Honors General Chemistry Final Exam - 1830 Verified Questions

Honors General Chemistry

Final Exam

Course Introduction

Honors General Chemistry is an accelerated introductory course designed for students with a strong interest and background in chemistry. The course covers fundamental concepts such as atomic and molecular structure, chemical bonding, stoichiometry, thermodynamics, kinetics, equilibrium, and electrochemistry. Emphasis is placed on developing critical thinking and problem-solving skills through in-depth discussions, laboratory experiments, and advanced applications of chemical principles. Students will engage in challenging coursework and laboratory work that foster a deeper understanding of chemical phenomena and prepare them for higher-level studies in chemistry and related fields.

Recommended Textbook

Principles of General Chemistry 2nd Edition by Martin Silberberg

Available Study Resources on Quizplus

23 Chapters

1830 Verified Questions

1830 Flashcards

Source URL: https://quizplus.com/study-set/3726 Page 2

Chapter 1: Keys to the Study of Chemistry

Available Study Resources on Quizplus for this Chatper

66 Verified Questions

66 Flashcards

Source URL: https://quizplus.com/quiz/74295

Sample Questions

Q1) The S.I.unit of speed (velocity)is

A)km/h

B)km/s

C)m/h

D)m/s

E)none of these choices is correct

Answer: D

Q2) An important aim in much chemical work is to use macroscopic measurements in order to gain an understanding of the microscopic world.

A)True

B)False

Answer: True

Q3) Use the relationship between temperatures in Celsius and Fahrenheit to calculate the temperature at which

a.the numerical value is the same on both scales.

b.the Fahrenheit number is exactly twice the Celsius number.

Answer: a.40.°F = - 40.°C

b.320.°F = 160.°C

To view all questions and flashcards with answers, click on the resource link above.

3

Chapter 2: The Components of Matter

Available Study Resources on Quizplus for this Chatper

91 Verified Questions

91 Flashcards

Source URL: https://quizplus.com/quiz/74296

Sample Questions

Q1) Which one of the following combinations of names and formulas of ions is incorrect?

A)O₂^- oxide

B)Al³⁺ aluminum

C)NO₃^- nitrate

D)PO₄^3- phosphate

E)CrO₄^2- chromate

Answer: A

Q2) What is the name of BBr₃?

A)boron bromide

B)boric bromide

C)boron tribromide

D)tribromoboride

E)bromine triboride

Answer: C

Q3) The formula C₉H₂₀ is an empirical formula.

A)True

B)False

Answer: True

To view all questions and flashcards with answers, click on the resource link above.

Chapter 3: Stoichiometry of Formulas and Equations

Available Study Resources on Quizplus for this Chatper

90 Verified Questions

90 Flashcards

Source URL: https://quizplus.com/quiz/74297

Sample Questions

Q1) A solution of methanol (CH₄O)in water has a concentration of 0.200 M.What mass of methanol,in grams,is present in 0.150 liters of this solution?

Answer: 0.961 g

Q2) How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides)are needed to form 485 g of sulfur tetrafluoride?

3SCl₂(l)+ 4NaF(s) \(\to\)

S₂Cl₂(l)+ 4NaCl(s)

A)1940 g

B)1510 g

C)754 g

D)205 g

E)51.3 g

Answer: C

SF₄(g)+

Q3) You are provided with a 250 mL volumetric flask,deionized water and solid NaOH.How much NaOH should be weighed out in order to make 250.mL of 0.100 M solution?

Answer: 1.000 g

To view all questions and flashcards with answers, click on the resource link above. Page 5

Chapter 4: Three Major Classes of Chemical Reactions

Available Study Resources on Quizplus for this Chatper

84 Verified Questions

84 Flashcards

Source URL: https://quizplus.com/quiz/74298

Sample Questions

Q1) Identify all the spectator ions in the following reaction. 2KMnO₄(aq)+ 10FeSO₄(aq)+ 8H₂SO₄(aq) \(\to\)K₂SO₄(aq)+ 2MnSO₄(aq)+ 5Fe₂(SO₄)₃(aq)+

8H₂O(l)

A)only K⁺

B)only SO₄^2-

C)only K⁺ and SO₄^2-

D)only K⁺,SO₄^2- and Fe²⁺

E)only K⁺,SO₄^2-,Fe²⁺ and Mn²⁺

Q2) Potassium carbonate,K₂CO₃,sodium iodide,NaI,magnesium chloride,MgCl₂,methanol,CH₃OH,and ammonium chloride,NH₄Cl,are soluble in water.Which produces the largest number of dissolved particles per mole of dissolved solute?

A)K₂CO₃

B)NaI

C)MgCl₂

D)CH₃OH

E)NH₄Cl

To view all questions and flashcards with answers, click on the resource link above. Page 6

Chapter 5: Gases and the Kinetic-Molecular Theory

Available Study Resources on Quizplus for this Chatper

93 Verified Questions

93 Flashcards

Source URL: https://quizplus.com/quiz/74299

Sample Questions

Q1) From the postulates of kinetic-molecular theory,it follows that the molecules of all gases at a given temperature have the same average speed.

A)True

B)False

Q2) Select the gas with the largest root-mean-square molecular speed at 25°C.

A)NH₃

B)CO

C)H₂

D)SF₆

E)All the gases have the same root-mean-square molecular speed at 25°C.

Q3) A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0°C and 1.00 atm.What is the molar mass of the gas?

A)7.76 g/mol

B)66.1 g/mol

C)74.0 g/mol

D)81.4 g/mol

E)144 g/mol

Q4) Briefly state the conditions corresponding to STP (standard temperature and pressure).

To view all questions and flashcards with answers, click on the resource link above. Page 7

Chapter 6: Thermochemistry: Energy Flow and Chemical Change

Available Study Resources on Quizplus for this Chatper

71 Verified Questions

71 Flashcards

Source URL: https://quizplus.com/quiz/74300

Sample Questions

Q1) Which one of the following statements about standard states is incorrect?

A)The standard state of a solid compound is the pure solid.

B)The standard state of a liquid compound is the pure liquid.

C)The standard state of a gaseous compound is the gas at a pressure of 1 atmosphere.

D)The standard state of an aqueous solute is a saturated solution in water.

E)The standard state of an element is the form in which it is stable at 1 atm and a specified temperature,usually 25°C.

Q2) A system which undergoes an adiabatic change and does work on the surroundings has

A)w < 0,\(\Delta\)E = 0

B)w > 0,\(\Delta\)E > 0

C)w > 0,\(\Delta\)E < 0

D)w < 0,\(\Delta\)E > 0

E)w < 0,\(\Delta\)E < 0

Q3) When 1.00 g of solid NH₄Cl is dissolved in 25.00 g of water contained in a coffee cup calorimeter,both reagents initially being at 25.0°C,the temperature falls to 22.4°C.Assuming that the heat capacity of the ammonium chloride solution is 4.18 J/(g·K),calculate the heat (enthalpy)of solution of NH₄Cl, (a)in J/g and (b)in kJ/mol.

Page 8

To view all questions and flashcards with answers, click on the resource link above.

Chapter 7: Quantum Theory and Atomic Structure

Available Study Resources on Quizplus for this Chatper

72 Verified Questions

72 Flashcards

Source URL: https://quizplus.com/quiz/74301

Sample Questions

Q1) In not more than three lines for each answer,briefly outline one important scientific contribution of each of the following.

a.Planck

b.de Broglie

c.Heisenberg

Q2) a.Use the Bohr equation to calculate the energy needed to ionize a hydrogen atom from its ground state.

b.What is the minimum wavelength of a photon needed for it to have the energy needed in (a)?

Q3) Use the Bohr equation to calculate the energy of

a.the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

b.the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

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

To view all questions and flashcards with answers, click on the resource link above.

9

Chapter 8: Electron Configuration and Chemical Periodicity

Available Study Resources on Quizplus for this Chatper

70 Verified Questions

70 Flashcards

Source URL: https://quizplus.com/quiz/74302

Sample Questions

Q1) Select the element with the greatest metallic character.

A)Li

B)Ca

C)Al

D)Pb

E)Cs

Q2) Define what is meant by ionization energy,and write a balanced chemical equation to represent the relevant process for element X.

Q3) An element with the electron configuration [noble gas]ns²(n1)d¹⁰np³ has ____________ valence electrons.

A)2

B)3

C)5

D)10

E)15

Q4) Electron affinities of neutral atoms may be positive or negative.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 10

Chapter 9: Models of Chemical Bonding

Available Study Resources on Quizplus for this Chatper

60 Verified Questions

60 Flashcards

Source URL: https://quizplus.com/quiz/74303

Sample Questions

Q1) Select the compound with the lowest lattice energy.

A)CsBr(s)

B)NaCl(s)

C)SrO(s)

D)CaO(s)

E)KBr(s)

Q2) Arrange the following bonds in order of increasing bond strength.

A)C-I < C-Br < C-Cl < C-F

B)C-F < C-Cl < C-Br < C-I

C)C-Br < C-I < C-Cl < C-F

D)C-I < C-Br < C-F< C-Cl

E)None of these orders is correct.

Q3) No real bonds are 100% ionic in character.

A)True

B)False

Q4) Electronegativities on Pauling's scale are calculated from ionization energies and electron affinities.

A)True

B)False

To view all questions and flashcards with answers, click on the resource link above. Page 11

Chapter 10: The Shapes of Molecules

Available Study Resources on Quizplus for this Chatper

94 Verified Questions

94 Flashcards

Source URL: https://quizplus.com/quiz/74304

Sample Questions

Q1) When resonance occurs,the bond lengths in a molecule fluctuate rapidly.

A)True

B)False

Q2) Boron never achieves an octet in any of its compounds.

A)True

B)False

Q3) According to VSEPR theory,a molecule with the general formula AX₆ will have a ______ molecular shape.

A)tetrahedral

B)trigonal planar

C)trigonal bipyramidal

D)hexagonal

E)octahedral

Q4) Name and outline the concept which is introduced when more than one valid Lewis structure can be drawn for a given molecule or ion.Use appropriate diagrams of the formate ion (HCO₂^-,carbon is the central atom)to illustrate.

Q5) What is the shape of the PF₃ molecule? Explain your answer,using VSEPR theory.

To view all questions and flashcards with answers, click on the resource link above. Page 12

Chapter 11: Theories of Covalent Bonding

Available Study Resources on Quizplus for this Chatper

49 Verified Questions

49 Flashcards

Source URL: https://quizplus.com/quiz/74305

Sample Questions

Q1) Carbon uses ______ hybrid orbitals in ClCN.

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q2) A molecule with the formula AX₃ uses __________ to form its bonds.

A)sp hybrid orbitals

B)sp² hybrid orbitals

C)sp³ hybrid orbitals

D)sp³d hybrid orbitals

E)sp³d² hybrid orbitals

Q3) 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.

To view all questions and flashcards with answers, click on the resource link above. Page 13

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

Available Study Resources on Quizplus for this Chatper

89 Verified Questions

89 Flashcards

Source URL: https://quizplus.com/quiz/74306

Sample Questions

Q1) In cubic closest packing,the unit cell is body-centered cubic.

A)True

B)False

Q2) a.Explain what is meant by the term "unit cell".

b.Copper metal has a face-centered cubic unit cell.The edge length of the unit cell is 361 pm,and the atomic weight of copper is 63.55 amu.Calculate the density of the copper in g/cm³.

(1 amu = 1.661 \(\times\) 10^-24 g. )

c.From the data in (b),calculate the radius of a copper atom in pm.

Q3) The maximum number of phases of a single substance which can coexist in equilibrium is two.

A)True

B)False

Q4) Strontium metal crystallizes in a cubic unit cell which has an edge length of 612 pm.If the mass of an atom of Sr is 87.62 amu,and the density of Sr metal is 2.54 g/cm³,calculate the number of atoms per unit cell.(1 amu = 1.661 \(\times\) 10^-24 g. )

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

To view all questions and flashcards with answers, click on the resource link above. Page 14

Chapter 13: The Properties of Solutions

Available Study Resources on Quizplus for this Chatper

73 Verified Questions

73 Flashcards

Source URL: https://quizplus.com/quiz/74307

Sample Questions

Q1) Potassium fluoride is used for frosting glass.Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution.

A)0.304 M

B)0.349 M

C)1.35 M

D)3.29 M

E)6.01 M

Q2) The density of pure water at 25°C is 0.997 g/mL.Considering water as being both solvent and solute,calculate its molarity.

Q3) Which of the following aqueous solutions should demonstrate the most ideal behavior?

A)0.1 M K₂SO₄

B)0.1 M CaCl₂

C)3.0 M LiF

D)0.1 M MgSO₄

E)0.1 M NaCl

Q4) A 7.112 M solution of sulfuric acid (H₂SO₄)in water has a density of 1.395 g/mL.What is its molality?

To view all questions and flashcards with answers, click on the resource link above. Page 15

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

Available Study Resources on Quizplus for this Chatper

58 Verified Questions

58 Flashcards

Source URL: https://quizplus.com/quiz/74308

Sample Questions

Q1) Dinitrogen monoxide,N₂O,is

A)a brown poisonous gas that is one of the chemicals involved in the production of photochemical smog.

B)a colorless gas used in the production of nitric acid.

C)a colorless gas used as an aerosol propellant.

D)a colorless gas that disproportionates into nitrogen and oxygen.

E)None of these choices is correct.

Q2) What are the products of the reaction of potassium hydride and water?

KH(s)+ H₂O(l) \(\to\)

A)K(s)+ H₂(g)+ OH^-(aq)

B)K(s)+ H₂(g)+ O₂(g)

C)KOH(s)+ O₂(g)

D)K⁺(aq)+ H₂(g)+ O₂(g)

E)K⁺(aq)+ H₂(g)+ OH^-(aq)

Q3) Name two different classes (types)of hydride.

Q4) Carbon monoxide's toxicity is related to its ability to bond to iron in hemoglobin.

A)True

B)False

Page 16

To view all questions and flashcards with answers, click on the resource link above.

Chapter 15: Organic Compounds and the Atomic Properties

of Carbon

Available Study Resources on Quizplus for this Chatper

95 Verified Questions

95 Flashcards

Source URL: https://quizplus.com/quiz/74309

Sample Questions

Q1) Carboxylic acids are weak acids.

A)True

B)False

Q2) The most abundant organic chemical on earth is A)glycogen.

B)starch.

C)cellulose.

D)glucose.

E)carbonate.

Q3) 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?

Q4) Ethane (C₂H₆)is much more reactive than disilane (Si₂H₆).

A)True

B)False

Q5) a.Draw two different structures with the molecular formula C₂H₆O.

b.Name the functional group in each structure.

c.Which one will have the higher boiling point,and why?

To view all questions and flashcards with answers, click on the resource link above. Page 17

Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Available Study Resources on Quizplus for this Chatper

76 Verified Questions

76 Flashcards

Source URL: https://quizplus.com/quiz/74310

Sample Questions

Q1) When a catalyst is added to a reaction mixture,it

A)increases the rate of collisions between reactant molecules.

B)provides reactant molecules with more energy.

C)slows down the rate of the back reaction.

D)provides a new pathway (mechanism)for the reaction.

E)does none of these

Q2) The rate constant for a reaction is 4.65 L mol^-1s^-1.What is the overall order of the reaction?

A)zero

B)first

C)second

D)third

E)More information is needed to determine the overall order.

Q3) Is a bimolecular reaction necessarily second-order? Is a second-order reaction necessarily bimolecular? Answer,with explanations and clarifications.

Q4) The rate law cannot be predicted from the stoichiometry of a reaction.

A)True

B)False

Page 18

To view all questions and flashcards with answers, click on the resource link above.

Chapter 17: Equilibrium: the Extent of Chemical Reactions

Available Study Resources on Quizplus for this Chatper

85 Verified Questions

85 Flashcards

Source URL: https://quizplus.com/quiz/74311

Sample Questions

Q1) There is a direct correlation between the speed of a reaction and its equilibrium constant.

A)True B)False

Q2) If Q > K,more products need to be formed as the reaction proceeds to equilibrium.

A)True

B)False

Q3) Changing the amount of reactant or product in an equilibrium reaction will always change the equilibrium position,regardless of the physical state of the substance involved.

A)True

B)False

Q4) Once a reaction system reaches equilibrium,the concentrations of reactions and products no longer change.

A)True

B)False

Q5) For some gas-phase reactions,K_p = K_c.

A)True B)False

To view all questions and flashcards with answers, click on the resource link above. Page 19

Chapter 18: Acid-Base Equilibria

Available Study Resources on Quizplus for this Chatper

90 Verified Questions

90 Flashcards

Source URL: https://quizplus.com/quiz/74312

Sample Questions

Q1) Define an acid according to the Lewis theory.Write a balanced equation in support of this definition,in which the acid is neither an Arrhenius acid nor a Brønsted-Lowry acid.

Q2) Ammonium chloride is used as an electrolyte in dry cells.Which of the following statements about a 0.10 M solution of NH₄Cl,is correct?

A)The solution is weakly basic.

B)The solution is strongly basic.

C)The solution is neutral.

D)The solution is acidic.

E)The values for K_a and K_b for the species in solution must be known before a prediction can be made.

Q3) Which one of the following substances will give an aqueous solution of pH < 7?

A)KI

B)NH₄Br

C)Na₂CO₃

D)CH₃COONa

E)CH₃OH

Q4) Define an acid according to the Arrhenius theory,and write a balanced equation to support this definition.

To view all questions and flashcards with answers, click on the resource link above.

Page 20

Chapter 19: Ionic Equilibria in Aqueous Systems

Available Study Resources on Quizplus for this Chatper

96 Verified Questions

96 Flashcards

Source URL: https://quizplus.com/quiz/74313

Sample Questions

Q1) A phosphate buffer (H₂PO₄^-/HPO₄^2-)has a pH of 8.3.Which of the following changes will cause the pH to increase?

A)dissolving a small amount of Na₂HPO₄

B)dissolving a small amount of NaH₂PO₄

C)adding a small amount of dilute hydrochloric acid

D)adding a small amount of dilute phosphoric acid

E)making the buffer more concentrated by removing some water

Q2) Which of the following indicators would be the best to use when 0.050 M benzoic acid (K_a = 6.6 \(\times\) 10^-5)is titrated with 0.05 M NaOH?

A)bromphenol blue,pH range: 3.0-4.5

B)bromcresol green,pH range: 3.8-5.4

C)alizarin,pH range: 5.7-7.2

D)phenol red,pH range: 6.9-8.2

E)phenolphthalein,pH range: 8.0-10.1

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

A)True B)False

To view all questions and flashcards with answers, click on the resource link above. Page 21

Chapter 20: Thermodynamics: Entropy,

Direction of Chemical Reactions

Available Study Resources on Quizplus for this Chatper

84 Verified Questions

84 Flashcards

Source URL: https://quizplus.com/quiz/74314

Sample Questions

Q1) Compare one mole of ice with one mole of liquid water,both at 1.0 atm and 0°C.The melting point of ice at 1.0 atm is 0°C.For the process H₂O(s) \(\to\) H₂O(l) under these conditions predict whether each of the following quantities will be greater than,less than,or equal to,zero .Explain each prediction in one sentence.

a.\(\Delta\)H°

b.\(\Delta\)S°

c.\(\Delta\)G°

Q2) A certain process has \(\Delta\)S_univ > 0 at 25°C.What does one know about the process?

A)It is exothermic.

B)It is endothermic.

C)It is spontaneous at 25°C.

D)It will move rapidly toward equilibrium.

E)None of these choices is correct.

Q3) In some spontaneous processes,the entropy of the surroundings decreases.

A)True

B)False

Q4) State the second and third laws of thermodynamics.

Page 22

To view all questions and flashcards with answers, click on the resource link above.

Chapter 21: Electrochemistry: Chemical Change and Electrical Work

Available Study Resources on Quizplus for this Chatper

97 Verified Questions

97 Flashcards

Source URL: https://quizplus.com/quiz/74315

Sample Questions

Q1) Consider the following redox equation Mn(OH)₂(s)+ MnO₄^-(aq) \(\to\)MnO₄^2-(aq)(basic solution)

When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq)and on which side of the equation is OH^-(aq)present?

A)4,reactant side

B)4,product side

C)6,reactant side

D)6,product side

E)None of these choices is correct.

Q2) A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V)and a Sn/Sn²⁺ electrode (E°= -0.14 V).Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

A)0.0001 M

B)0.0007 M

C)0.005 M

D)0.03 M

E)0.05 M

To view all questions and flashcards with answers, click on the resource link above. Page 23

Chapter 22: The Transition Elements and Their Coordination Compounds

Available Study Resources on Quizplus for this Chatper

72 Verified Questions

72 Flashcards

Source URL: https://quizplus.com/quiz/74316

Sample Questions

Q1) What is the difference between a coordination compound and a complex ion?

Q2) Which of the following will be the strongest oxidizing agent?

A)Cr

B)Cr(II)

C)Cr(III)

D)Cr(IV)

E)Cr(VI)

Q3) According to Valence Bond theory,in the square planar Ni(CN)₄^2- complex ion,the orbital hybridization pattern is A)sp³

B)dsp²

C)d²sp

D)d²sp³

E)None of these choices is correct.

Q4) The d_xy and the orbitals d_x²_y² both lie in the xy plane,yet for a metal ion in an octahedral complex the energy of the d_xy orbital is lower than that of the d_x²- _y² orbital.Explain this using the arguments of crystal field theory.

Q5) Why is the +2 oxidation state so common among transition elements?

To view all questions and flashcards with answers, click on the resource link above. Page 24

Chapter 23: Nuclear Reactions and Their Applications

Available Study Resources on Quizplus for this Chatper

75 Verified Questions

75 Flashcards

Source URL: https://quizplus.com/quiz/74317

Sample Questions

Q1) After 4 half-lives,the fraction of a radioactive isotope which still remains is approximately one eighth.

A)True

B)False

Q2) An isotope with Z > 83,which lies close to the band of stability,will generally decay through

A)(\(\alpha\) decay.)

B)(\(\beta\) decay.)

C)(\(\gamma\) decay.)

D)positron decay.

E)electron capture.

Q3) Write a complete,balanced equation to represent the formation of manganese-55 by the beta decay of another nuclide.

Q4) No alpha decay is observed for isotopes of elements with Z < 83.

A)True

B)False

Q5) Gamma rays are high energy electrons.

A)True

B)False

Q6) Write a complete,balanced equation to represent the beta decay of thallium-207.

To view all questions and flashcards with answers, click on the resource link above. Page 25