Survey of Chemistry Final Test Solutions - 3674 Verified Questions

Survey of Chemistry

Final Test Solutions

Course Introduction

Survey of Chemistry provides a broad introduction to the fundamental concepts of chemistry, emphasizing basic chemical principles and their applications to everyday life. Topics include atomic structure, chemical bonding, states of matter, chemical reactions, stoichiometry, solutions, acids and bases, and an overview of organic chemistry. Designed for non-science majors or students needing a general understanding of chemistry, the course combines theoretical discussions with practical examples to illustrate the relevance of chemistry in fields such as health, environment, and industry.

Recommended Textbook

Chemistry The Central Science 14th Edition by Theodore E. Brown

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24 Chapters

3674 Verified Questions

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Page 2

Chapter 1: Introduction: Matter, energy, and Measurement

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Sample Questions

Q1) Which of the items below would be considered the most dense?

A)a piece of wood with a volume of 2.5 L and a mass of 12.5 kg

B)a ball with a volume of 139 mL and a mass of 93 g

C)a tire with a volume of 2.12 L and a mass of 4.22 × 10⁴ mg

D)a wire with a volume of 3.91 × 10^-7L and a mass of 7.93 × 10^-1 ng

E)a block of metal with a volume of 1350 mL and a mass of 1.29 × 10³ g

Answer: A

Q2) For which of the following,can the composition vary?

A)pure substance

B)element

C)both homogeneous and heterogeneous mixtures

D)homogeneous mixture

E)heterogeneous mixture

Answer: C

Q3) Mass and volume are often referred to as ________ properties of substances.

Answer: extensive

Q4) Si is the symbol for the element ________.

Answer: Silicon

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) Which element forms an ion with the same charge as the sulfate ion?

A)magnesium

B)sodium

C)fluorine

D)vanadium

E)sulfur

Answer: E

Q2) Calcium forms an ion with a charge of ________.

A)1-

B)2-

C)1+

D)2+

E)0

Answer: D

Q3) The correct name for Na₃N is sodium azide.

A)True

B)False

Answer: False

Q4) Which element is found in Period 2 and Group VIIA?

Answer: fluorine

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Chapter 3: Chemical Reactions and Reaction Stoichiometry

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Sample Questions

Q1) Complete and balance the following reaction,given that elemental sodium reacts with elemental oxygen to form Na₂O (s).

K (s)+ S (s) ________

Answer: K₂S (s)

Q2) Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s) PbO (s)+ CO₂(g)

How many grams of lead (II)oxide will be produced by the decomposition of 2.50 g of lead (II)carbonate?

A)0.41

B)2.50

C)0.00936

D)2.09

E)2.61

Answer: D

Q3) The mass of a single atom of an element (in amu)is numerically equal to the mass in grams of that element.

A)True

B)False

Answer: False

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Page 5

Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) Which of the following is an oxidation-reduction reaction?

A)Cu (s)+ 2AgNO₃ (aq) 2Ag (s)+ Cu(NO₃)₂ (aq)

B)HCl (aq)+ NaOH (aq) H₂O (l)+ NaCl (aq)

C)AgNO₃(aq)+ HCl (aq) AgCl (s)+ HNO₃ (aq)

D)Ba(C₂H₃O₂)₂ (aq)+ Na₂SO₄ (aq) BaSO₄ (s)+ 2NaC₂H₃O₂(aq)

E)H₂CO₃ (aq)+ Ca(NO₃)₂(aq) 2HNO₃ (aq)+ CaCO₃ (s)

Q2) Which one of the following solutions will have the greatest concentration of hydroxide ions?

A)1.10 M rubidium hydroxide

B)0.368 M calcium hydroxide

C)0.368 M ammonium hydroxide

D)0.368 M potassium hydroxide

E)0.368 M sulfuric acid

Q3) The solvent in an aqueous solution is ________.

Q4) The compound HClO₄ is a weak acid.

A)True

B)False

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Chapter 5: Thermochemistry

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Sample Questions

Q1) A 100-watt electric incandescent light bulb consumes ________ J of energy in 24 hours.[1 Watt (W)= 1 J/sec]

A)2.40 × 10³

B)8.64 × 10³

C)4.17

D)2.10 × 10³

E)8.64 × 10⁶

Q2) How many kJ of heat are released when 15.75 g of Ba (s)reacts completely with oxygen gas to form BaO (s)? H° = -1107 kJ.

A)63.5 kJ

B)20.8 kJ

C)114 kJ

D)70.3 kJ

E)35.1 kJ

Q3) Work equals mass times distance.

A)True B)False

Q4) The primary component of natural gas is methane.

A)True B)False

Page 7

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) In the de Broglie formula describing the movement of an electron about the nucleus,the quantity "mv" is called its ________.

Q2) What is the frequency of light (s^-1)that has a wavelength of 3.12 × 10^-3 cm?

A)3.69 s^-1

B)2.44 × 10¹⁶ s^-1

C)9.62 × 10¹² s^-1

D)4.10 × 10^-17 s^-1

E)1.04 × 10^-13 s^-1

Q3) Which is the correct electron configuration for an oxide ion?

A)1s²2s²2p³

B)1s²2s²2p¹

C)1s²2s²2p⁶

D)1s²2s²3s²

E)1s²2s²2p²

Q4) The larger the principal quantum number of an orbital,the lower is the energy of the electrons in that orbital.

A)True

B)False

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) The element in the periodic table that looks like a metal,is a poor thermal conductor,and acts as an electrical semiconductor is ________.

A)Sn

B)B

C)As

D)Si

E)Ge

Q2) What is the coefficient of H₂O when the following equation is completed and balanced?

Ca (s)+ H₂O (l)

A)1

B)3

C)2

D)5

E)Ca(s)does not react with H₂O (l).

Q3) Which noble gas has the highest first ionization energy?

Q4) [He]2s²2p⁵ is the electron configuration for ________.

Q5) Which of the halogens has the highest first ionization energy?

Q6) [Kr]5s² is the electron configuration for ________.

Q7) Which metal is a liquid at room temperature?

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) How many different types of resonance structures can be drawn for the ion SO₃^2-?

A)1

B)2

C)3

D)4

E)5

Q2) The Lewis structure of PF₃ shows that the central phosphorus atom has ________ nonbonding and ________ bonding electron pair(s).

A)2, 2

B)1, 3

C)3, 1

D)1, 2

E)3, 3

Q3) The greater the lattice energy,the greater the charges on the participatory ions and the smaller their radii.

A)True

B)False

Q4) Which halogen,bromine or iodine,will form the more polar bond with phosphorus?

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) XeF₄ is a polar molecule.

A)True

B)False

Q2) Of the following molecules,only ________ is polar.

A)CCl₄

B)BCl₃

C)NCl₃

D)BeCl₂

E)Cl₂

Q3) The ________ hydrogen orbital overlaps with the ________ fluoride orbital in HF.

Q4) According to MO theory,overlap of two p atomic orbitals produces ________.

A)one MO and one ^* MO

B)one MO and one MO

C)one MO and one ^* MO or one MO and one ^*MO

D)one ⁺ MO and one ^*MO

E)two MOs, two ⁺MOs, one MO, and one ^* MO

Q5) Electron domains for single bonds exert greater force on adjacent domains than the electron domains for multiple bonds.

A)True

B)False

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Chapter 10: Gases

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Sample Questions

Q1) Ammonium nitrite undergoes thermal decomposition to produce only gases: NH₄NO₂ (s) N₂ (g)+ 2H₂O (g)

What volume (L)of gas is produced by the decomposition of 35.0 g of NH₄NO₂(s)at 525 °C and 1.5 atm?

A)48

B)160

C)15

D)72

E)24

Q2) How many moles of gas are there in a 36.3 L container at 25.2 °C and 570.3 mm Hg?

A)1.11

B)13.2

C)0.863

D)0.0110

E)16,700

Q3) How many liters of O₂ are consumed during the combustion of 60.0 grams of ethane at STP in the open atmosphere?

Q4) How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The phase diagram of a substance is shown above.The area labeled ________ indicates the gas phase for the substance.

A)w

B)x

C)y

D)z

E)y and z

Q2) When the phase diagram for a substance has a solid-liquid phase boundary line that has a ________ slope,the substance can go from solid to liquid,within a small temperature range,via the application of pressure.

A)positive

B)zero

C)y = 1

D)negative

E)y = 0

Q3) London Dispersion Forces tend to ________ in strength with increasing molecular weight.

Q4) In general,intramolecular forces determine the ________ properties of a substance and intermolecular forces determine its ________ properties.

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) When two different monomers combine to form a polymer,the resulting compound is called a ________.

Q2) Which of the following is an addition polymer?

A)polyethylene terephthalate

B)polyurethane

C)Nylon 6,6

D)polyvinyl chloride

E)polycarbonate

Q3) What happens to a polymer as it becomes more crystalline?

A)its melting point decreases

B)its density decreases

C)its yield stress decreases

D)its stiffness decreases

E)None of the above is correct.

Q4) All of the following are polymers except ________.

A)nylon

B)cellulose

C)bronze

D)starch

E)protein

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) What is the molarity of phosphoric acid in a 22.1% (by mass)aqueous solution?

A)0.0522 m

B)0.0248 m

C)0.0992 m

D)0.0496 m

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

Q2) Which of the following would be least soluble in a nonpolar solvent?

A)NaNO₃

B)C₅H₁₂

C)NH₃

D)HF

E)CH₃CH₂OH

Q3) The phrase "like dissolves like" refers to the fact that ________.

A)gases can only dissolve other gases

B)polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes

C)solvents can only dissolve solutes of similar molar mass

D)condensed phases can only dissolve other condensed phases

E)polar solvents dissolve nonpolar solutes and vice versa

Q4) What is the osmotic pressure (in atm)of a 0.0255 M NaCl solution at 25.0 °C?

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) What is the order of the reaction with respect to OH^-?

A)0

B)1

C)2

D)3

E)4

Q2) The rate limiting step in a reaction is the slowest step in the reaction sequence.

A)True

B)False

Q3) As the temperature of a reaction is increased,the rate of the reaction increases because the ________.

A)reactant molecules collide less frequently

B)reactant molecules collide more frequently and with greater energy per collision

C)activation energy is lowered

D)reactant molecules collide with greater energy

E)reactant molecules collide more frequently

Q4) The rate-determining step is the ________ elementary step.

Q5) Define a heterogeneous catalyst.

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Page 16

Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) Fritz Haber was awarded the ________ Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen.

A)1954

B)1918

C)1933

D)1900

E)1912

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

A)True

B)False

Q3) The effect of a catalyst on a chemical reaction is to speed up the rate of the reaction in the forward direction by lowering the activation energy.

A)True

B)False

Q4) If a reaction is endothermic,________ the reaction temperature results in an decrease in K.

Q5) Define the reaction quotient.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) Which of the following salts will produce a neutral solution?

A)NaBr

B)LiNO₂

C)LiF

D)Na₂CO₃

E)NH₄Cl

Q2) Calculate the pOH of a solution at 25.0 °C that contains 2.95 × 10^-12 M hydronium ions.

A)12.00

B)2.95

C)7.00

D)2.47

E)11.53

Q3) A substance that is capable of acting as both an acid and as a base is ________.

A)autosomal

B)conjugated

C)amphiprotic

D)saturated

E)miscible

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) Which one of the following pairs cannot be mixed together to form a buffer solution?

A)HONH₂, HONH₃Cl

B)NaCl, HCl

C)RbOH, HF

D)KOH, HNO₂

E)H₂SO₃, KHSO₃

Q2) In which of the following aqueous solutions would you expect PbCl₂ to have the lowest solubility?

A)0.020 M BaCl₂

B)0.020 M Pb(NO₃)₂

C)0.020 M NaCl

D)0.020 M KCl

E)pure water

Q3) CaCO₃ is very soluble in the presence of ________.

Q4) A complex ion is when a metal ion binds to a ________.

Q5) For any buffer system,the buffer capacity depends on the amount of acid and base from which the buffer is made.

A)True

B)False

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) Nitrogen oxides catalytically destroy ozone.

A)True

B)False

Q2) The acidic water of a lake (V = 4 × 10⁸ L)must be neutralized with lime,CaO.It will require a minimum of ________ grams of lime to adjust the pH from 5.6 to 6.5.

A)2 × 10⁴

B)5 × 10⁴

C)1 × 10⁵

D)3 × 10⁴

E)5

Q3) The absorption of a photon which results in bond breaking is known as ________.

Q4) List two of the three major sources of nitrogen and phosphorus in water.

Q5) The greenhouse effect of a methane molecule far exceeds the effect of a carbon dioxide molecule.

A)True

B)False

Q6) The salinity,density,and temperature of seawater varies with ________.

Q7) Clean rainwater is ________ mainly due to the presence of carbon dioxide.

Q8) The stratosphere contains approximately ________ of the earth's ozone.

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The value of H° for the formation of calcium chloride from its constituent elements, Ca (s)+ Cl₂ (g) CaCl₂ (s) Is ________ kJ/mol.

A)0.00

B)-397.9

C)+397.9

D)-795.8

E)+795.8

Q2) The value of S° for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, 2SO₃ (g) 2S (s,rhombic)+ 3O₂ (g) Is ________ J/K mol.

A)+19.3

B)-19.3

C)+493.1

D)+166.4

E)-493.1

Q3) A reversible change produces the maximum amount of ________ that can be achieved by the system on the surroundings.

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Page 21

Chapter 20: Electrochemistry

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Sample Questions

Q1) The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a ________ process.

A)four-electron

B)one-electron

C)two-electron

D)three-electron

E)six-electron

Q2) Define the Nernst equation.

Q3) The town of Natrium,West Virginia,derives its name from the sodium produced in the electrolysis of molten sodium chloride (NaCl)mined from ancient salt deposits.The number of kilowatt-hours of electricity required to produce 4.50 kg of metallic sodium from the electrolysis of molten NaCl(s)is ________ when the applied emf is 5.00 V.

A)26.2

B)0.0381

C)0.0262

D)52.5

E)13.1

Q4) Based on standard reduction potentials,the most difficult species to reduce and the poorest oxidizing agent is ________.

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Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) Positron emission causes an increase of one in the atomic number. A)True

B)False

Q2) Transuranium elements have atomic numbers greater than ________. A)90

B)91 C)92 D)93

E)94

Q3) How many radioactive decay series exist in nature? A)0

Q4) What was the purpose of the Manhattan project?

Q5) The energy produced by the sun is the result of nuclear fusion.

A)True

B)False

Q6) What is the predominant isotope of uranium?

Page 23

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) Which group 3A element is a metalloid?

A)B

B)Al

C)Ga

D)In

E)Tl

Q2) What sulfur compound is used to sterilize wine?

A)H₂SO₄

B)H₂S

C)Na₂SO₃

D)SO₂

E)Na₂S

Q3) The primary commercial use of oxygen is ________.

A)for the treatment of respiratory distress

B)in oxyacetylene welding

C)as a household bleach

D)as an oxidizing agent

E)to charge oxygen-containing cylinders used by deep-sea divers

Q4) Why does calcium carbonate dissolve in water containing carbon dioxide?

Q5) Low levels of arsenic consumption can lead to ________ or bladder cancer.

Page 24

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Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) A ligand with a single donor atom is called ________.

A)a chelon

B)a chelate

C)polydentate

D)monodentate

E)bidentate

Q2) What are the donor atoms in ferrichrome and how many of them are in one molecule?

A)Cr, 5

B)N, 4

C)O, 6

D)Fe, 4

E)S, 6

Q3) A complex that absorbs light at 700 nm will appear ________.

A)red

B)green

C)yellow

D)orange

E)violet

Q4) Myoglobin has ________ heme group(s)that bind(s)________.

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

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Sample Questions

Q1) The suffix used for organic molecules containing the ketone functional group is

A)-one

B)-oic acid

C)-oate

D)-amide

E)-ene

Q2) The secondary structure of a protein is the result of ________ bonding.

A)covalent

B)peptide

C)ionic

D)hydrogen

E)none of the above

Q3) In an addition reaction,H₂ is added to 1-propene in the presence of a nickel catalyst to form ________.

A)propanol

B)propyne

C)propane

D)2-butene

E)propanoic acid

Page 26

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