Fundamentals of Chemistry
Textbook Exam Questions
Course Introduction
Fundamentals of Chemistry introduces students to the basic principles and concepts underlying the science of chemistry. Topics covered include atomic structure, periodic trends, chemical bonding, stoichiometry, states of matter, chemical reactions, and thermochemistry. The course emphasizes both theoretical understanding and practical applications, providing foundational knowledge essential for advanced study in chemistry, biology, medicine, and related fields. Laboratory experiences complement lecture material, enabling students to develop key problem-solving and analytical skills through hands-on experimentation and observation.
Recommended Textbook
Introductory Chemistry 4th Edition by Steve Russo
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Page 2
Chapter 1: What Is Chemistry
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Sample Questions
Q1) Evaporated ethanol can be isolated by cooling, without changing its disinfectant properties.
A)True
B)False
Answer: True
Q2) If 1 gram of ice needs a certain amount of heat to melt, the same amount of energy must be removed to convert it back to ice at its melting point.
A)True
B)False
Answer: True
Q3) A theory summarizes facts in general statements.
A)True
B)False
Answer: False
Q4) Air is a homogeneous mixture of nitrogen, oxygen and hydrogen.
A)True
B)False
Answer: False
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Page 3
Chapter 2: The Numerical Side of Chemistry
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Sample Questions
Q1) Convert 16.8 meters to:
a)millimeters
b)centimeters c)kilometers.
Answer: a)16,800 mm
b)1,680 cm
c)0.0168 km
Q2) Which is the SI unit for temperature?
A)Fahrenheit
B)Celsius
C)Kelvin
D)either A or C
Answer: C
Q3) 2 × 10<sup>-</sup><sup>3</sup> meters is equal to 2 kilometers.
A)True
B)False
Answer: True
Q4) How many significant digits are there in the number 0.0038040?
Answer: 5
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Chapter 3: The Evolution of Atomic Theory
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Sample Questions
Q1) Which of the following elements is an actinide?
A)Np
B)Pr
C)W
D)Fr
Answer: A
Q2) How many protons does the nucleus of the sulfur-35 isotope have?
A)16
B)19
C)32
D)35
Answer: A
Q3) The law of definite proportion states that atoms must combine in a one to one ratio.
A)True
B)False
Answer: False
Q4) lead-207
Answer: atomic number 82, mass number 207, symbol Pb
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Page 5
Chapter 4: The Modern Model of the Atom
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Sample Questions
Q1) Which type of electromagnetic radiation is composed of photons having the largest energy?
A)microwaves
B)radio waves
C)x rays
D)gamma rays
Q2) Carbon can assume both +4 and -4 charges.
A)True
B)False
Q3) The wavelength is the distance measured between two crests, but not between two troughs.
A)True
B)False
Q4) The wavelengths in infrared radiation are larger than those of the ultraviolet region.
A)True
B)False
Q5) Blue visible light is of lower energy than red visible light.
A)True
B)False
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Chapter 5: Chemical Bonding and Nomenclature
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Sample Questions
Q1) Oxygen in water has two bonds and one non-bonded pair of electrons.
A)True
B)False
Q2) H<sub>2</sub>Se
Q3) The number of valence electrons that belong to the oxygens in the carbonate anion is ________.
A)15
B)18
C)20
D)24
Q4) The number of bonds phosphorus usually has is 3.
A)True
B)False
Q5) Which of the following does not have a charge of -2?
A)carbonate
B)chromate
C)dichromate
D)nitrate
Q6) O<sub>3</sub> (ozone)
Q7) NO<sub>3</sub><sup>-</sup>
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Chapter 6: The Shape of Molecules
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Sample Questions
Q1) Which of the following is bent?
A)water
B)sulfur dioxide
C)carbon dioxide
D)both A and B
Q2) The ball-and-stick model emphasizes the bonding pattern.
A)True
B)False
Q3) NO<sup>+</sup>
Q4) Which compound listed below has a bond angle of 180° around the central atom?
A)H<sub>2</sub>O
B)CO<sub>2</sub>
C)CC1<sub>4</sub>
D)NH<sub>3</sub>
Q5) PO<sub>4</sub><sup>3</sup><sup>-</sup>
Q6) CO<sub>3</sub><sup>2</sup><sup>-</sup>
Q7) A polar covalent compound is unaffected by the presence of an electric field.
A)True
B)False
Q8) BF<sub>3</sub>
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Chapter 7: Intermolecular Forces and the Phases of Matter
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Sample Questions
Q1) Which of the following experiences the strongest London forces?
A)carbon tetrachloride
B)water
C)hydrogen
D)helium
Q2) London forces are extremely weak for ________.
A)nitrogen gas
B)methane gas
C)oxygen gas
D)all of the above
Q3) Which of the three phases of matter (solid, liquid, or gas)has particles that are in a loose, changeable arrangement but do not completely fill the volume of a given container?
A)solid
B)liquid
C)gas
D)All of the above feature loose arrangements of particles.
Q4) Vancomycin is the first line of defense against bacteria.
A)True
B)False
Page 9
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Chapter 8: Chemical Reactions
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Sample Questions
Q1) Which of the following equations has 1:1:1:1 as the relative ratio of coefficients when balanced?
A)H<sub>2</sub>SO<sub>4</sub> + KOH K<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O
B)Zn + HCl H<sub>2</sub> + ZnCl<sub>2</sub>
C)CH<sub>4</sub> + O<sub>2</sub> CO<sub>2</sub> + H<sub>2</sub>O
D)NaOH + HCl NaCl + H<sub>2</sub>O
Q2) In a decomposition reaction one compound breaks down into two or more simpler compounds or elements.
A)True
B)False
Q3) Which of the following equations is not a single replacement reaction?
A)H<sub>2</sub>SO<sub>4</sub> + Mg(OH)<sub>2</sub> H<sub>2</sub>O + MgSO<sub>4</sub>
B)Zn + HCl H<sub>2</sub> + ZnCl<sub>2</sub>
C)Al + Fe<sub>2</sub>O<sub>3</sub> Al<sub>2</sub>O<sub>3</sub> + Fe
D)Na + H<sub>2</sub>O NaOH + H<sub>2</sub>
Q4) In a combustion reaction, oxygen is typically one of the reactants.
A)True
B)False
Page 10
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Chapter 9: Stoichiometry and the Mole
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Sample Questions
Q1) The % yield of an experiment in which two moles copper was used and 18 g water was isolated is ________.
A)100%
B)50%
C)37.5%
D)25%
Q2) Determine the molecular formula for a compound that weighs 44.1 g/mol and is 81.7% C and 18.3% H by mass.
Q3) The % yield of an experiment in which 1 mole C<sub>2</sub>H<sub>6</sub>O was used and 22 g carbon dioxide was isolated is ________.
A)100%
B)50%
C)37.5%
D)25%
Q4) One mole of oxygen gas has fewer atoms than one mole of ozone gas.
A)True
B)False
Q5) Determine the number of grams of copper present in a 4.0 kg sample of the mineral chalcopyrite (CuFeS<sub>2</sub>).
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Chapter 10: Electron Transfer in Chemical Reactions
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Sample Questions
Q1) Which atom in the compound KClO<sub>3</sub> has a negative oxidation state?
A)potassium
B)oxygen
C)both potassium and chlorine
D)both chlorine and oxygen
Q2) Which of the following is most easily oxidized?
A)Ni
B)Pb
C)Li
D)Cr
Q3) What is the oxidation state of chromium in the compound K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>?
A)+4
B)+6
C)+7
D)-1
Q4) A spontaneous electrochemical cell is called a galvanic cell.
A)True
B)False
Q5) Which of the reactions above are examples of electron transfer reactions?
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) Find the number of liters occupied by 3.0 g of nitrogen gas at STP.
A)67 L
B)7.5 L
C)2.4 L
D)0.13 L
Q2) 1 torr is equal to 1 cm Hg.
A)True
B)False
Q3) Imagine a balloon that you blow up to a given size (fill with a given amount of air at a given temperature and pressure). What do you expect to happen if you pour liquid nitrogen (at 77 K)over the surface of the balloon? (Assuming that the pressure does not change significantly).
A)increase slightly in size
B)decrease significantly in size
C)stay exactly the same size as before
D)One cannot say unless the composition of the gas is known.
Q4) 30.19 inches of Hg is equal to 1.009 atm.
A)True
B)False
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Chapter 12: Solutions
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Sample Questions
Q1) Alloys are solid solutions.
A)True
B)False
Q2) Briefly, how does increasing the pressure of a gas over a given solvent increase the amount of that gas that can be dissolved in that solvent?
Q3) What volume (in mL's)of a 1.05 M stock solution of HCl should be used to prepare 4.00 L of a 0.0920 M HCl solution?
Q4) A mixture is not necessarily a solution.
A)True
B)False
Q5) 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.
Q6) 25 mL of 0.2 M NaOH will neutralize 10 mL 0.5 M HCl solution.
A)True
B)False
Page 14
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Chapter 13: When Reactants Turn Into Products
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Sample Questions
Q1) In the diagram above, the two containers shown (Box A and BoxB)have exactly the same size (volume), are held at the same temperature, and contain reactant molecules (dots). In which box will the rate of reaction be faster?
A)Box A
B)Box B
C)The rate will be about the same in each box.
D)There is no way to tell which will be faster from this diagram.
Q2) It is possible to determine a given reaction's mechanism without performing any experiments of any kind.
A)True
B)False
Q3) If the kinetic energy of the reactant molecules is not high enough to overcome the activation energy barrier, ________.
A)the reverse reaction will occur
B)no reaction takes place
C)the reaction will occur anyway
D)the products will form at a slower rate
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15
Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Changing the temperature of a reaction will not change the equilibrium value.
A)True
B)False
Q2) 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>
Q3) Refer to the equilibrium shown above. If the reaction vessel is expanded, this will
A)shift the reaction to the right
B)shift the reaction to the left
C)have no effect
D)cannot be determined, since the temperature is unknown
Q4) If the solubility product of tin(II)carbonate is 1.03 × 10<sup>-</sup><sup>9</sup>, the molar solubility is 3.21 × 10<sup>-</sup><sup>5</sup> M.
A)True
B)False
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Chapter 15: Electrolytes, Acids, and Bases
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Sample Questions
Q1) The pH of a given aqueous solution of acetic acid is 3.76. What is the concentration of OH<sup>-</sup> in this solution?
Q2) Which of the following is a triprotic acid when dissolved in water?
A)hydrobromic
B)sulfuric
C)hypochlorous
D)phosphoric
Q3) Which of the following is a non-electrolyte when dissolved in distilled water?
A)sodium chloride
B)hydrochloric acid
C)sodium hydroxide
D)ethyl alcohol
Q4) A solution of HCl/Cl<sup>-</sup> can act as a buffer.
A)True
B)False
Q5) The hydrogen-ion concentration of a solution of pOH 10.5 is 3.16 × 10<sup>-4</sup> mol/L (remember that pH + pOH = 14 for aqueous systems).
A)True
B)False
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) <sup>35</sup>Cl and <sup>37</sup>Cl are isotopes.
A)True
B)False
Q2) <sup>12</sup>C is the most stable carbon isotope.
A)True
B)False
Q3) When an unstable nucleus emits a beta particle ________.
A)its mass number is decreased by four units
B)its atomic number is decreased by two units
C)its atomic number is increased by one unit
D)its mass number is decreased by one unit
Q4) The n/p ratio of stable isotopes becomes larger than 1, when the atomic number is larger than ________.
A)10
B)18
C)20
D)24
Q5) What is the mass defect of the lithium-9 isotope in g/mol? Lithium-9 has an atomic mass of 9.0273 g/mol.
Page 18
Q6) <sup>3</sup>H + <sup>2</sup>H ______ + <sup>1</sup>n
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Chapter 17: The Chemistry of Carbon
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Q1) Unlike carbon, nitrogen has the potential of bonding to other atoms of itself, but cannot form long chains.
A)True
B)False
Q2) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,2,4-trimethylpentane.
Q3) Construct a line drawing for the hydrocarbon whose IUPAC name is 2,4,4-trimethyl-2-pentene.
Q4) The formula C<sub>5</sub>H<sub>10</sub>O may be applicable to an aldehyde or a ketone.
A)True
B)False
Q5) 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>
Q6) Diamond is a hydrocarbon.
A)True
B)False
Page 19
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Chapter 18: Synthetic and Biological Polymers
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Q1) The complete human genetic "blueprint" (the human genome)was determined many years ago, and is really not all that complicated.
A)True
B)False
Q2) The bond found in Nylon-66 is a(n)________ bond.
A)amide
B)ester
C)ketone
D)alcohol
Q3) DNA molecules contain "codes," from which proteins and other materials can eventually be synthesized.
A)True
B)False
Q4) Polymers are very large molecules.
A)True
B)False
Q5) The human body is able to synthesize as much of every type of amino acid as it needs.
A)True
B)False
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