Fundamentals of Chemistry Textbook Exam Questions - 2610 Verified Questions

Fundamentals of Chemistry

Textbook Exam Questions

Course Introduction

Fundamentals of Chemistry provides an introduction to the basic concepts and principles of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and thermodynamics. The course covers the periodic table, chemical reactions, properties of gases, solutions, acids and bases, and introduces laboratory techniques. Emphasis is placed on developing problem-solving skills and an understanding of chemistrys role in real world applications, preparing students for more advanced study in the field.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) Calculate the mass of aluminum that occupies the same volume as 95.7 g of cobalt.The density of cobalt is 8.90 g/cm³ and the density of aluminum is 2.71 g/cm³.

A)0.252 g

B)29.1 g

C)2 × 10³ g

D)0.00318 g

E)3.96 g

Answer: B

Q2) A student is working on converting a number that has a unit with the SI prefix milli- to a unit that has the prefix mega-.Using your knowledge about the relative sizes that milliand mega- represent,how should the student convert the number?

A)The student should multiply the number by 10⁹.

B)The student should multiply the number by 10⁶.

C)The student should divide the number by 10⁶.

D)The student should use the number as is.

E)The student should divide the number by 10⁹.

Answer: E

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) The name of the SO₄^2- ion is A)persulfate.

B)thiosulfite.

C)sulfite.

D)sulfate.

E)sulfide.

Answer: D

Q2) A reaction occurs between sodium carbonate and hydrochloric acid,producing sodium chloride,carbon dioxide,and water.Which is the correct set of coefficients,respectively,for the balanced reaction?

A)3 6 6 3 4

B)8 6 5 10 5

C)5 10 10 5 5

D)1 2 2 1 1

E)none of these

Answer: D

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Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) What is the molar mass of ammonium sulfite,(NH₄)₂SO₃?

A)98 g/mol

B)116 g/mol

C)55 g/mol

D)180 g/mol

E)84 g/mol

Answer: B

Q2) _____ is the calculation of the quantities of reactants and products involved in a chemical reaction.

A)Allotropy

B)Congruence

C)Allometry

D)Isometry

E)Stoichiometry

Answer: E

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) Which one of the following is necessary in order for a metal to be oxidized?

A)addition of electrons

B)removal of electrons

C)addition of oxygen

D)removal of oxygen

E)addition of hydrogen

Q2) What is the net ionic equation for the reaction that occurs between nitrous acid and barium hydroxide?

A)HNO₂(aq)+ OH^-(aq) NO₂^-(aq)+ H₂O(l)

B)2HNO₂(aq)+

Ba(OH)₂

Ba(NO₂)₂(aq)+ H₂O(l)

C)2H⁺(aq)+ 2NO₂^-(aq)+ Ba²⁺(aq)+ 2OH^-(aq) Ba(NO₂)₂(aq)+ H₂O(l)

D)2H⁺(aq)+ 2NO₂^-(aq)+ Ba²⁺(aq)+ 2OH^-(aq) Ba²⁺(aq)+ 2NO₂^-(aq)+ 2H₂O(l)

E)H⁺(aq)+ OH^-(aq) H₂O(l)

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Chapter 5: The Gaseous State

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Sample Questions

Q1) The behavior of PH₃(g)is most likely to approach ideal behavior at

A)1.0 atm and 100°C.

B)0.10 atm and -100°C.

C)10 atm and 100°C.

D)0.10 atm and 100°C.

E)1.0 atm and 0°C.

Q2) A particular gas exerts a pressure of 731 mmHg.What is this pressure in units of atmospheres?

A)5.48 × 10⁵ atm

B)5.63 × 10⁵ atm

C)721 atm

D)0.974 atm

E)0.961 atm

Q3) A particular gas exerts a pressure of 4.09 × 10⁴ Pa.What is this pressure in units of atmospheres?

A)0.403 atm

B)4.04 × 10⁹ atm

C)0.414 atm

D)0.409 atm

E)4.14 × 10⁹atm

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Chapter 6: Thermochemistry

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Sample Questions

Q1) What is H° for the following reaction?

2C₂H₂(g)+ 5O₂(g) 4CO₂(g)+ 2H₂O(l)

Substance

H°_f (kJ/mol)

C₂H₂(g)

+226.7

CO₂(g) -393.5

H₂O(l)

-285.8

A)+1692.2 kJ

B)-452.6 kJ

C)-1692.2 kJ

D)+2599.0 kJ

E)-2599.0 kJ

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Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) Which type of electromagnetic radiation has the lowest frequency?

A)microwaves

B)visible

C)ultraviolet

D)infrared

E)radio waves

Q2) The _____ of a wave is the number of wavelengths of that wave that pass a fixed point in one unit of time and its unit is _____.

A)frequency,hertz

B)wavelength,meter

C)intensity,candela

D)current,ampere

E)period,second

Q3) An orbital with the quantum numbers n = 5,l = 2,m_l = -1 may be found in which subshell?

A)5f

B)5d

C)5p

D)5g

E)5s

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Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) How many valence electrons does an arsenic atom have?

A)5

B)6

C)7

D)2

E)33

Q2) An atom of which of the following elements has the largest atomic radius?

A)Ge

B)Rb

C)F

D)Ca

E)P

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

A)Tl

B)B

C)In

D)Ga

E)Al

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Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) Which pair of species is isoelectronic?

A)Na⁺ and K⁺

B)K⁺ and Cl^-

C)Be²⁺ and Na⁺

D)Ne and Ar

E)Li⁺ and Ne

Q2) In the Lewis formula for ClF₃,how many lone pairs are around the central atom?

A)0

B)4

C)3

D)2

E)1

Q3) The concept of resonance describes molecular structures

A)that have several different geometric arrangements.

B)that have delocalized bonding.

C)that are formed from hybridized orbitals.

D)that have different molecular formulas.

E)that have electrons resonating.

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Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) What is the molecular geometry around an atom in a molecule or ion which is surrounded by five single bonds and no lone pairs of electrons.

A)trigonal bipyramidal

B)octahedral

C)linear

D)trigonal planar

E)tetrahedral

Q2) Which of the following statements is not correct?

A)Hybrid orbitals are made by the combination of atomic orbitals on a given atom.

B)In both valence bond theory and molecular orbital theory bonding result from the overlap of occupied atomic orbitals.

C)Valence bond theory does not account for the experimentally observed paramagnetism of molecules like O₂.

D)Pi bonds may be formed from s or p orbital overlap.

E)In molecular orbital theory a molecular orbital may encompass more than two atoms.

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) The boiling point of a liquid is

A)always the temperature at which the vapor pressure equals 760 mmHg (1 atm).

B)always the temperature at which the liquid phase of a substance is in equilibrium with the vapor phase.

C)always the temperature at which the vapor pressure equals the pressure exerted on the liquid.

D)always equal to the vapor pressure of the liquid at a given temperature.

E)independent of the pressure exerted on the liquid.

Q2) A particular compound has an enthalpy of vaporization of 28400 J/mol.At 274 K it has a vapor pressure of 122 mmHg.What is its vapor pressure at 311 K? (R = 8.31 J/(K· mol))

A)117 mmHg

B)262 mmHg

C)27.6 mmHg

D)538 mmHg

E)126 mmHg

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Chapter 12: Solutions

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Sample Questions

Q1) Determine the osmotic pressure of a solution that contains 0.018 g of a hydrocarbon solute (molar mass = 340 g/mol)dissolved in benzene to make a 350-mL solution.The temperature is 20.0°C.

A)1.2 torr

B)2.5 torr

C)0.18 torr

D)0.9 torr

E)2.7 torr

Q2) The dissolution of ionic compounds in water depends only on the hydration energy of the ions.

A)1 only

B)2 only

C)3 only

D)1 and 2

E)1,2,and 3

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Chapter 13: Rates of Reaction

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Sample Questions

Q1) For a certain reaction of the general form aA products,the experimental data plotted as 1/[A] versus time is linear.The slope of this plot must equal A)-1.

B)the rate constant.

C)one over the rate constant.

D)the negative of the rate constant. E)1.

Q2) For the first-order reaction

1/2 N₂O₄(g) NO₂(g); H = 28.6 kJ

The rate constant is k = 3.24 × 10⁵ s^-1 at -7°C,and the activation energy is 53.7 kJ/mol.What is the rate constant at 26°C?

A)3.64 × 10⁵ s^-1

B)3.24 × 10⁵ s^-1

C)6.08 × 10⁵ s^-1

D)4.73 × 10⁶ s^-1

E)1.00 × 10⁵ s^-1

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) 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

Q2) The _____ is a relation that states that the values of the equilibrium-constant expression K_c are constant for a particular reaction at a given temperature,whatever equilibrium concentrations are substituted.

A)law of gravity

B)law of thermodynamics

C)law of mass action

D)law of definite proportions

E)law of combining volumes

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Chapter 15: Acids and Bases

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Sample Questions

Q1) Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)CH₄

B)HSO₃^-

C)H₂SO₃

D)H₃O⁺

E)HCl

Q2) The acid strength decreases in the series HBr > HSO₄^- > CH₃COOH > HCN > HCO₃^-.Which of the following is the strongest base?

A)SO₄^2-

B)CO₃^2-

C)CH₃COO^-

D)Br^-

E)CN^-

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) A solution contains 0.08 M acetic acid,HC₂H₃O₂ (K_a = 1.7 × 10⁵ at 25°C),and 0.15 M sodium acetate,NaC₂H₃O₂.What is the pH of the solution at 25°C?

A)5.04

B)6.02

C)4.28

D)3.86

E)7.05

Q2) 15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO₂ (K_a for HNO₂ = 4.0 × 10^-4).What is the equilibrium concentration of NO₂^- ions?

A)4.2 × 10^-1 M

B)1.7 × 10^-4 M

C)5.1 × 10^-2 M

D)2.6 × 10^-3 M

E)none of these

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Chapter 17: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) What is the molar solubility of zinc hydroxide at pH 12.34? For Zn(OH)₂,K_sp = 2.1 × 10^-16; for Zn(OH)₄^2-,K_f = 2.8 × 10¹⁵.

A)1.2 × 10^-25 M

B)1.3 × 10^-2 M

C)2.8 × 10^-4 M

D)3.7 × 10^-6 M

E)1.4 × 10^-8 M

Q2) In which of the following solutions would CaC₂O₄ have the highest molar solubility?

A)0.01 M Na₂C₂O₄

B)0.01 M NaCl

C)0.01 M HCl

D)0.01 M Ca(NO₃)₂

E)0.01 M NaHC₂O₄

Q3) What is the solubility product expression for Pb(IO₃)₄?

A)K_sp = [Pb⁴⁺][4IO₃^-]⁴

B)K_sp = [Pb⁴⁺][IO₃^-]

C)K_sp = [Pb][IO₃]⁴

D)K_sp = [Pb⁴⁺][IO₃^-]⁴

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Chapter 18: Thermodynamics and Equilibrium

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Q1) A system under constant external pressure undergoes a decrease in volume.What is the effect on the surroundings?

A)Energy is transferred as pressure-volume work done by the surroundings on the system.

B)Energy is transferred as pressure-volume work done on the surroundings.

C)Energy is transferred as heat from the system to the surroundings.

D)Energy is transferred as heat from the surroundings to the system.

E)None of the above.

Q2) If a process is both endothermic and spontaneous,then

A) H = 0.

B) G > 0.

C) S > 0.

D) U < 0.

E) H < 0.

Q3) Condensation is a process for which

A) G is negative at high temperature but positive at low temperature.

B) H, S,and G are positive at all temperatures.

C) G is positive when condensation occurs spontaneously.

D) H and S are positive at all temperatures.

E) H and S are negative at all temperatures.

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Chapter 19: Electrochemistry

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Sample Questions

Q1) In the following electrochemical cell,what is the role of the platinum? Cu(s)| Cu²⁺(aq)|| Fe³⁺(aq),Fe²⁺(aq)| Pt(s)

A)The platinum serves as the anode.

B)The oxidation of Fe²⁺ takes place at the surface of the platinum as the cell discharges.

C)The reduction of Fe³⁺ takes place at the surface of the platinum as the cell discharges.

D)A and C.

E)A and B.

Q2) A current of 13.0 A is passed through molten magnesium chloride for 16.0 h.How many moles of magnesium metal could be produced via this electrolysis?

A)0.0647 mol

B)3.88 mol

C)0.37 mol

D)0.22 mol

E)7.76 mol

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Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) A scintillation counter measures radiation by detecting A)cations produced from radiation colliding with phosphor gases.

B)electrons released when gas atoms are ionized by the radiation.

C)alpha and beta particles as they strike a detector window.

D)the increase in temperature when a gas is struck by radiation.

E)flashes of light emitted from a phosphor affected by radiation.

Q2) Metastable isotopes,such as Technetium-99m and those produced from neutron activation analysis decay by what process?

A)gamma emission

B)alpha emission

C)beta emission

D)positron emission

E)all of the above

Q3) Which of the following nuclides will produce ²³³Pa upon undergoing alpha decay?

A)(²³⁴Pa)

B)(²³³U)

C)(²²⁹Ra)

D)(²³⁷Np)

E)(²³³Th)

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Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) Which element reacts most vigorously with water?

A)Al

B)Li

C)Ba

D)Mg

E)Cs

Q2) Which of the following statements is true?

A)An alloy may also be an ore.

B)A metal may also be a mineral.

C)A mineral may also be an alloy.

D)A mineral may also be an ore.

E)All of these statements are true.

Q3) Cryolite,Na₃AlF₆,is used in the production of A)HF.

B)NaF.

C)Na.

D)Al.

E)F₂.

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Chapter 22: The Transition Elements and Coordination Compounds

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Sample Questions

Q1) What is the correct formula for sodium tetrachlorocuprate(II)?

A)Na₃[CuCl₄]

B)Na₂[CuCl₄]

C)Na[CuCl₄]

D)Na₄[CuCl₄]

E)Na₂[CuCl₆]

Q2) What is the total number of geometric isomers possible for the octahedral complex [Co(NH₃)₃(H₂O)₃]?

A)1

B)4

C)5

D)2

E)3

Q3) Which of the following salts would not be expected to be colored in aqueous solution?

A)CoCl₂

B)FeCl₂

C)CuCl₂

D)CuCl

E)CrCl₃

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) What is the major product after addition of two HF to propyne,CH₃C CH?

A)CH₃CHFCH₂F

B)CH₂FCH₂CH₂F

C)CH₃CF₂CH₃

D)CH₃CH₂CF₂H

E)CH₃CHF=CH₂

Q3) Which substance is a weak Brønsted-Lowry acid in aqueous solution?

A)CH₃OCH₃

B)CH₃COOCH₃

C)CH₃OH

D)CH₃NH₂

E)CH₃COOH

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Chapter 24: Polymer Materials: Synthetic and Biological

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Q1) A hemiacetal is formed from

A)an alcohol and a ketone.

B)a carboxylic acid and a mercaptan.

C)an alcohol and an ether.

D)an aldehyde and an alcohol.

E)an ester and an amine.

Q2) What is the type of polymer formed when 1,5-pentanediol,HOCH₂CH₂CH₂CH₂CH ₂OH,reacts with 1,6-hexanedicarboxylic acid,HOOCCH₂CH₂CH₂CH₂COOH?

A)polyacetylene

B)polyester

C)polyamide

D)polypropylene

E)polyolefin

Q3) The alpha helix and beta sheet are examples of A)protein denaturation.

B)protein primary structure.

C)complementary bases.

D)protein tertiary structure.

E)protein secondary structure.

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