Download Chemistry 3100H Quarter 2 Semester Practice Exam

Name: ________________________ Class: ___________________ Date: __________ Mr. Dennis F. Goode ID: A
Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam.
This Chemistry 3100H Quarter 2 Semester Exam Study Guide is provided to help the Chemistry learner prepare for
a rigorous Chemistry Exam. Tackle this study guide to prepare yourself to do your best.
This Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam will assess your knowledge,
understanding, and some higher level thinking in the following Chemistyry content areas:
The Science Of Chemistry
Chemistry Measurement And Calculations
Atoms: Building Blocks Of Matter
Arrangements Of Electrons In Atoms
The Periodic Law
Chemical Bonding
Chemical Formulas/Compounds
Prepare the questions below. Print. Bring to the Semester Exam Study Sessions for review.
Good Luck!!! Remember: Hard work and smart work pay dividends!!!
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Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. Biochemistry is the study of
a. properties, changes, and relationships between energy and matter.
b. the chemistry of living things.
c. crystals and minerals.
d. carbon-containing compounds.
____
2. Organic chemistry is the study of
a. properties, changes, and relationships between energy and matter.
b. the chemistry of living things.
c. crystals and minerals.
d. carbon-containing compounds.
____
3. Matter includes all of the following except
a. air.
b. light.
c.
d.
smoke.
water vapor.
____
4. A true statement about mass is that
a. mass if often measured with a spring scale.
b. mass is expressed in pounds.
c. as the force of Earth's gravity on an object increases, the object's mass increases.
d. mass is determined by comparing the mass of an object with a set of standard masses that
are part of a balance.
____
5. Which of the following is not a physical change?
a. grinding
c.
b. cutting
d.
1
boiling
burning
Name: ________________________
ID: A
____
6. A solid substance is
a. always frozen regardless of its container.
b. always a crystal regardless of its container.
c. always the same shape regardless of its container.
d. always losing particles regardless of its container.
____
7. Plasma is the fourth state of matter. In the plasma state
a. atoms gain electrons.
b. atoms lose electrons.
c. atoms form molecules.
d. atomic nuclei break down.
____
8. The only pure substance listed below is
a. bread dough.
b. vinegar (5% acetic acid).
____
c.
d.
9. If a mixture is not uniform throughout, it is called
a. homogeneous.
c.
b. heterogeneous.
d.
vitamin C (ascorbic acid).
seawater.
chemically bonded.
a solution.
____ 10. A theory is accepted as the explanation of an observed phenomenon until
a. one study contradicts the theory.
b. repeated observations conflict with the theory.
c. a new method is discovered.
d. a leading scientist declares that it is invalid.
____ 11. Which of these statements does not describe a measurement standard?
a. Measurement standards avoid ambiguity.
b. Measurement standards must be unchanging.
c. A standard can be easily changed to suit the experiment.
d. Confusion is eliminated when the correct measurement is applied.
____ 12. The SI base units for length and time are
a. centimeter and second.
b. meter and hour.
c.
d.
centimeter and hour.
meter and second.
____ 13. The metric unit for length that is closest to the diameter of a pencil is the
a. micrometer.
c. centimeter.
b. millimeter.
d. decimeter.
____ 14. The symbols for units of length in order from largest to smallest are
a. m, cm, mm, km.
c. km, mm, cm, m.
b. mm, m, cm, km.
d. km, m, cm, mm.
____ 15. A volume of 1 milliliter is equivalent to
a. 1 cubic centimeter.
b. 1 gram.
c.
d.
1 liter.
10–1 cubic decimeters.
____ 16. The SI base unit for time is the
a. day.
b. hour.
c.
d.
minute.
second.
2
Name: ________________________
ID: A
____ 17. Which of these is the abbreviation for the SI base unit of time?
a. hr
c. sec
b. h
d. s
____ 18. Which of these statements about mass is true?
a. Mass is expressed in pounds or newtons.
b. Mass is usually measured with a spring scale.
c. The mass of an object depends on the force of gravity acting on it.
d. The mass of an object is determined by comparing it to an object of known mass.
____ 19. The relationship between the mass m of a material, its volume V, and its density D is
a. D = mV.
c. D = m/V.
b. D = V/m.
d. D = m + v.
____ 20. 0.25 g is equivalent to
a. 250 kg.
b. 250 mg.
c.
d.
0.025 mg.
0.025 kg.
____ 21. 0.05 cm is the same as
a. 0.000 05 m.
b. 0.005 mm.
c.
d.
0.05 m.
0.5 mm.
____ 22. If repeated measurements agree closely but differ widely from the accepted value, these measurements are
a. neither precise nor accurate.
b. accurate, but not precise.
c. both precise and accurate.
d. precise, but not accurate.
____ 23. The measurement 0.035550 g rounded off to two significant figures would be
a. 0.03 g.
c. 0.036 g.
b. 0.35 g.
d. 3.5  102 g.
____ 24. The number of significant figures in the measured value 0.032 0 g is
a. 2.
c. 4.
b. 3.
d. 5.
____ 25. When 5.7 m is divided by 2 s, the quotient is correctly reported as
a. 2.8 m/s.
c. 2.9 m/s.
b. 2.85 m/s.
d. 3 m/s.
____ 26. How many significant figures would the answer to the following calculation have?
3.475  1.97 + 2.4712 is
a.
b.
2
3
c.
d.
4
5
____ 27. How many significant digits should be shown in the product of 1.6 cm and 2.4 cm?
a. 1
c. 3
b. 2
d. 4
3
Name: ________________________
ID: A
____ 28. How would 0.00930 m be expressed in scientific notation?
a. 93  10–4 m
c. 9.30  10–3 m
–4
b. 9.3  10 m
d. 9.30  10–5 m
____ 29. The result of dividing 107 by 10–3 is
a. 10–4.
b. 102.5.
c.
d.
104.
1010.
____ 30. The graph of two variables that are directly proportional to one another is
a. a straight line.
c. a parabola.
b. an ellipse.
d. a hyperbola.
____ 31. Which of these statements about y = kx is not true?
a. y is directly proportional to x.
b. x is a variable.
c. The product of y and x is a constant.
d. The graph of y versus x is be a straight line.
____ 32. If each atom of element D has 3 mass units and each atom of element E has 5 mass units, a molecule
composed of one atom each of D and E has
a. 2 mass units.
c. 15 mass units.
b. 8 mass units.
d. 35 mass units.
____ 33. In oxides of nitrogen, such as N2O, NO, NO2, and N2O3, atoms combine in small whole-number ratios. This
evidence supports the law of
a. conservation of mass.
c. definite composition.
b. multiple proportions.
d. mass action.
____ 34. Which of the following statements is true according to modern atomic theory?
a. Atoms of the same element may have different masses.
b. Atoms may be divided in ordinary chemical reactions.
c. Atoms can never combine with any other atoms.
d. Cathode rays are composed of protons..
____ 35. Which concept in Dalton's atomic theory has been modified?
a. All matter is composed of atoms.
b. Atoms of different elements have different properties and masses.
c. Atoms can combine in chemical reactions.
d. Atoms cannot be divided.
____ 36. An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____ 37. The charge due to the electrons of a neutral atom
a. prevents compounds from forming.
c.
b. balances the charge on the nucleus.
d.
4
attracts electrons in other atoms.
does not exist.
Name: ________________________
____ 38. The most common form of hydrogen has
a. no neutrons.
b. one neutron.
ID: A
c.
d.
two neutrons.
three neutrons.
____ 39. As the atomic number increases, the number of electrons in a neutral atom
a. decreases.
c. remains the same.
b. increases.
d. is undetermined.
____ 40. Atoms of the same element can differ in
a. chemical properties.
b. mass number.
c.
d.
atomic number.
number of protons and electrons.
____ 41. The number of atoms in a mole of any pure substance is called
a. its atomic number.
c. its mass number.
b. Avogadro's constant.
d. its gram-atomic number.
____ 42. Avogadro's number is
a. the maximum number of electrons that all the energy levels can accommodate.
b. the number of protons and neutrons that can fit in the shells of the nucleus.
c. the number of particles in 1 mole of a pure substance.
d. the number of particles in exactly 1 gram of a pure substance.
____ 43. Because c, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is
a. proportional to its frequency.
c. inversely proportional to its frequency.
b. equal to its frequency.
d. double its frequency.
____ 44. As it travels through space, electromagnetic radiation
a. exhibits wavelike behavior.
c. varies in speed.
b. loses energy.
d. releases photons.
____ 45. If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B,
the wavelength of A is
a. longer.
c. equal.
b. shorter.
d. exactly half the length of B's wavelength.
____ 46. The distance between two successive peaks on adjacent waves is its
a. frequency.
c. quantum number.
b. wavelength.
d. velocity.
____ 47. Max Planck proposed that a hot object radiated energy in small, specific amounts called
a. quanta.
c. hertz.
b. waves.
d. electrons.
____ 48. Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that
hydrogen
a. had no electrons.
c. released photons of only certain energies.
b. did not release photons.
d. could only exist in the ground state.
5
Name: ________________________
ID: A
____ 49. Which energy-level change shown in the diagram below emits the highest energy?
a.
b.
c.
d.
an electron moving from E6 to E5
an electron moving from E2 to E4
an electron moving from E2 to E3
an electron moving from E2 to E1
____ 50. The electron in a hydrogen atom has its lowest total energy when the electron is in its
a. neutral state.
c. ground state.
b. excited state.
d. quantum state.
____ 51. The French scientist Louis de Broglie theorized that
a. electrons could have a dual wave-particle nature.
b. light waves did not have a dual wave-particle nature.
c. the natures of light and quantized electron orbits were not similar.
d. Bohr's model of the hydrogen atom was completely correct.
____ 52. The equation E = h helped Louis de Broglie determine
a. how protons and neutrons behave in the nucleus.
b. how electron wave frequencies correspond to specific energies.
c. whether electrons behave as particles.
d. whether electrons exist in a limited number of orbits with different energies.
____ 53. The region outside the nucleus where an electron can most probably be found is the
a. electron configuration.
c. s sublevel.
b. quantum.
d. electron cloud.
____ 54. The quantum number that indicates the position of an orbital about the three axes in space is the
a. principal quantum number.
b. angular momentum quantum number.
c. magnetic quantum number.
d. spin quantum number.
6
Name: ________________________
ID: A
____ 55. The spin quantum number indicates that the number of possible spin states for an electron in an orbital is
a. 1.
c. 3.
b. 2.
d. 5.
____ 56. The spin quantum number of an electron can be thought of as describing
a. the direction of electron spin.
b. whether the electron's charge is positive or negative.
c. the electron's exact location in orbit.
d. the number of revolutions the electron makes about the nucleus per second.
____ 57. An electron for which n = 4 has more ____ than an electron for which n = 2.
a. spin
c. energy
b. particle nature
d. wave nature
____ 58. The letter designations for the first four sublevels with the maximum number of electrons that can be
accommodated in each sublevel are
a. s:2, p:4, d:6, and f:8.
b. s:1, p:3, d:5, and f:7.
c. s:2, p:6, d:10, and f:14.
d. s:1, p:2, d:3, and f:4.
____ 59. How many electrons are needed to completely fill the fourth energy level?
a. 8
c. 32
b. 18
d. 40
____ 60. If 8 electrons completely fill a main energy level, what is n?
a. 2
c. 8
b. 4
d. 32
____ 61. "Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and
all electrons in singly occupied orbitals must have the same spin" is a statement of
a. the Pauli exclusion principle.
c. the quantum effect.
b. the Aufbau principle.
d. Hund's rule.
____ 62. Which of the following rules requires that each of the p orbitals at a particular energy level receive one
electron before any of them can have two electrons?
a. Hund's rule
c. the Aufbau principle
b. the Pauli exclusion principle
d. the quantum rule
____ 63. Which of the following lists atomic orbitals in the correct order they are filled according to the Aufbau
principle?
a. 1s 2s 2p 3s 4s 3p 3d 4p 5s
b. 1s 2s 2p 3s 3p 4s 3d 4p 5s
c. 1s 2s 2p 3s 3p 4s 4p 3d 4d
d. 1s 2s 2p 3s 3p 3d 4s 4p 5s
____ 64. If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
a. 2
c. 10
b. 8
d. 32
7
Name: ________________________
ID: A
____ 65. The periodic table
a. permits the properties of an element to be predicted before the element is discovered.
b. will be completed with element 118.
c. has been of little use to chemists since the early 1900s.
d. was completed with the discovery of the noble gases.
____ 66. The atomic number of lithium, the first element in Group 1, is 3. The atomic number of the second element in
this group is
a. 4.
c. 11.
b. 10.
d. 18.
____ 67. Krypton, atomic number 36, is the fourth element in Group 18. What is the atomic number of xenon, the fifth
element in Group 18?
a. 54
c. 72
b. 68
d. 90
____ 68. Barium, atomic number 56, is the fifth element in Group 2. What is the atomic number of radium, the next
element in Group 2?
a. 64
c. 88
b. 74
d. 103
____ 69. Refer to the figure above. Potassium and bromine belong to
a. Period 4.
c. Period 1.
b. Group 4.
d. Group 1.
____ 70. In Period 3 there are 8 elements. What sublevel(s) is (are) being filled?
a. s
c. s and p
b. s and d
d. d and f
____ 71. To which block do the actinide elements belong?
a. d block
c.
b. s block
d.
f block
p block
____ 72. Titanium, atomic number 22, has the configuration [Ar] 3d2 4s2. To what group does titanium belong?
a. Group 2
c. Group 4
b. Group 3
d. Group 5
____ 73. The most reactive group of the nonmetals is the
a. lanthanides.
c.
b. transition elements.
d.
halogens.
noble gases.
____ 74. The group of soft, silvery, reactive metals, all of which have one electron in an s orbital, is known as the
a. alkaline-earth metals.
c. alkali metals.
b. transition metals.
d. metalloids.
____ 75. The most characteristic property of the noble gases is that they
a. have low boiling points.
b. are radioactive.
c. are gases at ordinary temperatures.
d. are largely unreactive.
8
Name: ________________________
ID: A
____ 76. A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the
compound is called
a. electron affinity.
c. electronegativity.
b. electron configuration.
d. ionization potential.
____ 77. One-half the distance between the nuclei of identical atoms that are bonded together is called the
a. atomic radius.
c. atomic volume.
b. atomic diameter.
d. electron cloud.
____ 78. A positive ion is known as a(n)
a. ionic radius.
b. valence electron.
c.
d.
cation.
anion
____ 79. Within a group of elements, as the atomic number increases, the atomic radius
a. increases.
b. remains approximately constant.
c. decreases regularly.
d. varies unpredictably.
____ 80. In the alkaline-earth group, atoms with the smallest radii
a. are the most reactive.
b. have the largest volume.
c. are all gases.
d. have the highest ionization energies.
____ 81. Which is the best reason that the atomic radius generally increases with atomic number in each group of
elements?
a. The nuclear charge increases.
b. The number of neutrons increases.
c. The number of occupied energy levels increases.
d. A new octet forms.
____ 82. The first electrons to be removed when d-block elements form ions are the
a. d electrons.
c. s electrons.
b. p electrons.
d. f electrons.
____ 83. Which groups in the main group have lower electronegativity than d-block elements?
a. groups 1 and 2
c. groups 17 and 18
b. groups 13 through 18
d. groups 13 through 17
____ 84. The electrons involved in the formation of a chemical bond are called
a. dipoles.
c. Lewis electrons.
b. s electrons.
d. valence electrons.
____ 85. Atoms naturally move
a. toward high potential energy.
b. toward low potential energy.
c.
d.
toward less stability.
away from each other.
____ 86. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
a. nonpolar.
c. ionic.
b. polar.
d. dipolar.
9
Name: ________________________
ID: A
____ 87. The greater the electronegativity difference between two bonded atoms, the greater the percentage of ____ in
the bond.
a. ionic character
c. metallic character
b. covalent character
d. electron sharing
____ 88. The pair of elements that forms a bond with the least ionic character is
a. Na and Cl.
c. O and Cl.
b. K and Cl.
d. Mg and Cl.
____ 89. In a molecule of fluorine, the two shared electrons give each fluorine atom how many electron(s) in the outer
energy level?
a. 1
c. 8
b. 2
d. 32
____ 90. To draw a Lewis structure, one must know the
a. number of valence electrons in each atom.
b. atomic mass of each atom.
c. bond length of each atom.
d. ionization energy of each atom.
____ 91. What is the correct Lewis structure for hydrogen chloride, HCl?
a.
b.
A
B
c.
d.
C
D
____ 92. The chemical formula for an ionic compound represents the
a. number of atoms in each molecule.
b. number of ions in each molecule.
c. ratio of the combined ions present in a sample.
d. total number of ions in the crystal lattice.
____ 93. The chemical formula for water, a covalent compound, is H2O. This formula is an example of a(n)
a. formula unit.
c. ionic formula.
b. Lewis structure.
d. molecular formula.
____ 94. Compared with ionic compounds, molecular compounds
a. have higher boiling points.
c. have lower melting points.
b. are brittle.
d. are harder.
____ 95. How many electrons must be shown in the Lewis structure of the hydroxide ion, OH –?
a. 1
c. 9
b. 8
d. 10
____ 96. In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)
a. Lewis structure.
c. electron cloud.
b. electron sea.
d. dipole.
10
Name: ________________________
ID: A
____ 97. To appear shiny, a material must be able to
a. form crystals.
b. absorb and re-emit light of many wavelengths.
c. absorb light and change it all to energy as heat.
d. change light to electricity.
____ 98. According to VSEPR theory, the shape of an AB3 molecule is
a. trigonal-planar.
c. linear.
b. tetrahedral.
d. bent.
____ 99. Use VSEPR theory to predict the shape of the magnesium hydride molecule, MgH 2.
a. tetrahedral
c. bent
b. linear
d. octahedral
____ 100. Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI 4.
a. tetrahedral
c. bent
b. linear
d. trigonal-planar
____ 101. Four hybrid sp3 orbitals are formed from
a. two s orbitals and two p orbitals.
b. an s orbital and a p orbital.
c. three s orbitals and one p orbital.
d. one s orbital and three p orbitals.
____ 102. What is the formula for the compound formed by calcium ions and chloride ions?
a. CaCl
c. CaCl3
b. Ca2Cl
d. CaCl2
____ 103. Name the compound Ni(ClO3)2.
a. nickel(II) chlorate
b. nickel(II) chloride
c.
d.
nickel(II) chlorite
nickel(II) peroxide
____ 104. Name the compound KClO3.
a. potassium chloride
b. potassium trioxychlorite
c.
d.
potassium chlorate
hypochlorite
____ 105. Name the compound N2O3.
a. dinitrogen oxide
b. nitrogen trioxide
c.
d.
nitric oxide
dinitrogen trioxide
____ 106. What is the formula for diphosphorus pentoxide?
a. P2PeO5
c.
b. PO5
d.
P2O4
P2O5
____ 107. What is the oxidation number of hydrogen in compounds containing metals?
a. –1
c. +1
b. 0
d. the charge on the metal ion
____ 108. What is the oxidation number of oxygen in CO2?
a. –4
c.
b. –2
d.
11
0
+4
Name: ________________________
____ 109. What is the percentage composition of CO?
a. 50% C, 50% O
b. 12% C, 88% O
ID: A
c.
d.
25% C, 75% O
43% C, 57% O
____ 110. The empirical formula for a compound shows the symbols of the elements with subscripts indicating the
a. actual numbers of atoms in a molecule.
b. number of moles of the compound in 100 g.
c. smallest whole-number ratio of the atoms.
d. atomic masses of each element.
____ 111. Of the following molecular formulas for hydrocarbons, which is an empirical formula?
a. CH4
c. C3H6
b. C2H2
d. C4H10
____ 112. A compound's empirical formula is C2H5. If the formula mass is 58 amu, what is the molecular formula?
a. C3H6
c. C5H8
b. C4H10
d. C5H15
____ 113. A compound's empirical formula is N2O5. If the formula mass is 108 amu, what is the molecular formula?
a. N2O5
c. NO3
b. N4O10
d. N2O4
Completion
Complete each statement.
114. The study of matter and changes that occur in matter best describes the science of ____________________.
115. A scientist is working to determine the properties and changes of matter and their relation to energy of a
newly discovered mineral. She is working in the field of ____________________ chemistry.
116. A scientist is working to develop better dating methods for substances that contain carbon. He is working in
the field of ____________________ chemistry.
117. A team of scientists is working to discover how an enzyme affects blood cells in sheep. They are working in
the field of ____________________ chemistry.
118. A chemistry student is studying the formation of quartz crystals. She is studying ____________________
chemistry.
119. A scientist is using mathematical models to isolate a new chemical process. He is working in the field of
____________________ chemistry.
120. Two scientists are trying to determine the exact nature of the chemicals in a lava flow. They are working in
the field of ____________________ chemistry.
121. Basic research is performed to increase ____________________.
12
Name: ________________________
ID: A
122. Applied research is often performed to find the answer to a particular ____________________.
123. Technological development is performed to better our ____________________.
124. In a bonfire, oxygen allows wood to combust, leaving behind ashes. In this process, oxygen and wood are the
reactants, and ashes are the ____________________.
125. When examining a mineral, hardness and color are two of the properties used for identification. Hardness and
color are examples of ____________________ properties.
126. An apple turning brown after being cut is an example of a ____________________ change.
127. The melting of butter is a ____________________ change because it does not produce any new substances.
128. Iron and sulfur, when heated, form an iron sulfide that has different properties from either iron or sulfur. The
formation of iron sulfide is an example of a ____________________ change.
129. The oxygen in air causes iron to rust. Iron and oxygen are ____________________ in this process, and rust is
the product.
130. Some iron and sulfur are mixed together, then heated. When the result is cooled, the iron can no longer be
separated from the sulfur with a magnet. The result of heating the mixture was the formation of a(n)
____________________.
131. A sample of matter can be poured from container to container. It takes the shape of its container but only
takes up a certain volume. Based on this information, the sample is in the ____________________ state.
132. The particles of a substance in the ____________________ are able to slide past each other.
133. Any substance with a definite composition is a ____________________.
134. Matter that has neither a definite volume nor a definite shape is in the ____________________ state.
135. The two types of matter that are pure substances are ____________________ and ____________________.
136. An alloy such as a gold ring is an example of a(n) ____________________ mixture.
137. Gravel is an example of a(n) ____________________ mixture.
Use a periodic table to answer the following questions.
138. Find the name for the element whose symbol is Pb. ____________________
139. Find the name for the element whose symbol is Mg. ____________________
140. Find the name for the element whose symbol is H. ____________________
13
Name: ________________________
ID: A
141. Find the name for the element whose symbol is P. ____________________
142. Find the name for the element whose symbol is Al. ____________________
143. Find the name for the element whose symbol is Bi. ____________________
144. Find the symbol for the element helium. ____________________
145. Find the symbol for the element tin. ____________________
146. Find the symbol for the element neon. ____________________
147. Find the symbol for the element iodine. ____________________
148. Find the symbol for the element chlorine. ____________________
149. In which period can you find the element iron? ____________________
150. In which period can you find the element gold? ____________________
151. In which period can you find the lanthanide series? ____________________
152. In which period can you find the actinide series? ____________________
153. In which group can you find the element lithium? ____________________
154. In which group can you find the element nickel? ____________________
155. In which group can you find the element neon? ____________________
156. In which group can you find the element carbon? ____________________
157. Find the symbol for the element argon. ____________________
158. The name and formula for the compound formed by strontium ions and sulfite ions are
____________________.
159. The Stock name for the compound P2O5 is ____________________.
2
160. The name for the CrO 4 ion is ____________________.
161. The oxidation numbers for each atom in NH 4 are ____________________.
162. The oxidation numbers for each atom in H2CO3 are ____________________.
14
Name: ________________________
ID: A
Essay
163. Compare and contrast solids, liquids, gases, and plasma by explaining the behavior of their particles. Draw
models to illustrate your answer.
164. Use examples to show how the properties and classifications of elements change as you move across a period
of the periodic table.
165. Using the two models shown below explain how each model resembles the object it represents. Explain how
each model differs from the object it represents.
166. The table below show measurements made on samples of three unknown materials. Explain how this data
could be used to identify the three materials.
Material
1
2
3
Mass and Volume Data
Mass (g)
Volume (mL)
6.02
2.23
18.42
2.34
35.15
3.10
167. Explain what is meant by the law of definite proportions, the law of conservation of mass, and the law of
multiple proportions.
168. Why do scientists use Dalton's theory, even though parts of it have been proven wrong? How much of
Dalton's theory do scientists still accept?
169. What can you determine about the atomic structure of an element if you know the atomic number of the
element and mass numbers of its isotopes? What additional information is needed to determine the average
atomic mass of the element? How do you determine the average atomic mass of the element?
170. Explain the significance of Avogadro's constant, 6.022  1023. What is the relationship between it and the
molar mass of oxygen, 16.00 g/mol?
171. Elements of the fourth period fill the 4s sublevel with electrons before filling the 3d sublevels. Also, some
elements move an electron from a filled 4s sublevel to an unoccupied 3d sublevel. Explain these behaviors.
172. Explain nuclear charge and how it affects the general trend in radii of atoms of elements going from left to
right across a period in the periodic table.
15
Name: ________________________
ID: A
173. How many different kinds of covalent bonds can a nitrogen atom form? Explain.
174. HO and H2O2 are examples of the empirical and molecular formula of a compound, respectively. Explain the
relationship between these two types of formulas.
Problem
175. How many atoms are present in 8.00 mol of chlorine atoms?
176. How many atoms are present in 80.0 mol of zirconium?
177. How many moles of platinum are equivalent to 1.20  1024 atoms?
178. How many moles of iron are equivalent to 1.11  1025 atoms?
179. Determine the mass in grams of 5.00 mol of oxygen. The molar mass of oxygen is 16.00 g/mol.
180. Determine the mass in grams of 10.0 mol of bromine. The molar mass of bromine is 79.90 g/mol.
181. Determine the number of moles of helium in 10.0 g of helium. The molar mass of helium is 4.00 g/mol.
182. Determine the number of moles in 100. g of potassium. The molar mass of potassium is 39.10 g/mol.
183. The mass of 1 mol of gold atoms is 196.97 g. Find the mass of 1 atom of gold.
184. Calculate the mass in grams of 9.00 mol of potassium (molar mass 39.10 g/mol).
185. Calculate the number of atoms in 10.0 g of sulfur (molar mass 32.07 g/mol).
186. Write the electron configuration for nitrogen, atomic number 7.
16
Name: ________________________
ID: A
Use the periodic table below to answer the following questions.
187. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
188. Write the noble-gas electron configuration for silicon.
189. Draw the orbital diagram for phosphorus.
190. Draw the orbital diagram for argon.
191. Write the noble-gas electron configuration represented in the orbital diagram below.
17
Name: ________________________
ID: A
192. What element's orbital diagram is shown in the figure below?
193. Draw a Lewis structure for the oxalate ion, C2O42–.
194. Draw a Lewis structure for carbon disulfide, CS2.
195. Draw a Lewis structure for the nitrate ion, NO 3 . Use VSEPR theory to predict its molecular geometry.
196. Draw a ball-and-stick model of a water molecule. Label that atoms, include the polarities of the bonds using
arrows, and indicate net molecular dipole.
197. The molar mass of aluminum is 26.98 g/mol and the molar mass of fluorine is 19.00 g/mol. Calculate the
molar mass of aluminum trifluoride, AlF3.
198. The molar mass of copper is 63.55 g/mol, the molar mass of sulfur is 32.07 g/mol, and the molar mass of
oxygen is 16.00 g/mol. Calculate the molar mass of copper(II) sulfate, CuSO 4.
199. The molar mass of iron is 55.85 g/mol, the molar mass of silicon is 28.08 g/mol, and the molar mass of
oxygen is 16.00 g/mol. Calculate the molar mass of iron(II) silicate, Fe 2SiO4.
200. The molar mass of aluminum is 26.98 g/mol and the molar mass of oxygen is 16.00 g/mol. Determine the
molar mass of Al2O3.
18
ID: A
Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam.
Answer Section
MULTIPLE CHOICE
1. ANS:
OBJ:
2. ANS:
OBJ:
3. ANS:
OBJ:
4. ANS:
OBJ:
5. ANS:
OBJ:
6. ANS:
OBJ:
7. ANS:
OBJ:
8. ANS:
OBJ:
9. ANS:
OBJ:
10. ANS:
OBJ:
11. ANS:
OBJ:
12. ANS:
OBJ:
13. ANS:
OBJ:
14. ANS:
OBJ:
15. ANS:
OBJ:
16. ANS:
OBJ:
17. ANS:
OBJ:
18. ANS:
OBJ:
19. ANS:
OBJ:
20. ANS:
OBJ:
B
2
D
2
B
1
D
1
D
2
C
3
B
3
C
5
B
5
B
3
C
1
D
2
C
2
D
2
A
2
D
2
D
2
D
3
C
4
B
5
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
III
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
III
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
II
REF: 2
1
ID: A
21. ANS:
OBJ:
22. ANS:
OBJ:
23. ANS:
OBJ:
24. ANS:
OBJ:
25. ANS:
OBJ:
26. ANS:
OBJ:
27. ANS:
OBJ:
28. ANS:
OBJ:
29. ANS:
OBJ:
30. ANS:
OBJ:
31. ANS:
OBJ:
32. ANS:
OBJ:
33. ANS:
OBJ:
34. ANS:
OBJ:
35. ANS:
OBJ:
36. ANS:
OBJ:
37. ANS:
OBJ:
38. ANS:
OBJ:
39. ANS:
OBJ:
40. ANS:
OBJ:
41. ANS:
OBJ:
42. ANS:
OBJ:
43. ANS:
OBJ:
D
5
D
1
C
2
B
2
D
3
B
3
B
3
C
4
D
4
A
5
C
5
B
1
B
1
A
3
D
3
C
3
B
4
A
1
B
2
B
2
B
4
C
4
C
1
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 1
2
ID: A
44. ANS:
OBJ:
45. ANS:
OBJ:
46. ANS:
OBJ:
47. ANS:
OBJ:
48. ANS:
OBJ:
49. ANS:
OBJ:
50. ANS:
OBJ:
51. ANS:
OBJ:
52. ANS:
OBJ:
53. ANS:
OBJ:
54. ANS:
OBJ:
55. ANS:
OBJ:
56. ANS:
OBJ:
57. ANS:
OBJ:
58. ANS:
OBJ:
59. ANS:
OBJ:
60. ANS:
OBJ:
61. ANS:
OBJ:
62. ANS:
OBJ:
63. ANS:
OBJ:
64. ANS:
OBJ:
65. ANS:
OBJ:
66. ANS:
OBJ:
A
2
A
2
B
2
A
3
C
3
C
4
C
4
A
1
B
1
D
2
C
4
B
4
A
4
C
4
C
5
C
1
A
1
D
2
A
2
B
3
B
3
A
2
C
4
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
II
REF: 1
3
ID: A
67. ANS:
OBJ:
68. ANS:
OBJ:
69. ANS:
OBJ:
70. ANS:
OBJ:
71. ANS:
OBJ:
72. ANS:
OBJ:
73. ANS:
OBJ:
74. ANS:
OBJ:
75. ANS:
OBJ:
76. ANS:
OBJ:
77. ANS:
OBJ:
78. ANS:
OBJ:
79. ANS:
OBJ:
80. ANS:
OBJ:
81. ANS:
OBJ:
82. ANS:
OBJ:
83. ANS:
OBJ:
84. ANS:
OBJ:
85. ANS:
OBJ:
86. ANS:
OBJ:
87. ANS:
OBJ:
88. ANS:
OBJ:
89. ANS:
OBJ:
A
4
C
4
A
4
C
1
C
2
C
3
C
4
C
4
D
4
C
1
A
1
C
2
A
2
D
2
C
2
C
4
A
4
D
1
B
2
B
3
A
4
D
5
C
3
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
I
REF: 1
PTS: 1
DIF:
III
REF: 1
PTS: 1
DIF:
II
REF: 2
4
ID: A
90. ANS: A
OBJ: 4
91. ANS: D
OBJ: 5
92. ANS: C
OBJ: 1
93. ANS: D
OBJ: 1
94. ANS: C
OBJ: 4
95. ANS: B
OBJ: 4
96. ANS: B
OBJ: 1
97. ANS: B
OBJ: 2
98. ANS: A
OBJ: 1
99. ANS: B
OBJ: 2
100. ANS: A
OBJ: 2
101. ANS: D
OBJ: 3
102. ANS: D
OBJ: 2
103. ANS: A
OBJ: 3
104. ANS: C
OBJ: 3
105. ANS: D
OBJ: 4
106. ANS: D
OBJ: 5
107. ANS: A
OBJ: 1
108. ANS: B
OBJ: 2
109. ANS: D
Solution:
PTS: 1
DIF:
I
REF: 2
PTS: 1
DIF:
III
REF: 2
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
II
REF: 3
PTS: 1
DIF:
I
REF: 3
PTS: 1
DIF:
III
REF: 3
PTS: 1
DIF:
I
REF: 4
PTS: 1
DIF:
I
REF: 4
PTS: 1
DIF:
I
REF: 5
PTS: 1
DIF:
III
REF: 5
PTS: 1
DIF:
III
REF: 5
PTS: 1
DIF:
II
REF: 5
PTS: 1
DIF:
III
REF: 1
PTS: 1
DIF:
III
REF: 1
PTS: 1
DIF:
III
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
II
REF: 1
PTS: 1
DIF:
II
REF: 2
PTS: 1
DIF:
III
REF: 2
percentage composition 
percentage carbon 
PTS: 1
mass of element
 100
total mass
12.01 g
 100 = 42.88% C, 100%  42.88%  57.12% O
28.01 g
DIF:
III
REF: 3
5
OBJ: 4
ID: A
110. ANS: C
PTS: 1
OBJ: 1
111. ANS: A
PTS: 1
OBJ: 3
112. ANS: B
Solution:
molecular mass
58 amu

 2.0
empirical mass 29.07 amu
DIF:
I
REF: 4
DIF:
III
REF: 4
Molecular formula is C 4 H 10 .
PTS: 1
DIF: III
113. ANS: A
Solution:
molecular mass
108 amu

 1.0
empirical mass 108.02 amu
REF: 4
OBJ: 4
Molecular formula is N 2 O 5 .
PTS: 1
DIF:
III
REF: 4
OBJ: 4
PTS: 1
115. ANS: physical
DIF:
I
REF: 1
OBJ: 1
PTS: 1
116. ANS: organic
DIF:
II
REF: 1
OBJ: 2
PTS: 1
DIF:
117. ANS: biochemistry
II
REF: 1
OBJ: 2
PTS: 1
118. ANS: inorganic
DIF:
II
REF: 1
OBJ: 2
PTS: 1
119. ANS: analytical
DIF:
II
REF: 1
OBJ: 2
PTS: 1
120. ANS: analytical
DIF:
II
REF: 1
OBJ: 2
PTS: 1
121. ANS: knowledge
DIF:
II
REF: 1
OBJ: 2
DIF:
II
REF: 1
OBJ: 3
COMPLETION
114. ANS: chemistry
PTS: 1
6
ID: A
122. ANS: problem
PTS: 1
123. ANS: lives
DIF:
II
REF: 1
OBJ: 3
PTS: 1
124. ANS: product
DIF:
II
REF: 1
OBJ: 3
PTS: 1
125. ANS: physical
DIF:
II
REF: 2
OBJ: 1
PTS: 1
126. ANS: chemical
DIF:
I
REF: 2
OBJ: 1
PTS: 1
127. ANS: physical
DIF:
II
REF: 2
OBJ: 2
PTS: 1
128. ANS: compound
DIF:
II
REF: 2
OBJ: 2
PTS: 1
129. ANS: reactants
DIF:
II
REF: 2
OBJ: 2
PTS: 1
130. ANS: compound
DIF:
II
REF: 2
OBJ: 2
PTS: 1
131. ANS: liquid
DIF:
II
REF: 2
OBJ: 2
PTS: 1
132. ANS: liquid
DIF:
II
REF: 2
OBJ: 3
PTS: 1
133. ANS: chemical
DIF:
I
REF: 2
OBJ: 3
PTS: 1
134. ANS: gaseous
DIF:
I
REF: 2
OBJ: 3
PTS: 1
DIF: I
135. ANS: elements, compounds
REF: 2
OBJ: 3
PTS: 1
DIF:
136. ANS: homogeneous
II
REF: 2
OBJ: 5
PTS: 1
DIF:
137. ANS: heterogeneous
I
REF: 2
OBJ: 5
II
REF: 2
OBJ: 5
PTS: 1
DIF:
7
ID: A
138. ANS: lead
PTS: 1
139. ANS: magnesium
DIF:
I
REF: 3
OBJ: 1
PTS: 1
140. ANS: hydrogen
DIF:
I
REF: 3
OBJ: 1
PTS: 1
DIF:
141. ANS: phosphorous
I
REF: 3
OBJ: 1
PTS: 1
142. ANS: aluminum
DIF:
I
REF: 3
OBJ: 1
PTS: 1
143. ANS: Bismuth
DIF:
I
REF: 3
OBJ: 1
PTS: 1
144. ANS: He
DIF:
I
REF: 3
OBJ: 1
PTS: 1
145. ANS: Sn
DIF:
I
REF: 3
OBJ: 2
PTS: 1
146. ANS: Ne
DIF:
I
REF: 3
OBJ: 2
PTS: 1
147. ANS: I
DIF:
I
REF: 3
OBJ: 2
PTS: 1
148. ANS: Cl
DIF:
I
REF: 3
OBJ: 2
PTS: 1
149. ANS: 4
DIF:
I
REF: 3
OBJ: 2
PTS: 1
150. ANS: 6
DIF:
I
REF: 3
OBJ: 3
PTS: 1
151. ANS: 6
DIF:
I
REF: 3
OBJ: 3
PTS: 1
152. ANS: 7
DIF:
I
REF: 3
OBJ: 3
PTS: 1
153. ANS: 1
DIF:
I
REF: 3
OBJ: 3
PTS: 1
DIF:
I
REF: 3
OBJ: 3
8
ID: A
154. ANS: 10
PTS: 1
155. ANS: 18
DIF:
I
REF: 3
OBJ: 3
PTS: 1
156. ANS: 14
DIF:
I
REF: 3
OBJ: 3
PTS: 1
157. ANS: Ar
DIF:
I
REF: 3
OBJ: 3
PTS: 1
DIF: I
158. ANS: strontium sulfite, SrSO3
REF: 3
OBJ: 2
PTS: 1
DIF: III
159. ANS: phosphorus(V) oxide
REF: 1
OBJ: 3
PTS: 1
DIF:
160. ANS: chromate ion
III
REF: 1
OBJ: 3
PTS: 1
161. ANS: N –3, H +1
DIF:
III
REF: 1
OBJ: 3
PTS: 1
DIF:
162. ANS: H +1, C +4, O –2
III
REF: 2
OBJ: 2
III
REF: 2
OBJ: 2
PTS: 1
DIF:
ESSAY
163. ANS:
The arrangement of the particles in the three states accounts for their different properties. Particles in a solid
move very little; particles in a liquid move more; and gas particles and plasma particles move the most. In
drawn models, particles in solids should be closely packed and structured; particles in liquids should appear
able to flow randomly past one another; and particles in gases should appear sparsely and randomly spaced.
Plasma particles should have lost some of their electrons.
PTS: 1
DIF: III
REF: 2
OBJ: 3
164. ANS:
The closer two elements are within a period, the more similar their properties are. Moving across a period,
elements progress from metals to metalloids, to nonmetals, to noble gases.
PTS: 1
DIF:
III
REF: 3
9
OBJ: 3
ID: A
165. ANS:
The model of the sun is accurate in showing that the sun is round and has a fiery surface. The model of an
atom shows that the atom is a particle.
The sun model is inaccurate because it is only two-dimensional, and it is smaller than the real sun. In
addition, it does not show the sun's composition. The atomic model is inaccurate because it is larger than a
real atom, because it is only two-dimensional, and because it does not depict the atom's composition and
chemical properties.
PTS: 1
DIF: III
REF: 1
OBJ: 3
166. ANS:
The density of each sample could be calculated. Then each value could be compared to known values to
identify the substances.
PTS: 1
DIF: III
REF: 2
OBJ: 4
167. ANS:
Definite proportions: regardless of the origin or size of samples of a particular compound, their elements are
always in the same proportion. Conservation of mass: the mass of the elements combined in a compound is
the same as the sum of the masses of the individual elements. Multiple proportions: when two elements
combine to form two different compounds, the ratio of the masses of one element that combine with a fixed
mass of the other element is a small whole number.
PTS: 1
DIF: III
REF: 1
OBJ: 1
168. ANS:
Dalton's theory led to the modern theory of the atom. Although scientists now know that atoms can be
divided and that elements exist as isotopes, most of his early theory is still accepted.
PTS: 1
DIF: II
REF: 1
OBJ: 3
169. ANS:
The atomic number equals the number of protons in the nucleus of an atom and also equals the number of
electrons in the neutral atom. The mass number is the sum of the number of protons and neutrons and can be
used, with the atomic number, to find the number of neutrons in each isotope. Each isotope of the element
has a different mass number but the same atomic number as the element.
In order to determine the average atomic mass of the element, you needed to know the relative
abundance and the exact mass of each isotope. Then, multiply the relative abundance (in decimal form) times
the atomic mass for each isotope, and adding the results.
PTS: 1
DIF: II
REF: 3
OBJ: 2
170. ANS:
Avogadro's constant is the number of particles in 1 mol of a substance. Because the molar mass of oxygen
atoms is 16.00 g/mol, the mass of 1 mol, or 6.022  1023, oxygen atoms is 16.00 g.
PTS: 1
DIF:
II
REF: 3
10
OBJ: 4
ID: A
171. ANS:
Elements fill the 4s sublevel with electrons before filling the 3d sublevels because the 4s sublevel is lower in
energy than the 3d sublevels. According to the Aufbau principle, an electron occupies the lowest energy level
that can receive it. Some elements move an electron from a filled 4s sublevel to an unoccupied 3d sublevel so
they can have more unpaired electrons in their configuration. This minimizes electron repulsions and is
therefore a more stable arrangement.
PTS: 1
DIF: III
REF: 3
OBJ: 2
172. ANS:
Nuclear charge is the attraction an atomic nucleus has on the electrons surrounding it. As you move from left
to right across a period, the atomic number increases, and therefore the number of protons in the nucleus
increases. The more protons within a nucleus, the greater is the nuclear charge. A greater nuclear charge pulls
the electrons closer to the nucleus, decreasing the atomic radius.
PTS: 1
DIF: II
REF: 3
OBJ: 2
173. ANS:
A nitrogen atom has five valence electrons. To have a complete octet of electrons, the nitrogen atom forms
three covalent bonds. It could form three single bonds, one single, and one double bond, or one triple bond.
PTS: 1
DIF: II
REF: 2
OBJ: 5
174. ANS:
The empirical formula is related to the molecular formula by the relationship x(empirical formula) =
molecular formula. The x is a whole-number factor by which the subscripts in the empirical formula must be
multiplied. The product is the correct molecular formula. In this case, x = 2.
PTS: 1
DIF:
I
REF: 4
OBJ: 4
PROBLEM
175. ANS:
4.821024Cl
Solution:
8.00 mol Cl 
PTS: 1
176. ANS:
4.821025 atoms Zr
Solution:
PTS: 1
DIF:
III
80.0 mol Zr 
DIF:
6.022  10 23 atoms Cl
= 4.82  10 24 atoms Cl
1 mol Cl
REF: 3
OBJ: 5
6.022 x 10 23 atoms Zr
= 4.82  10 25 atoms Zr
1 mol Zr
III
REF: 3
11
OBJ: 5
ID: A
177. ANS:
1.99 mol Pt
Solution:
PTS: 1
178. ANS:
18.4 mol Fe
Solution:
PTS: 1
179. ANS:
80.0 g O
Solution:
PTS: 1
180. ANS:
799 g Br
Solution:
PTS: 1
181. ANS:
2.50 mol He
Solution:
PTS: 1
182. ANS:
2.56 mol K
Solution:
1.20  1024 atoms Pt 
DIF:
1 mol Pt
= 1.99 mol Pt
6.022 × 10 23 atoms Pt
III
1.11  10 25 atoms Fe 
DIF:
III
III
10.0 mol Br ×
DIF:
DIF:
100 g K ×
1 mol Fe
= 18.4 mol Fe
6.022  10 23 atoms Fe
REF: 3
OBJ: 5
REF: 3
OBJ: 5
79.90 g Br
= 799 g Br
1 mol Br
III
10.0 g He ×
OBJ: 5
16.00 g O
= 80.0 g O
1 mol O
5.00 mol O ×
DIF:
REF: 3
REF: 3
OBJ: 5
1 mol He
= 2.50 mol He
4.00 g He
III
REF: 3
OBJ: 5
1 mol K
= 2.56 mol K
39.10 g K
PTS: 1
DIF: III
REF: 3
OBJ: 5
183. ANS:
3.2710-22 g/atom Au
196.97 g Au
1 mol Au
×
= 3.27 × 10 -22 g/atom Au
Solution:
23
1 mol Au
6.022 × 10
PTS: 1
DIF:
III
REF: 3
12
OBJ: 5
ID: A
184. ANS:
352 g K
Solution:
9.00 mol K ×
PTS: 1
185. ANS:
1.881023 atoms S
Solution:
DIF:
10.0 g S ×
39.10 g K
 352 g K
1 mol K
III
REF: 3
OBJ: 5
1 mol S
6.022 × 10 23 atoms S
×
= 1.88  10 23 atoms S
32.07 g S
1 mol S
PTS: 1
186. ANS:
1s2 2s2 2p3
DIF:
III
REF: 3
OBJ: 5
PTS: 1
187. ANS:
bromine
DIF:
III
REF: 3
OBJ: 3
PTS: 1
188. ANS:
[Ne] 3s2 3p2
DIF:
III
REF: 3
OBJ: 3
PTS: 1
189. ANS:
DIF:
III
REF: 3
OBJ: 3
PTS: 1
190. ANS:
DIF:
III
REF: 3
OBJ: 3
PTS: 1
DIF:
III
OBJ: 4-3.3
13
ID: A
191. ANS:
[Ne] 3s2 3p4
PTS: 1
192. ANS:
fluorine
DIF:
III
REF: 3
OBJ: 3
PTS: 1
DIF: III
REF: 3
193. ANS:
2 C atoms with 4 valence electrons  2  4  8
OBJ: 3
4 O atoms with 6 valence electrons  4  6  24
8  24  32 valence electrons
2  charge  2 extra electrons
32  2  34 electrons totals
PTS: 1
DIF: III
REF: 3
194. ANS:
1 C atom with 4 valence electrons  1  4  4
OBJ: 5
2 S atoms with 6 valence electrons  2  6  12
4  12  16 valence electrons
PTS: 1
195. ANS:
DIF:
III
REF: 3
OBJ: 5
DIF:
III
REF: 3
OBJ: 5
trigonal-planar
PTS: 1
14
ID: A
196. ANS:
δ-
δ+
PTS: 1
DIF: III
REF: 5
197. ANS:
83.98 g/mol AlF3
Solution:
26.98 g/mol Al + (3  19.00 g/mol F) = 89.3 g/mol AlF 3
OBJ: 5
PTS: 1
DIF: III
REF: 3
OBJ: 1
198. ANS:
159.62 g/mol CuSO4
Solution:
63.55 g/mol Cu + 32.07 g/mol S + (4  16.00 g/mol O) = 159.62 g/mol CuSO4
PTS: 1
DIF: III
REF: 3
OBJ: 1
199. ANS:
203.78 g/mol Fe2SiO4
Solution:
(2  55.85 g/mol Fe) + (28.08 g/mol Si) + (4  16.00 g/mol O) = 203.78 g/mol Fe2SiO4
PTS: 1
DIF: III
REF: 3
OBJ: 1
200. ANS:
101.96 g/mol Al2O3
Solution:
(2  26.98 g/mol Al) + (3  16.00 g/mol O) = 101.96 g/mol Al2O3
PTS: 1
DIF:
III
REF: 3
15
OBJ: 1
Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam.
[Answer Strip]
C
_____
6.
D 17.
_____
C 28.
_____
A 38.
_____
D 18.
_____
D 29.
_____
B 39.
_____
A 30.
_____
B 40.
_____
C 31.
_____
B 41.
_____
B
_____
7.
C 19.
_____
C
_____
8.
B 20.
_____
C 42.
_____
B
_____
9.
D 21.
_____
B 32.
_____
B 10.
_____
D 22.
_____
B
_____
1.
C 43.
_____
B 33.
_____
A 44.
_____
C 11.
_____
C 23.
_____
D
_____
2.
A 34.
_____
A 45.
_____
D 12.
_____
B 24.
_____
D 35.
_____
B
_____
3.
C 13.
_____
D 25.
_____
D 14.
_____
B 26.
_____
B 46.
_____
A 47.
_____
D
_____
4.
C 36.
_____
C 48.
_____
A 15.
_____
D
_____
5.
D 16.
_____
B 27.
_____
B 37.
_____
ID: A
Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam.
[Answer Strip]
C 49.
_____
B 55.
_____
A 65.
_____
C 76.
_____
A 87.
_____
A 77.
_____
D 88.
_____
C 78.
_____
C 89.
_____
A 56.
_____
C 66.
_____
C 57.
_____
A 67.
_____
A 79.
_____
A 90.
_____
C 58.
_____
C 68.
_____
D 80.
_____
D 91.
_____
C 59.
_____
A 69.
_____
A 60.
_____
C 70.
_____
C 50.
_____
C 81.
_____
A 51.
_____
C 92.
_____
D 61.
_____
B 52.
_____
C 71.
_____
C 72.
_____
C 82.
_____
D 93.
_____
A 62.
_____
C 73.
_____
D 53.
_____
A 83.
_____
C 94.
_____
B 63.
_____
C 74.
_____
D 84.
_____
B 95.
_____
C 54.
_____
D 75.
_____
B 85.
_____
B 96.
_____
B 64.
_____
B 86.
_____
ID: A
Chemistry 3100H Quarter 2 Semester Exam Study Guide And Practice Exam.
[Answer Strip]
B 97.
_____
D
_____109.
C
_____110.
A 98.
_____
B 99.
_____
A
_____111.
A
_____100.
B
_____112.
D
_____101.
A
_____113.
D
_____102.
A
_____103.
C
_____104.
D
_____105.
D
_____106.
A
_____107.
B
_____108.
ID: A