Survey of Chemistry Final Exam Questions - 3679 Verified Questions

Survey of Chemistry

Final Exam Questions

Course Introduction

Survey of Chemistry provides a broad introduction to the fundamental concepts of chemistry for non-majors and those seeking a general understanding of the subject. The course covers basic topics including atomic structure, chemical bonding, states of matter, chemical reactions, stoichiometry, solutions, acids and bases, and an overview of organic and biochemistry. Emphasis is placed on real-world applications and the relevance of chemistry in everyday life, environmental issues, health, and technology. This course also serves as a preparatory foundation for students who may pursue further studies in science-related fields.

Recommended Textbook

Chemistry The Central Science 13th Edition by Theodore E. Brown

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Chapter 1: Introduction: Matter and Measurement

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Sample Questions

Q1) Which one of the following has the element name and symbol correctly matched?

A)Ne, nitrogen

B)Si, sulfur

C)Ca, carbon

D)Be, beryllium

E)None of the symbols are correctly matched to the element name.

Answer: D

Q2) Which of the following liquids has the greatest density?

A)13 cm³ with a mass of 23 g

B)3.5 cm³ with a mass of 10 g

C)0.022 cm³ with a mass of 0.10 g

D)54 cm³ with a mass of 45 g

E)210 cm³ with a mass of 12 g

Answer: C

Q3) The symbol for the element phosphorus is ________.

Answer: P

Q4) 1 milligram = ________ micrograms

Answer: 1,000

Q5) 1.035 × 10^-4 L = ________ mL

Answer: 0.1035

Page 3

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be ________.

A)oxygen

B)fluorine

C)chlorine

D)nitrogen

E)sulfur

Answer: D

Q2) The charge on an electron was determined in the ________.

A)cathode ray tube, by J. J. Thomson

B)Rutherford gold foil experiment

C)Millikan oil drop experiment

D)Dalton atomic theory

E)atomic theory of matter

Answer: C

Q3) The correct name for Na₃N is sodium azide.

A)True

B)False

Answer: False

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Chapter 3: Stoichiometry: Calculations With Chemical

Formulas and Equations

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Sample Questions

Q1) A great deal of the carbon dioxide produced by the combustion of fossil fuels is absorbed into the oceans.

A)True

B)False

Answer: True

Q2) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO (s) + H₂O (l) Ca(OH)₂ (s)

A 3.50-g sample of CaO is reacted with 3.38 g of H₂O. How many grams of water remain after completion of reaction?

A)0.00

B)0.00694

C)2.25

D)1.04

E)0.125

Answer: C

Q3) Determine the mass percent (to the hundredths place)of C in sodium bicarbonate (NaHCO₃).

Answer: 14.30

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Chapter 4: Aqueous Reactions and Solution Stoichiometry

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Sample Questions

Q1) What are the spectator ions in the reaction between KOH (aq)and HNO₃(aq)?

A)K⁺ and H⁺

B)H⁺and OH^-

C)K⁺and NO₃^-

D)H⁺and NO₃^-

E)OH^-only

Q2) A 24.5 mL aliquot of 0.0938 M H₂SO₄ (aq)is to be titrated with 0.0295 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

A)156

B)0.136

C)77.9

D)39.0

E)4430

Q3) How many grams of CH₃OH must be added to water to prepare 175 mL of a solution that is 1.0 M CH₃OH?

Q4) Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250 mL.

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Chapter 5: Thermochemistry

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Sample Questions

Q1) Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. (1 mile = 1.6093 km, 1lb = 453.59 g).

A)5.5 × 10^{5 J}

B)5.5 × 10^-⁵ J

C)1.1 × 10⁶ J

D)2.2 × 10⁶ J

E)2.2 × 10^-⁶ J

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 of Ga is ________.

A)1s²2s²3s²3p⁶4s²3d<su p>10</sup>4p¹

B)1s²2s²2p⁶3s²3p⁶4s<su p>2</sup>4d¹⁰4p¹

C)1s²2s²2p⁶3s²3p⁶4s<su p>2</sup>3d¹⁰4p¹

D)1s²2s²2p⁶3s²3p⁶4s<su p>2</sup>3d¹⁰4d¹

E)[Ar]4s²3d¹¹

Q2) The uncertainty principle states that ________.

A)matter and energy are really the same thing

B)it is impossible to know anything with certainty

C)it is impossible to know the exact position and momentum of an electron

D)there can only be one uncertain digit in a reported number

E)it is impossible to know how many electrons there are in an atom

Q3) Blackbody radiation is the emission of light from metal surfaces.

A)True

B)False

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) Ca reacts with element X to form an ionic compound with the formula CaX. Al will react with X to form ________.

A)AlX₂

B)AlX

C)Al₂X₃

D)Al₃X₂

E)Al₃X

Q2) Xenon can form compounds with fluorine.

A)True

B)False

Q3) Which of the following generalizations cannot be made with regard to reactions of alkali metals? (The symbol M represents any one of the alkali metals.)

A)M (s) + O₂ (g) MO₂ (s)

B)2M (s) + 2H₂O (l) 2MOH (aq) + H₂ (g)

C)2M (s) + H₂ (g) 2MH (s)

D)2M (s) + Cl₂ (g) 2MCl (s)

E)2M (s) + S (s) M₂S (s)

Q4) Which noble gas has the highest first ionization energy?

Q5) Of the alkaline earth metals, which two elements are the least reactive?

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) In a reaction, if the bonds in the reactants are stronger than the bonds in the product, the reaction is ________.

Q2) Of the atoms below, ________ is the most electronegative.

A)Ba

B)Sr

C)Ca

D)Mg

E)Be

Q3) The electron configuration of the S^2- ion is ________.

A)[Ar]3s²3p⁶

B)[Ar]3s²3p²

C)[Ne]3s²3p²

D)[Ne]3s²3p⁶

E)[Kr]3s²2p⁶

Q4) There are ________ unpaired electrons in the Lewis symbol for an oxygen atom. A)0 B)1

Page 10

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) The electron-domain geometry of a boron-centered compound BH₃ is trigonal planar. The hybridization of the central boron atom is ________.

A)sp²

B)sp³d²

C)sp³

D)sp³d

E)sp

Q2) Using the VSEPR model, the electron-domain geometry of the central atom in ClO₃^- is ________.

A)linear

B)trigonal planar

C)tetrahedral

D)trigonal bipyramidal

E)octahedral

Q3) Nitrogen is colorless because the minimum energy to excite an electron is in the ultraviolet section of the spectrum.

A)True

B)False

Q4) What are the three bond angles in the trigonal bipyramidal structure?

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Chapter 10: Gases

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Sample Questions

Q1) A sample of oxygen gas (O₂)was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is ________ g/mol.

A)288

B)96

C)55

D)4

E)10.7

Q2) Kinetic-molecular theory assumes that attractive and repulsive forces between gas particles are stronger than those between gas particles and container walls. A)True

B)False

Q3) How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?

Q4) The density of krypton gas at 0.866 atm and 44.4 °C is ________ g/L.

A)0.0332

B)0.359

C)0.238

D)2.78

E)5.57

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the ________ segment corresponds to the heat capacity of the gas.

A)AB

B)BC

C)CD

D)DE

E)EF

Q2) Some things take longer to cook at high altitudes than at low altitudes because

A)water boils at a lower temperature at high altitude than at low altitude

B)water boils at a higher temperature at high altitude than at low altitude

C)heat isn't conducted as well in low density air

D)natural gas flames don't burn as hot at high altitudes

E)there is a higher moisture content in the air at high altitude

Q3) Heats of vaporization are greater than heats of fusion.

A)True

B)False

Q4) London Dispersion Forces tend to ________ in strength with increasing molecular weight.

13

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Which will have a larger band gap: GaN, GaP, GaAs, or GaSb?

A)GaN

B)GaP

C)GaAs

D)GaSb

E)All choices have identical band gaps.

Q2) If the electronic structure of a solid substance consists of a valence band that is completely filled with electrons and there is a large energy gap to the next set of orbitals, then this substance will be a(n)________.

A)alloy

B)insulator

C)conductor

D)semiconductor

E)nonmetal

Q3) What two metals are alloyed to produce sterling silver?

Q4) The process of adding controlled amounts of impurity atoms to a material is known as ________.

Q5) Nylon is formed by the reaction of a(n)________ with a(n)________.

Q6) Semiconductor particles with diameters of 1-10 nm are called ________.

Q7) Polymers formed from two different monomers are called ________.

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) Calculate the molarity of phosphoric acid (H₃PO₄)in a 22.1% (by mass)aqueous solution.

A)0.0522 m

B)0.0992 m

C)0.0248 m

D)0.0496 m

E)The density of the solution is needed to solve the problem.

Q2) Hydration is a specific example of the phenomenon known generally as ________.

A)salutation

B)disordering

C)solvation

D)condensation

E)dilution

Q3) Calculate the molarity of a 10.0% (by mass)aqueous solution of hydrochloric acid.

A)0.274 m

B)2.74 m

C)3.04 m

D)4.33 m

E)The density of the solution is needed to solve the problem.

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) The reaction 2NOBr (g) 2 NO (g)+ Br₂ (g) Is a second-order reaction with a rate constant of 0.80 M^-1s^-1at 11 °C. If the initial concentration of NOBr is 0.0440 M, the concentration of NOBr after 6.0 seconds is ________.

A)0.0276 M

B)0.0324 M

C)0.0363 M

D)0.0348 M

E)0.0402 M

Q2) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂ 2NO + O₂

In a particular experiment at 300 °C, [NO₂] drops from 0.0143 to 0.00701 M in 261 s. The rate of disappearance of NO₂ for this period is ________ M/s.

A)2.79 × 10^-5

B)-8.16 × 10^-5

C)5.59 × 10^-5

D)1.40 × 10^-5

E)35,800

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) What role did Karl Bosch play in development of the Haber-Bosch process?

A)He discovered the reaction conditions necessary for formation of ammonia.

B)He originally isolated ammonia from camel dung and found a method for purifying it.

C)Haber was working in his lab with his instructor at the time he worked out the process.

D)He developed the equipment necessary for industrial production of ammonia.

E)He was the German industrialist who financed the research done by Haber.

Q2) In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

A)True

B)False

Q3) How is the reaction quotient used to determine whether a system is at equilibrium?

A)The reaction quotient must be satisfied for equilibrium to be achieved.

B)At equilibrium, the reaction quotient is undefined.

C)The reaction is at equilibrium when Q < K_eq.

D)The reaction is at equilibrium when Q > K_eq.

E)The reaction is at equilibrium when Q = K_eq.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Classify the following compounds as weak acids (W)or strong acids (S): hypochlorous acid perchloric acid chloric acid

A)W S S

B)S S S

C)S W W

D)W W W

E)W S W

Q2) The magnitude of K_w indicates that ________.

A)water autoionizes very slowly

B)water autoionizes very quickly

C)water autoionizes only to a very small extent

D)the autoionization of water is exothermic

Q3) Classify the following compounds as weak bases (W)or strong bases (S): methylamine carbonate ion potassium hydroxide

A)W W S

B)S S S

C)S W W

D)W S S

E)W S W

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Q1) A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is ________ M.

A)11.7

B)0.00214

C)0.0856

D)0.267

E)0.139

Q2) The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 35.0 mL of 0.145 M HCl is ________.

A)1.314

B)1.403

C)0.00824

D)12.597

E)12.923

Q3) Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) The concentration of Mg in seawater is 0.054 M. How many grams of Mg can be extracted from 10.0 kg of seawater if the recovery rate is 20.0%?

A)13.9

B)6.50

C)11.3

D)2.62

E)5.25

Q2) Of the reactions involved in the photodecomposition of ozone (shown below), which are photochemical? 1. O₂ (g) + h O (g) + O (g)

2. O (g) + O₂(g) + M (g) O₃(g) + M^* (g)

3. O₃ (g) + h O₂(g) + O (g)

4. O (g) + O (g) + M (g) O₂(g) + M^* (g)

A)2 and 4

B)1, 2, and 4

C)1 and 3

D)1 only

E)all of them

Q3) Describe the process of reverse osmosis that is used to desalinate seawater.

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Chapter 19: Chemical Thermodynamics

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Q1) The value of S° for the formation of POCl₃ from its constituent elements, P₂(g) + O₂ (g) + 3Cl₂ (g) 2POCl₃ (g) Is ________ J/K mol.

A)-442.0

B)+771.0

C)-321.0

D)-771.0

E)+321.0

Q2) The value of S° for the formation of phosphorous trichloride from its constituent elements, P₂ (g) + 3Cl₂ (g) 2PCl₃ (g) Is ________ J/K mol.

A)-311.7

B)+311.7

C)-263.6

D)+129.4

E)-129.4

Q3) Find the temperature (in K)above which a reaction with a H of 123.0 kJ/mol and a S of 90.00 J/K mol becomes spontaneous.

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Chapter 20: Electrochemistry

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Q1) Which of the halogens in Table 20.1 is the strongest oxidizing agent?

A)Cl₂

B)Br₂

C)F₂

D)I₂

E)All of the halogens have equal strength as oxidizing agents.

Q2) 1V = ________.

A)1 amp s

B)1 J/s

C)96485 C

D)1 J/C

E)1 C/J

Q3) The anode of the alkaline battery is powdered zinc in a gel that contacts ________.

Q4) In a half reaction, the amount of a substance that is reduced or oxidized is directly proportional to the number of electrons generated in the cell.

A)True

B)False

Q5) The major product of a hydrogen fuel cell is ________.

Q6) In the formula G = -nFE, F is the ________.

Page 22

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Chapter 21: Nuclear Chemistry

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Q1) If we start with 1.000 g of strontium-90, 0.805 g will remain after 9.00 yr. This means that the half-life of strontium-90 is ________ yr.

A)7.74

B)11.2

C)28.8

D)7.25

E)41.6

Q2) All atoms of a given element have the same ________.

A)mass number

B)number of nucleons

C)atomic mass

D)number of neutrons

E)atomic number

Q3) The use of radioisotopes in tracing metabolism is possible because ________.

Q4) The major type of cancer caused by radiation is ________.

Q5) The SI unit of an absorbed dose of radiation is the gray.

A)True

B)False

Q6) When an isotope undergoes electron capture, what happens to the captured electron?

Page 23

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Chapter 22: Chemistry of the Nonmetals

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Q1) A carbonyl compound contains ________.

A)a carbon-oxygen double bond

B)a carbon-oxygen triple bond

C)a carbon atom with a lone pair of electrons

D)a carbon-carbon triple bond

E)a carbon-carbon double bond

Q2) Of Li, K, P and Ne which is the least electronegative?

Q3) The oxidation numbers of nitrogen in the nitride ion, hydrazine, ammonium cation, and nitrate ion are ________, ________, ________, and ________, respectively.

A)-3, -2, -3, +5

B)+3, -2, -3, +5

C)+3, -2, +1, +3

D)-3, +2, +1, +5

E)-3, +2, -3, +3

Q4) Oxides can react with water to form acids or bases.

A)True

B)False

Q5) Compounds containing only boron and hydrogen are called ________.

Q6) In a discussion of oxygen compounds, a disproportionation reaction is ________.

Q7) What group 5A element is the most metallic?

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Chapter 23: Transition Metals and Coordination Chemistry

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Q1) A geometrical isomer with like groups located on opposite sides of the metal atom is denoted with the prefix ________.

A)cis-

B)trans-

C)bis-

D)tetrakis-

E)d-

Q2) Which of the following is a polydentate ligand?

A)ethylenediamine

B)water

C)cyanide ion

D)nitrite ion

E)ammonia

Q3) A substance is ________ if its ions or atoms have one or more unpaired electrons.

Q4) Name the compound, Ca[AlH₄]₂.

Q5) Draw a diagram of the short-hand ground state electron configuration of zinc.

Q6) How does an elevated body temperature deprive some bacteria in the body of iron?

Q7) Name the compound, [Os(en)₃]₂ [NiCl₂Br₂]₃.

Page 25

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

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Q1) Ethers can be made by condensation of two ________ molecules by splitting out a molecule of water.

A)alkyne

B)alcohol

C)ketone

D)aldehyde

E)olefin

Q2) The doubly ionized form of an amino acid is called a(n)________.

Q3) Consider the following types of compounds: (i)amino acid

(ii)nitrogen-containing organic base

(iii)phosphoric acid

(iv)five-carbon sugar

From which of the above compounds are the monomers of nucleic acids, called nucleotides, formed?

A)none

B)(i)and (ii)

C)(ii)and (iv)

D)(ii), (iii), and (iv)

E)all

Q4) The primary ingredient in vinegar is ________.

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