General Chemistry I Test Bank - 2610 Verified Questions

General Chemistry I Test Bank

Course Introduction

General Chemistry I introduces students to the fundamental principles of chemistry, covering topics such as atomic structure, chemical bonding, stoichiometry, chemical reactions, thermochemistry, the periodic table, and properties of gases, liquids, and solids. Through a combination of lectures, laboratory experiments, and problem-solving exercises, students gain a solid understanding of chemical concepts and quantitative reasoning skills necessary for advanced study in the sciences. This course provides a foundational framework for exploring the behavior of matter and the chemical processes that underlie both natural phenomena and technological applications.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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24 Chapters

2610 Verified Questions

2610 Flashcards

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Page 2

Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) A particular sheet of paper measures 8.5 × 6.5 inches.What is the surface area of one side of the paper in cm²? (2.54 cm = 1 in exactly)

A)1 × 10² cm²

B)6 × 10¹ cm²

C)4 × 10² cm²

D)2 × 10¹ cm²

E)8.6 cm²

Answer: C

Q2) Convert 12.36 cm³ to cubic inches (in³)given that 1 inch = 2.54 cm (exact).

A)0.754 in³

B)4.865 in³

C)31.390 in³

D)202.500 in³

E)1.325 in³

Answer: A

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which of the following chemical equations is not balanced?

A)NH₄NO₃ N₂O + 2H₂O

B)C₁₂H₂₂O₁₁ 12C + 11H₂O

C)2NH₄SCN + Ba(OH)₂ 8H₂O 2NH₃ + 10H₂O + Ba(SCN)₂ D)(NH₄)₂Cr₂O₇ N₂O + Cr₂O₃ + 4H₂O

E)2Mg + CO₂ 2MgO + C

Answer: D

Q2) What is the name of the compound whose formula is Al₂(SO₄)₃?

A)aluminum sulfate

B)dialuminum tri(sulfur tetraoxygen)

C)aluminum sulfide

D)aluminum persulfate

E)aluminum sulfite

Answer: A

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Page 4

Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) Pure copper may be produced by the reaction of copper(I)sulfide with oxygen gas as follows:

Cu₂S(s)+ O₂(g) 2Cu(s)+ SO₂(g)

If 0.190 kg of copper(I)sulfide reacts with excess oxygen,what mass of copper metal may be produced?

A)0.19 kg

B)0.0379 kg

C)0.0758 kg

D)0.151 kg

E)0.38 kg

Answer: D

Q2) A compound is composed of only C and H.It contains 92.26 % C.What is its empirical formula?

A)C₂H₅

B)C₂H₃

C)C₃H₄

D)CH

E)CH₂

Answer: D

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) A precipitate will form when a freshly prepared aqueous carbonic acid solution is added to an aqueous solution of A)potassium carbonate.

B)ammonium chloride.

C)nitrous acid.

D)calcium hydroxide.

E)sodium chloride.

Q2) A 38.0-g sample of NaOH is dissolved in water,and the solution is diluted to give a final volume of 1.70 L.The molarity of the final solution is

A)22.3 M.

B)0.558 M.

C)0.95 M.

D)0.0447 M.

E)0.619 M.

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Chapter 5: The Gaseous State

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Sample Questions

Q1) Which of the following statements is incorrect regarding a 128-g sample of gaseous sulfur dioxide at 0°C and 760 mmHg pressure?

A)The density of the gas is 2.86 g/L.

B)There are 2 × 6.02 × 10²³ atoms of oxygen present.

C)There are 2 mol of gas present.

D)The molar mass of the gas is 64 g/mol.

E)The volume of the gas is 44.8 L.

Q2) A flexible vessel contains 78.00 L of gas at a pressure of 1.50 atm.Under conditions of constant temperature and moles of gas,what is the pressure of the gas when the volume of the vessel is tripled?

A)0.572 atm

B)4.5111 atm

C)2.38 atm

D)1.5 atm

E)0.025578 atm

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Chapter 6: Thermochemistry

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Sample Questions

Q1) A 70.4-L sample of a gaseous hydrocarbon,measured at 1.00 atm pressure and 25.0°C,is burned in excess oxygen,liberating 4.06 × 10³ kJ of heat at constant pressure.What is the identity of the hydrocarbon? (R = 0.0821 L atm/(K mol))

Substance

H°_f (kJ/mol)

CO₂(g)

-393.5

H₂O(l)

-285.8

A)propylene (C₃H₆, H°_f = 20.41 kJ/mol)

B)propane (C₃H₈, H°_f = -104.7 kJ/mol)

C)acetylene (C₂H₂, H°_f = 226.73 kJ/mol)

D)ethylene (C₂H₄, H°_f = 52.47 kJ/mol)

E)ethane (C₂H₆, H°_f = -84.68 kJ/mol)

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Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) The square of the wave function, ²,of an electron in an atom

A)is inversely proportional to the distance between the electron and the nucleus.

B)specifies the momentum of the electron.

C)describes the energy of the electron.

D)is proportional to the velocity of the electron.

E)gives the probability of finding the electron in a region of space.

Q2) When a particular metal is illuminated with photons,one electron is observed for each absorbed photon.What effect would decreasing the wavelength and number of photons have on the electrons leaving the surface?

A)There would be more electrons leaving the surface.

B)They would have higher kinetic energy.

C)The electron velocity would be lower.

D)The kinetic energy of the electrons would be lower.

E)Two photons might be required to eject the electrons.

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9

Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) Which of the following elements would be expected to have chemical and physical properties most similar to those of the krypton (Kr)?

A)neon (Ne)

B)gallium (Ga)

C)sodium (Na)

D)tin (Sn)

E)chlorine (Cl)

Q2) What is the maximum number of electrons in an atom that have the set of quantum numbers n= 2 and l= 1?

A)10

B)2

C)14

D)18

E)6

Q3) An atom of which of the following elements has the smallest atomic radius?

A)Cl

B)Rb

C)Mg

D)Si

E)As

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Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) A bond in which an electron pair is unequally shared by two atoms is

A)polar covalent.

B)coordinate covalent.

C)ionic.

D)nonpolar covalent.

E)metallic.

Q2) An atom of which of the following elements has the highest electronegativity?

A)K

B)As

C)Ba

D)Si

E)Br

Q3) Which of the following compounds would be expected to have the highest melting point?

A)NCl₃

B)OCl₂

C)MgCl₂

D)LiCl

E)CCl₄

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Page 11

Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) Which of the following molecules is polar?

A)SF₆

B)CCl₄

C)BF₃

D)NO₂

E)CO₂

Q2) Which molecule or ion does not have a planar molecular geometry?

A)NO₃^-

B)BF₃

C)F₂CO

D)C₂H₄

E)SO₃^2-

Q3) Which molecule or ion has the highest bond order?

A)F₂^-

B)O₂

C)O₂^2-

D)N₂

E)F₂

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) Which of the following indicates the existence of strong intermolecular forces of attraction in a liquid?

A)a very low critical temperature

B)a very low boiling point

C)a very low vapor pressure

D)a very low viscosity

E)a very low enthalpy of vaporization

Q2) How much heat is released at constant pressure if a 15.0-L tank containing 47.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0^oC? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0^oC.(R = 0.0821 L atm/(K mol))

A)1.31 × 10² J

B)2.68 × 10⁶ J

C)4.64× 10² J

D)1.87× 10⁴ J

E)7.54 × 10⁵ J

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Chapter 12: Solutions

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Sample Questions

Q1) What is the mole fraction of water in a solution that contains 8.0 mol of ethanol (C₂H₅OH)and 1.6 mol of water?

A)0.17

B)0.08

C)0.50

D)0.20

E)0.83

Q2) Calculate the molecular weight of a small protein if a 0.25-g sample dissolved in 180 mL of water has an osmotic pressure of 9.2 mmHg at 25°C.(R = 0.0821 L · atm/(K · mol))

A)2.4 × 10² g/mol

B)2.8 × 10³ g/mol

C)3.6 g/mol

D)2.7 × 10² g/mol

E)3.7 × 10^-3 g/mol

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Chapter 13: Rates of Reaction

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Sample Questions

Q1) At 500^oC,cyclopropane (C₃H₆)reacts to form its isomer,propene (C₃H₆).The reaction is first-order,and the rate constant is 6.7 × 10^-4 s^-1.If the initial concentration of cyclopropane is 0.500 M and the initial concentration of propene is 0,determine the time required for the concentration of propene to reach 0.100 M.

A)3.4 × 10³ s

B)3.3 × 10² s

C)1.2 × 10⁴ s

D)7.5 × 10² s

E)2.4 × 10³ s

Q2) In a first-order reaction,the half-life is 139 minutes.What is the rate constant?

A)1.20 × 10^-4 s^-1

B)5770 s^-1

C)0.299 s^-1

D)4.99 × 10^-3 s^-1

E)8.31 × 10^-5 s^-1

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) For which of the following values of the equilibrium constant does the reaction mixture contain mostly products?

A)10⁰

B)10¹

C)10⁹

D)10^-1

E)10^-9

Q2) Which of the following represents a dynamic equilibrium?

A)a stoppered flask half full of water

B)a coin spinning in mid-air

C)two people of equal mass balanced on the ends of a seesaw

D)an open pan of boiling water

E)an object traveling at a constant speed

Q3) A(n)_____ is a substance that increases the rate of a reaction but is not consumed by it.

A)antimatter

B)dark matter

C)beta particle

D)pansmer

E)catalyst

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Chapter 15: Acids and Bases

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Sample Questions

Q1) What is the pH of the final solution when 25 mL of 0.023 M HCl has been added to 35 mL of 0.040 M HCl at 25°C?

A)3.22

B)1.81

C)1.48

D)2.70

E)3.41

Q2) What is the pOH of a 0.0032 M CsOH solution?

A)2.49

B)16.49

C)8.26

D)5.74

E)11.51

Q3) Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)ClO₄^-

B)HClO₃

C)H₂SO₃

D)H₃PO₄

E)HSO₄^-

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) What is the percent ionization of a solution prepared by dissolving 0.0175 mol of chloroacetic acid,(HC₂H₂O₂Cl)in 1.30 L of water? For chloroacetic acid,K_a = 1.4 × 10^-3.

A)1.3 %

B)100 %

C)27 %

D)72 %

E)0.36 %

Q2) What is the hydroxide-ion concentration in a 0.16 M solution of Na₂CO₃? For carbonic acid,Ka₁ = 4.2 × 10^-7 and Ka₂ = 4.8 × 10^-11.(K_w = 1.0 × 10^-14)

A)5.8 × 10^-3 M

B)2.0 × 10^-4 M

C)6.2 × 10^-5 M

D)4.5 × 10^-9 M

E)2.8 × 10^-6 M

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18

Chapter 17: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) The insoluble salts

AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed from the metal ions A⁺,B⁺,C³⁺,D²⁺,and E³⁺ and the nonmetals V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

A)AV

B)EZ₃

C)DY₂

D)B₂W

E)C₂X₃

Q2) What is the pH of a saturated solution of Zn(OH)₂? For Zn(OH)₂,K_sp = 2.1 × 10^-16.

A)5.13

B)8.57

C)5.43

D)8.87

E)7.00

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Chapter 18: Thermodynamics and Equilibrium

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Sample Questions

Q1) For which of the following reactions is S° > 0 at 25°C?

A)2H₂(g)+ O₂(g) 2H₂O(g)

B)2ClBr(g) Cl₂(g)+ Br₂(g)

C)I₂(g) I₂(s)

D)2NO(g)+ O₂(g) 2NO₂(g)

E)NH₄HS(s) NH₃(g)+ H₂S(g)

Q2) Which of the following equations is correct?

A)G = S - TH

B)G = H - PV

C)G = H - TS

D) G = G_initial - G_final

E)G = S - PV

Q3) The reaction C(s)+ CO₂(g) 2CO(g)is spontaneous only at temperatures in excess of 1100 K.We can conclude that

A) G° is negative for all temperatures.

B) H° is negative and S° is negative.

C) H° is positive and S° is positive.

D) H° is negative and S° is positive.

E) H° is positive and S° is negative.

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Page 20

Chapter 19: Electrochemistry

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Sample Questions

Q1) What is the cell reaction for the following electrochemical cell?

Zn | Zn²⁺(aq)|| Sc³⁺(aq)| Sc

A)3Zn(s)+ 2Sc³⁺(aq) 2Sc(s)+ 3Zn²⁺(aq)

B)2Sc(s)+ 3Zn²⁺(aq) 3Zn(s)+ 2Sc³⁺(aq)

C)Zn(s)+ Zn²⁺(aq) Sc(s)+ Sc³⁺(aq)

D)Zn(s)+ Sc³⁺(aq) Sc(s)+ Zn²⁺(aq)

E)Sc(s)+ Zn²⁺(aq) Zn(s)+ Sc³⁺(aq)

Q2) What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr₂(SO₄)₃ for 155 min using a constant current of 10.0 A? (F = 96485 C/mol)

A)0.278 g

B)16.7 g

C)150.4 g

D)0.187 g

E)25.1 g

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Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) ⁵⁵Mn can be prepared by electron capture from which of the following?

A)(⁵⁶Mn)

B)(⁵⁵Fe)

C)(⁵⁵Cr)

D)(⁵¹V)

E)(⁵⁷Co)

Q2) For which of the following radioactive decay processes does the atomic number not change?

A)electron capture

B)positron emission

C)alpha emission

D)gamma emission

E)beta emission

Q3) The half-life of phosphorus-33 is 25 days.How much of a 128-g sample will remain after 160 days?

A)1.5 g

B)16 g

C)1.0 g

D)8.0 g

E)4.0 g

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Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) What makes metals a good conductor of heat and electricity?

A)Overlapping of the molecular orbitals

B)Mobility of positively charged positrons

C)Mobility of valence electrons

D)High mass of the atomic nucleus

E)Low mass of the atomic nucleus

Q2) Most HCl(g)is obtained commercially

A)by reaction of MnO₂ with concentrated HCl.

B)by reaction of NaCl with concentrated H₂SO₄.

C)by electrolysis of NaCl.

D)by distillation of HCl(aq).

E)as a by-product from the chlorination of hydrocarbons.

Q3) Which molecule does not have a bent molecular geometry?

A)H₂O

B)SO₂

C)N₂O

D)O₃

E)H₂S

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Page 23

Chapter 22: The Transition Elements and Coordination Compounds

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Sample Questions

Q1) Copper metal can be oxidized by which of the following acids?

A)H₃PO₄

B)HBr

C)H₂SO₄

D)CH₃COOH

E)HCl

Q2) Which of the following is a dark green solid?

A)CrO₃

B)KCr(SO₄)₂·12H₂O

C)Na₂Cr₂O₇

D)Na₂CrO₄

E)Cr₂O₃

Q3) Transition metals can be distinguished from main-group metals by the fact that

A)main-group metals have only +1 or +2 oxidation states.

B)transition metals have higher relative atomic weights than main-group metals.

C)transition metals have a greater tendency to form colored compounds than main-group metals.

D)main-group metals have higher relative atomic weights than transition metals.

E)only the main-group metals can form complex ions.

Page 24

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Chapter 23: Organic Chemistry

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Sample Questions

Q1) What is the molecular geometry around each carbon atom in a saturated hydrocarbon?

A)tetrahedral

B)trigonal planar

C)trigonal bipyramidal

D)linear

E)bent

Q2) Which substance is a weak Brønsted-Lowry acid in aqueous solution?

A)CH₃OCH₃

B)CH₃COOCH₃

C)CH₃OH

D)CH₃NH₂

E)CH₃COOH

Q3) All of the following molecules except _________ make up a homologous series.

A)CH₃C

H₂CH₂CH₂CH₂CH₃

B)CH₃CH₂CH₃

C)CH₃CH₂CH₂CH₃

D)CH₃CH₂CH₂CH₂CH₃

E)CH₃CHCHCH₃

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Chapter 24: Polymer Materials: Synthetic and Biological

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Sample Questions

Q1) What is the nitrogenous base that is found in RNA but not in DNA?

A)thymine

B)guanine

C)uracil

D)cytosine

E)adenine

Q2) What is the cell structure that contains the cell's DNA?

A)chromosome

B)codon

C)ribosome

D)gene

E)nucleus

Q3) A(n)_____ is a linear polymer of nucleotide units linked from the hydroxyl group at the 3' carbon of the pentose of one nucleotide to the phosphate group of the other nucleotide.

A)ribonucleotide

B)polysaccharide

C)polynucleotide

D)ketopentose

E)aldopentose

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