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CHEMISTRY I
FINAL ASSESSMENT
Indicate the letter of the best answer on your answer sheet.
Objective 1.01: Design, conduct and analyze investigations to answer questions related to chemistry.
Objective 1.02: Evaluate reports of scientific investigations from an informed scientifically-literate viewpoint.
Objective 1.03: Evaluate experimental designs with regard to safety.
1. Which of the following is a qualitative measurement?
a. 27.0g
b. 312 m
c. blue
d. 523 ml
2. In the chemistry lab, chemicals that you are finished working with should be —
a. poured into the sink
b. returned to their original containers
c. mixed together and dumped in a designated container
d. disposed of as directed by your teacher
3. For an experiment in which you are determining the freezing point of an unknown chemical, you record
the temperature every minute for 20 minutes. In this example, time is the —
a. control
b. dependent variable
c. independent variable
d. hypothesis
Objective 2.01: Analyze the historical development of the current atomic theory.
4. Which sequence represents a correct order of historical developments leading to the modern model of the atom?
a. The atom is a hard sphereelectrons exist in orbitals outside the nucleusmost of the atom is
empty space with a small dense nucleus.
b. The atom is a hard spheremost of the atom is empty space with a small dense
nucleuselectrons exist in orbitals outside the nucleus
c. Most of the atom is empty space with a small, dense nucleuselectrons exist in orbitals outside
the nucleusthe atom is a hard sphere.
d. Most of the atom is empty space with a small dense nucleusthe atom is a hard
sphereelectrons exist in orbitals outside the nucleus.
5. The diagram below shows the results of Rutherford’s experiment in which he used a radioactive source to
“shoot” alpha particles at a thin sheet of gold foil. Based on these results, what were Rutherford’s conclusions?
a.
b.
c.
d.
Atoms
Atoms
Atoms
Atoms
are solid matter with positive and negative charges scattered throughout.
are solid, positively charged matter with negatively charged electrons scattered throughout.
are mostly empty space with small, dense, negatively charged centers.
are mostly empty space with small, dense, positively charged centers.
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6. The arrangement of electrons in an atom of an element determines the chemical properties of that
element. Our present-day understanding of how electrons are arranged in an atom is the result of which
of these scientific models —
a. Rutherford’s model based on the gold foil experiment that proved the existence of the nucleus.
b. Dalton’s model that was based on the law of definite composition.
c. The quantum (wave) mechanical model which explains the most probable location of the electron in the
electron cloud.
d. Thompson’s model based on his discovery of the electron using the cathode ray tube.
Objective 2.02:
Examine the nature of atomic structure including subatomic particle, mass number, atomic number and isotopes.
7. Which statement correctly describes the charge of the nucleus and the charge of the electron
cloud of an atom?
a. The nucleus is positive and the electron cloud is positive.
b. The nucleus is positive and the electron cloud is negative.
c. The nucleus is negative and the electron cloud is positive.
d. The nucleus is negative and the electron cloud is negative.
Use the chart on the right to answer question 8.
8. The chart shows isotopes of some common elements. In what
two properties do the isotopes of oxygen differ?
a. Number of protons and number of neutrons
b. Atomic mass and number of protons
c. Atomic number and number of neutrons
d. Atomic mass and number of neutrons
9. An ion with 20 protons, 20 neutrons, and 18 electrons
is represented by
a. Ne
b. Ca+2
c. Ca-2
d. Ca
Objective 2.03: Apply the language and symbols of chemistry.
You may need to use your reference tables to answer these questions.
10. What is the formula for a compound formed from sodium ions (Na1+) and oxygen ions (O2–)?
a. NaO
b. Na2O
c. NaO2
d. Na4O2
11. What is the Stock system name for CuO?
a. Copper (I) oxide
b. Copper (II) oxide
c. Copper (III) oxide
12. What is the correct name for the compound HNO2?
a. Hydronitric acid
b. Nitric acid
c. Nitrous acid
d. Hyponitrous acid
13. What is the formula for sulfuric acid?
a. H2S
b. H2SO4
c. H2SO3
d. H3N
2
d. copper oxide
14. The table shows some of the prefixes used to name binary covalent compounds. What name would be
given to the compound P2Br10?
a. Phosphorus tetrabromide
b. Monophosphorus pentabromide
c. Diphosphorus decabromide
d. Phosphorus hexabromide
15. Sodium Citrate has a formula of Na3C6H5O7. What would be the formula for magnesium citrate?
a. Mg (C6H5O7)2
b. MgC6H5O7
c. Mg3(C6H5O7)2
d. Mg3 C6H5O7
Objective 2.04: Identify substances using their physical properties.
You may need to use your reference tables to answer these questions.
Use the graph on the right to answer questions 16-17
16. According to these data, what is the approximate
number of grams of sodium nitrate that can be
dissolved in 100ml of water at a temperature of 50ºC?
a. 95 g
b. 105 g
c. 115 g
d. 125 g
17. Based on the information in the graph, a solution of 130 g of
sodium nitrate in 100 ml of water at 60C is
a. dilute b. unsaturated
c. saturated d. supersaturated
18. A nonpolar solvent will most likely dissolve in what type of solute?
a. polar
b. nonpolar
c. ionic
d. metallic.
19. Which of the following is a possible freezing to boiling point temperature range for a solution of sugar in
water?
a. 0C to 115.3 C
b. 0C to 100 C
c. -5C to 100  C
d. -6.3  C to 102.6  C
20. When making a solution of calcium chloride in water, the water would be the
a. solution
b. precipitate
c. solvent
d. solute
21. Bubbles arise on the surface of a newly opened bottle of a carbonated beverage. This action is explained
by the fact that the carbon dioxide is less soluble when
a. Temperature is increased
b. Temperature is decreased
c. Pressure is decreased
d. Pressure in increased
22. Which compound is insoluble in water?
a. BaSO4
b. KClO3
23. Which process is a chemical change?
a. melting of ice
b. boiling of water
c. CaBr2
d. Na2S
c. subliming of ice
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d. decomposing water into hydrogen and oxygen
24. 11.2 liters of a gas at STP has a mass of 35.5 grams. What is the identity of the gas?
a. Chlorine
b. Hydrogen chloride
c. Nitrogen
d. Hydrogen
Objective 2.05: Analyze the basic assumptions of kinetic molecular theory and apply the gas laws.
25.
D
26. A sample of a gas is contained in a closed rigid cylinder. According to kinetic molecular theory, what occurs
when the gas inside the cylinder is heated?
a. The number of gas molecules increases.
b. The number of collisions between gas molecules per unit time decreases.
c. The average velocity of the gas molecules increases.
d. The volume of the gas decreases.
27. The stronger the intermolecular forces in a substance, the higher the boiling point of the substance.
Which of the following substances would be predicted to have the highest boiling point?
a. O2
b. Ar
c. He
d. NH3
28. The density of a substance undergoes the greatest change when
a. A liquid changes to gas
b. A liquid changes to a solid
c. A solid changes to a liquid
d. When a gas changes to a solid
29. What is the volume of 40.0 g of helium at STP?
a. 11.2 L
b. 22.4 L
c. 112 L
d. 224 L
30. A diver finds the best corals at a depth of 10.0 m. The diver’s lung capacity at the surface is 2.40 L. The
surface air temperature is 32.0 C and the pressure is 101.3 kPa. What is the volume of the diver’s lungs at
10.0 m at a temperature of 21.0  C and a pressure of 141.2 kPa?
a. 1.12 L
b. 1.66 L
c. 1.78 L
d. 4.86 L
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31. How many moles of Nitrogen gas, N2, are present in a 45.0 liter container at a pressure of 0.50 atm and a
temperature of 82 C?
a. 7.72 mol
b. 3.34 mol
c. 0.772 mol
d. 1.23 mol
Objective 2.06: Assess bonding in metals and ionic compounds as related to chemical and physical properties.
32. Which substance contains bonds that involved the transfer of electrons from one atom to another?
a. CO2
b. KBr
c. NH3
d. Cl2
33. An atom of which element is larger than its iona. calcium
b. chlorine
c. oxygen
d. iodine
34. This apparatus was most likely designed to show that —
a.
b.
c.
d.
the formation of an ionic compound is an exothermic reaction
ionic compounds conduct a current in solution
the formation of an ionic compound is an endothermic reaction
water is a good conductor of electricity
Use the chart below on questions 35-36
35. What type of bonding is mostly likely in compound A?
a. non-polar covalent
b. polar covalent
c. ionic
d. metallic
36. What type of bonding is most likely in compound D?
a. non-polar covalent
b. polar covalent
c. ionic
d. metallic
Use the diagram below in question 37.
37. The diagram represents the arrangement of atoms in a metallic solid. Scientists believe that electrons in
the outer energy levels of the bonding metallic atoms are free to move from one atom to the next. Because
they are free to move, these electrons are often referred to delocalized electrons and give metals ALL of
the following properties EXCEPT.
a. Malleable and ductile.
c. Conduct heat and electricity in the solid state.
b. Luster
d. Brittle, break easily
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Objective 2.07: Assess covalent bonding in molecular compounds as related to chemical and physical properties
and molecular geometry.
38. The boiling point of HBr is lower than that of HF because:
a. HBr is heavier than HF and therefore it requires less energy to vaporize.
b. HBr has dipole-dipole attractions which are weaker than the hydrogen bonding found in HF.
c. The dispersion forces are weaker in HBr than in HF.
d. All of the above are correct.
39. Which substance(s) will exhibit hydrogen bonding between its molecules?
a. H2O
b. N2
c. CH4
d. H2
40. Which of these molecules would be expected to be polar?
a. O2
b. HCl
c. CO2
d. CCl4
41. What is the total number of pairs of electrons shared in a molecule of N2?
a. one pair
b. three pairs
c. two pairs
d. four pairs
42. The ammonia, NH3, gas molecule exhibits what type of geometric shape?
a. trigonal planar
b. tetrahedral
c. bent or V-shaped d. trigonal pyramidal
C 43. Which diagram best represents the structure of a water molecule?
Objective 2.08: Assess the dynamics of physical equilibrium
44. What are the best conditions for condensing a gas into a liquid?
a. high temperature, high pressure
b. low temperature, high pressure
c. high temperature, low pressure
d. low temperature, low pressure.
Use the graph on the right for questions 45-46
45. What phase change takes place as a substance moves
from A to B?
a. condensation
b. melting
c. boiling
d. sublimation
46. What is the boiling point of this liquid at 0.8 atm of
pressure?
a. 81.0 K
b. 83.5 K
c. 85.5 K
d. 87.5K
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Ö
A
Ö
B Ö
normal
B.P .
Objective 3.01: Analyze periodic trends in chemical properties and use the periodic table to predict properties of elements.
47. Which Period 4 element has the most metallic properties?
a. As
b. Ge
c. Br
d. Sc
48. If two elements have similar chemical properties, which of the following would be similar in
both elements?
a. atomic radii
c. number of energy levels
b. number of valence electrons
d. atomic mass
49. Which of the following is the correct noble gas representation for calcium?
a. [Ar] 4s2
b. [Ne] 3s23p64s2
c. [Xe] 4s6
d. [Br] 4s2
Use the Chart Below to Answer Questions 50-52
1
A
2
B
3
4
5
6
7
8
9 10
11 12
18
13 14 15 16 17
C
D
E
50. Which element has the lowest ionization energy?
a. A
b. B
c. C
d. D
51. What is the electron configuration of element D?
a. 1s2, 2s2, 2p6
b. 1s2, 2s2, 2p5
c. 1s2, 2s2, 3s1
d. 2s2, 2p3
52. What is the most common oxidation number for element C?
a. +3
b. +2
c. -2
d. -3
Objective 3.02: Apply the mole concept, Avogadro’s number and conversion factors to chemical calculations.
53. The gram molecular mass of oxygen (O2) is 32.0 grams/mol.
How many ATOMS of oxygen does this quantity represent?
a. 6.02 x 1023 atoms b. 2.0 atoms
c. 2 x 6.02 x 1023 atoms
d. 32.0 atoms
54. What is the number of moles of hydrogen contained in 1.0 mol of NH4HCO3?
a. 4.0 moles
b. 1.0 mole
c. 5.0 moles
d. 10.0 moles
55. What is the molarity of a solution of 3.2L which contains 0.32moles of solute?
a. 1.0 M
b. 0.1 M
c. 0.01 M
d. 10.0 M
56. How many grams of solute are contained in 125 mL of 0.0500 M solution of NaOH?
a. 0.00625 g
b. 6.25 g
c. 2.50 g
d. 0.250 g
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57. 7.00 moles of sodium have a mass of
a. 280 g
b. 161 g
c. 224 g
d. 3.29 g
58. What is the empirical formula for the compound C6H12O6?
a. CH2O
b. C3H6O3
c. C2H4O2
d. C6H12O6
59. Calculate the percent of oxygen in Ca(OH)2 calcium hydroxide?
a. 0.28%
b. 28%
c. 43%
d. 0.43%
Objective 3.03: Calculate quantitative relationships in chemical relationships (stoichiometry)
60. For the reaction: 2 HNO3 + Mg(OH)2  Mg(NO3)2 + 2 H2O, how many grams of magnesium nitrate are
produced from 8.00 moles of nitric acid?
a. 9.40 g
b. 37.0 g
c. 592 g
d. 818 g
61. In the chemical reaction A + B  C + D, if one knows the mass of A, one could determine
a. Only the mass of A and B combined
b. The mass of any other reactant or product
c. Only the mass of C and D combines
d. Only the mass of B
62. What is the mole-to-mole ratio between nitrogen gas and hydrogen gas in the equation
3H2 + N2  2 NH3
a. 1:2
b. 2:2
c. 1:3
d. 2:3
63.
2Al(s) + 3Br2(l) ➔ 2AlBr3(s)
The above equation represents the reaction of aluminum and bromine to form aluminum bromide.
If 3.0 moles of Aluminum are used, how many moles of AlBr 3 are produced?
a. 4.5 moles of AlBr3
b. 2.0 moles of AlBr3
c. 1.0 moles of AlBr3
d. 3.0 moles of AlBr3
64.
3H2(g) + N2(g)  2 NH3(g)
If 28.0 g of nitrogen are combined with hydrogen, what volume of ammonia, NH 3(g), is produced at STP?
a. 44.8 liters
b. 22.4 liters
c. 6.02 x 1023 ml
d. 17.0 liters
Objective 4.01: Analyze the Bohr model in terms of electron energies in the hydrogen atom.
Use the Reference Tables to answer questions 65-66.
65. The mathematical equation c= λf means that as the wavelength (λ) increases, the frequency (f)
decreases. The equation E = hf means that as frequency increases, energy increases. Using this
information and the reference tables, which color of visible light has the most energy?
a. Red
b. Yellow
c. Green
d. Violet
66. If an electron drops from n=4 to n=2, what type of electromagnetic radiation is emitted?
a. Ultraviolet (UV)
b. Visible
c. Infrared (IR)
d. Radiowaves
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Objective 4.02: Analyze the law of conservation, energy changes, and the various forms of energy involved in chemical and
physical processes.
67. What is the best way to describe the change that occurs when propane is burned?
a. chemical, exothermic
b. chemical, endothermic
c. physical, exothermic
d. physical, endothermic
Tempearture
68. The graph below represents the uniform heating of a substance, starting with the substance as a solid
below its melting point.
F
D
B
E
C
A
Time
Which line segment represents an increase in potential energy and no change in average kinetic energy?
a. AB
b. BC
c. CD
69. All of the following represent an endothermic chemical change except?
a.
b. 2H2O(l)  2H2 (g) + O2 (g)
∆H = +483.6 Kj
c. Two clear colorless solutions are mixed and the
temperature of the mixture decreases.
d. CO2(g) + 2H2O(l) + 891Kj  CH4(g) + 2O2(g)
Objective 4.03: Analyze the relationship between entropy and disorder in the universe.
70. Which 10-milliliter sample of water has the greatest degree of disorder?
a. H2O(g) at 1200C
b. H2O(g) at 800C
c. H2O(l) at 90C
d. H2O(s) at 0
Objective 4.04: Analyze nuclear energy.
71. Which of these particles has the greatest mass?
a. alpha
b. neutron
c. beta
d. positron
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d. EF
72. In the reaction 4Be9 + X -> 6C12 + 0n1, the X represents
a. an alpha particle
b. a beta particle
c. an electron
d. a proton
73. How much of a 40.0g sample of element X remains after 3.99 days? The half-life of element X is 1.33 days.
a. 5.0 g
b. 10.0 g
c. 20.0 g
d. 40.0 g
Objective 5.01: Evaluate various types of chemical reactions.
74. Which of the following metals would replace Zn in a single replacement reaction?
a. Cr
b. Cu
c. Fe
d. Ca
75. The equation below is an example of a ___________reaction.
2KClO3  2KCl
+ 3O2
a. synthesis
b. decomposition
c. double replacement
d. combustion
76. The equation below is an example of a ___________reaction.
CH4 + 2O2  CO2 + 2H2O
a. synthesis
b. decomposition
77. What are the products of this reaction?
a.
c. double replacement
Ca(OH)2
d. combustion
+ HCl 
calcium chloride and water
b. calcium hydroxide and hydrochloric acid
c.
chlorine, water, and calcium
d. calcium, oxygen, hydrogen and chlorine
Objective 5.02: Evaluate the Law of Conservation of Matter (balancing equations)
78. When the reaction below is correctly balanced, what will be the coefficient of Lead(II) Chloride?
___Pb(NO3)2(aq) + ____KCl(aq)  ____KNO3(aq) + _____PbCl2(s)
a. 1
b. 2 c. 3 d. 4
79. When the reaction: Ca(ClO3)2  ___ CaCl2 + ___ O2
is correctly balanced, what will be the coefficient of oxygen?
a. 1 b. 2 c. 3
d. 4
80. A chemist wrote down the following equation on a chalkboard: Ti + Cl2➝TiCl3 . Which set of
coefficients will balance the equation?
a. 1:1:1
b. 1:2:1
c. 2:1: 3
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d.
2: 3:2
Objective 5.03: Identify and predict the indicators of chemical change
81. Two clear colorless solutions are mixed in a test tube. A blue solution is formed and the test tube becomes
cold. What is the best way to describe the change that occurred?
a) chemical, exothermic
b) chemical, endothermic
c) physical, exothermic+
d) physical, endothermic
Objective 5.04: Identify the physical and chemical behaviors of acids and bases.
82. Hydrogen chloride, HCl, is classified as an Arrhenius acid because it produces
a. H+ ions in aqueous solution
b. Cl- ions in aqueous solution
c. OH- ions in aqueous solution
d. NH4+ ions in aqueous solution
83. An acid has as a [H+] = 1.0 x 10-4 . What is the pH of the solution?
a. 7
b. 4
c.
10
d. -4
84. Which equation represents a neutralization reaction?
a) 4Fe(s) + 3O2(g)  2Fe2O3(s)
b) 2H2(g) + O2(g) 
2H2O(l)
c) HNO3(aq) + KOH(aq)  KNO3(aq) + H2O(l)
d) AgNO3(aq) + KCl(aq)  KNO3(aq) + AgCl(s)
85. How many milliliters of 0.20 M NaOH are needed to neutralize 12.0 mL of 16M HNO3?
a. 600 ml
b. 800 ml
c. 960 ml
d. 1200 ml;
Objective 5.05: Analyze the oxidation/reduction reactions with regard to the transfer of electrons.
86. Given the balanced equation representing a redox reaction:
2Al + 3Cu2+  2Al3+ + 3Cu
Which statement is true about this reaction?
a. Each Al loses 2e– and each Cu2+ gains 3e–.
b. Each Al loses 3e– and each Cu2+ gains 2e–.
c. Each Al3+ gains 2e– and each Cu loses 3e–.
d. Each Al3+ gains 3e– and each Cu loses 2e–.
87. The principle characteristic of all redox reactions is:
a. the production of non-ionized compounds
b. complete irreversibility;
c. the transfer of electrons
d. the formation of water.
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88. What element is being reduced in the following equation:
A) zinc; B) sulfur; C) oxygen;
D) hydrogen.
Zn + H 2SO4  ZnSO4 + H2
Objective 5.06: Assess the factor that affect the rates of chemical reactions.
89. Given the reaction at 25°C:
Zn(s) + 2 HCl(aq)  ZnCl2(aq) + H2(g)
The rate of this reaction can be increased by using 5.0 grams of powdered zinc instead of a 5.0-gram strip of
zinc because the powdered zinc has
a. lower kinetic energy
b. lower concentration
c. more surface area
d. more zinc atoms
Use the diagram on the right to answer question 90.
90. How would the addition of a catalyst affect this reaction?
a. The presence of a catalyst would decrease the activation energy.
b. The catalyst would increase the activation energy.
c. The presence of a catalyst would make the reaction more spontaneous.
d. The catalyst would be consumed during the reaction and make more product
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