Survey of Chemistry Exam Practice Tests
Course Introduction
Survey of Chemistry provides a comprehensive introduction to the fundamental principles of chemistry for students pursuing diverse academic paths. The course covers essential topics such as atomic structure, chemical bonding, stoichiometry, states of matter, solutions, acids and bases, chemical reactions, and basic thermodynamics. Emphasis is placed on the relevance of chemistry in everyday life and its connections to other scientific disciplines. Through lectures, discussions, and laboratory experiments, students develop critical thinking skills and gain hands-on experience with chemical concepts, preparing them for advanced study or informed citizenship in a technologically driven world.
Recommended Textbook
Introductory Chemistry 4th Edition by Steve Russo
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18 Chapters
1785 Verified Questions
1785 Flashcards
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Page 2
Chapter 1: What Is Chemistry
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46 Verified Questions
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Sample Questions
Q1) When milk goes "sour," only a physical change has occurred.
A)True
B)False
Answer: False
Q2) Which of the following is an example of a heterogeneous mixture?
A)seawater
B)steel
C)milk
D)chicken noodle soup
Answer: D
Q3) The earth, taken together as a unit, may be considered one very large piece of heterogeneous matter.
A)True
B)False
Answer: True
Q4) Iced tea, with sugar completely dissolved in it, is an example of homogeneous matter.
A)True
B)False
Answer: True
Page 3
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Chapter 2: The Numerical Side of Chemistry
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140 Flashcards
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Sample Questions
Q1) What is the symbol and name borrowed from Greek which signifies one thousand? Answer: k, for kilo
Q2) If the speed limit is 120 km/hr, its equivalent in mi/hr is ________.
A)75
B)192
C)133
D)210
Answer: A
Q3) For the final sum of 544.36 + 455.64, the number of significant figures is ________.
A)6
B)5
C)4
D)2
E)1 Answer: A
Q4) Oil "floats" on water because oil weighs less than water.
A)True
B)False Answer: False
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Chapter 3: The Evolution of Atomic Theory
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87 Flashcards
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Sample Questions
Q1) According to the experiments of Ernest Rutherford, where can a majority of a given atom's mass be found?
A)scattered randomly throughout an approximately cube-shaped atom
B)at the center of an approximately spherical atom
C)in concentric layers of spherical shape
D)as small pieces orbiting a common center in circular paths
Answer: B
Q2) What is the mass of the single product that is formed from the reaction between 2.5 g hydrogen and 7.5 g oxygen?
A)5.0 g
B)7.5 g
C)9.5 g
D)10.0 g
Answer: D
Q3) Which of the following is a transition element?
A)Co
B)Eu
C)Es
D)He
Answer: A
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Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) Which of the following does not include [Kr] in its shorthand electron configuration?
A)Sr<sup>2+</sup>
B)Te<sup>2-</sup>
C)Se<sup>6+</sup>
D)Mo
Q2) Blue visible light is of lower energy than red visible light.
A)True
B)False
Q3) Below are four pairs of atoms and ions. In which pair is the larger of the two species written first?
A)S<sup>2-</sup> and S
B)Cu<sup>2+</sup> and Cu
C)O and O<sup>2-</sup>
D)Cr<sup>3+</sup> and Cr
Q4) The correct order of increasing energy in the following subshells is:
A)2p, 3s, 4s, 3p, 3d
B)2p, 3s, 3p, 4s, 3d
C)2p, 3s, 3p, 3d, 4s
D)2p, 3s, 3d, 3p, 4s
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Chapter 5: Chemical Bonding and Nomenclature
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230 Verified Questions
230 Flashcards
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Sample Questions
Q1) Which of the following does not have a charge of -1?
A)bicarbonate
B)bisulfate
C)hydrogen phosphate
D)nitrite
Q2) What is the chemical formula of the compound named potassium bicarbonate?
A)KHCO<sub>3</sub>
B)K<sub>2</sub>(HCO<sub>3</sub>)
C)K(HCO<sub>3</sub>)<sub>2</sub>
D)K<sub>3</sub>HCO<sub>3</sub>
Q3) Consider a bond A-B. If the difference in electronegativity is 0.0, the bond is considered ________.
A)ionic
B)covalent
C)polar covalent
D)hydrogen
Q4) Sulfur in hydrogen sulfide has two bonds and one non-bonded pair of electrons.
A)True
B)False
Q5) NO<sub>3</sub><sup>-</sup>
Page 7
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) Which of the following chlorine-containing species is not polar?
A)CHCl<sub>3</sub>
B)CH<sub>2</sub>Cl<sub>2</sub>
C)HCl
D)CCl<sub>4</sub>
Q2) When drawing the three-dimensional structure diagram of a molecule the bold line
A)projects out from the page B)goes back behind the page C)the bond is in the plane of the page D)One cannot say unless the formula of the molecule is known.
Q3) Which of the following will be affected by the presence of an electric field?
A)H<sub>2</sub>
B)O<sub>2</sub>
C)HCl
D)N<sub>2</sub>
Q4) CHC1<sub>3</sub>
Q5) O<sub>3</sub> (ozone)
Q6) CS<sub>2</sub>
Q7) BF<sub>3</sub>
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) The attractive forces between carbon dioxide molecules are considerably stronger than those found in water molecules.
A)True
B)False
Q2) Which of the following intermolecular force is the strongest?
A)London forces
B)van der Waals forces
C)hydrogen bonding
D)dipole forces
Q3) Nonpolar molecules may exhibit ________.
A)London forces
B)hydrogen bonding
C)dipolar forces
D)all of the above
Q4) Which intermolecular force is important for the function of the antibiotic vancomycin?
A)London forces
B)van der Waals forces
C)hydrogen bonding
D)dipole forces
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) When aqueous solutions of calcium hydroxide and hydrobromic acid are mixed, the spectator ions are ________.
A)calcium and bromide
B)hydrogen and hydroxide
C)calcium and hydroxide
D)hydrogen and bromide
Q2) In a decomposition reaction one compound breaks down into two or more simpler compounds or elements.
A)True
B)False
Q3) Which sulfate is water insoluble?
A)ammonium sulfate
B)strontium sulfate
C)sodium sulfate
D)potassium sulfate
Q4) Which chloride is water soluble?
A)lead (II)chloride
B)calcium chloride
C)mercury (I)chloride
D)silver (I)chloride
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Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) The % yield of an experiment in which 1 mole C<sub>6</sub>H<sub>14</sub> was used and 22 g carbon dioxide was isolated is ________.
A)100%
B)50%
C)17.5%
D)8.3%
Q2) Which of the following pairs does not share the same empirical formula?
A)CH<sub>2</sub>O and C<sub>3</sub>H<sub>6</sub>O<sub>3</sub>
B)C<sub>6</sub>H<sub>6</sub> and C<sub>2</sub>H<sub>2</sub>
C)C<sub>2</sub>H<sub>6</sub>O and CH<sub>3</sub>O
D)C<sub>3</sub>H<sub>4</sub>Br<sub>2</sub> and
C<sub>9</sub>H<sub>12</sub>O<sub>6</sub>
Q3) Which contains the highest % of oxygen?
A)H<sub>2</sub>O<sub>2</sub>
B)Na<sub>2</sub>O<sub>2</sub>
C)HgO
D)CO<sub>2</sub>
Q4) One mole of oxygen gas has fewer atoms than one mole of ozone gas.
A)True
B)False
Page 11
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) Which of the following is most easily oxidized?
A)Ni
B)Pb
C)Li
D)Cr
Q2) What is reduction?
A)loss of electrons
B)increase in oxidation number
C)gain of electrons
D)two of the above
Q3) Consult the EMF activity series and predict which of the following changes will occur if an 24K gold ring (pure gold)is placed in an aqueous solution containing hydrochloric acid.
A)Nothing at all will happen (no reaction).
B)Hydrogen will be further oxidized.
C)Gold will be reduced.
D)Gold will be oxidized.
Q4) The cathode is the electrode where oxidation occurs.
A)True
B)False
Page 12
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Chapter 11: What If There Were No Intermolecular Forces
the Ideal Gas
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Sample Questions
Q1) Which statement is true for an ideal gas?
A)The pressure of a gas increases when its volume decreases.
B)The pressure of a gas increases when its temperature increases.
C)The pressure of a gas increases when the number of gas moles increases.
D)All of the above statements are correct.
Q2) The value of the gas constant R is equal to ________ Latm/ Kmole.
A)0.0821
B)8.21
C)82.1
D)0.00821
Q3) Increasing the temperature of a gas from 100 °C to 200 °C will cause the volume to double.
A)True
B)False
Q4) 1 torr is equal to 1 cm Hg.
A)True
B)False
Q5) The lowest temperature that can theoretically be achieved is -273.16 °C
A)True
B)False
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Chapter 12: Solutions
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Sample Questions
Q1) Sterling silver is a solution (ALLOY)of ________.
A)silver and zinc
B)silver and gold
C)silver and copper
D)silver and iron
Q2) 4.173 g of an organic compound (non-electrolyte)lowered the freezing point of 100.0 g nitrobenzene by 2.6 °C. If the K<sub>f</sub> of nitrobenzene is 8.1 °C, the molecular mass of the non-electrolyte is ________.
A)260
B)195
C)65
D)130
Q3) NH<sub>3</sub> will dissolve in BF<sub>3</sub>.
A)True
B)False
Q4) Which of the following is not a solution?
A)ice in water
B)vinegar in water
C)sugar in water
D)metal alloys
14
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Chapter 13: When Reactants Turn Into Products
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Sample Questions
Q1) An exothermic reaction would feel cold.
A)True
B)False
Q2) In the diagram above, the containers shown (Box A and BoxB)contain exactly the same number of reactant molecules and are at the same temperature. In which box will the rate of reaction be faster?
A)Box A
B)Box B
C)Rate is about the same in each box.
D)No way to tell which is faster from this picture.
Q3) Which of the following is true about a catalyst?
A)It increases the rate of a reaction.
B)It lowers the energy of activation.
C)It is not used up in the process.
D)All of the above are true.
Q4) Which statement is true about the reaction energy profile?
A)plots the relative energies of both the reactants and products
B)plots energy on the y-axis
C)traces the progress of the reaction on the x-axis
D)All of the above are true.
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) If the solubility of calcium fluoride is 2.0 × 10<sup>-</sup><sup>4 </sup><sup>M</sup>, the solubility product value is ________.
A)1.6 × 10<sup>-</sup><sup>12</sup>
B)3.2 × 10<sup>-</sup><sup>11</sup>
C)4.0 × 10<sup>-</sup><sup>8</sup>
D)8.0 × 10<sup>-</sup><sup>12</sup>
Q2) If the value of the equilibrium constant for the reverse reaction is 2.5 × 10<sup>-</sup><sup>6</sup>, the value of the equilibrium constant for the forward reaction is ________.
A)-2.5 × 10<sup>-</sup><sup>6</sup>
B)4.0 × 10<sup>5</sup>
C)2.5 × 10<sup>6</sup>
D)4.0 × 10<sup>7</sup>
Q3) Consider the reaction: A + 3B 2C. Equal numbers of moles for A and B are added to the reaction vessel and equilibrium established. At that point ________.
A)[A] < [B]
B)[A] > [B]
C)[A] = [B]
D)One cannot say unless the equilibrium constant value is known.
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Page 16
Chapter 15: Electrolytes, Acids, and Bases
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Sample Questions
Q1) Which of the following does not produce more than one H<sub>3</sub>O<sup>+</sup> ion per molecule of acid when dissolved in water?
A)carbonic
B)sulfurous
C)phosphoric
D)acetic
Q2) Water can serve both as a Bronsted-Lowry acid and Bronsted-Lowry base. A)True
B)False
Q3) What is the hydroxide-ion concentration of an aqueous solution having a pH of 4.72?
A)4.7 × 10<sup>-5</sup> mol/L
B)1.9 × 10<sup>-</sup><sup>14</sup> mol/L
C)5.3 × 10<sup>-</sup><sup>10</sup> mol/L
D)1.9 × 10<sup>-5</sup> mol/L
Q4) Which is the most acidic solution?
A)a solution whose [H<sup>+</sup>] = 10<sup>-</sup><sup>1</sup>
B)a solution whose [OH<sup>-</sup>] = 10<sup>-</sup><sup>10</sup>
C)a solution whose pH = 0
D)All of the above have the same degree of acidity.
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) When a neutron is transformed into a proton what else is emitted?
A)a beta particle
B)an electron
C)an alpha particle
D)Either A or B; both of them represent the same particle.
Q2) Identify X in the reaction below. X + <sup>1</sup>n <sup>142</sup>Ba + <sup>91</sup>Kr + 3 <sup>1</sup>n
A)(<sup>235</sup>Th)
B)(<sup>238</sup>U)
C)(<sup>235</sup>U)
D)(<sup>234</sup>Pa)
Q3) When radium-226 is converted to radon-222 ________.
A)an electron is captured
B)an alpha particle is emitted
C)an electron is released
D)a neutron is released
Q4) <sup>12</sup>C is the most stable carbon isotope.
A)True
B)False
Q5) <sup>1</sup>n + ______ <sup>141</sup>Ba + <sup>92</sup>Kr + 3 <sup>1</sup>n
Page 18
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Chapter 17: The Chemistry of Carbon
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Sample Questions
Q1) Which compounds typically have an unpleasant smell?
A)amines
B)esters
C)alcohols
D)ethers
Q2) The ability of carbon to connect and link together is called ________.
A)isomerism
B)allotropism
C)catenation
D)ring formation
Q3) No other element in the periodic table is able to covalently bond with other atoms of its own kind as extensively as carbon.
A)True
B)False
Q4) Which of the following is a hydrocarbon?
A)C<sub>4</sub>H<sub>8</sub>O
B)C<sub>4</sub>H<sub>10</sub>O
C)C<sub>4</sub>H<sub>8</sub>O<sub>2</sub>
D)C<sub>4</sub>H<sub>6</sub>
Q5) Draw the structure of butanal.
Page 19
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Chapter 18: Synthetic and Biological Polymers
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Sample Questions
Q1) Human DNA molecules consist of just a single strand, just like protein molecules.
A)True
B)False
Q2) Which of the following does not appear in a DNA strand?
A)deoxyribose sugar
B)phosphate
C)amino acids
D)amine base
Q3) The name of the bond that combines two amino acids together is called ________.
A)peptide
B)glycoside
C)acetal
D)ketal
Q4) Construct the complementary strand of this piece of a DNA molecule:
G T A C C T T G G T A A T T G
Q5) Nylon contains only one type of monomer.
A)True
B)False
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