Fundamentals of Chemistry Exam Practice Tests - 1830 Verified Questions

Fundamentals of Chemistry Exam Practice Tests

Course Introduction

Fundamentals of Chemistry introduces students to the basic principles and concepts underlying the science of chemistry. This course covers essential topics such as atomic structure, the periodic table, chemical bonding, stoichiometry, chemical reactions, states of matter, and thermodynamics. Emphasis is placed on developing problem-solving skills, understanding laboratory techniques, and applying chemical concepts to real-world scenarios. Through lectures, discussions, and hands-on experiments, students will gain a solid foundation in chemistry, preparing them for advanced study in scientific and health-related fields.

Recommended Textbook

Principles of General Chemistry 2nd Edition by Martin Silberberg

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23 Chapters

1830 Verified Questions

1830 Flashcards

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Page 2

Chapter 1: Keys to the Study of Chemistry

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Sample Questions

Q1) The numerical value of any temperature expressed in Celsius is always different from the numerical value of the same temperature in Fahrenheit.

A)True

B)False

Answer: False

Q2) The numerical value of any temperature expressed in Celsius is always different from the numerical value of the same temperature in kelvin.

A)True

B)False

Answer: True

Q3) Which of the following activities is not a part of good science?

A)proposing a theory

B)developing a hypothesis

C)making quantitative observations

D)designing experiments

E)indulging in speculation

Answer: E

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Chapter 2: The Components of Matter

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Sample Questions

Q1) Who is credited with discovering the atomic nucleus?

A)Dalton

B)Gay-Lussac

C)Thomson

D)Millikan

E)Rutherford

Answer: E

Q2) What is the name of the acid formed when HCN gas is dissolved in water?

A)cyanic acid

B)hydrocyanic acid

C)cyanous acid

D)hydrocyanous acid

E)hydrogen cyanide

Answer: B

Q3) Name the three important "laws" that were accounted for by Dalton's atomic theory.

Answer: Laws of conservation of mass;definite composition;multiple proportions

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Chapter 3: Stoichiometry of Formulas and Equations

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Sample Questions

Q1) Lead(II)nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography.Calculate the mass of lead in 139 g of Pb(NO₃)₂.

A)107 g

B)90.8 g

C)87.0 g

D)83.4 g

E)62.6 g

Answer: C

Q2) Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain.Calculate the mass in grams of 3.65 \(\times\) 10²⁰ molecules of SO₃.

A)6.06 \(\times\) 10^-4 g

B)2.91 \(\times\) 10^-2 g

C)4.85 \(\times\) 10^-2 g

D)20.6 g

E)1650 g

Answer: C

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Chapter 4: Three Major Classes of Chemical Reactions

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Sample Questions

Q1) Write down the oxidation number of the indicated atom in each of the following formulas:

a.Si in SiO₂

b.Cl in ClO₂^- c.Mn in KMnO₄ d.C in C₆H₁₂O₆

Q2) Which of the following is a strong base?

A)NH₃

B)Ca(OH)₂

C)Al(OH)₃

D)B(OH)₃

E)CH₃OH

Q3) All combustion reactions are classified as combination reactions. A)True B)False

Q4) For each of the following species,write down,next to the formula,the oxidation number of the indicated atom.

a.P in H₂PO₂^-

b.S in Na₂S₂O₃ c.C in CH₂O

Page 6

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Chapter 5: Gases and the Kinetic-Molecular Theory

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Sample Questions

Q1) A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L.What is its volume when the temperature is -15.8°C and its pressure is 524 torr?

A)3.69 L

B)11.6 L

C)20.2 L

D)63.5 L

E)It is not possible,since the volume would have to be negative.

Q2) What is the density of carbon dioxide gas at -25.2°C and 98.0 kPa?

A)0.232 g/L

B)0.279 g/L

C)0.994 g/L

D)1.74 g/L

E)2.09 g/L

Q3) The air pressure in a volleyball is 75 psi.What is this pressure in torr?

A)520 torr

B)562 torr

C)3900 torr

D)7600 torr

E)75,000 torr

Q4) State Avogadro's Law.

Page 7

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Chapter 6: Thermochemistry: Energy Flow and Chemical Change

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Sample Questions

Q1) a.Write a balanced equation for the combustion of benzene,C₆H₆(l)in oxygen.

b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation,\(\Delta\)H°_f ,given the data: \(\Delta\)H°_f [CO₂(g)] = -394 kJ;\(\Delta\)H°_f [H₂O(l)] = -286 kJ

Q2) A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings.If the initial internal energy,E,is 61.2 kJ,what is the final value of E?

A)32.7 kJ

B)46.5 kJ

C)75.9 kJ

D)82.8 kJ

E)89.7 kJ

Q3) For a reaction in a sealed,rigid container,\(\Delta\)H is always greater than \(\Delta\)E.

A)True

B)False

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Page 8

Chapter 7: Quantum Theory and Atomic Structure

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Sample Questions

Q1) A radio wave has a frequency of 8.6 \(\times\) 10⁸ Hz.What is the energy of one photon of this radiation?

A)7.7 \(\times\) 10^-43 J

B)2.3 \(\times\) 10^-34 J

C)5.7 \(\times\) 10^-25 J

D)1.7 \(\times\) 10^-16 J

E)> 10^-15 J

Q2) Continuous spectra are characteristic of heated solids.

A)True

B)False

Q3) In the Bohr model of the hydrogen atom,the electron moves in a circular path which Bohr referred to as an orbital.

A)True

B)False

Q4) In the quantum mechanical treatment of the hydrogen atom,the probability of finding an electron at any point is proportional to the wave function \(\varPsi\) .

A)True

B)False

Q5) What is the speed of an electron in m/s if its wavelength is 0.155 nm?

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Chapter 8: Electron Configuration and Chemical Periodicity

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Sample Questions

Q1) In moving down a group in the periodic table,the oxides of the elements become more acidic in nature.

A)True

B)False

Q2) What is the correct order of decreasing size of the following ions?

A)P^3- > Cl^- > K⁺ > Ca²⁺

B)Ca²⁺ > K⁺ > Cl^- > P^3-

C)K⁺ > Cl^- > Ca²⁺ > P^3-

D)K⁺ > Cl^- > P^3- > Ca²⁺

E)None of these is correct.

Q3) Which of the following electron configurations represents the ground state for an element?

A)[Ne]3s¹3p¹

B)[He]2s¹2p³

C)[Ne]3s²3p²3d¹

D)[Ne]3s²3p³3d¹

E)[Ne]3s²3p³

Q4) First ionization energies of neutral atoms may be positive or negative.

A)True

B)False

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Chapter 9: Models of Chemical Bonding

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Sample Questions

Q1) Which one of the following properties is least characteristic of substances composed of small,covalently-bonded molecules?

A)low melting point

B)low boiling point

C)weak bonds

D)poor electrical conductor when solid

E)poor electrical conductor when molten

Q2) A hypothetical ionic substance will not form merely because it has a high lattice energy.Explain why,using energy-based arguments.

Q3) Which of the following contains ionic bonding?

A)CO

B)SrF₂

C)Al

D)OCl₂

E)HCl

Q4) In not more than three sentences,describe the electron arrangement responsible for bonding in Cl₂ molecules.

Q5) Covalent bonding typically occurs when a ______________ bonds with a

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Chapter 10: The Shapes of Molecules

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Sample Questions

Q1) According to VSEPR theory,a molecule with the general formula

AX₄E₂ will have a _____ molecular shape.

A)tetrahedral

B)square pyramidal

C)square planar

D)octahedral

E)see-saw

Q2) Which of the following has no net dipole moment?

A)N₂O

B)NF₃

C)H₂Se

D)TeO₃

E)CH₃Cl

Q3) Predict the actual bond angle in SeCl₂ using the VSEPR theory.

A)more than 120°

B)between 109° and 120°

C)between 90° and 109°

D)exactly 90°

E)less than 90°

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Page 12

Chapter 11: Theories of Covalent Bonding

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Sample Questions

Q1) A molecule with the formula AX₃E uses _________ to form its bonds.

A)s and p atomic orbitals

B)sp³ hybrid orbitals

C)sp² hybrid orbitals

D)sp hybrid orbitals

E)sp³d² hybrid orbitals

Q2) The nitrosonium ion,NO⁺,forms a number of interesting complexes with nickel,cobalt,and iron.According to molecular orbital theory,which of the following statements about NO⁺ is correct?

A)NO⁺ has a bond order of 2 and is paramagnetic.

B)NO⁺ has a bond order of 2 and is diamagnetic.

C)NO⁺ has a bond order of 3 and is paramagnetic.

D)NO⁺ has a bond order of 3 and is diamagnetic.

E)None of these statements is correct.

Q3) A molecule with the formula AX₄E uses _________ to form its bonds.

A)sp² hybrid orbitals

B)sp³ hybrid orbitals

C)sp³d hybrid orbitals

D)sp³d² hybrid orbitals

E)None of these choices is correct.

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Chapter 12: Intermolecular Forces: Liquids,solids,and Phase Changes

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Sample Questions

Q1) Which of the following should have the lowest boiling point?

A)C₅H₁₂

B)C₆H₁₄

C)C₈H₁₈

D)C₁₀H₂₂

E)C₁₂H₂₆

Q2) The surface tension of water is lowered when a detergent is present in solution.

A)True

B)False

Q3) Which of the following terms refers to the resistance of a liquid to flow?

A)surface tension

B)capillary action

C)viscosity

D)adhesion

E)cohesion

Q4) In the packing of identical atoms with cubic unit cells,the packing efficiency increases as the coordination number increases.

A)True

B)False

Page 14

Q5) How do the electrical properties of semiconductors differ from those of metals?

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Chapter 13: The Properties of Solutions

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Sample Questions

Q1) For a given solution,which of the following concentration values will change as temperature changes?

A)mass percent

B)molality

C)mole fraction

D)molarity

E)None of these choices is correct.

Q2) If the shell of a raw egg is carefully dissolved away,and the egg in its flexible membrane is then placed in distilled water,the egg's volume will expand.Explain.

Q3) The solubility of gases in water increases with increase in the pressure of the gas.

A)True

B)False

Q4) When two pure substances are mixed to form a solution

A)heat is released.

B)heat is absorbed.

C)there is an increase in entropy.

D)there is a decrease in entropy.

E)entropy is conserved.

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Chapter 14: The Main-Group Elements: Applying Principles of Bonding and Structure

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Sample Questions

Q1) Name the three allotropes of carbon and briefly describe their properties and structures.

Q2) Which of the following oxides will be the most acidic?

A)Al₂O₃

B)Ga₂O₃

C)In₂O₃

D)Tl₂O₃

E)None of these oxides is acidic.

Q3) Predict the products for the following set of reactants.

Cl₂(g)+ I^-(aq) \(\to\)

A)ICl

B)ICl₂

C)ICl₃

D)I₂ + Cl^-

E)I + Cl₂^-

Q4) Phosphoric acid (H₃PO₄)is a strong acid.

A)True

B)False

Q5) Name two different classes (types)of hydride.

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Chapter 15: Organic Compounds and the Atomic Properties of

Carbon

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Sample Questions

Q1) Given that each 3-base sequence in DNA is a "code word" for a particular amino acid,how many different code words are possible using a 3-base sequence and the bases available in DNA?

Q2) Carboxylic acids are weak acids.

A)True

B)False

Q3) Esters can be formed by the dehydration-condensation of a carboxylic acid and an alcohol.

A)True

B)False

Q4) A characteristic reaction of alkenes is addition.

A)True

B)False

Q5) Explain what is meant by "complementary" in the context of DNA strands.

Q6) All the carbon atoms in a molecule of benzene lie in the same plane.

A)True

B)False

Q8) Name the three component parts of a nucleotide. Page 17

Q7) Draw and name four alkenes with the formula C₄H₈.

Q9) Draw and name all stable molecules with the formula C₅H₁₂.

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Page 18

Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions

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Sample Questions

Q1) The reaction CH₃NC(g) \(\to\) CH₃CN(g)is first-order with respect to methyl isocyanide,CH₃NC.If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react,what is the rate constant in units of min^-1?

A)-0.135 min^-1

B)0.0279 min^-1

C)0.089 min^-1

D)0.135 min^-1

E)35.8 min^-1

Q2) Which of the following sets of units could be appropriate for a zero-order rate constant?

A)s^-1

B)L mol^-1 s^-1

C)L² mol^-2 s^-1

D)L³ mol^-3 s^-1

E)mol L^-1 s^-1

Q3) The rate of a reaction is determined by the rate of the fastest step in the mechanism.

A)True

B)False

Page 19

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Chapter 17: Equilibrium: the Extent of Chemical Reactions

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Sample Questions

Q1) Unless \(\Delta\)H°_rxn = 0,a change in temperature will affect the value of the equilibrium constant K_c.

A)True

B)False

Q2) Which of the following has an effect on the magnitude of the equilibrium constant?

A)activation energy of the forward reaction

B)concentrations of the reactants and products

C)presence of a catalyst

D)change in volume of container

E)change in temperature

Q3) Once a reaction system reaches equilibrium,the concentrations of reactions and products no longer change.

A)True

B)False

Q4) For some gas-phase reactions,K_p = K_c.

A)True

B)False

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Chapter 18: Acid-Base Equilibria

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Sample Questions

Q1) Calcium oxide,CaO,also known as quick lime,will react with carbon dioxide to form calcium carbonate,CaCO₃.Which species,if any,acts as a Lewis acid in the reaction?

A)Ca²⁺

B)O^2-

C)CO₂

D)CaCO₃

E)None of the species acts as a Lewis acid in this reaction.

Q2) Which one of the following pairs is not a conjugate acid-base pair?

A)H₂O/OH^-

B)H₂O₂/HO₂^-

C)OH^-/O^2-

D)H₂PO₄^-/HPO₄^2-

E)HCl/H⁺

Q3) Which of the following pairs has the stronger acid listed first?

A)H₂AsO₃,H₂AsO₄ B)HI,HBr

C)HClO,HClO₃

D)H₂S,HCl

E)H₂SO₃,H₂SO₄

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Chapter 19: Ionic Equilibria in Aqueous Systems

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Sample Questions

Q1) A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH₃COOH).What is the pH of the buffer?

A)The pH will be pK_a - 0.30,where pK_a is that of acetic acid.

B)The pH will be greater than the pK_a for acetic acid.

C)The pH will be less than the value in answer a.

D)The pH will be equal to the pK_a for acetic acid.

E)More information is needed to solve the problem.

Q2) If the pH of a buffer solution is greater than the pK_a value of the buffer acid,the buffer will have more capacity to neutralize added base than added acid.

A)True

B)False

Q3) A CH₃COOH/CH₃COO^- buffer can be produced by adding a strong acid to a solution of CH₃COO^- ions.

A)True

B)False

Q4) Make a clear distinction between buffer range and buffer capacity.

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22

Chapter

Direction of Chemical Reactions

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Sample Questions

Q1) Which relationship or statement best describes \(\Delta\)S° for the following reaction?

2NH₃(g)+ 2ClF₃(g) \(\to\) 6HF(g)+ N₂(g)+ Cl₂(g)

A)(\(\Delta\)S° \(\approx\) 0)

B)(\(\Delta\)S° < 0)

C)(\(\Delta\)S° > 0)

D)(\(\Delta\)S° = \(\Delta\)H°/T)

E)More information is needed to make a reasonable prediction.

Q2) For a chemical reaction to be non-spontaneous at any temperature,which of the following conditions must be met?

A)(\(\Delta\)S° > 0,\(\Delta\)H° > 0)

B)(\(\Delta\)S° > 0,\(\Delta\)H° < 0)

C)(\(\Delta\)S° < 0,\(\Delta\)H° < 0)

D)(\(\Delta\)S° < 0,\(\Delta\)H° > 0)

E)(All reactions are spontaneous at some temperature.

Q3) For what signs of \(\Delta\)H and \(\Delta\)S will a process

a.be spontaneous at high temperatures but not at low temperatures?

b.not be spontaneous at any temperatures?

Q4) State the second and third laws of thermodynamics.

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Chapter 21: Electrochemistry: Chemical Change and Electrical Work

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Q1) A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V)and a Cu/Cu²⁺ electrode (E° = 0.34 V).Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

A)0.001 M

B)0.002 M

C)0.01 M

D)0.02 M

E)0.04 M

Q2) Consider the reaction in the lead-acid cell Pb(s)+ PbO₂(s)+ 2H₂SO₄(aq) \(\to\) 2PbSO₄(aq)+ 2H₂O(l)

For which E°_cell = 2.04 V at 298 K.\(\Delta\)G° for this reaction is

A)-3.94 \(\times\) 10⁵ kJ

B)-3.94 \(\times\) 10² kJ

C)-1.97 \(\times\) 10⁵ kJ

D)-7.87 \(\times\) 10² kJ

E)None of these choices is correct.

Q3) Explain what is meant by a fuel cell.Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Page 24

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Chapter 22: The Transition Elements and Their Coordination Compounds

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Q1) Which of the following atoms has the biggest radius?

A)Ti

B)Cr

C)Fe

D)Ni

E)Zn

Q2) Square planar complexes can exhibit both geometric and optical isomerism.

A)True

B)False

Q3) In complexes of transition metals,the maximum coordination number of the metal is equal to its number of d electrons.

A)True

B)False

Q4) In the spectrochemical series,which one of the following ligands has the strongest field?

A)H₂O

B)CN^-

C)NH₃

D)OH^-

E)Cl^-

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Chapter 23: Nuclear Reactions and Their Applications

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Q1) Briefly explain the relationship between the rad and the rem as units of radiation dosage.

Q2) An 85-kg person exposed to barium-141 receives 2.5 \(\times\) 10⁵ \(\beta\) particles,each with an energy of 5.2 \(\times\) 10^-13 J.How many rads does the person receive?

A)2.4 \(\times\) 10^-20

B)1.5 \(\times\) 10^-7

C)1.8 \(\times\) 10^-16

D)6.1 \(\times\) 10^-15

E)None of these choices is correct.

Q3) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable mode of decay.Illustrate your answer with a schematic graph,properly labeled,showing stable nuclides (nuclei)in relation to number of protons and neutrons.

Q4) Gamma rays are not deflected by an electric field.

A)True

B)False

Q5) Gamma rays are high energy electrons.

A)True

B)False

26

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