Course Introduction
Chemical Principles
Exam Questions
Chemical Principles is an introductory course designed to provide a foundational understanding of the core concepts in chemistry. The course covers atomic and molecular structure, stoichiometry, chemical reactions, thermodynamics, equilibrium, kinetics, and the properties of gases, liquids, and solids. Emphasis is placed on the application of quantitative reasoning and problem-solving skills to understand and predict the behavior of matter. Students will engage with both theoretical concepts and practical laboratory techniques, preparing them for advanced studies in chemistry, biology, and related scientific disciplines.
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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Sample Questions
Q1) What is the name of the element whose symbol is "Co"?
A)Carbon
B)Chromium
C)Coal
D)Cobalt
Answer: D
Q2) It is scientifically proper to construct a theory without then doing any experiments to test it.
A)True
B)False
Answer: False
Q3) The only way one can change an element to another is via ________.
A)a chemical reaction
B)a physical reaction
C)a nuclear reaction
D)applying heat
Answer: C
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Page 3
Chapter 2: The Numerical Side of Chemistry
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Sample Questions
Q1) Specific heat may be measured as cal. g/°C.
A)True
B)False
Answer: False
Q2) Which of the following temperatures are not possible?
A)2000 °C
B)-425 °F
C)-425 °C
D)5 K
Answer: C
Q3) The Fahrenheit temperature is always numerically higher than the equivalent Celsius temperature.
A)True
B)False
Answer: False
Q4) Trailing zeros are also called place-holding zeros.
A)True
B)False
Answer: False
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Chapter 3: The Evolution of Atomic Theory
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Sample Questions
Q1) One needs to supply energy from an outside source to form a cation from a neutral atom.
A)True
B)False
Answer: True
Q2) Which of the following elements is a chalcogen?
A)H
B)N
C)O
D)F
Answer: C
Q3) The breakthrough Dmitri Mendeleev had when constructing the periodic table occurred ________.
A)when J. J. Thomson discovered the electron
B)when Sir James Chadwick discovered the neutron
C)when Thomson and E. Goldstein discovered the proton
D)when Mendeleev placed the elements in a sequence of increasing atomic mass
Answer: D
Q4) cobalt-60
Answer: atomic number 27, mass number 60, symbol Co
Page 5
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Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) The number of electrons in the valence shell of an atom is equal to the group number for the representative elements.
A)True
B)False
Q2) H<sup>+</sup> has one electron.
A)True
B)False
Q3) Once an atom gets excited, it may remain in that excited state indefinitely.
A)True
B)False
Q4) The total number of electrons that can be accommodated in 3d is ________.
A)5
B)2
C)6
D)10
Q5) Halogens have large electron affinity values.
A)True
B)False
Q6) Which element is the more reactive, sodium (Na)or potassium (K)?
Page 6
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Chapter 5: Chemical Bonding and Nomenclature
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Sample Questions
Q1) In the set H, S, Cl, Na, sodium is the least electronegative.
A)True
B)False
Q2) How many unpaired electrons does the oxide anion (O<sup>2-</sup>)have?
A)3
B)2
C)1
D)0
Q3) Which of the following elements has the highest number of valence electrons?
A)magnesium
B)lithium
C)argon
D)phosphorus
Q4) Which of the following polyatomic ions has the least atoms per formula unit?
A)ammonium
B)carbonate
C)dihydrogen phosphate
D)acetate
Q5) O<sub>3</sub> (ozone)
Q6) H<sub>2</sub>Se
Page 7
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) What is the steric number of the central atom in carbon disulfide?
A)1
B)2
C)3
D)4
Q2) What is the molecular shape of NO<sub>2</sub><sup>-</sup>
A)tetrahedral
B)pyramidal
C)linear
D)bent
Q3) Which of the following will be the least soluble in water?
A)CH<sub>3</sub>OH
B)CH<sub>4</sub>
C)NH<sub>3</sub>
D)CH<sub>3</sub>CH<sub>2</sub>OH
Q4) The angle around the central atom in the pyramidal structure is very close to that of the tetrahedral one.
A)True
B)False
Q5) H<sub>2</sub>S
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) Which of the following may not be considered an ionic compound?
A)sodium chloride
B)magnesium oxide
C)ammonia
D)potassium bromide
Q2) The solid to gas conversion is called ________.
A)melting
B)sublimation
C)evaporation
D)condensation
Q3) Between individual molecules of NO<sub>2</sub> in the solid state, which of the following types of intermolecular forces would you expect to be dominant?
A)hydrogen bonding
B)London forces
C)van der Waals forces
D)dipole forces
Q4) magnesium chloride, MgC1<sub>2</sub>, m.p.: 714 °C
Q5) chromium, Cr
Q6) silicon carbide, SiC, m.p.: 2700 °C
Q7) glucose, C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) Which of the following salts is water insoluble?
A)K<sub>2</sub>SO<sub>4</sub>
B)AgNO<sub>3</sub>
C)CaCO<sub>3</sub>
D)Na<sub>3</sub>PO<sub>4</sub>
Q2) Which sulfide is water insoluble?
A)lead (II)sulfide
B)potassium sulfide
C)ammonium sulfide
D)sodium sulfide
Q3) Which hydroxide is water insoluble?
A)sodium hydroxide
B)barium hydroxide
C)aluminum hydroxide
D)calcium hydroxide
Q4) Ammonium phosphate is water soluble but ammonium carbonate is water insoluble.
A)True
B)False
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Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) A chromium-silicon compound contains 73.52% chromium. The empirical formula is
A)CrSi
B)CrSi<sub>2</sub>
C)Cr<sub>2</sub>Si
D)Cr<sub>3</sub>Si<sub>2</sub>
Q2) The % yield of an experiment in which 1 mole NaHCO<sub>3</sub> was used and 22 g carbon dioxide was isolated is ________.
A)100%
B)50%
C)37.5%
D)25%
Q3) What is the theoretical mass of carbon dioxide produced from one mole of C<sub>2</sub>H<sub>6</sub>O?
A)6 g
B)44 g
C)88 g
D)176 g
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) Assign oxidation states to each of the atoms in the following chemical species:
a)SiO<sub>2</sub>
b)NO<sup>-</sup>
c)TlCl
d)V<sub>2</sub>O<sub>5</sub>
Q2) The reducing agent is ________.
A)reduced in a redox equation
B)oxidized in a redox equation
C)reduced in an oxidation reaction
D)oxidized in a reduction reaction
Q3) In a chemical bond, which atom gets to own the shared electrons?
A)the larger element
B)the smaller element
C)the more electronegative element
D)the most electropositive element
Q4) In which case is the least number of electrons transferred?
A)NaClO NaClO<sub>2</sub>
B)2 Mg + O<sub>2</sub> 2 MgO
C)CuCl CuCl<sub>2</sub>
D)NaClO<sub>2</sub> NaClO<sub>4</sub>
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Chapter 11: What If There Were No Intermolecular Forces
the Ideal Gas
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Sample Questions
Q1) The molar volume of an ideal gas is ________.
A)always equal to 22.4 L at room temperature
B)proportional to the molecular weight of the gas
C)always equal to 22.4 L at STP
D)inversely proportional to the molecular weight of the gas
Q2) The molar volume of water vapor at its boiling point is 22.4 L.
A)True
B)False
Q3) 88 g of carbon dioxide gas will occupy ________ at STP.
A)11.2 L
B)22.4 L
C)44.8 L
D)67.2 L
Q4) A gas occupies a volume of 0.500 L at 125 °C and 0.443 atm. What mathematical expression will yield the correct temperature at 0.750 L and 0.689 atm?
A)(0.689 × 0.750 × 125)/(0.443 × 0.500)
B)(0.443 × 0.500 × 398)/(0.689 × 0.750)
C)(0.443 × 0.500)/(0.689 × 0.750 × 398)
D)(0.689 × 0.750 × 398)/(0.443 × 0.500)
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Chapter 12: Solutions
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Sample Questions
Q1) 500 mL 0.4 M potassium dichromate contains ________ moles of potassium ions and ________ moles of dichromate ions.
A)0.4; 0.2
B)0.2; 0.4
C)0.4; 0.6
D)0.2; 0.2
Q2) If a solute is to be soluble in a given solvent, which step in the solution-making process must have a negative value for its energy?
A)the physical separation of solvent particles
B)the physical separation of solute particles
C)the formation of solvent/solute interactions
D)All three of the preceding steps must be negative for a solute to be soluble.
Q3) 10.0 mL 0.5 M HCl neutralizes ________ mL 0.5 M NaOH.
A)5.0
B)10.
C)20.
D)40.
Q4) How does the phrase "like dissolves like" help to explain why a solute like sodium chloride (NaCl)and a solvent like water should form a solution?
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Chapter 13: When Reactants Turn Into Products
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Sample Questions
Q1) If the forward reaction is exothermic, the reverse is endothermic.
A)True
B)False
Q2) A catalyst lowers the activation energy for a chemical reaction.
A)True
B)False
Q3) An exothermic reaction usually leads to a release in energy.
A)True
B)False
Q4) Generally in a biochemical reaction the first step involves ________.
A)the reaction of the enzyme with the active site of the substrate
B)the reaction of the substrate with the active site of the enzyme
C)the reaction of the substrate with the enzyme-substrate complex
D)the reaction of the enzyme with the enzyme-substrate complex
Q5) For chemical reactions to occur at all, "old" bonds must be broken and "new" bonds must form.
A)True
B)False
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) The equilibrium constant expression for the reaction 2SO<sub>3</sub> (g)+ 2Cl<sub>2</sub> (g) 2SO<sub>2</sub>Cl<sub>2</sub> (g)+ O<sub>2</sub> (g)is
A)K<sub>eq</sub> = [SO<sub>2</sub>Cl<sub>2</sub>] × [O<sub>2</sub>] / [SO<sub>3</sub>] × [Cl<sub>2</sub>]
B)K<sub>eq</sub> = [SO<sub>3</sub>] × [Cl<sub>2</sub>] / [SO<sub>2</sub>Cl<sub>2</sub>] × [O<sub>2</sub>]
C)K<sub>eq</sub> = [SO<sub>2</sub>Cl<sub>2</sub>]<sup>2</sup> × [O<sub>2</sub>] / [SO<sub>3</sub>]<sup>2</sup> × [Cl<sub>2</sub>]<sup>2</sup>
D)K<sub>eq</sub> = [SO<sub>3</sub>]<sup>2</sup> × [Cl<sub>2</sub>]<sup>2</sup> / [SO<sub>2</sub>Cl<sub>2</sub>]<sup>2</sup> × [O<sub>2</sub>]
Q2) Refer to the equilibrium shown above. Adding iron(III)chloride will ________.
A)turn the solution red.
B)turn the solution less red.
C)turn the solution clear.
D)have no effect on the color.
Q3) HCl (g)+ H<sub>2</sub>O (l) H<sub>3</sub>O<sup>+</sup> (aq)+ Cl<sup>-</sup> (aq)
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Page 16
Chapter 15: Electrolytes, Acids, and Bases
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Sample Questions
Q1) Basic solutions ________.
A)have a higher concentration of hydronium ions than hydroxide ions
B)have a lower concentration of hydronium ions than hydroxide ions
C)turn blue litmus paper to pink
D)decolorize phenolphthalein solutions
Q2) Hydrochloric, hypochlorous and hydrobromic acids produce only one H<sub>3</sub>O<sup>+</sup> ion per molecule of acid when dissolved in water.
A)True
B)False
Q3) The conjugate base of HCO<sub>3</sub><sup>-</sup> is ________.
A)H<sub>2</sub>CO<sub>3</sub>
B)CO<sub>3</sub><sup>-</sup><sup>2</sup>
C)CO<sub>2</sub><sup>-</sup><sup>2</sup>
D)H<sub>3</sub>CO<sub>3</sub><sup>+</sup>
Q4) An aqueous solution of pOH 5 is more basic than an aqueous solution of pOH 8. A)True
B)False
Q5) The pH of natural rainwater is 5.6 due to the carbon dioxide in the atmosphere. A)True
B)False
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) Which of the following transformations is not an alpha emission?
A)(<sup>14</sup>C <sup>14</sup>N)
B)(<sup>225</sup>Ac <sup>221</sup>Fr)
C)(<sup>241</sup>Am <sup>237</sup>Np)
D)(<sup>218</sup>Po <sup>214</sup>Pb)
Q2) <sup>3</sup>H + <sup>2</sup>H ______ + <sup>1</sup>n
Q3) The daughter isotope of <sup>196</sup>Po when it undergoes alpha-emission is <sup>200</sup>Pb.
A)True
B)False
Q4) Nuclear fission is sometimes referred to as the "holy grail" for energy production.
A)True
B)False
Q5) Isotopes with the lowest possible n/p ratio are the most stable.
A)True
B)False
Q6) <sup>14</sup>N + <sup>4</sup>He ______ + <sup>1</sup>H
Q7) <sup>1</sup><sup>35</sup>Nd <sup>24</sup>Mg + ______
Q8) <sup>22</sup>Na ______ + <sub>+</sub><sub>1</sub>e
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Chapter 17: The Chemistry of Carbon
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Sample Questions
Q1) Which of the following formulas may be attributed to an amine?
A)C<sub>4</sub>H<sub>10</sub>S
B)CH<sub>5</sub>N
C)C<sub>4</sub>H<sub>8</sub>O<sub>2</sub>
D)C<sub>4</sub>H<sub>6</sub>
Q2) Which hydrocarbon has the lowest boiling point?
A)C<sub>6</sub>H<sub>14</sub>
B)C<sub>4</sub>H<sub>10</sub>
C)C<sub>2</sub>H<sub>6</sub>
D)C<sub>3</sub>H<sub>8</sub>
Q3) Methanol is the compound used in automobile radiators as antifreeze.
A)True
B)False
Q4) Ethanol may be obtained via the fermentation of grains.
A)True
B)False
Q5) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,2,4-trimethylpentane.
Q6) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,4,4-trimethyl-2-pentene.
Page 19
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Chapter 18: Synthetic and Biological Polymers
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Sample Questions
Q1) Viruses are not, technically, truly living organisms.
A)True
B)False
Q2) DNA molecules contain "codes," from which proteins and other materials can eventually be synthesized.
A)True
B)False
Q3) The term used to describe a substance with a medium number of amino acids is
A)peptide
B)polypeptide
C)protein
D)polymer
Q4) Think for a moment about the terms "polymer" and "polysaccharide". Is it right to refer to polysaccharides as "nature's polymers"? Why or why not?
Q5) Polymers are very large molecules.
A)True
B)False
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