Course Introduction
Preparatory Chemistry
Test Preparation
Preparatory Chemistry is designed to provide students with a foundational understanding of essential chemical concepts and skills necessary for success in college-level chemistry courses. Topics covered include atomic and molecular structure, chemical nomenclature, stoichiometry, the periodic table, chemical reactions, and the properties of gases, liquids, and solids. The course emphasizes problem-solving, laboratory techniques, and the development of scientific reasoning, preparing students for further study in general chemistry and related scientific fields.
Recommended Textbook Chemistry A Molecular Approach 4th Edition by Nivaldo J. Tro
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25 Chapters
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Page 2
Chapter 1: Matter, measurement, and Problem Solving
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Sample Questions
Q1) Identify a gas.
A) definite volume and definite shape
B) definite volume and no definite shape
C) definite shape and no definite volume
D) no definite shape and no definite volume
Answer: D
Q2) Choose the element from the list below.
A) sodium chloride
B) table salt
C) hydrogen peroxide
D) iron
E) rust
Answer: D
Q3) How many cm<sup>3</sup> are contained in 5.83 × 10<sup>6 </sup>mm<sup>3</sup>?
A) 5.83 × 10<sup>6</sup> cm<sup>3</sup>
B) 5.83 × 10<sup>3</sup> cm<sup>3</sup>
C) 5.83 × 10<sup>-</sup><sup>10</sup>cm<sup>3</sup>
D) 5.83 × 10<sup>18</sup> cm<sup>3</sup>
E) 5.83 × 10<sup>12</sup> cm<sup>3</sup>
Answer: B
Page 3
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Chapter 2: Atoms and Elements
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Sample Questions
Q1) How many protons (p)and neutrons (n)are in an atom of calcium-46?
A) 20 p, 26 n
B) 20 p, 46 n
C) 26 p, 20 n
D) 46 p, 20 n
Answer: A
Q2) All samples of a given compound,regardless of their source or how they were prepared,have the same proportions of their constituent elements.Which law does this refer to?
A) Law of Definite Proportions
B) Law of the Conservation of Mass
C) Law of Modern Atomic Theory
D) Law of Multiple Proportions
E) First Law of Thermodynamics
Answer: A
Q3) Give the name of the instrument that is used to measure masses of atoms and the percent abundance of isotopes.
Answer: mass spectrometer
Q4) The atomic number is equal to the number of ________.
Answer: protons
4
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Chapter 3: Molecules,compounds,and Chemical Equations
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Sample Questions
Q1) Give the mass percent of carbon in C<sub>14</sub>H<sub>19</sub>NO<sub>2</sub>.
A) 72.07%
B) 8.21%
C) 6.00%
D) 13.72%
Answer: A
Q2) The ion ClO<sub>2</sub><sup>-</sup> is named
A) chlorate ion.
B) chlorite ion.
C) chlorine dioxide ion.
D) chlorine(II) oxide ion.
Answer: B
Q3) How many sodium ions are contained in 99.6 mg of Na<sub>2</sub>SO<sub>3</sub>? The molar mass of Na<sub>2</sub>SO<sub>3</sub><sub> </sub>is 126.05 g/mol.
A) 1.52 × 10<sup>27</sup> sodium ions
B) 4.76 × 10<sup>20</sup> sodium ions
C) 2.10 × 10<sup>21</sup> sodium ions
D) 1.05 × 10<sup>21</sup> sodium ions
E) 9.52 × 10<sup>20</sup> sodium ions
Answer: E
Page 5
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Chapter 4: Chemical Quantities and Aqueous Reactions
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Sample Questions
Q1) What is the oxidation number of the chromium atom in H<sub>2</sub>CrO<sub>4</sub>?
A) +2
B) +4
C) +6
D) -7
E) -3
Q2) Determine the oxidation state of carbon in CO<sub>2</sub>.
A) +5
B) +3
C) 0
D) +2
E) +4
Q3) Identify barium hydroxide.
A) strong electrolyte, strong base
B) strong electrolyte, weak base
C) weak electrolyte, strong base
D) weak electrolyte, weak base
E) nonelectrolyte
Q4) How can you tell if a reaction is an oxidation-reduction reaction?
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Chapter 5: Gases
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Sample Questions
Q1) A gas bottle contains 0.450 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?
A) 0.0471 mol
B) 0.0888 mol
C) 0.497 mol
D) 0.539 mol
Q2) Which of the following gases has the highest average speed at 400K?
A) NO<sub>2</sub>
B) O<sub>2</sub> <sub> </sub>
C) F<sub>2</sub>
D) Cl<sub>2</sub>
Q3) Which of the following compounds will behave least like an ideal gas at low temperatures?
A) Ar
B) CCl<sub>4</sub>
C) O<sub>2</sub>
D) Kr
E) F<sub>2</sub>
Q4) Why does the rate of effusion increase with a decrease in the molar mass?
Q5) Give the major gas in dry air.
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Chapter 6: Thermochemistry
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Sample Questions
Q1) When 1.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C,33.9 kJ are absorbed and P V for the vaporization process is equal to 2.90 kJ,then
A) E = 31.0 kJ and H = 33.9 kJ.
B) E = 36.8 kJ and H = 33.9 kJ.
C) E = 33.9 kJ and H = 31.0 kJ.
D) E = 33.9 kJ and H = 36.8 kJ.
Q2) Where does the energy absorbed during an endothermic reaction go?
Q3) A piece of iron (mass = 25.0 g)at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K.Assuming that no heat is lost to the cup or the surroundings,what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.
A) 348 K
B) 308 K
C) 287 K
D) 325 K
E) 388 K
Q4) Explain the difference between H and DE.
Q5) Give the temperature and pressure for the standard state for a liquid.
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Chapter 7: The Quantum-Mechanical Model of the Atom
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Sample Questions
Q1) What is the maximum number of f orbitals that are possible?
A) 0
B) 3
C) 7
D) 8
E) 9
Q2) When an electric current is passed through a tube containing mercury,mercury atoms absorb some of the electrical energy and reemit it as a ________ color.
A) white
B) yellow
C) violet
D) blue
E) red
Q3) What is the maximum number of p orbitals that are possible?
A) 0
B) 3
C) 6
D) 12
E) 9
Q4) Give an example of a d orbital.
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Chapter 8: Periodic Properties of the Elements
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Sample Questions
Q1) Choose the paramagnetic species from below.
A) Ba
B) O<sup>2</sup>
C) Zn<sup>2</sup>
D) Cd
E) Nb<sup>3</sup>
Q2) The element that corresponds to the electron configuration 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<sup> 1</sup>3d<sup>5</sup> is
A) titanium.
B) vanadium.
C) chromium.
D) manganese.
E) iron.
Q3) Give the number of valence electrons for Te.
A) 1
B) 7
C) 3
D) 5
E) 6
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Chapter 9: Chemical Bonding I: Lewis Theory
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Sample Questions
Q1) Identify the compound with atoms that have an incomplete octet.
A) ICl<sub>5</sub>
B) CO<sub>2</sub>
C) BF<sub>3</sub>
D) Cl<sub>2</sub>
E) CCl<sub>4</sub>
Q2) Which of the following elements can form compounds with an expanded octet?
A) Br
B) O
C) Na
D) H
E) All of the above elements can form compounds with an expanded octet.
Q3) How many electrons does an hydroxyl radical contain?
A) 7 electrons
B) 6 electrons
C) 8 electrons
D) 9 electrons
E) 5 electrons
Q4) Describe the difference between a pure covalent bond and a polar covalent bond.
Q5) Draw the Lewis Dot structure for Al<sup>3+</sup>.
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Chapter 10: Chemical Bonding Ii: Molecular Shapes,valence
Bond Theory,
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Sample Questions
Q1) Give the molecular geometry and number of electron groups for SF<sub>4</sub>.
A) square planar, 6 electron groups
B) square pyramidal, 6 electron groups
C) T-shaped, 5 electron groups
D) octahedral, 6 electron groups
E) seesaw, 5 electron groups
Q2) Use molecular orbital theory to determine whether He<sub>2</sub><sup>2</sup> or He<sub>2</sub> is more stable.Draw the molecular orbital diagram for each and explain your answer.
Q3) Place the following in order of decreasing dipole moment. I.cis-CHCl=CHCl II.trans-CHCl=CHCl III.cis-CHF=CHF
A) III > I > II
B) II > I > III
C) I > III > II
D) II > III > I
E) I = III > II
Q4) According to molecular orbital theory,what is an antibonding orbital?
Q5) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.
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Chapter 11: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) Identify the characteristics of a gas.
A) indefinite shape and volume
B) indefinite shape, but definite volume
C) definite shape and volume
D) none of the above
E) all of the above
Q2) Define vaporization.
A) A liquid becomes a gas.
B) A gas becomes a liquid.
C) A gas becomes a solid.
D) A solid becomes a gas.
E) A solid becomes a liquid.
Q3) Why is the H<sub>vap</sub> higher than H<sub>fus </sub>for a given compound?
Q4) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.
A) absolute temperature
B) definite temperature
C) fluid temperature
D) critical temperature
E) solid temperature
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Chapter 12: Solids and Modern Materials
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Sample Questions
Q1) Identify a use for ceramics.
A) beakers
B) bridges
C) furniture
D) wooden decks
E) bricks
Q2) Give the coordination number for a face-centered cubic cell.
A) 2
B) 8
C) 12
D) 10
E) 6
Q3) Which of the following substances should have the highest melting point?
A) Fe
B) Ne
C) Xe
D) N<sub>2</sub>
E) CO
Q4) Give the edge length in terms of r for a simple cubic cell.
Q5) Describe the difference between the conduction band and the valence band.
Page 14
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Chapter 13: Solutions
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Sample Questions
Q1) Determine the partial pressure of oxygen necessary to form an aqueous solution that is 7.1 × 10<sup>-4</sup><sup> </sup>M O<sub>2</sub> at 25°C.The Henry's law constant for oxygen in water at 25°C is 1)3 × 10<sup>-3</sup> M/atm.
A) 1.1 atm
B) 0.92 atm
C) 0.88 atm
D) 1.8 atm
E) 0.55 atm
Q2) A solution of CsF in water has X<sub>CsF</sub> = 0.0700.What is the molality?
A) 3.55 m CsF
B) 3.89 m CsF
C) 4.18 m CsF
D) 7.53 m CsF
Q3) Give the preparation of rock candy.
Q4) Explain why the van't Hoff factor for MgCl<sub>2</sub> is less than its predicted value.
Q5) Define colloid.
Q6) Explain why water does not dissolve in gasoline.
Q7) Define osmosis.
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Chapter 14: Chemical Kinetics
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Sample Questions
Q1) What is the overall order of the following reaction,given the rate law? X + 2Y 4Z Rate = k[X][Y]
<sup> </sup>
A) 3rd order
B) 5th order
C) 2nd order
D) 1st order
E) 6th order
Q2) What is the overall order of the following reaction,given the rate law? 2X + 3Y 2Z Rate = k[X]<sup>1</sup>[Y]<sup>2</sup>
<sup> </sup>
A) 3rd order
B) 5th order
C) 2nd order
D) 1st order
E) 0th order
Q3) Define half-life.
Q4) Define the frequency factor.
Q5) What happens in the concentration of reactants and products during a chemical reaction?
16
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Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) Consider the following reaction at equilibrium.What will happen if the volume increased? 4 FeS<sub>2</sub>(s)+ 11 O<sub>2</sub>(g) 2 Fe<sub>2</sub>O<sub>3</sub>(s)+ 8 SO<sub>2</sub>(g)
A) The equilibrium constant will increase.
B) The equilibrium will change in the direction of the reactants.
C) The equilibrium will change in the direction of the products.
D) No change in equilibrium is observed.
E) The equilibrium constant will decrease.
Q2) Consider the following reaction at equilibrium.What effect will decreasing the temperature have on the system? CO<sub>2</sub>(g)+ 2 H<sub>2</sub>O(l) CH<sub>4</sub>(g)+ 2 O<sub>2</sub>(g) H° = +890 kJ
A) The reaction will shift to the left in the direction of reactants.
B) The equilibrium constant will decrease.
C) The equilibrium constant will increase.
D) The reaction will shift to the right in the direction of products.
E) No effect will be observed.
Q3) Define Le Chatelier's Principle.
Q4) Can the K<sub>p</sub> and K<sub>c</sub> for a reaction ever have the same value? Why or why not?
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Chapter 16: Acids and Bases
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Sample Questions
Q1) Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C.
A) 7.1 × 10<sup>-5</sup> M
B) 4.2 × 10<sup>-10</sup> M
C) 8.7 × 10<sup>-10</sup> M
D) 6.5 × 10<sup>-5</sup> M
E) 1.4 × 10<sup>-10</sup> M
Q2) Determine the pH of a 0.188 M NH<sub>3</sub> solution at 25°C.The K<sub>b </sub>of NH<sub>3</sub> is 1.76 × 10<sup>-5</sup>.
A) 5.480
B) 2.740
C) 8.520
D) 11.260
E) 12.656
Q3) Determine the [OH ] concentration in a 0.344 M Ba(OH)<sub>2</sub> solution.
A) 0.688 M
B) 0.344 M
C) 0.463
D) 0.334
E) 13.666
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Chapter 17: Aqueous Ionic Equilibrium
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Sample Questions
Q1) Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10<sup>-4</sup>.
A) 1.12 × 10<sup>-4</sup>
B) 0.0450
C) 4.25
D) 0.342
E) 5.53
Q2) Determine the solubility of the ions that is calculated from the Ksp for Na<sub>3</sub>PO<sub>4</sub>.
A) S<sup>4</sup>
B) 27S<sup>3</sup>
C) 3S<sup>2</sup>
D) 27S<sup>4</sup>
E) 9S<sup>4</sup>
Q3) Explain the common ion effect with respect to molar solubility.
Q4) Define a buffer.
Q5) Give the name of the compound that is in antifreeze and is toxic to pets.
Q6) Identify the compound that is in stalactites and stalagmites.
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Chapter 18: Free Energy and Thermodynamics
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Sample Questions
Q1) What is true if ln K is 1?
A) G°<sub>rxn</sub> is positive and the reaction is spontaneous in the forward direction.
B) G°<sub>rxn</sub> is negative and the reaction is spontaneous in the forward direction.
C) G°<sub>rxn</sub> is negative and the reaction is spontaneous in the reverse direction.
D) G°<sub>rxn</sub> is positive and the reaction is spontaneous in the reverse direction.
E) G°<sub>rxn</sub> is zero and the reaction is at equilibrium.
Q2) Determine G°<sub>rxn</sub> for the following reaction at 338 K. FeO(s)+ CO(g) Fe(s)+ CO<sub>2</sub>(g) H°= -11.0 kJ; S°= -17.4 J/K
A) +191.0 kJ
B) -5.1 kJ
C) +5.1 kJ
D) -16.1 kJ
E) +16.1 kJ
Q3) Why is heating your home with gas more efficient than heating it with electricity?
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Chapter 19: Electrochemistry
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Sample Questions
Q1) In a nickel-cadmium battery,NiO(OH)is reduced to
A) Ni(OH)<sub>4</sub>.
B) NiO<sub>2</sub>.
C) Ni.
D) Ni(OH)<sub>2</sub>.
E) NiOH.
Q2) Which of the following metals will dissolve in nitric acid but NOT hydrochloric?
A) Li
B) Zn
C) Mg
D) Ag
E) Al
Q3) Identify the battery that is used as a common flashlight battery.
A) dry-cell battery
B) lithium ion battery
C) lead-acid storage battery
D) NiCad battery
E) fuel cell
Q4) Why,if we multiply a reaction by 2,don't we multiply its E°<sub>red</sub> by 2?
Q5) Why is sugar water NOT a good conductor of current?
Page 21
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Chapter 20: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Explain the concept of "magic numbers."
Q2) Which of the following nuclides are most likely to decay via positron emission?
A) Cs-137
B) I-131
C) Al-24
D) K-42
E) N-14
Q3) Determine the binding energy per nucleon of an Mg-24 nucleus.The Mg-24 nucleus has a mass of 23.985045.A proton has a mass of 1.00728 amu,a neutron has a mass of 1.008665 amu,and 1 amu is equivalent to 931.5 MeV of energy.
A) 0.3050 MeV
B) 8.83 MeV
C) 0.113 MeV
D) 192 MeV
E) 4.41 MeV
Q4) What is the "mass defect"?
Q5) Define radioactivity.
Q6) Describe what is meant by the term "valley of stability"?
Q7) Define chain reaction in terms of the fission of uranium nucleus.
Q8) List two problems associated with nuclear power.
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Chapter 21: Organic Chemistry
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Sample Questions
Q1) Which of the following names is correct?
A) 2-methyl-5-hexyne
B) 3-propyl-1-butyne
C) 3-butyl-3-propyl-1-pentyne
D) 3-methyl-1-pentyne
E) 3-ethyl-3-butyl-1-hexyne
Q2) Why doesn't benzene typically undergo addition reactions like the alkenes do?
Q3) Choose the weak base from the compounds below.
A) (CH<sub>3</sub>)<sub>2</sub>NH
B) CH<sub>3</sub>COOH
C) CH<sub>3</sub>SCH<sub>3</sub>
D) CH<sub>3</sub>CH<sub>3</sub>
E) CH<sub>3</sub>CH<sub>2</sub>I
Q4) Identify the formula for an alkane.
A) C<sub>n</sub>H<sub>2n+2</sub>
B) C<sub>n</sub>H<sub>2n-2</sub>
C) C<sub>n</sub>H<sub>2n</sub>
D) C<sub>n</sub>H<sub>n</sub>
E) C<sub>n</sub>H<sub>2n+4</sub>
Q5) What does the term "racemic mixture" mean?
Page 23
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Chapter 22: Biochemistry
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Sample Questions
Q1) In the protein,Arg-Pro-Lys-Val,which amino acid contains the C-terminal group?
A) arginine
B) lysine
C) valine
D) proline
Q2) Identify the smallest amino acid.
A) glycine
B) isoleucine
C) phenylalanine
D) cysteine
E) aspartic acid
Q3) Which of the following shows all of the tripeptides that can be formed from one molecule each of lysine (Lys),threonine (Thr),and hisitidine (His)?
A) LysThrHis
B) LysThrHis, LysHisThr, HisThrLys, HisLysThr, ThrLysHis, ThrHisLys
C) LysThrHis, LysHisThr, HisLysThr, ThrHisLys
D) LysThrHis, LysHisThr, HisLysThr
E) LysThrHis and LysHisThr
Q4) Why does the melting point of fatty acids decrease with the number of double bonds present?
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Chapter 23: Chemistry of the Nonmetals
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Sample Questions
Q1) Give the formula of the compound that is in quartz.
A) SiO<sub>4</sub>
B) Si<sub>2</sub>O<sub>3</sub>
C) SiO<sub>3</sub>
D) Si<sub>2</sub>O<sub>4</sub>
E) SiO<sub>2</sub>
Q2) Which of the following statements is TRUE?
A) Ionic carbides form between carbon and another high electronegativity element.
B) Carbides are soft materials with low melting points.
C) Metallic carbides are more malleable than the pure metal.
D) Covalent carbides are formed between carbon and a low electronegativity nonmetal.
E) None of the above is true.
Q3) Determine the oxidation state of carbon in the carbon monoxide,CO.
A) +2
B) +4
C) +3
D) +6
E) +8
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Chapter 24: Metals and Metallurgy
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Q1) Chromate,CrO<sub>4</sub><sup>-</sup>,has a(n)________ shape.
A) octahedral
B) trigonal bipyramidal
C) trigonal pyramidal
D) tetrahedral
E) square
Q2) Identify the metal most commonly used for wires in the electrical industry.
A) copper
B) silver
C) lead
D) aluminum
E) potassium
Q3) ________ is a soft-white metal that has been found as a contaminant in crude oil.
A) Vanadium
B) Gold
C) Silver
D) Mercury
E) Copper
Q4) Why does a "two-phase" structure occur in a substitutional alloy?
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Chapter 25: Transition Metals and Coordination Compounds
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Q1) Identify the isomers that occurs when a coordinated ligand exchanges places with the uncoordinated counterion.
A) linkage isomers
B) geometric isomers
C) coordination isomers
D) optical isomers
E) stereoisomers
Q2) Which of the following compounds can exhibit cis-trans isomerism?
A) [Fe(CO)<sub>5</sub>NO<sub>2</sub>]<sup>2+</sup>
B) [Cu(CO)<sub>5</sub>Br]<sup>+</sup>
C) [MnClBr<sub>3</sub>]<sup>2-</sup>
D) [Mn(H<sub>2</sub>O)<sub>6</sub>]3<sup>+</sup>
E) [Ni(CO)<sub>2</sub>(NH<sub>3</sub>)<sub>2</sub>]<sup>2+</sup>
Q3) Identify the geometry around the Fe<sup>2+</sup> ion in the hemoglobin complex.
A) octahedral
B) tetrahedral
C) pentadral
D) hexadral
E) heptadral
Q4) Why is +2 a common oxidation state for transition elements?
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