and common SI prefixes.
STA: 5.3.B.1
ANS: B
PTS: 1
DIF: L1
REF: p. 91
OBJ: 3.4.2 Describe how density varies with temperature.
97. ANS:
OBJ:
98. ANS:
OBJ:
99. ANS:
OBJ:
STA:
100. ANS:
OBJ:
A
PTS: 1
DIF: L1
REF: p. 112 | p. 113
4.3.1 Explain what makes elements and isotopes different from each other.
D
PTS: 1
DIF: L1
REF: p. 114
4.3.3 Calculate the atomic mass of an element.
A
PTS: 1
DIF: L1
REF: p. 164
6.1.1 Explain how elements are organized in a periodic table.
5.6.A.5
C
PTS: 1
DIF: L1
REF: p. 800
25.1.2 Describe the three main types of nuclear radiation.