Preparatory Chemistry
Textbook Exam Questions
Course Introduction
Preparatory Chemistry is an introductory course designed to equip students with the foundational concepts and problem-solving skills necessary for success in college-level chemistry. The course covers essential topics such as atomic structure, chemical bonding, periodic trends, stoichiometry, chemical reactions, states of matter, and basic laboratory techniques. Emphasis is placed on developing quantitative reasoning, understanding scientific notation and measurement, and applying principles to solve real-world problems. By the end of the course, students will be prepared for more advanced studies in general chemistry and related scientific fields.
Recommended Textbook Chemistry 10th Edition by Raymond Chang
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Chapter 1: Chemistry: The Study of Change
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Sample Questions
Q1) Define element.
Answer: An element is a substance that cannot be separated into simpler substances by chemical means.
Q2) What is the density of a salt solution if 50.0 mL of the solution has a mass of 57.0 g?
Answer: 1.14 g/mL
Q3) Give three examples of mixtures.
Answer: (Answers will vary.)Air, gasoline, sea water, salt and sand, iron filings and sand
Q4) The diameter of Earth is 12.7 Mm. Express this diameter in centimeters.
A)1.27 * 10<sup>5</sup> cm
B)1.27 * 10<sup>6</sup> cm
C)1.27 * 10<sup>7</sup> cm
D)1.27 * 10<sup>8</sup> cm
E)1.27 * 10<sup>9</sup> cm
Answer: E
Q5) Give examples of three physical properties.
Answer: (Answers will vary.)Melting point, boiling point, density, color
Q6) Name two types of mixtures.
Answer: Homogeneous mixture and heterogeneous mixture
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Chapter 2: Atoms, Molecules, and Ions
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Sample Questions
Q1) Write the formula for the acid formed from the permanganate anion, and then name the acid.
Answer: HMnO<sub>4</sub>, permanganic acid
Q2) Name the following ternary compound: CuCO<sub>3</sub>.
Answer: copper(II)carbonate
Q3) The elements known as the halogens are useful as disinfectants.Name two halogens.
Answer: (two of these)fluorine, chlorine, bromine, iodine
Q4) The correct name for Ba(OH)<sub>2</sub> is
A)barium hydrogen oxide.
B)boron hydroxide.
C)barium hydrate.
D)beryllium hydroxide.
E)barium hydroxide.
Answer: E
Q5) Give the formula for nickel(II)sulfate.
Answer: NiSO<sub>4</sub>
Q6) Name the following binary compound: NaH. Answer: sodium hydride
Page 4
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Chapter 3: Mass Relationships in Chemical Reactions
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Sample Questions
Q1) A silver wire has a diameter of 0.500 mm. What length of this wire contains exactly 1.00 mol of silver? (density of Ag = 10.5 g/cm<sup>3</sup>)
A)52.3 m
B)222 m
C)13.1 m
D)2.01 m
E)890 m
Answer: A
Q2) A 0.600 g sample of a compound of arsenic and oxygen was found to contain 0.454 g of arsenic. What is the empirical formula of the compound? Answer: As<sub>2</sub>O<sub>3</sub>
Q3) What is the mass of 0.20 mole of C<sub>2</sub>H<sub>6</sub>O (ethanol)?
A)230 g
B)46 g
C)23 g
D)4.6 g
E)None of these.
Answer: E
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Chapter 4: Reactions in Aqueous Solution
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Sample Questions
Q1) Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: NH<sub>4</sub>Cl.
Q2) Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s)+ 2HCl(aq)\(\rarr\)ZnCl<sub>2</sub>(aq)+ H<sub>2</sub>(g)
What mass of hydrogen gas is produced when a 7.35 g chunk of zinc dissolves in 500. mL of 1.200M HCl?
A)0.605 g
B)0.113 g
C)0.302 g
D)0.453 g
E)0.227 g
Q3) A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250.mL. What is the concentration of nitric acid in the final solution?
A)1.27 M
B)8.12 * 10<sup>-3</sup> M
C)0.406 M
D)3.25 * 10<sup>-2</sup> M
E)5.08 * 10<sup>-4</sup> M
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Chapter 5: Gases
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Sample Questions
Q1) Calculate the volume occupied by 35.2 g of methane gas (CH<sub>4</sub>)at 25°C and 1.0 atm.R = 0.08206 L.atm/K.mol.
A)0.0186 L
B)4.5 L
C)11.2 L
D)49.2 L
E)53.7 L
Q2) Many automobiles produce about 5 grams of NO for each mile they are driven. How many liters of NO gas at STP would be produced on a 100-mile trip?
Q3) A pressure that will support a column of Hg to a height of 256 mm would support a column of water to what height? The density of mercury is 13.6 g/cm<sup>3</sup>; the density of water is 1.00 g/cm<sup>3</sup>.
A)1.00 * 10<sup>2</sup> ft
B)18.8 mm
C)33.8 ft
D)76.0 cm
E)348 cm
Q4) Give five examples of compounds that exist as gases at room temperature and pressure.
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Chapter 6: Thermo-Chemistry
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Sample Questions
Q1) Given the thermochemical equation 2SO<sub>2</sub>(g)+ O<sub>2</sub>(g)\(\rarr\)2SO<sub>3</sub>(g), \(\Delta\)H°<sub>rxn</sub>= -198 kJ/mol, how much heat is evolved when 600.g of SO<sub>2</sub> is burned?
A)5.46 * 10<sup>-2</sup> kJ
B)928 kJ
C)1.85 * 10<sup>3</sup> kJ
D)59,400 kJ
E)3.71 * 10<sup>3</sup> kJ
Q2) How many grams of ethylene (C<sub>2</sub>H<sub>4</sub>)would have to be burned to produce 450 kJ of heat?
C<sub>2</sub>H<sub>4</sub>(g)+ 3O<sub>2</sub>(g)\(\rarr\)2CO<sub>2</sub>(g)+ H<sub>2</sub>O(l)\(\Delta\)H°<sub>rxn</sub> = -1411 kJ/mol
Q3) Find \(\Delta\)H°<sub>rxn</sub> for the reaction
2Ag<sub>2</sub>S(s)+ 2H<sub>2</sub>O(l)\(\rarr\) 4Ag(s)+ 2H<sub>2</sub>S(g)+ O<sub>2</sub>(g).
[\(\Delta\)H°<sub>f</sub> (Ag<sub>2</sub>S(s))= -32.6 kJ/mol; \(\Delta\)H°<sub>f</sub> (H<sub>2</sub>S(g))= -20.5 kJ/mol; \(\Delta\)H°<sub>f</sub> (H<sub>2</sub>O(l))= -285.5 kJ/mol]
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Chapter 7: Quantum Theory and the Electronic Structure of Atoms
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Sample Questions
Q1) Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E<sub>n</sub> = -2.18 * 10<sup>-18</sup> J(1/n<sup>2</sup>)
A)97.2 nm
B)82.6 nm
C)365 nm
D)0.612 nm
E)6.8 * 10<sup>-18</sup> nm
Q2) A ground-state atom of manganese has ___ unpaired electrons and is _____.
A)0, diamagnetic
B)2, diamagnetic
C)3, paramagnetic
D)5, paramagnetic
E)7, paramagnetic
Q3) The colors of the visible spectrum are blue, green, orange, red, violet, and yellow.Of these colors, ______ has the shortest wavelength.
Q4) With regard to electron behavior, what happens when light is absorbed or emitted by an atom?
Q5) Write the ground state electron configuration for the phosphorus atom.
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Chapter 8: Periodic Relationships Among the Elements
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Sample Questions
Q1) Electron affinity is always a positive quantity.
A)True
B)False
Q2) Which one of the following elements is a transition element?
A)Sr
B)Pb
C)As
D)Fe
E)H
Q3) Since arsenic is a nonmetal, As<sub>2</sub>O<sub>3</sub> is expected to be a/an _____ oxide.
A)acidic
B)ionic
C)amphoteric
D)neutral
E)basic
Q4) Write the ground-state electron configuration for Mg<sup>2+</sup>.
Q5) Consider the following reaction 2A + 3F<sub>2</sub> \(\rarr\) 2AF<sub>3</sub>.What is a reasonable guess for the identity element A?
Q6) Write the ground-state electron configuration for Al<sup>3+</sup>.
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Chapter 9: Chemical Bonding I: Basic Concepts
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Sample Questions
Q1) The bond in which of the following pairs of atoms would be the least polar (i.e., lowest percent ionic character)?
A)C - Cl
B)C - C
C)C - H
D)O - C
E)N - C
Q2) Write a Lewis structure for OF<sub>2</sub>.
Q3) Which of the elements listed below has the greatest electronegativity?
A)Se
B)Sb
C)K
D)Ga
E)Fe
Q4) The number of lone electron pairs in the CO<sub>3</sub><sup>2-</sup> ion is ___.
A)4
B)5
C)6
D)7
E)8
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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization of
Atomic Orbitals
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Q1) Consider the species O<sub>2</sub><sup>-</sup>, O<sub>2</sub>, and O<sub>2</sub><sup>+</sup>. Which of these species will be paramagnetic?
A)O<sub>2</sub> and O<sub>2</sub><sup>-</sup>
B)O<sub>2</sub><sup>+</sup> and O<sub>2</sub>
C)O<sub>2</sub><sup>+</sup> and O<sub>2</sub><sup>-</sup>
D)only O<sub>2</sub>
E)all three are paramagnetic
Q2) In benzene (C<sub>6</sub>H<sub>6</sub>), what is the hybridization of each carbon atom?
Q3) What bond angles are predicted by VSEPR theory for the F -P -F bonds in PF<sub>5</sub>?
Q4) The bond angle in ICl<sub>2</sub><sup>-</sup> is expected to be
A)a little less than 109.5°.
B)109.5°.
C)a little more than 109.5°.
D)120°.
E)180°.
Q5) Which should have the longer bond, O<sub>2</sub> or O<sub>2</sub><sup>+</sup>?
Page 12
Q6) Explain why CO<sub>2</sub> is nonpolar, but OCS is polar.
Q7) According to the VSEPR theory, the geometrical structure of PF<sub>5</sub> is
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Chapter 11: Intermolecular Forces and Liquids and Solids
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Sample Questions
Q1) Find the temperature at which water boils on a day in the mountains when the barometric pressure is 593 mmHg.(Given: the heat of vaporization of water is 40.79 kJ/mol)
A)93.1°C
B)117°C
C)41.5°C
D)97.0°C
E)68.1°C
Q2) What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 10<sup>5</sup> J of heat from your body? H<sub>2</sub>O(l)\(\rarr\)H<sub>2</sub>O(g)\(\Delta\)H<sub>vap</sub> = 40.7 kJ/mol
A)7.52 * 10<sup>4</sup> g
B)418 g
C)75.2 g
D)58.4 g
E)6.92 * 10<sup>6</sup> g
Q3) Magnesium oxide, MgO, melts at 2,800°C and is very hard.The liquid conducts electricity very well.What kind of crystal is this?
Q4) Indicate all the types of intermolecular forces of attraction in HF(l).
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Chapter 12: Physical Properties of Solutions
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Sample Questions
Q1) Calculate the molality of 6.0 M H<sub>2</sub>SO<sub>4</sub> solution. The density of the solution is 1.34 g/mL.
A)4.48 m
B)7.98 m
C)8.10 m
D)8.43 m
E)10.2 m
Q2) A 100.mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.
Q3) A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 3.85 g.Calculate the original concentration of NaCl, in g per liter, in the water sample.
Q4) Automobile radiators usually carry a sticker that indicates that they must contain an antifreeze solution for proper operation, winter or summer.Why should you not use ordinary water during the summer?
Q5) Define solvation.
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Chapter 13: Chemical Kinetics
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Q1) The activation energy for the following reaction is 60.kJ/mol. Sn<sup>2+</sup> + 2Co<sup>3+</sup> F1F1F1S1 F1F1F10 Sn<sup>4+</sup> + 2Co<sup>2+</sup> <sup> </sup>By what factor (how many times)will the rate constant increase when the temperature is raised from 10°C to 28°C?
A)1.002
B)4.6
C)5.6
D)2.8
E)696
Q2) For the reaction whose rate law is rate = k[X], a plot of which of the following is a straight line?
A)[X] versus time
B)ln [X] versus time
C)1/[X] versus time
D)[X] versus 1/time
E)ln [X] versus 1/time
Q3) The rate constant for a certain first-order reaction is 0.40/min.What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?
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Chapter 14: Chemical Equilibrium
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Q1) The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10<sup>-18</sup>.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?
Q2) Which of these statements is true about chemical equilibria in general?
A)At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants].
B)Equilibrium is the result of the cessation of all chemical change. C)There is only one set of equilibrium concentrations that equals the K<sub>c</sub> value.
D)At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction.
E)At equilibrium, the rate of the forward reaction is equal to as the rate of the reverse reaction.
Q3) What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.
Q4) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.
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Chapter 15: Acids and Bases
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Q1) Write the chemical formula for nitric acid.
Q2) For H<sub>3</sub>PO<sub>4</sub>, K<sub>a1</sub> = 7.3 * 10<sup>-3</sup>, K<sub>a2</sub> = 6.2 *10<sup>-6</sup>, and K<sub>a3</sub> = 4.8 *10<sup>-13</sup>.
An aqueous solution of Na<sub>3</sub>PO<sub>4</sub> therefore would be
A)neutral
B)basic
C)acidic
Q3) The pH of coffee is approximately 5.0. How many times greater is the [H<sup>+</sup>] in coffee than in neutral water?
A)200
B)100
C)5.0
D)1.4
E)0.01
Q4) If the pH of tomato juice is 4.0, what is the hydroxide ion concentration in this solution?
Q5) Will a 0.1 M solution of NaH<sub>2</sub>PO<sub>4</sub>(aq)be acidic, basic, or neutral?
Q6) Write the chemical formula for sulfuric acid.
Page 18
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Chapter 16: Acid-Base Equilibria and Solubility Equilibria
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Q1) Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3?
A)CH<sub>3</sub>COONa / CH<sub>3</sub>COOH (K<sub>a</sub> = 1.8 * 10<sup>-5</sup>)
B)NH<sub>3</sub> / NH<sub>4</sub>Cl (K<sub>a</sub> = 5.6 * 10<sup>-10</sup>)
C)NaOCl / HOCl (K<sub>a</sub> = 3.2 * 10<sup>-8</sup>)
D)NaNO<sub>2</sub> / HNO<sub>2</sub> (K<sub>a</sub> = 4.5 * 10<sup>-4</sup>)
E)NaCl / HCl
Q2) A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution. The solubility product constant for sodium carbonate at this temperature is
A)79.0
B)0.316
C)0.0790
D)36.8
E)316
Q3) The solubility of a salt increases as its K<sub>sp</sub> increases.
A)True
B)False
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Chapter 17: Chemistry in the Atmosphere
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Q1) The average person breathes about 20 m<sup>3</sup> of air a day.What mass of particulates would a person breathe in a day if the particulate level were 400 micrograms per cubic meter?
Q2) Write out the steps in the mechanism of ozone destruction by chlorine atoms.
Q3) Which of the following cannot be plausibly linked to the destruction of the ozone layer?
A)Damage to crops.
B)Increased number of skin cancer cases.
C)Genetic mutations.
D)Increasing global CO<sub>2</sub> concentrations.
Q4) Which region of the atmosphere contains the ozone layer?
A)thermosphere
B)mesosphere
C)stratosphere
D)troposphere
Q5) Write chemical equations that show what happens when acid rain reacts with limestone rock
Q6) Excluding water vapor, list the four most prevalent gases in our atmosphere from most abundant to least abundant.
Q7) Name four "greenhouse gases" besides carbon dioxide.
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Chapter 18: Entropy, Free Energy, and Equilibrium
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Q1) Which of these species would you expect to have the lowest standard entropy (S°)?
A)CH<sub>4</sub>(g)
B)HF(g)
C)NH<sub>3</sub>(g)
D)H<sub>2</sub>O(g)
Q2) Which response includes all the following processes that are accompanied by an increase in entropy?
1)2SO<sub>2</sub>(g)+ O<sub>2</sub>(g)\(\to\) SO<sub>3</sub>(g)
2)H<sub>2</sub>O(l)\(\to\) H<sub>2</sub>O(s)
3)Br<sub>2</sub>(l)\(\to\) Br<sub>2</sub>(g)
4)H<sub>2</sub>O<sub>2</sub>(l)\(\to\) H<sub>2</sub>O(l)+ <sup>1</sup>/<sub>2</sub>O<sub>2</sub>(g)
A)1, 2, 3, 4
B)1, 2
C)2, 3, 4
D)3, 4
E)1, 4
Q3) How does the entropy change when a solid is melted?
Q4) Predict the sign of \(\Delta\)S for the reaction O<sub>2</sub>(g)\(\to\) 2O(g).
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Chapter 19: Electrochemistry
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Q1) Find the emf of the cell described by the cell diagram Fe | Fe<sup>2+</sup> (1.500M)|| Au<sup>3+</sup> (0.00400M)| Au
A)1.99 V
B)1.89 V
C)1.94 V
D)1.66 V
E)1.91 V
Q2) Aluminum metal is formed by the electrolysis of Al<sub>2</sub>O<sub>3 </sub>in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?
Q3) An electrochemical cell based on the following reaction has a standard cell voltage (E°<sub>cell</sub>)of 0.48 V: Sn(s)+ Cu<sup>2+</sup>(aq)\(\to\) Sn<sup>2+</sup>(aq)+ Cu(s)
What is the standard reduction potential of tin(II)? (E°(Cu<sup>2+</sup>/Cu)= 0.34 V)
A)-0.14 V
B)0.14 V
C)-0.82 V
D)0.82 V
E)none of these
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Chapter 20: Metallurgy and the Chemistry of Metals
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Q1) In the Hall process, ____________ is reduced ____________.
A)nickel; electrolytically
B)aluminum; electrolytically
C)nickel; by reaction with metallic sodium
D)aluminum; by reaction with metallic sodium
E)copper; electrolytically
Q2) What effect does increasing temperature have on the conductivities of semiconductors?
A)increases
B)decreases
C)no change
D)cannot be predicted
Q3) Which of these statements does not describe a property of aluminum?
A)Al is an efficient electrical conductor.
B)Al has a low density compared to other metals.
C)Al forms an amphoteric hydroxide.
D)Al is generally considered toxic to humans.
E)Al has a great affinity for oxygen.
Q4) Write the chemical formula of magnetite.
Q5) Write the chemical formula of corundum.
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Chapter 21: Nonmetallic Elements and Their Compounds
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Q1) When in the liquid state, which one of these substances resembles water, insofar as it is a solvent for many electrolytes and even undergoes autoionization as water does?
A)N<sub>2</sub>
B)Cl<sub>2</sub>
C)NH<sub>3</sub>
D)N<sub>2</sub>O
E)Xe
Q2) Hydrogen plays an important role in many industrial processes. Write a balanced chemical equation for its production by the water gas reaction.
Q3) Which of these substances is the active ingredient in ordinary household bleach?
A)HCl
B)Cl<sub>2</sub>
C)NaCl
D)NaClO
E)NaClO<sub>4</sub>
Q4) Write the chemical formula of the peroxide ion.
Q5) Write a balanced chemical equation to show the production of chlorine by the chlor-alkali process.
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Chapter 22: Transition Metal Chemistry and Coordination Compounds
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Q1) The numbers of geometrical isomers and optical isomers of the complex ion [Co(en)<sub>3</sub>]<sup>3+</sup> are, respectively, A)2 and 2.
B)1 and 1.
C)3 and 2.
D)1 and 2.
E)2 and 4.
Q2) Which of these complex ions would absorb light with the longest wavelength?
A)[Co(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup>
B)[Co(NH<sub>3</sub>)<sub>6</sub>]<sup>2+</sup>
C)[CoF<sub>6</sub>]<sup>4-</sup>
D)[Co(CN)<sub>6</sub>]<sup>4-</sup>
E)[Co(en)<sub>6</sub>]<sup>2+</sup>
Q3) How many 3d electrons does a V<sup>3+</sup> ion have?
A)6
B)5
C)4
D)3
E)2
Q4) Write the chemical formula of diamminedichloroplatinum(II).
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Chapter 23: Nuclear Chemistry
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Q1) Which of the following is an advantage of nuclear power plants over coal-burning plants? Nuclear power plants
A)produce radioactive byproducts with very short half-lives, reducing the need for waste storage.
B)do not pollute the air with SO<sub>2</sub>, soot, and fly-ash.
C)create no thermal pollution.
D)generate radioactive byproducts that can be sold for use in secondary applications.
Q2) Which type of radiation is the least penetrating?
A)alpha
B)beta
C)gamma
Q3) What nuclear fuel is produced in a breeder reactor?
Q4) The mass of a nucleus is always less than the sum of the masses of the nucleons. A)True
B)False
Q5) Protactinium-234 has a half-life of 1 minute.How much of a 400.g sample protactinium would remain after 4 minutes?
Q6) Thorium-225 undergoes alpha decay.Write a balanced equation for this reaction.
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Chapter 24: Organic Chemistry
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57 Verified Questions
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Sample Questions
Q1) How many structural isomers are there of C<sub>4</sub>H<sub>10</sub>?
A)4
B)6
C)2
D)8
E)10
Q2) The formula CH<sub>3</sub>CH<sub>2</sub>CH<sub>2</sub>CH=CH<sub>2</sub> represents
A)an alkane.
B)a cycloalkane.
C)an alkene.
D)an alkyne.
E)an aromatic compound.
Q3) The reaction of hydrogen chloride gas with propene will yield 1-chloropropane as the main product.
A)True
B)False
Q4) A compound with the formula C<sub>6</sub>H<sub>12</sub> may or may not be a saturated hydrocarbon.Explain.
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Chapter 25: Synthetic and Natural Organic Polymers
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Sample Questions
Q1) Which of the following statements about the binding of oxygen to deoxyhemoglobin is correct?
A)The binding of oxygen to Fe<sup>2+</sup> in the first heme pulls the iron ion into the porphyrin ring, decreasing the affinity for the second oxygen.
B)The binding of oxygen to Fe<sup>2+</sup> in the first heme pushes the iron ion out of the porphyrin ring, decreasing the affinity for the second oxygen.
C)The binding of oxygen to Fe<sup>2+</sup> in the first heme pulls the iron ion into the porphyrin ring, increasing the affinity for the second oxygen.
D)The binding of oxygen to Fe<sup>2+</sup> in the first heme pushes the iron ion out of the porphyrin ring, increasing the affinity for the second oxygen.
E)Oxygen does not bind to deoxyhemoglobin.
Q2) Which choice contains all three molecular units found in nucleotides?
A)phosphate, sugar, amino acid
B)amino acid, nitrogen-containing base, sugar
C)carboxylic acid, sugar, protein
D)phosphate, nitrogen-containing base, sugar
E)sugar, amino acid, protein
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