Preparatory Chemistry Exam Answer Key - 3674 Verified Questions by Quizplus

Preparatory Chemistry

Exam Answer Key

Course Introduction

Preparatory Chemistry is an introductory course designed to provide students with a solid foundation in the fundamental concepts of chemistry. The course covers essential topics such as atomic structure, chemical bonding, the periodic table, chemical reactions, stoichiometry, states of matter, and basic laboratory techniques. Emphasis is placed on problem-solving skills and conceptual understanding to prepare students for success in college-level general chemistry courses. Through lectures, discussions, and hands-on laboratory experiences, students develop the analytical and practical skills necessary for further study in the sciences.

Recommended Textbook

Chemistry The Central Science 14th Edition by Theodore E. Brown

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24 Chapters

3674 Verified Questions

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Page 2

Chapter 1: Introduction: Matter, energy, and Measurement

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Sample Questions

Q1) Which one of the following is a pure substance?

A)tap water

B)rock

C)air

D)elemental oxygen

E)apple

Answer: D

Q2) In the following list,only ________ is not an example of a chemical reaction.

A)dissolution of a penny in nitric acid

B)the condensation of water vapor

C)a burning candle

D)the formation of polyethylene from ethylene

E)the rusting of iron

Answer: B

Q3) 1.035 × 10-4 L = ________ mL

Answer: 0.1035

Q4) Sn is the symbol for the element ________.

Answer: Tin

Q5) Si is the symbol for the element ________.

Answer: Silicon

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Magnesium reacts with a certain element to form a compound with the general formula MgX.What would the most likely formula be for the compound formed between potassium and element X?

A)K2X

B)KX2

C)K2X3

D)K2X2

E)KX

Answer: A

Q2) The charge on the silver ion in the salt AgCl is ________.

A)+2

B)+1

C)+3

D)+4

E)+5

Answer: B

Q3) Which element is found in Period 2 and Group VIIA?

Answer: fluorine

Q4) What is the name of an alcohol derived from hexane?

Answer: hexanol

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Chapter 3: Chemical Reactions and Reaction Stoichiometry

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Sample Questions

Q1) Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO3 (s) PbO (s)+ CO2 (g)

If the reaction yield is 92.4%,how many grams of lead (II)oxide will be produced by the decomposition of 1.30 g of lead (II)carbonate?

A)1.00

B)1.18

C)1.20

D)1.09

E)1.41

Answer: A

Q2) Balance the following reaction and determine the coefficient of potassium hydroxide. K (s)+ H2O (l) KOH (aq)+ H2 (g)

A)1

B)2

C)3

D)4

E)5

Answer: B

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) In which species does nitrogen have the highest oxidation number?

A)NaNO3

B)HNO2

C)NO2-

D)NH3

E)N2

Q2) All of the following are true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2 except for ________.

A)This solution contains 0.200 mol of Ca3(PO4)2.

B)1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions.

C)There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution.

D)This solution contains 0.800 mol of oxygen atoms.

E)This solution contains 0.600 mol of Ca2+.

Q3) How many grams of an unknown substance with a molar mass of 40.0 are there in 500.0 mL of a 0.175 M solution of the unknown?

Q4) The solvent in an aqueous solution is ________.

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Chapter 5: Thermochemistry

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Sample Questions

Q1) A chemical reaction that releases heat to the surroundings is said to be ________ and has a ________ H at constant pressure.

A)endothermic, positive

B)endothermic, negative

C)exothermic, negative

D)exothermic, positive

E)exothermic, neutral

Q2) In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g)+ 2O2 (g)

CO2 (g)+ 2H2O (l) H = -890.0 kJ

Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

A)-100.1 kJ

B)0.0324 kJ

C)-0.0100 kJ

D)30.9 kJ

E)-1.00 × 105 kJ

Q3) ________ is defined as the energy used to move an object against a force.

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) The ground-state electron configuration for Zn is ________.

A)[Kr]4s23d10

B)[Ar]4s23d10

C)[Ar]4s13d10

D)[Ar]3s23d10

E)[Kr]3s23d10

Q2) Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number?

A)4f

B)4d

C)4p

D)4s

E)none of the above

Q3) Which of the following is not a valid set of four quantum numbers? (n,l,ml,ms)

A)2, 0, 0, +1/2

B)2, 1, 0, -1/2

C)3, 1, -1, -1/2

D)1, 0, 0, +1/2

E)1, 1, 0, +1/2

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) This element reacts with hydrogen to produce a gas with the formula HX.When dissolved in water,HX forms an acidic solution.X is ________.

A)chlorine

B)calcium

C)oxygen

D)germanium

E)arsenic

Q2) Oxides of the active metals combine with acid to form ________.

A)hydrogen gas

B)metal hydrides

C)water and a salt

D)oxygen gas

E)metal hydroxides

Q3) ________ compounds in fireworks are responsible for the observed green colors.

A)barium

B)strontium

C)calcium

D)copper

E)sodium

Q4) [Kr]5s2 is the electron configuration for ________.

Page 9

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) Using the noble gas shorthand notation,write the electron configuration for Fe2+.

Q2) In ionic bond formation,the lattice energy of ions ________ as the magnitude of the ion charges ________ and the radii ________. A)increases, decrease, increase B)increases, increase, increase C)decreases, increase, increase D)increases, increase, decrease E)increases, decrease, decrease

Q3) A triple bond consists of ________ pairs of electrons shared between two atoms. A)1

B)2

C)3

D)4

E)6

Q4) An exothermic reaction should have ________ chemical bonds and decompose to a molecule with ________ bonds.

Q5) Which halogen,bromine or iodine,will form the more polar bond with phosphorus?

Q6) Give the electron configuration of Zn2+.

Page 10

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) How many unhybridized p atomic orbital(s)are found in an sp-hybridized carbon atom?

A)4

B)2

C)0

D)1

E)3

Q2) What is the molecular geometry of ICl5?

Q3) Using the VSEPR model,the electron-domain geometry of the central atom in O3 is ________.

A)linear

B)trigonal planar

C)tetrahedral

D)trigonal bipyramidal

E)octahedral

Q4) The ________ hydrogen orbital overlaps with the ________ bromide orbital in HBr.

Q5) What are the three bond angles in the trigonal bipyramidal structure?

Q6) A ________ compound would display unpaired electrons in the molecular orbital diagram.

Q7) The ________ hydrogen orbital overlaps with the ________ fluoride orbital in HF.

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Chapter 10: Gases

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Sample Questions

Q1) One significant difference between gases and liquids is that ________.

A)a gas is made up of molecules

B)a gas expands to fill its container

C)a gas may consist of both elements and compounds

D)gases are always mixtures

E)All of the above answers are correct.

Q2) A vessel contained N2,Ar,He,and Ne.The total pressure in the vessel was 987 torr.The partial pressures of nitrogen,argon,and helium were 44.0,486,and 218 torr,respectively.The partial pressure of neon in the vessel was ________ torr.

A)42.4

B)521

C)19.4

D)239

E)760

Q3) The temperature and pressure specified by STP are ________ °C and ________ atm.

Q4) What is the rms speed (m/s)of oxygen molecules at 36.0 °C?

Q5) The effusion rate of a gas is proportional to the square root of its molar mass.

A)True

B)False

Page 12

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The property responsible for the "beading up" of water is ________.

A)density

B)viscosity

C)vapor pressure

D)surface tension

E)hydrogen bonding

Q2) Which species has London dispersion forces as the only intermolecular force?

A)CH3CH2OH

B)Ar

C)NH3

D)HBr

E)H2O

Q3) The conversion of a solid to a liquid is called ________.

Q4) On a phase diagram,the critical temperature is ________.

A)the temperature below which a gas cannot be liquefied

B)the temperature above which a gas cannot be liquefied

C)the temperature at which all three states are in equilibrium

D)the temperature required to melt a solid

E)the temperature required to cause sublimation of a solid

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) For a substitutional alloy to form,the two metals combined must have similar

A)ionization potential and electron affinity

B)number of valance electrons and electronegativity

C)reduction potential and size

D)atomic radii and chemical bonding properties

E)band gap and reactivity

Q2) The type of solid that is characterized by low melting point,softness,and low electrical conduction is a molecular solid.

A)True

B)False

Q3) Define a body-centered cubic lattice.

Q4) Trends in melting points for metals can be explained with the ________.

A)intermolecular model

B)electron-sea model

C)thermal conductivity model

D)covalent bonding model

E)ionic bonding model

Q5) Define a face-centered cubic lattice.

Q6) What is an alloy?

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) An aqueous solution with a concentration of 12.5 ppb indicates that there is ________ per liter of solution.

Q2) Of the following,a 0.1 M aqueous solution of ________ will have the lowest freezing point.

A)NaCl

B)Al(NO3)3

C)K2CrO4

D)Na2SO4 E)sucrose

Q3) A solution is prepared by dissolving 15.0 g of NH3 in 250.0 g of water.The density of the resulting solution is 0.974 g/mL.The molarity of NH3 in the solution is ________ M.

A)0.00353

B)0.882

C)60.0

D)3.24

E)3.53

Q4) The ________ is a phenomenon used to differentiate colloids and correct solutions.

Q5) What is the osmotic pressure (in atm)of a 0.0255 M NaCl solution at 25.0 °C?

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) What is the average rate of disappearance (M/s)of I- between 800.0 s and 1200.0 s?

A)2.8 × 10-5

B)3.3 × 10-5

C)5.8 × 104

D)2.3 × 10-5

E)2.6 × 10-4

Q2) The enzyme ________ converts nitrogen into ammonia.

A)oxygenase

B)hydrogenase

C)oxidase

D)nitroglycerine

E)nitrogenase

Q3) A reaction was found to be third order in A.Increasing the concentration of A by a factor of 3 will cause the reaction rate to ________.

A)remain constant

B)increase by a factor of 27

C)increase by a factor of 9

D)triple

E)decrease by a factor of the cube root of 3

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) Le Châtelier's principle states that if a system at equilibrium is disturbed,then more reactants are produced.

A)True

B)False

Q2) If the reaction quotient Q for a reaction is equal to the value of the equilibrium constant K for that reaction at a given temperature,then the reaction is at ________.

Q3) In the coal-gasification process,carbon monoxide reacts with water to produce carbon dioxide and hydrogen gas.In an experiment,0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel.At equilibrium,there were 0.22 mol of CO remaining.Keq at the temperature of the experiment is

A)5.5

B)0.28

C)0.75

D)3.5

E)1.0

Q4) The equilibrium-constant expressed as 1/Keq is for a reaction written in the ________ direction.

Q5) Define the reaction quotient.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) What is the pH of a 0.030 M aqueous solution of calcium hydroxide?

A)1.52

B)12.48

C)10.41

D)12.78

E)1.22

Q2) What is the pOH of a 0.030 M solution of calcium hydroxide?

A)12.78

B)1.22

C)12.48

D)10.41

E)1.52

Q3) Calculate the concentration (in M)of hydroxide ions in a solution at 25.0 °C with a pOH of 3.58.

A)2.63 × 1010

B)3.80 × 10-11

C)1.00 × 10-7

D)3.80 × 103

E)2.63 × 10-4

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Page 18

Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) Which one of the following is not amphoteric?

A)Al(OH)3

B)Ca(OH)2

C)Cr(OH)3

D)Zn(OH)2

E)Sn(OH)2

Q2) Which one of the following is amphoteric?

A)H2SO4

B)H2O2

C)CO2

D)H2O

E)NaOH

Q3) In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

A)0.0100 M KBr

B)0.040 M CuNO3

C)0.030 M NaBr

D)0.020 M LiBr

E)CuBr will have the same solubility in all solutions.

Q4) A complex ion is when a metal ion binds to a ________.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) The C-Cl and C-F bond dissociation energies in CF3Cl are 339 kJ/mol and 482 kJ/mol,respectively.The maximum wavelengths of electromagnetic radiation required to rupture these bonds are ________ and ________,respectively.

A)45.0 nm, 307 nm

B)742 nm, 654 nm

C)482 nm, 248 nm

D)353 nm, 248 nm

E)979 nm, 953 nm

Q2) The amount of atomic O relative to O2 ________.

A)is highest in the troposphere

B)is highest in the stratosphere

C)increases with altitude in the thermosphere

D)decreases with altitude in the thermosphere

E)is essentially independent of altitude in the thermosphere

Q3) THMs are ________.

A)non-toxic

B)natural

C)used in green chemistry

D)suspected carcinogens

E)atmospheric pollutants

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The value of S° for the catalytic hydrogenation of acetylene to ethene, C2H2 (g)+ H2 (g) C2H4 (g)

Is ________ J/K mol.

A)+18.6

B)+550.8

C)+112.0

D)-112.0

E)-18.6

Q2) The standard Gibbs free energy of formation of ________ is zero.

(a) H2O (l) (b)O(g)

A)(a)only

B)(b)only

C)(c)only

D)(b)and (c)

E)(a), (b), and (c)

Q3) The vaporization of a substance at its boiling point is an isothermal process.

A)True B)False

Page 21

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Chapter 20: Electrochemistry

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Sample Questions

Q1) What is the anode in an alkaline battery?

A)MnO2

B)KOH

C)Zn powder

D)Mn2O3

E)Pt

Q2) The standard cell potential (E°cell)for the voltaic cell based on the reaction below is ________ V. Sn2+ (aq)+ 2Fe3+ (aq) 2Fe2+ (aq)+ Sn4+ (aq)

A)+0.46

B)+0.617

C)+1.39

D)-0.46

E)+1.21

Q3) The standard reduction potential of X is 1.23 V and that of Y is -0.44 V; therefore X is oxidized by Y.

A)True

B)False

Q4) What is a galvanized iron nail?

Q5) Define a coulomb.

Page 22

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Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) The half-life of 218Po is 3.1 minutes.How much of a 155 gram sample remains after 0.40 hours?

A)0.00067 g

B)0.0072 g

C)0.72 g

D)0.0047 g

E)none of the above

Q2) What exposure level to radiation is fatal to most humans?

A)100 rem

B)200 rem

C)600 rem

D)300 rem

E)1000 rem

Q3) Control rods in a nuclear reactor are composed of boron and ________.

Q4) What isotope of what element is produced if uranium-238 undergoes alpha decay?

Q5) Electrons do not exist in the nucleus,yet beta emission is ejection of electrons from the nucleus.How does this happen?

Q6) The SI unit of an absorbed dose of radiation is the gray.

A)True

B)False

Page 23

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) Which form of elemental sulfur is the most stable at room temperature?

A)rhombic sulfur

B)monoclinic

C)hexagonal

D)triclinic

E)tetraclinic

Q2) ________ are typically basic while ________ are typically acidic.

A)Nonmetal oxides, metal oxides

B)Metals, nonmetals

C)Metal oxides, nonmetal oxides

D)Nonmetals, metals

Q3) Compounds containing only boron and hydrogen are called ________.

Q4) The most nonmetallic element is ________.

A)S

B)P

C)Cl

D)Br

E)Se

Q5) KNO3 and NaNO3 are also known as ________.

Q6) What are the principal components used in making soda-lime glass?

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Chapter 23: Transition Metals and Coordination Chemistry

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Q1) What is the oxidation number of the central metal in [Mo(H2O)5NO3]Cl2

Q2) What is the oxidation number of chromium in Cr[(NH3)4Cl2]Cl?

A)-3

B)+3

C)+2

D)-2

E)0

Q3) What is the mechanism used in humans to combat blood bacterial growth via deprivation of iron?

Q4) Green and orange are complementary colors.

A)True

B)False

Q5) Which of the following can form both high- and low-spin octahedral complexes?

A)Cr2+

B)Cr3+

C)Zn2+

D)Cu+

E)All of the above can form either high- or low-spin complexes.

Page 25

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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

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Sample Questions

Q1) How many isomers are possible for C4H10?

A)1

B)2

C)3

D)4

E)10

Q2) Which of the following compounds do not contain an sp3 hybridized oxygen atom?

A)ketones

B)alcohols

C)ethers

D)esters

E)water

Q3) The octane number of straight-run gasoline is about ________.

A)0

B)25

C)50

D)75

E)93

Q4) Why is cyclopropane more reactive than propane?

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