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Chemistry Fall 2014 Review
PART IV On the line to the left of each symbol, write the letter of the correct element name.
a. silicon
b. sodium
c. cobalt
d. iron
e. tin
f. tungsten
g. chlorine
h. gold
i. copper
j. silver
____ 1. W
____ 2. Cl
____ 3. Co
____ 4. Si
____ 5. Na
____ 6. Cu
____ 7. Fe
____ 8. Au
____ 9. Sn
Choose the best answer from the options that follow each question.
____ 10. A scientist is working in the lab, with compounds containing carbon. She is most likely working in the field
of
a. inorganic chemistry.
b. theoretical chemistry.
c. organic chemistry.
d. None of the above.
____ 11. The branch of chemistry called analytical chemistry most likely would be used in determining the
a. economic effects of a new substance.
b. chemical composition of a new substance.
c. effect of a chemical compound on living things.
d. uses of a particular metal.
____ 12. A scientist is working with mathematical and computer models to learn about the principles at work in a
chemical reaction. He is working in the field of
a. theoretical chemistry.
b. physical chemistry.
c. biochemistry.
d. analytical chemistry.
____ 13. Research that is carried out for the sake of increasing knowledge, such as research into the properties of a
substance, is considered to be
a. applied research.
b. basic research.
c. technological development.
d. none of the above.
____ 14. A scientist is working to improve a product that uses fiber optics. This is an example of
a. applied research.
b. basic research.
c. technological development.
d. both (a) and (c).
____ 15. To find a safer chemical for industrial purposes, a scientist is working with chemicals that do not cause
depletion of ozone in the atmosphere. This is an example of
a. green chemistry.
b. forensic chemistry.
c. pharmaceuticals.
d. alchemy.
____ 16. The smallest unit of matter that retains the properties of that matter is
a. a molecule.
b. a compound.
c. a mixture.
d. an atom.
____ 17. Which statement best describes an element?
a. any combination of two or more atoms of different types
b. a pure substance made up of only one kind of atom
c. a substance containing only carbon atoms
d. any kind of crystal
____ 18. Which of the following is an extensive property of matter?
a. boiling point
b. density
c. volume
d. melting point
____ 19. Which of the following is an intensive property of matter?
a. energy content
b. density
c. volume
d. mass
____ 20. Which of the following changes is a physical change of matter?
a. water evaporating
b. paper burning
c. a nail rusting
d. a silver spoon tarnishing
____ 21. Which state of matter is composed of atoms that have lost many of their electrons?
a. solid
b. liquid
c. gas
d. plasma
____ 22. Which of the following changes is a chemical change of matter?
a. ice melting to produce water
b. vinegar combining with baking soda to produce carbon dioxide
c. water boiling to produce water vapor
d. liquid silica solidifying to form glass
____ 23. A homogeneous mixture is one that
a. contains only one element.
b. is uniform in composition.
c. cannot change state easily.
d. acts as a solvent.
____ 24. Which of the following is an example of a heterogeneous mixture?
a. tap water
b. chunky peanut butter
c. orange-colored sugar water
d. gold ring
____ 25. What is the difference between a mixture and a compound?
a. All mixtures have a uniform composition.
b. Mixtures can be separated by physical processes.
c. Mixtures are made of at least two different elements.
d. All mixtures are heterogeneous.
____ 26. Which of the following is a pure substance?
a. air
b. granite
c. water
d. stainless steel
____ 27. Homogeneous mixtures are also called
a. atoms.
b. solutions.
c. molecules.
d. compounds.
____ 28. One way to separate the different kinds of matter in a mixture is through
a. filtration.
b. decomposition.
c. electrolysis.
d. chemical reactions.
____ 29. In general, which properties are common to elements within a single group on the periodic table?
a. atomic number and atomic weight
b. chemical properties and ability to bond to other atoms
c. color and luster
d. boiling point and freezing point
____ 30. The horizontal rows of the periodic table are called
a. periods.
b. columns.
c. groups.
d. families.
____ 31. Which property would be least helpful in determining whether a substance is a metal or a nonmetal?
a. conductivity
b. luster
c. ductility
d. state
____ 32. Noble gases are generally
a. semiconductors.
b. malleable.
c. brittle.
d. unreactive.
____ 33. Which is an example of a nonmetal?
a. copper
b. phosphorus
c. mercury
d. cadmium
____ 34. An element near argon in the periodic table would probably be
a. a good electrical conductor.
b. a poor heat conductor.
c. solid at room temperature.
d. shiny and malleable.
____ 35. In an experiment, onion plants of different ages were exposed to various amounts of caffeine to determine the
effect of caffeine on cell growth. Temperature, amount of water, and light were kept constant. Which of these
statements about the experiment is definitely true?
a. The results may not be valid because there were two variables.
b. The amount of caffeine used was a control.
c. Temperature, water, and light were the only variables.
d. Onion plants can be used to model the effects of caffeine on living things.
____ 36. Which of these is the variable in an experiment designed to determine whether steel rusts more quickly near a
lake or in a desert in one year?
a. amount of rust
b. time of exposure
c. amount of water in the air
d. mass of the steel
____ 37. Which of these recorded observations is qualitative, rather than quantitative?
a. A chemical reaction is complete in 2.3 s.
b. The solid has a mass of 23.4 g.
c. The compound melts at 87.5°C.
d. Iron is denser than aluminum.
____ 38. Which of these statements is true of the scientific method?
a. The steps may vary somewhat to suit the experiment.
b. Working scientists rarely use it.
c. Scientists must follow its steps exactly.
d. Scientists rarely publish results of experiments.
____ 39. Theories are considered successful only if they
a. can be used to make accurate predictions.
b. can be stated in simple terms.
c. can be written in the form of an equation.
d. have been accepted by all scientists.
____ 40. An experiment is designed to measure the effect of global temperature increase on ocean levels. In this
experiment, if the ocean level is compared to the average ocean level over the last 100 years, then the average
ocean level over the last 100 years would be considered
a. a model.
b. a variable.
c. the hypothesis.
d. the control.
____ 41. The unit cm3 is used to express
a. length.
b. mass.
c. volume.
d. time.
____ 42. The SI base units for time and temperature are
a. hour and degree Celsius.
b. second and degree Celsius.
c. hour and kelvin.
d. second and kelvin.
____ 43. Which of these shows SI unit prefixes arranged in order from smallest to largest?
a. centi, milli, kilo
b. milli, centi, kilo
c. kilo, milli, centi
d. kilo, centi, milli
____ 44. The conversion factor would be used to change
a. milliliters to liters.
b. liters to milliliters.
c. units of volume to units of length.
d. units of length to units of volume.
____ 45. A sample of bismuth has a mass of 343 g and a volume of 35.0 cm3.
What is the density of bismuth?
a. 0.102 g/cm3
b. 9.80 g/cm3
c. 378 g/cm3
d. 1.20 104 g/cm
3
____ 46. Which of these statements about density is true?
a. Density is proportional to the amount of a substance.
b. Density is expressed in units of mL/cm3.
c. Density does not change with temperature.
d. Density may be used to help identify a material.
____ 47. An object’s weight is a measure of
a. the force with which it is attracted by gravity.
b. the pressure exerted on a scale.
c. the amount of material per unit volume.
d. the force causing the object to move.
____ 48. The SI base unit for mass is the
a. gram.
b. cubic centimeter.
c. meter.
d. kilogram.
____ 49. Which of these is not an SI base unit?
a. meter
b. pound
c. kelvin
d. ampere
____ 50. Precision is related to all of these except
a. reproducibility of measurements.
b. range of measurement values.
c. number of significant figures.
d. closeness of a measurement to the accepted value.
____ 51. A student determined the density of aluminum by averaging the results of three density calculations. Each
value was different, but the average was equal to the accepted value for aluminum’s density. The results of
this investigation are best described as
a. accurate, but not precise.
b. precise, but not accurate.
c. both precise and accurate.
d. neither precise nor accurate.
____ 52. The measurement 0.0265 g, rounded off to two significant figures, would be
a. 0.026 g.
b. 0.027 g.
c. 0.03 g.
d. 0.030 g.
____ 53. In division and multiplication, the answer should have the same number of significant figures as the
a. number in the calculation with the fewest significant figures.
b. number in the calculation with the most significant figures.
c. average number of significant figures in the calculation.
d. total number of significant figures in the calculation.
____ 54. The number of significant figures in the measurement 170.040 km is
a. three.
b. four.
c. five.
d. six.
____ 55. The dimensions of rectangular solid are measured to be 1.27 cm, 1.3 cm, and 2.5 cm. The volume should be
recorded as
a. 4.128 cm3.
b. 4.12 cm3.
c. 4.13 cm3.
d. 4.1 cm3.
____ 56. Samples with masses of 0.12 g, 1.8 g, and 0.562 g are mixed together. The combined mass of the three
samples, expressed to the correct number of significant figures, should be recorded as
a. 2.4 g.
b. 2.48 g.
c. 2.482 g.
d. 2.5 g.
____ 57. Expressed in scientific notation, 0.0930 m is
a. 93 10-3
m.
b. 9.3 10-3
m.
c. 9.30 10-2
m.
d. 9.30 10-4
m.
____ 58. When 6.02 1023
is multiplied by 9.1 10-31
, the product is
a. 5.5 10-8
.
b. 5.5 1055
.
c. 5.5 10-7
.
d. 5.5 10-53
.
____ 59. Chemistry is a natural science that deals with the study of
a. living things and their life processes.
b. the physical features of Earth.
c. the composition, structure, properties, and changes of matter.
d. the composition, motion, and relative positions of stars and planets.
____ 60. The branch of chemistry in which the compositions of materials are identified is known as
a. biochemistry.
b. organic chemistry.
c. physical chemistry.
d. analytical chemistry.
____ 61. Which of these is an example of an extensive property?
a. mass
b. density
c. color
d. boiling point
____ 62. Which of these is an example of an element?
a. sugar
b. soil
c. water
d. oxygen
____ 63. Which of these is an example of a heterogeneous mixture?
a. salt
b. nitrogen
c. mud
d. air
____ 64. Which process is a chemical change?
a. heating to boiling
b. dissolving in alcohol
c. burning in air
d. slicing into two pieces
____ 65. At sea level, water boils at 100°C. This is an example of a(n)
a. chemical property.
b. extensive property.
c. physical property.
d. chemical change.
____ 66. Every pure chemical compound consists of two or more elements that
a. are combined chemically.
b. can be separated by a physical change.
c. cannot be separated.
d. are combined in any proportion.
____ 67. The study of the composition, structure, and properties of matter; the processes that matter undergoes; and the
energy changes that accompany those processes best describes the science of
a. biology.
b. physics.
c. astronomy.
d. chemistry.
____ 68. The branch of chemistry that involves the study of substances and processes occurring in living things is
called
a. biochemistry.
b. organic chemistry.
c. physical chemistry.
d. theoretical chemistry.
____ 69. The branch of chemistry that deals with substances containing carbon is called
a. biochemistry.
b. organic chemistry.
c. physical chemistry.
d. analytical chemistry.
____ 70. Using mathematical models and computer models to understand a chemical principle is an example of
a. biochemistry.
b. physical chemistry.
c. analytical chemistry.
d. theoretical chemistry.
____ 71. A team of scientists is analyzing evidence from a crime scene and keeping records that might be used in court.
The best description of their work is
a. forensic chemistry.
b. green chemistry.
c. pharmeceutical chemistry.
d. alchemy.
____ 72. Two chemistry students are investigating the properties of quartz crystals. They are most likely studying in
the field of
a. biochemistry.
b. physical chemistry.
c. organic chemistry.
d. inorganic chemistry.
____ 73. The definition of a chemical is
a. a toxic substance made in a laboratory.
b. an unnatural material added to foods.
c. any substance that has a definite composition.
d. anything that has mass and takes up space.
____ 74. The goal of basic research is to
a. find a solution to a particular problem.
b. produce new chemicals.
c. increase knowledge.
d. discover new technologies.
____ 75. A scientist is working on developing refrigerants that do not release chemicals that destroy the ozone layer.
This is best described as an example of
a. basic research.
b. applied research.
c. technological development.
d. biochemistry.
____ 76. Technological applications often
a. occur by accident.
b. degrade our quality of life.
c. lag far behind basic and applied research.
d. have little effect on our lives.
____ 77. Mass is a measurement of
a. how much space an object occupies.
b. how dense an object is.
c. the amount of matter in an object.
d. the volume of an object.
____ 78. The fundamental building block of matter is the
a. atom.
b. molecule.
c. cell.
d. proton.
____ 79. An element is made of one type of
a. molecule.
b. atom.
c. compound.
d. mixture.
____ 80. A compound is
a. a substance that is composed of two or more elements that are chemically bonded.
b. a molecule formed by atoms of the same element.
c. another word for an atom.
d. any substance that can be split apart.
____ 81. Extensive properties
a. include boiling point.
b. do not depend on the amount of matter present.
c. include volume and mass.
d. all depend on the chemical composition of the matter present.
____ 82. Which of the following is an intensive property of matter?
a. volume
b. mass
c. energy content
d. density
____ 83. A change in a substance that does not involve a change in the identity of the substance is called a(n)
a. chemical change.
b. physical change.
c. extensive property.
d. intensive property.
____ 84. In every chemical change, two or more reactants form at least one
a. product.
b. gas.
c. precipitate.
d. reaction.
____ 85. Which is not true about the liquid state of matter?
a. The liquid state has a definite volume and a definite shape.
b. The liquid state takes on the shape of its container.
c. The liquid state has a definite volume and an indefinite shape.
d. The particles in a liquid can easily move past each other.
____ 86. If a mixture is uniform in composition, it is considered to be
a. heterogeneous.
b. molecular.
c. homogeneous.
d. elemental.
____ 87. All known elements are organized into a chart known as the
a. element table.
b. group table.
c. periodic table.
d. metal-nonmetal table.
____ 88. The vertical columns of the periodic table are called
a. periods.
b. rows.
c. groups.
d. chemicals.
____ 89. A period is
a. a horizontal row of elements in the periodic table.
b. a vertical column of elements in the periodic table.
c. a region of two or more columns in the periodic table.
d. another name for the periodic table.
____ 90. Which of the following is not a property of metals?
a. malleability
b. good electrical conductivity
c. brittleness
d. good heat conductivity
____ 91. Metalloids lie between metals and nonmetals on the periodic table. They tend to be
a. nonconductors.
b. conductors.
c. semiconductors.
d. unreactive.
____ 92. The “shininess” of a metal is called its
a. luster.
b. color.
c. streak.
d. malleability.
____ 93. The element carbon is classified as a
a. metal.
b. nonmetal.
c. metalloid.
d. noble gas.
____ 94. Which of the following is not true of nonmetals?
a. Many are gases.
b. Many are ductile.
c. As solids, they tend to be brittle.
d. Most are poor heat and electrical conductors.
____ 95. Which of the following elements is a metalloid?
a. neon
b. selenium
c. mercury
d. silicon
____ 96. Which of these describes noble gases?
a. massless
b. unreactive
c. good heat conductors
d. good electrical conductors
____ 97. Which of the following is not a stage of the scientific method?
a. using a hypothesis to sell a new product
b. observing, collecting, and communicating data
c. formulating theories
d. formulating hypotheses
____ 98. By making several measurements of a sample with the same balance, a chemist obtained values of 5.224 g,
5.235 g, and 5.259 g for the mass of a sample. Without knowing the actual mass of the sample, we can tell
that these measurements have
a. high precision.
b. high accuracy.
c. low precision.
d. low accuracy.
____ 99. Which equation represents an inverse proportion between the variables?
a.
b. c. d.
____ 100. The average distance between the sun and Earth is about 150 million km. Light travels at a speed of
m/s. Dividing the distance by the speed and then multiplying by the number of meters in a kilometer will
result in units of
a. seconds.
b. meters per second.
c. kilometers squared.
d. kilometers per second.
____ 101. If some measurements agree closely with each other but differ widely from the actual value, these
measurements are
a. both accurate and precise.
b. neither precise nor accurate.
c. precise but not accurate.
d. accurate but not precise.
____ 102. In which of the following measurements are all the zeros considered to be nonsignificant figures?
a. 506 mL
b. 60.0 mL
c. 0.0037 mL
d. 400. mL
____ 103. If two quantities are directly proportional and one quantity increases by 10%, the other
a. increases by 10%.
b. decreases by 10%.
c. increases by 90%.
d. decreases by 90%.
____ 104. In division and multiplication, the answer must have the same number of significant figures as the
a. number in the calculation with the fewest significant figures.
b. number in the calculation with the most significant figures.
c. average number of significant figures in the problem.
d. total number of significant figures in the problem.
____ 105. Which of these observations is qualitative rather than quantitative?
a. A chemical reaction is complete in 2.3 s.
b. The solid has a mass of 23.4 g.
c. The density of aluminum is 2.70 g/cm3.
d. Salt deposits form from an evaporated liquid.
____ 106. All of the following are steps in the scientific method except
a. observing and recording data.
b. forming a hypothesis.
c. discarding data inconsistent with the hypothesis.
d. making predictions based on a theory.
____ 107. Which of these statements about the scientific method is not true?
a. All experiments must follow the same step-by-step procedure.
b. Experiments may be repeated several times.
c. Some unexpected results can be beneficial.
d. Experimental results may or may not support the hypothesis.
____ 108. Ten plants are grown in equal amounts of sunlight with equal amounts of water and varying amounts of
fertilizer. Sunlight and water are
a. variables.
b. experiments.
c. systems.
d. controls.
____ 109. An experiment was designed to measure the effect of sulfur dioxide emissions from a power plant on the pH
of rain falling downwind of the plant. In this experiment, the average pH of rainwater upwind from the plant
would be considered
a. a model.
b. a variable.
c. the hypothesis.
d. the control.
____ 110. Which of these best describes a scientific model?
a. a small version of a large object
b. the most recent version of a theory
c. a way of explaining a complex concept
d. a detailed description of a natural event
____ 111. A proposed explanation that is based on observations and that can be tested is known as a(n)
a. principle.
b. experiment.
c. law.
d. hypothesis.
____ 112. For each investigation, the scientific method
a. requires that the same set of procedures be followed.
b. provides a logical set of procedures.
c. is abandoned if there are unexpected results.
d. helps to predict the results.
____ 113. A theory is likely to be revised as the explanation of an observed phenomenon when
a. one study contradicts the theory.
b. repeated observations conflict with the theory.
c. a new method is used to gather data.
d. a leading scientist feels that it is invalid.
____ 114. The unit m3 is used to express
a. length.
b. mass.
c. volume.
d. density.
____ 115. SI base units for length and mass are
a. centimeter and gram.
b. meter and gram.
c. centimeter and kilogram.
d. meter and kilogram.
____ 116. The abbreviations for units of length in order from smallest to largest are
a. m, cm, mm, km.
b. mm, m, cm, km.
c. km, mm, cm, m.
d. mm, cm, m, km.
____ 117. The conversion factor would be used to change
a. mass to density.
b. liters to milliliters.
c. units of volume to units of length.
d. units of length to units of volume.
____ 118. A measure of the quantity of matter is
a. density.
b. weight.
c. volume.
d. mass.
____ 119. All of the following are examples of units except
a. weight.
b. kilometer.
c. gram.
d. teaspoon.
____ 120. Which of these abbreviations represents a volume unit?
a. mL
b. mg
c. mm
d. mm
____ 121. The metric unit for length that is closest to the thickness of a dime is the
a. micrometer.
b. millimeter.
c. centimeter.
d. decimeter.
____ 122. One cubic centimeter is equivalent to
a. 1 milliliter.
b. 1 gram.
c. 1 liter.
d. 1 kilogram.
____ 123. The relationship between the mass m of a material, its volume V, and its density D is
a. V = mD.
b. Vm = D.
c. m = DV.
d. D + V = m.
____ 124. A chemical reaction was carried out three times. The mass of the product was 8.93 g for the first trial, 8.94 g
for the second trial, and 8.92 g for the third trial. Under the conditions of the experiment, the reaction is
known to yield 8.60 g of product. The three mass values measured are
a. accurate.
b. precise.
c. both accurate and precise.
d. neither accurate nor precise.
____ 125. For numbers less than 0.1, such as 0.06, the zeros to the right of the decimal point but before the first nonzero
digit
a. are significant.
b. show the decimal place of the first digit.
c. show that the zero on the left side of the decimal is not significant.
d. are always uncertain.
____ 126. The number of significant figures in the measurement 0.000 305 kg is
a. two.
b. three.
c. six.
d. seven.
____ 127. When the difference between a measured value and the known value is expressed as percentage error, it is
usually written as
a. a positive number.
b. a negative number.
c. both positive and negative.
d. either a negative number or a positive number.
____ 128. A measurement is accurate if it
a. is reproducible.
b. is close to the true value.
c. has many decimal places.
d. has many significant figures.
____ 129. To determine the number of significant digits in a measurement, follow the rule that
a. all zeros are significant.
b. all nonzero digits are significant.
c. zeros between digits are not significant.
d. final digits less than 5 are not significant.
____ 130. The measurement 0.0255 g, rounded off to two significant figures, would be
a. 0.02 g.
b. 0.025 g.
c. 0.026 g.
d. 2.5 102 g.
____ 131. What is 1 102 divided by 1 10
-3?
a. 1 10-6
b. 1 10-1
c.
1 100
d. 1 105
____ 132. What is the sum of 100.0 g and 0.01 g, expressed in scientific notation and written with the correct number of
significant figures?
a. 10 001 10-2
g
b. 1.0 102 g
c. 1.000 102 g
d. 1.00 102 g
Choose the best answer from the options that follow each question. For calculations that require the
atomic mass of an element, round the atomic mass found on the periodic table to two decimal places.
____ 133. What follows an element’s symbol in a chemical formula to indicate the number of atoms of that element in
one molecule of the compound?
a. charge sign
b. superscripted number
c. number in parentheses
d. subscripted number
____ 134. The chemical formula for an ionic compound represents one
a. formula unit.
b. ion.
c. molecule.
d. cation.
____ 135. What is the correct notation for a calcium ion whose outer shell is a full octet?
a. Ca1+
b. Ca2+
c. Ca1-
d. Ca2-
____ 136. What is the correct name for the NO ion?
a. nitrate
b. nitrite
c. nitride
d. nitrogen oxide
____ 137. What is the correct formula for copper(I) cyanide?
a. CuCy
b. CuCy2
c. CuCN
d. Cu2CN
____ 138. What is the correct name for the acid CH3COOH?
a. carbonic acid
b. carbonate acid
c. acetic acid
d. acetous acid
____ 139. What is the correct name for the compound P2Cl4?
a. phosphorus chloride
b. phosphorus tetrachloride
c. diphosphorus chloride
d. diphosphorus tetrachloride
____ 140. What is the correct formula for the compound made of magnesium and nitrogen?
a. Mg2N3
b. Mg3N2
c. MgN2
d. MgN
____ 141. Oxidation numbers are used to indicate the
a. charge on an ion.
b. number of atoms or ions in a compound.
c. type of bond holding particles together in a compound.
d. distribution of electrons among the bonded particles in a compound.
____ 142. Atoms have an oxidation number of zero in a(n)
a. pure element.
b. acid.
c. ionic compound.
d. molecular compound.
____ 143. What is the oxidation number of nickel in NiCO3?
a. 0
b. 1
c. 2
d. 3
____ 144. What is the correct name for the compound Ni2O3 using the Stock system?
a. nickel(II) oxide
b. dinickel trioxide
c. nickel trioxide
d. nickel(III) oxide
____ 145. What is the oxidation number of phosphorus in the PO ion?
a. -3
b. 0
c. 5
d. 8
____ 146. What is the correct formula for the compound platinum(VI) fluoride?
a. PtF3
b. PtF6
c. Pt6F2
d. Pt6F
____ 147. The formula mass of any compound is described in units of
a. grams.
b. u.
c. moles.
d. grams per mole.
____ 148. The molar mass of water is equal to
a. 1 g of O plus 2 g of H.
b. 1 g of O plus 1 g of H.
c. the mass of 1 mol of O plus the mass of 1 mol of H.
d. the mass of 1 mol of O plus the mass of 2 mol of H.
____ 149. What is the molar mass of pure tin?
a. 1.00 g/mol
b. 47.88 g/mol
c. 118.71 g/mol
d. 237.42 g/mol
____ 150. How many moles of compound are there in 15.0 g of potassium dichromate, K2Cr2O7? (The molar mass of
K2Cr2O7 is 294.2 g.)
a. 0.0510 mol
b. 11.0 mol
c. 15.0 mol
d. 294 mol
____ 151. What is the mass percentage of cobalt in cobalt(II) fluoride, CoF2?
a. 33.33%
b. 39.20%
c. 60.80%
d. 96.93%
____ 152. What is the mass of 4.80 mol of barium hydride, BaH2?
a. 4.80 g
b. 29.0 g
c. 139 g
d. 669 g
____ 153. The simplest whole-number ratio of moles of each element in a compound is known as the
a. percent composition.
b. empirical formula.
c. Stock formula.
d. molecular formula.
____ 154. What is the empirical formula for a compound that contains 12.62% Li, 29.17% S, and 58.21% O?
a. LiSO2
b. LiS2O6
c. Li2SO4
d. Li2SO3
____ 155. What is the molecular formula for the compound with a formula mass of 58.12 u and an empirical formula of
C2H5?
a. C2H5
b. C4H10
c. C6H15
d. C8H20
____ 156. What is the molecular formula for the compound that is made up of 30.45 g N and 69.55 g O, and has a
formula mass of 92.02 u?
a. NO
b. N2O2
c. NO2
d. N2O4
PART I Choose the best answer from the options that follow each question.
____ 157. Changing a subscript in a correctly written chemical formula will
a. change the electron configuration of that element.
b. change the charges on the other ions in the compound.
c. change the formula so that it no longer represents the same compound.
d. have no effect on the formula.
____ 158. Using the Stock system of nomenclature, Cr2(SO4)3 is named
a. chromium(II) sulfate.
b. chromic sulfate.
c. dichromium trisulfate.
d. chromium(III) sulfate.
____ 159. In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to
a. 0.
b. 10.
c. the number of atoms in the ion.
d. the charge on the ion.
____ 160. The first part of the name of a binary ionic compound is the
a. cation.
b. polyatomic ion.
c. oxyanion.
d. anion.
____ 161. The formula for phosphoric acid is
a. HPO4.
b. H(PO4)2.
c. H2PO3.
d. H3PO4.
____ 162. The term formula mass can be applied to both ionic compounds and molecular compounds because
a. ionic compounds exist as individual molecules.
b. not all molecular formulas are empirical formulas.
c. not all formulas represent individual molecules.
d. all molecular formulas are Lewis formulas.
____ 163. To determine the correct molecular formula of a compound from an empirical formula, one must determine
the
a. density.
b. formula mass.
c. structural formula.
d. crystal lattice.
____ 164. An ion of bromine with a single negative charge has the symbol and the name
a. Br+, bromide ion.
b. Br-, bromide ion.
c. Br+, bromium ion.
d. Br-, bromium ion.
____ 165. The platinum(II) ion and the platinum(IV) ion
a. are anions.
b. are polyatomic ions.
c. have charges of 2+and 4+, respectively.
d. have charges of 1+ and 3+, respectively.
____ 166. What is the name of the compound made of zinc ions, Zn2+
, and fluoride ions, F-?
a. zinc difluoride
b. zinc fluorate
c. zinc fluoride
d. zinc(II) fluorite
____ 167. What is the chemical formula for the compound made of tin(IV) ions and chloride, Cl-, ions?
a. SnCl4
b. Sn2Cl2
c. SnCl2
d. Sn4Cl
____ 168. What is the formula for the compound made of aluminum ions, Al3+
, and sulfate ions, SO-?
a. AlSO4
b. Al3SO4
c. Al(SO4)3
d. Al2(SO4)3
____ 169. How many atoms are present in one formula unit of barium acetate, Ba(C2H3O2)2?
a. 4
b. 8
c. 15
d. 16
____ 170. What is the formula for the compound dinitrogen tetroxide?
a. N2O3
b. N2O4
c. N3O2
d. N3O4
____ 171. The term acid usually refers to
a. a solution of the acid compound in water.
b. only the acid compound.
c. a compound containing hydrogen.
d. a compound containing hydrogen and oxygen.
____ 172. What is the formula for carbonic acid?
a. CH3COOH
b. HClO3
c. CH4
d. H2CO3
____ 173. The salt calcium nitrate, Ca(NO3)2, contains the anion from
a. calcium.
b. nitrogen.
c. nitric acid.
d. nitrous acid.
____ 174. An oxidation number
a. is always negative.
b. is always positive.
c. has no exact physical meaning.
d. is the same in each compound that an element forms.
____ 175. Which element has the same oxidation number in all of its compounds?
a. oxygen
b. fluorine
c. hydrogen
d. chlorine
____ 176. What is the oxidation number of an atom of nitrogen in the compound N2?
a. 0
b. +3
c. -3
d. -6
____ 177. What is the oxidation number of phosphorus in H3PO4?
a. +1
b. +4
c. +5
d. +8
____ 178. What is the correct Stock name for Cr(CH3COO)3
a. chromium acetate
b. chromium triacetate
c. trichromium acetate
d. chromium(III) acetate
____ 179. What is the correct prefix-based name for selenium(II) fluoride?
a. selenium fluoride
b. diselenium fluoride
c. diselenium difluoride
d. selenium difluoride
____ 180. What is the formula for copper(I) oxide?
a. CuO
b. Cu2O
c. CuO2
d. Cu2O2
____ 181. A monatomic ion has an oxidation number
a. of zero.
b. indicated by the ion’s prefix.
c. equal to the charge of the ion.
d. equal to its subscript.
____ 182. What is the correct Stock name for SnBr4?
a. tin(IV) bromide
b. tin bromide
c. tin tetrabromide
d. tin(IV) tetrabromide.
____ 183. The mass of a molecule is found by
a. adding the masses of all the atoms in the molecule.
b. dividing the total mass of all the atoms in the molecule by 6.022 1023
.
c. multiplying the total mass of all the atoms in the molecule by 6.022 1023
.
d. dividing the total mass of all the atoms in the molecule by the total number of atoms.
____ 184. For any molecule, formula unit, or ion, the sum of the average atomic masses of all the atoms represented in a
formula is the
a. formula mass.
b. ionic mass.
c. molecular mass.
d. atomic mass.
____ 185. What is the correct formula mass for zinc hydroxide, Zn(OH)2?
a. 83.41 g
b. 99.41 g
c. 83.41 u
d. 99.41 u
____ 186. One mole of potassium atoms has a mass of
a. 1 g.
b. 39.10 g.
c. 78.20 g.
d. 6.022 1023
g.
____ 187. A compound’s molar mass is numerically equal to
a. the total number of atoms in the molecule.
b. the total number of moles of the compound.
c. its mass number.
d. its formula mass.
____ 188. How many total moles of atoms are there in one mole of silver(I) phosphate, Ag3PO4?
a. 3
b. 7
c. 8
d. 11
____ 189. What is the correct molar mass of Ag3PO4?
a. 418.58 g/mol
b. 387.61 g/mol
c. 154.84 g/mol
d. 52.32 g/mol
____ 190. Which statement shows how to correctly convert from the mass of a compound in grams to the amount of that
compound in moles?
a. molar mass (g/mol) = amount (moles)
b. molar mass (g/mol) 6.022 1023
= amount (moles)
c. mass (grams) = amount (moles)
d. mass (grams) molar mass (g/mol) = amount (moles)
____ 191. The percentage composition of a compound is
a. the percentage by volume of each element in the compound.
b. the percentage by mass of each element in the compound.
c. the molar mass of the compound the mass of each element in 1 mol of the compound.
d. the mass of each element in 1 mol of the compound the molar mass of the compound.
____ 192. What is the percentage of iron in iron(III) chloride, FeCl3? The molar mass of FeCl3 is 162.2 g/mol.
a. 25.00%
b. 34.43%
c. 61.17%
d. 65.57%
____ 193. The smallest whole-number ratio of atoms of each element, combined in the simplest unit of a chemical
compound is known as a(n)
a. molecular formula.
b. formula unit.
c. empirical formula.
d. molecule.
____ 194. What is the empirical formula for benzene, C6H6?
a. CH
b. C2H2
c. C3H3
d. C6H6
____ 195. What other information do you need in order to determine the molecular formula from the empirical formula
of a compound?
a. the number of moles of the compound
b. the formula mass of the compound
c. the oxidation numbers of all the elements in the compound
d. the smallest whole-number mole ratio of the atoms in the compound
____ 196. What is the empirical formula for a compound that contains 1.18 mol Na, 1.18 mol N, and 3.53 mol O?
a. NaNO
b. NaNO2
c. Na2NO
d. NaNO3
____ 197. What is the empirical formula for a compound that contains 83.01% K and 16.98% O by mass?
a. KO
b. KO2
c. K2O
d. K5O
____ 198. What is the empirical formula of a compound that contains 79.86% I and 20.14% O by mass?
a. IO
b. I2O2
c. IO2
d. I4O
____ 199. What is the empirical formula for lactic acid, which has a molecular formula of C3H6O3?
a. CH2O
b. C2H3O2
c. C3H6O3
d. CHO
____ 200. NaCl is
a. a molecular formula only.
b. an empirical formula only.
c. both an empirical formula and a chemical formula.
d. both a molecular formula and an emipirical formula.
____ 201. What is the empirical formula mass of the compound C2H4?
a. 13.02 g
b. 14.03 g
c. 26.04 g
d. 28.05 g
____ 202. What is the molecular formula for the compound with an empirical formula of NO2 and a formula mass of
92.02 u?
a. NO2
b. N2O4
c. N4O8
d. NO
PART VI Write the answers to the following questions on separate paper.
203. Explain the differences between solid, liquid, and gaseous states in terms of the arrangement of the particles.
204. Contrast mixtures and pure substances.
205. State the law of conservation of energy.
206. Contrast heterogeneous and homogeneous mixtures.
207. List several ways to test an advertisement's claim that a cleaning product is safe for the environment.
208. How does a theory differ from a hypothesis?
209. How does weight differ from mass?
210. What is a model and what is the function of models in science?
211. Sketch the graph of two quantities, y and x, that are directly proportional to one another and sketch the graph
of two quantities that are inversely proportional to each other. Label, title, and identify each graph.
PART VI Write the answers to the questions on separate paper, and show your work. Express each
answer to the correct number of significant digits.
212. The mass of a 5.00 cm3 sample of clay is 11.0 g. What is the density of the clay?
213. A length measurement is 1.40 cm. The correct value is 1.36 cm. Calculate the percentage error.
214. The density of lead is 11.35 g/cm3. What is the mass of a piece of lead with a volume of 10.0 cm
3?
215. What is the volume in liters of a cube whose edge is 4.33 cm long?
216. What is the sum of 3.089 g and 0.074 52 g?
PART II
Write the oxidation number for the given element in the space provided.
217. Sulfur in H2SO4
218. Oxygen in peroxides
219. Magnesium in MgO
220. Silicon in SiCl4
Write the formulas for the following compounds in the space provided.
221. Silicon dioxide
222. Carbon tetriodide
223. Tin(IV) chromate
224. Barium hydroxide
Write the names of the following compounds in the space provided. Use the Stock system or prefixes, as
indicated.
225. PI3
226. N2O4
227. Fe(NO2)2
228. CCl4
229. CO
230. CuCO3
Write the formulas and give the names of the compounds formed by the following ions in the space
provided.
231. Ca2+
and Cl
232. Pb2+
and CrO
233. Al3+
and SO
234. Sn4+
and PO
Name each of the following ions in the space provided.
235. CN
236. O2
237. OH
Write the formulas and indicate the charges for the following ions in the space provided.
238. sulfide ion
239. copper(I) ion
Write each atom and its oxidation number in the space provided.
240. carbonate ion
241. H2O2
242. CO
243. NH
