Download File

Name ___________________________________________ Date ____________ Period ______
BENCHMARK TEST – POWER STANDARDS
1a. Students know how to relate the position of an element in the periodic table to its atomic number and
atomic mass
1. What is the charge of a proton?
A. Positive (+)
B. Negative (-)
C. Neutral (0)
D. Undefined
2. What is the charge of a neutron?
A. Positive (+)
B. Negative (-)
C. Neutral (0)
D. Undefined
3. Where are electrons located in an atom?
A. In the nucleus
B. orbiting the nucleus
C. attached to the protons
D. negative
4. Which particles always have the same quantity in a neutral atom?
A. Protons and neutrons
B. Protons and electrons
C. Electrons and neutrons
D. Electrons and orbitals
5. What does the atomic number tell you about an element?
A. The number of neutrons in the atom
B. The number of protons in the atom
C. The number of protons plus the number of neutrons
D. The mass of the atom
6. How many protons are in an atom of Boron, B?
A. 5
B. 6
C. 10
D. 11
7. Which of the following ordered pairs of elements shows an increase in atomic number, but a
decrease in average atomic mass?
A. Ag to Pd
B. Co to Ni
C. Ge to Sn
D. Cr to Mo
8. Why is the atomic mass of an element on the periodic table a decimal?
A. It is an average of the number of neutrons in the atoms of an element.
B. It is an average of the masses of the naturally occurring isotopes.
C. It is an average of the atomic numbers of the naturally occurring isotopes.
D. None of the above.
9. Which element has the greatest atomic number?
A. Ni - Nickle
B. Cd - Cadmium
C. Hg – Mercury
D. Fr – Francium
1b. Students know how to use the periodic table to identify metals, semimetals, nonmetals, and halogens
For #10-12 classify each element as a
10. K
11. Cl
12. H
A) metal B) nonmetal C) Metalloid
1c. Students know how to use the periodic table to identify alkali metals, alkaline earth metals, transition
metals, trends in ionization energy, electronegativity, and the relative sizes of ions and atoms
13. Name the family that is in group 18 or 8A on the periodic table.
A. Halogen
B. Alkali Metals
C. Noble Gases
D. Transition Metals
Use the letters on the periodic table to label 14-17:
14. Alkali metals
15. Halogens
16. Alkaline earth metals
17. Transition metals
E
B
D
C
A
Use the following for 23-29:
A. Increases
B. Decreases
C. Stays the same
In general, as you go from LEFT to RIGHT across the periodic table…
18. atomic radius
19. electronegativity
20. ionization energy
In general, as you go from TOP to BOTTOM down the periodic table…
21. electronegativity
22. the number of valence electrons
23. ionization energy
24. atomic radius
25. What is ionization energy?
A. The ability of an atom to attract bonded electrons to itself
B. A measure of the size of an atom
C. The energy required to remove an electron from a neutral atom
D. The energy released when an atom loses or gains electrons
26. Which of the following elements has the highest ionization energy?
A. Cl
B. Al
C. Fe
D. Ba
27.
The chart above shows the relationship
between the first ionization energy and the increase
in atomic number. The letter on the chart for the
alkali family of elements is
A. W
B. X
C. Y
D. Z
28. Put the following in order of increasing (smallest to largest) atomic size: O, S, Po, Te
A. O, Po, S, Te
B. Po, Te, S, O
C. O, S, Te, Po
D. O, S, Po, Te
29. Which of the following is an alkali metal with the largest atomic radius?
A. Na
B. Ba
C. Mg
D. Cs
30. What is electronegativity?
A. A measure of the ability of an atom to attract bonded electrons towards itself
B. A partial negative charge
C. A polar molecule
D. The energy required to remove one electron from a neutral atom.
31. Which of the following elements is most electronegative?
A. Potassium (K)
B. Calcium (Ca)
C. Chlorine (Cl)
D. Aluminum (Al)
1d. Students know how to use the periodic table to determine the number of electrons available for bonding.
32. How many valence electrons are in a neutral atom of Chlorine?
A. 17
B. 7
C. 10
D. 35
33. Which of the following atoms has six valence electrons?
A. Magnesium (Mg)
B. silicon (Si)
C. sulfur (S)
D. argon (Ar)
1e. Students know the nucleus of the atom is much smaller than the atom yet contains most of the mass.
34. Which statement best describes the density of an atom’s nucleus?
A. The nucleus occupies most of the atom’s volume but contains little of its mass.
B. The nucleus occupies very little of the atom’s volume and contains little of its mass.
C. The nucleus occupies most of the atom’s volume and contains most of its mass.
D. The nucleus occupies very little of the atom’s volume but contains most of its mass.
35. If a tiny particle is shot into the middle of an atom, it hits something in the center and
bounces back. If the particle is shot into the edges of the atom, it goes through. This
discovery led to a model of the atom with
A. electrons
B. a neutral charge
C. a nucleus
D. electron orbital shells
36. Use the table below to answer the question:
Results of Firing Alpha Particles at Gold Foil
Observations
Alpha Particles went straight through gold foil
Alpha particles went through gold foil but were
deflected at large angles
Alpha particles bounced off gold foil
Proportion
> 98%
= 2%
=0.01 %
What information do the experimental results above reveal about the nucleus of the gold
atom?
A.
B.
C.
D.
The nucleus contains less than half the mass of the atom.
The nucleus is small and is the densest part of the atom.
The nucleus contains small positive and negative particles.
The nucleus is large and occupies most of the atom’s space.
2a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds
or by exchanging electrons to form ionic bonds
37. Why don’t noble gases lose or gain electrons?
A. They are unstable
B. They have 10 electrons in their outer shell
C. They have a full valence shell
D. None of the above
38. Iodine would have chemical properties most like:
A. manganese (Mn)
B. tellurium (Te)
C. Chlorine (Cl)
D. Xenon (Xe)
39. Fluorine gains one electron and becomes a Fluorine ion with a negative charge. Why
doesn’t it become a Neon atom?
A. The neutrons did not change, and the neutrons determine the identity of an atom.
B. The number of protons did not change, and the protons determine the identity of an
atom.
C. Electrons cannot be lost or gained.
D. None of the above
40. Which of the following is a monatomic gas?
A. Chlorine
B. Fluorine
C. Helium
D. Nitrogen
41. Which of the following is a diatomic gas?
A. Argon
B. Chlorine
C. Boron
D. Helium
42. What is an ion?
A. a neutral atom
B. an atom that has gained or lost neutrons and therefore has an overall charge
C. atoms of the same element that have different numbers of neutrons
D. an atom that has gained or lost electrons and therefore has an overall charge
43. Which of the following is a cation?
A) K+
B) BrC) H2
D) Li
For # 63-65: A. ionic bond B. covalent bond
C. metallic bond
44. involves sharing electrons
45. bendable solids
46. conducts electricity when dissolved in water
47. What type of bond will form between two atoms with very different electronegativities?
A. Ionic
B. Polar covalent
C. Nonpolar covalent
D. Metallic
2e. Students know how to draw Lewis dot structures
48. Which of the following is the correct dot symbol for Phosphorus
A)
B)
C)
D)
49. Which of the following elements has the same dot symbol as silicon?
A. germanium (Ge)
B. aluminum (Al)
C. arsenic (As)
D. gallium (Ga)
50. Which of the following is the correct Lewis Dot Structure for NH3?
A)
B)
A.
C)
A.
D)
A.
H N H
H
H N H
H
H N H
H
H N H
H
3a. Students know how to describe chemical reactions by writing balanced equations
(For 70-72) When zinc is added to hydrochloric acid, the following reaction occurs:
Zn(s) +
HCl(aq) 
ZnCl2(aq) +
H2(g)
51. In the equation above the reactants are
A. ZnCl2 and H2
B. ZnCl2
C. Zn and HCl
D. on the right
52. The abbreviation (aq) means
A. gas
B. dissolved in water
C. aquafina
D. liquid
53. The total mass of the reactants before the chemical reactants is 50g. What will the mass of the
products be?
A. 50g
B. Slightly less than 50g.
C. More than 50g
D. None of the above
54. The correct balanced equation for
A. 2N2 + H2  2NH3
B. N2 + H2  2NH3
C. N2 + 3H2  2NH3
D. 2N2 + 2H2  2NH3
55.
N2 + H2  NH3
C3H8 +
O2 
CO2 + ? H2O
This chemical equation represents the combustion of propane. When correctly balanced, the
coefficient for water is
A. 2
B. 4
C. 8
D. 16
56. Which of the following is a balanced equation for the combustion of ethanol (CH3CH2OH)?
A. CH3CH2OH + 3O2  CO2 + 2H2O
B. CH3CH2OH + 3O2  2CO2 + 3H2O
C. CH3CH2OH + O2  2CO2 + 3H2O
D. CH3CH2OH + 2O2  3CO2 + 2H2O
57. Which of the following is NOT part of the Law of Conservation of Matter?
A. Matter cannot be created or destroyed.
B. Atoms cannot come in and out of existence.
C. Mass can increase during a chemical reaction.
D. Mass does not change during a chemical reaction.
3c. Students know one mole equals 6.02 x 1023particles (atoms or molecules)
58. How many particles are in a mole?
A. 62
B. 6.02 x 102
C. 1.204 x 1023
D. 6.02 x 1023
59. How many atoms are in one mole of Lithium?
A. 1 million
B. 6.02 x 1023
C. 1.204 x 1024
D. 6.94
3d. Students know how to determine the molar mass of a molecule from its molecular substance to moles,
number of particles, or volume of a gas at standard temperature and pressure.
60. What is molar mass?
A. The number of particles in 12 grams of carbon-12
B. 6.02 x 1023 particles
C. The mass of an element
D. The mass of one mole of a substance
61. What is the molar mass of CO2?
A. 22 g/mol
B. 44 g/mol
C. 18 g/mol
D. 40 g/mol
62. What is the mass of 3 moles of Helium, He?
A. 2 g
B. 8 g
C. 12 g
D. 1.204 x 1024 g
63. How many moles of CH4 are contained in 96.0 grams of CH4?
A. 3.00 moles
B. 6.00 moles
C. 12.0 moles
D. 16.0 moles
64. How many atoms are contained in 80 grams of NaOH?
A. 5.16 x 1030
B. 3.01 x 1023
C. 1.20 x 1024
D. 6.02 x 1023
4c. Students know how to apply the gas laws to relations between the pressure, temperature, and volume of
any amount of an ideal gas or any mixture of ideal gases.
65. The volume of 400 mL of chlorine gas at 400mmHg is decreased to 200mL at constant temperature.
What is the new gas pressure?
A. 400 mmHg
B. 300 mmHg
C. 800 mmHg
D. 650 mmHg
66. If a sealed bag of chips is left in a hot car, what happens to the volume of bag?
A. volume increases
B. volume decreases
C. volume stays the same
D. cannot be determined
67. A balloon has a volume of 9 L at 27°C. What will the volume of the balloon be if the temperature
decreases to -73°C?
A. 4.5 L
B. 6 L
C. 18 L
D. 3 L
(For 68-69) A beach ball has a volume of 2 L at sea level where the pressure is 1.0 atm. You take the
ball to the top of a mountain where pressure is 0.8 atm.
68. What happens to the volume of the ball?
A. volume increases
B. volume decreases
C. volume stays the same
D. cannot be determined
69. Calculate the new volume of the balloon
A. 1.6 L
B. 1 L
C. 2.5 L
D. 2.5 atm.
70. What happens to the pressure of the air inside a flask when the flask is heated?
A. pressure increases
B. pressure decreases
C. pressure stays the same
D. pressure decreases and then increases
5a. Students know the observable properties of acids, bases, and salt solutions
Use the following for 17-19:
A = Acid
B = Base
C = Neutral
71. A solution has a pH of 6.7
72. Bleach has a pH of 12.6
73. A mixture of two substances has a pH of 7
74. The picture to the right shows a light bulb connected to a battery with
the circuit interrupted by a solution. When dissolved in the water to
form a 1 molar solution, all of the following substances will complete a
circuit allowing the bulb to light except
A. Hydrochloric acid
B. Sodium nitrate
C. Sucrose
D. Ammonium sulfate
75. Which of the following is an observable property of many acids?
A. They become slippery when reacting with water
B. They react with metals to release hydrogen gas
C. The produce salts when mixed with other acids
D. They become more acidic when mixed with a base
Use the following for 17-22:A = Acid
B = Base
C = Neutral D = Acid and Base
76. Burns to the touch
77. Turns litmus paper red
78. Pure water
79. Turns litmus paper blue
80. Has a bitter taste
81. Can conduct electricity when dissolved in water
82. You put something in your mouth and it tastes sour. It is most likely a(an)…
A. egg
B. base
C. soap
D. acid
5d. Students know how to use the pH scale to characterize acid and base solutions
83. Of the four different laboratory solutions, the solution with the highest acidity has a pH of
A. 11
B. 7
C. 5
D. 3
84. Stomach acid has a pH of 2 and apple juice has a pH of 3. Which statement is true?
A. Stomach acid is 100 times more acidic than apple juice
B. Apple juice is twice as acidic as stomach acid
C. Stomach acid is 10 times more acidic than apple juice
D. Apple juice is 10 times more acidic than stomach acid
85. The diagram above shows a pH scale with four regions identified. A chemist measures the pH of a
solution that is strongly acidic. Which region of the pH scale gives the approximate pH of the
chemist’s solution?
A. Region 1
B. Region 2
C. Region 3
D. Region 4
6a. Students know the definitions of solute and solvent.
86. What is a solution?
A. a mixture that is uniform throughout
B. the substance that is being dissolved
C. the substance present in the greatest amount
D. a heterogeneous mixture
87. When a sugar cube dissolves in a beaker of water, water is the ___________.
A. solute
B. solvent
C. solution
D. concentration
88. If a gummy bear dissolves in a cup of water, which substance is the solute?
A. gummy bear
B. water
C. salt
D. none of the above
89. Which of the substances in the table
can act as either the solute or the
solvent when mixed with 100 grams of
water at 20ºC? (Std 6A)
A. NH3
B. C6H5COOH
C. MgCl2
D. CH3CH2OH
7d. Students know how to solve problems involving heat flow and temperature changes, using known values
of specific heat and latent heat of phase change.
90. The specific heat of copper is about 0.4 joules/gram ºC. How much heat is needed to change the
temperature of a 30 gram sample of copper from 20 ºC to 60 ºC? (Std 7D)
A. 1000 J
B. 720 J
C. 480 J
D. 240 J
Use the diagram below for 46-50:
F
D
E
B
C
A
91. What phase change occurs as you move from D to E on the diagram above?
A. melting
B. freezing
C. evaporation
D. condensation
92. What phase change occurs as you move from C to B on the diagram above?
A. melting
B. freezing
C. evaporation
D. condensation
93. During which phase changes is energy absorbed?
A. melting
B. freezing
C. both A and B
D. neither A nor B
94. During which phase changes is energy released?
A. condensation
B. freezing
C. both A and B
D. neither A nor B
95. What happens during a phase change?
A. Energy is added and temperature increases
B. Energy is taken away and temperature decreases
C. Energy is added or removed and temperature stays the same
D. None of the above
96. What is specific heat?
A. a measure of kinetic energy
B. the energy of motion
C. how much space something takes up
D. the amount of energy required to raise the temperature of a substance
97. Which requires the most energy to raise the temperature by 1°C
A. gold (c = 0.13 J/g°C)
B. silver (c = 0.24 J/g°C)
C. copper (c = 0.39 J/g°C)
D. iron (c = 0.45 J/g°C)
(58-60) You are making pasta and need to bring a pot of water to a boil. If you start with 1000 grams
of water at room temperature (25°C) and need to boil it at 100°C, how much heat do you need? The
specific heat of water is about 4.2 J/g°C.
98. What values are you given in the problem?
A. m=1000g; ∆T=100°C; c= 4.2J/g°C
B. m=1000g; ∆T=75°C; Q= 4.2J/g°C
C. m=1000g; ∆T=75°C; c=4.2J/g°C
D. m=1000g; ∆T=25°C; Q=4.2J
99. What is your unknown?
A. mass
B. specific heat
C. change in temperature
D. heat
100.
A.
B.
C.
D.
How much heat do you need to bring the water to a boil?
4.2 J
17,857 J
315,000 J
315,000 J/g°C
8c. Students know the role a catalyst plays in increasing the reaction rate.
101. Which reaction diagram shows the effect of using the appropriate catalyst in a chemical
reaction?
102.
A.
B.
C.
D.
What is activation energy?
the energy released from a chemical reaction
the random motion of molecule
a measure of the kinetic energy of particles in a substance
the energy required for a reaction to occur
103. H2O2, hydrogen peroxide, naturally breaks down into H2O and O2 over time. MnO2, manganese
dioxide, can be used to lower the energy of activation needed for this reaction to take place and,
thus, increase the rate of reaction. What type of substance is MnO2? (Std 8c)
A. A catalyst
B. An enhancer
C. An inhibitor
D. A reactant
104.
A.
B.
C.
D.
Which of the following is NOT a characteristic of a catalyst?
increases the rate of a reaction
is chemically unchanged at the end of the reaction
decreases the chances of reactants colliding
is a protein
105.
A.
B.
C.
D.
How does a catalyst change the speed of a reaction?
A catalyst forces the molecules to collide
A catalyst lowers the activation energy of a reaction
A catalyst raises the activation energy of a reaction
A catalyst gives the particles in a reaction more energy
9a. Students know how to use Le Chatelier's principle to predict the effect of changes in concentration,
temperature, and pressure.
106. Which of the following is true of a reaction at equilibrium:
A. the forward and reverse reaction occur at the same rate
B. the concentration of products stays the same
C. the concentration of the reactants stays the same
D. all of the above
107. When a reaction is at equilibrium and more reactant is added, which of the following changes is
the immediate result? (Std 9A)
A. The reverse reaction rate remains the same.
B. The forward reaction rate increases
C. The reverse reaction rate decreases
D. The forward reaction rate remains the same.
108. In which of the following reactions involving gases would the forward reaction be favored by an
increase in pressure? (Std 9A)
 AB
A. A + B 
 C + D
B. A + B 
 C + 2D
C. 2A + B 
 A + C
D. AC 
109.
 2H2 + 2Cl2(g) + 113 kJ
4HCl(g) + O2(g) 
Which action will drive the reaction to the right? (Std 9A)
A. Heating the equilibrium mixture
B. Adding water to the system
C. Decreasing the oxygen concentration
D. Increasing the system’s pressure
110.
 NO(g) + CO2(g)
NO2(g) + CO(g) 
The reaction shown above occurs inside a closed flask. What action will shift the reaction to the
left? (Std 9A)
A. Pumping CO gas into the closed flask
B. Raising the total pressure inside the flask
C. Increasing the NO concentration in the flask
D. Venting some CO2 gas from the flask
111. In a sealed bottle that is half full of water, equilibrium will be attained when water molecules
A. Cease to evaporate
B. Begin to condense
C. Are equal in number for both the liquid and the gas phase
D. Evaporate and condense at equal rates
112. At equilibrium:
A. The rate of the forward reaction is greater than the rate of the reverse reaction
B. There is the same amount of reactant as there is product
C. The concentration of reactant doesn’t change
D. The reaction stops
113. Le Chatelier’s Principle states
A. If a system in equilibrium is stressed or disturbed the system will respond to relieve the stress
until a new equilibrium is reached.
B. At equilibrium, the rate of the forward and reverse reaction is the same.
C. The rate of formation of products is the same as the rate of decomposition of the reactants
D. Matter is neither created nor destroyed during a chemical reaction.
(74-76) The reaction of propane with oxygen is: C3H8 + 5O2 ⇄ 3CO2 +4H2O + 2043 kJ
114. Which direction will the reaction shift if the concentration of C3H8 increases?
A. towards the products (right)
B. towards the reactants (left)
C. no change
D. cannot be determined
115.
A.
B.
C.
D.
Which direction will the reaction shift if CO2 is removed from the system?
towards the products (right)
towards the reactants (left)
no change
cannot be determined
116.
A.
B.
C.
Which of the following would cause the reaction to shift towards the products?
Adding O2
Removing O2
Increasing temperature
D. Increasing pressure
10b. Students know the bonding characteristics of carbon that result in the formation of a large variety of
structures ranging from simple hydrocarbons to complex polymers and biological molecules.
117.
A.
B.
C.
D.
118.
A.
B.
C.
What element is involved in all organic compounds?
Carbon
Oxygen
Nitrogen
Gold
Carbon bonds _______ times giving the element unique bonding capabilities.
8
10
4
D. 2
11b. Students know the energy release per gram of material is much larger in nuclear fusion or fission
reactions than in chemical reactions. The change in mass (calculated by E = mc 2 ) is small but significant in
nuclear reactions.
119. During a nuclear reaction a large amount of energy can be released from a very small
amount of matter. The equations used to describe this relationship is
A. E=mc2
B. y=mx + b
C. q=mcT
D. F=ma
11c. Students know some naturally occurring isotopes of elements are radioactive, as are isotopes formed in
nuclear reactions.
120.
What are isotopes?
A. atoms of the same element
B. atoms that have the same number of electrons
C. atoms of the same element that have different numbers of neutrons
D. atoms that have the same number of neutrons
(For 38-41) Find the following for a neutral atom of Aluminum-27:
121. mass number
A) 13
B) 27
C) 14
D) 26.98
122. number of protons
A) 13
B) 27
C) 14
D) 26.98
123. number of neutrons
A) 13
B) 27
C) 14
D) 26.98
124. number of electrons
A) 13
B) 27
C) 14
D) 26.98
125. Which of the following is an isotope of Boron-10?
A. Helium
B. Neon
C. B3+
D. Boron-11
126.
Which of the following describes what happens to radioactive isotopes?
A. Stable nuclei break apart over time to form new elements
B. Unstable nuclei break apart over time to form new elements
C. Unstable elements join together
D. Stable nuclei join together