Chemistry for Non-Majors Exam Review

Course Introduction

Chemistry for Non-Majors provides an engaging introduction to the foundational concepts of chemistry with an emphasis on real-world applications and societal relevance. Tailored for students from diverse academic backgrounds, this course explores topics such as atomic structure, chemical bonding, states of matter, reactions, and energy, emphasizing how chemical principles affect everyday life, health, environment, and technology. Laboratory activities and interactive demonstrations reinforce theoretical understanding, fostering scientific literacy and critical thinking skills without requiring advanced mathematics or prior chemistry experience.

Recommended Textbook

Introductory Chemistry An Active Learning Approach 6th Edition by Mark S. Cracolice

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21 Chapters

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Chapter 2: Matter and Energy

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Sample Questions

Q1) Which of the following changes is/are exothermic for the underlined object?

i.ice melts

ii.hot french fries cool

iii.a beaker warms as chemicals react within it

iv.a hot plate warms a beaker of water

v.water evaporates off of skin

A)iii and iv

B)i and v

C)ii only

D)All are exothermic

E)None is exothermic

Answer: C

Q2) Which of the following does not describe the gaseous state?

A)Same shape as a closed container

B)Same volume of a closed container

C)Random, independent particle movement

D)Easily compressed

E)All describe the gaseous state

Answer: E

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Page 3

Chapter 3: Measurement and Chemical Calculations

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Sample Questions

Q1) A filled shipping box weighs 12 lb.How many kilograms is this? 1 lb = 453.59237 g

A)5.4 kg

B)5.4 × 103 kg

C)5.4 × 106 kg

D)26 kg

E)2.6 × 10-5 kg

Answer: A

Q2) Which of the following is the best mathematical expression to represent the fact that the pressure of a gas (P),at constant volume and temperature,is directly proportional to the mass of that gas (m)?

A)P m

B)P = m

C)Pm

D)P m

E)P m

Answer: A

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Chapter 4: Introduction to Gases

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Sample Questions

Q1) A bubble of steam rises to the top of a container of boiling water.Which of the following features of the ideal gas model best explains this phenomenon?

A)Gases consist of molecular particles moving at any instant in straight lines

B)Molecules collide with each other and with the container walls without loss of energy

C)Gas molecules behave as independent particles

D)Gas molecules are very widely spaced

E)The actual volume of molecules is negligible compared to the space they occupy

Q2) The volume of a sealed gas balloon is changed from 953 mL to 808 mL at constant temperature.The original pressure was 155 kPa.What is the pressure after the volume is reduced ?

A)0.00547 kPa

B)0.00761 kPa

C)131 kPa

D)183 kPa

E)1.19 × 108 kPa

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Chapter 5: Atomic Theory: The Nuclear Model of the Atom

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Sample Questions

Q1) Which of the three major subatomic particles has/have a charge of -1?

i.electron

ii.proton

iii.neutron

A)i only

B)ii only

C)iii only

D)i and ii

E)ii and iii

Q2) Which of the following statements is false?

A)The atomic mass unit is exactly 1/12 of the mass of a carbon-12 atom

B)Both protons and neutrons have atomic masses very close to 1 u

C)A carbon-12 atom with six electrons has a mass of 12.6 u

D)The atomic mass of an element is the average mass of the atoms of an element compared to an atom of carbon-12 at exactly 12 u

E)To find the atomic mass of an element, you must know the atomic mass of each isotope and the fraction of each isotope in a sample

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Chapter 6: Chemical Nomenclature

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Sample Questions

Q1) What is the name of Cu(NO3)2 3 H2O?

A)Copper nitrate terthydrate

B)Copper(II) nitrate trihydrate

C)Copper nitrate terhydrate

D)Copper(II) nitrate terhydrate

E)Copper nitrate trihydrate

Q2) For each of the following formulas,choose the correct name.

i.Pb2+

ii.S2-

iii.Ni2+

I ii iii

A)lead ion sulfur ion nickel ion

B)lead ion sulfur ion nickelide ion

C)lead(II) ion sulfur ion nickel ion

D)lead(II) ion sulfide ion nickel ion

E)lead(II) ion sulfide ion nickel(II) ion

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Chapter 7: Chemical Formula Relationships

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Sample Questions

Q1) Which of the following are empirical formulas?

i.C10H8

ii.CH2

iii.Al2Cl6

iv.NO2

v.Hg2Cl2

A)i only

B)i and ii

C)ii and iv

D)i, ii, and v

E)iii, iv, and v

Q2) List the number of atoms of each element in a formula unit of ammonium sulfate.

A)1 nitrogen atom, 4 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

B)1 nitrogen atom, 3 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

C)2 nitrogen atoms, 6 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

D)2 nitrogen atoms, 8 hydrogen atoms, 1 sulfur atom, 4 oxygen atoms

E)1 nitrogen atom, 4 hydrogen atoms, 2 sulfur atoms, 8 oxygen atoms

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Chapter 8: Chemical Reactions

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Sample Questions

Q1) Calcium reacts with the oxygen in the air,forming calcium oxide.Write the balanced chemical equation for this reaction.What is the sum of the coefficients?

A)3 or less

B)4

C)5

D)6

E)7 or more

Q2) Calcium combines with bromine to make calcium bromide.Write the balanced chemical equation for this reaction.What is the coefficient for bromine?

A)1

B)2

C)3

D)4

E)5

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Chapter 9: Chemical Change

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Sample Questions

Q1) What is the net ionic equation for the preparation of Ca3(PO4)2(s)from aqueous solution?

A)3 Ca2+(aq) + 2 PO43-(aq) Ca3(PO4)2(s)

B)3 Ca(s) + 2 PO4(aq) Ca3(PO4)2(s)

C)3 CaO(aq) + 2 P2(s) + 3 O2(g)

Ca3PO4(aq) + 2 PO4(g)

D)3 Ca2+(aq) + 2 PO3-(aq) + 2 O2-(g) Ca3(PO4)2(aq)

E)3 Ca+(aq) + 2 PO4-(aq)

Ca3(PO4)2(s)

Q2) Which of the following is the best explanation of why a strong acid is an excellent conductor?

A)It is almost completely ionized in water

B)It undergoes a vigorous chemical reaction with the water molecules

C)It is immiscible in water

D)All acids are natural conductors

E)It reduces electronic vibration and thus allows greater conductivity

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Chapter 10: Quantity Relationships in Chemical Reactions

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Sample Questions

Q1) A chemist combines hydrochloric acid with a sodium hydroxide solution,transferring 5.75 kJ of heat.Express this in calories.

A)2.41 × 10-2 cal

B)2.41 × 101 cal

C)2.41 × 104 cal

D)1.37 × 10-3 cal

E)1.37 × 103 cal

Q2) If the reaction N2 + 3 H2 2 NH3 is carried out using 1.40 g of N2 and 0.400 g of H2,what mass of excess reactant will remain?

A)0.200 g N2

B)1.00 g N2

C)0.100 g H2

D)0.300 g H2

E)Both reactants will be completely consumed

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Chapter 11: Atomic Theory: The Quantum Model of the Atom

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Sample Questions

Q1) What is the ground state electron configuration of potassium?

A)[Ar] 3d1

B)1s22s22p63s23p63d<su p>1

C)[Ar] 4s1

D)1s22s22p62d103s1

E)None of the above is correct

Q2) Which of the following pairs of atomic numbers belong to elements whose atoms have the highest occupied energy level electron configuration of the form ns2np4?

A)16 and 52

B)40 and 72

C)24 and 42

D)9 and 17

E)14 and 32

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Chapter 12: Chemical Bonding

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Sample Questions

Q1) In a covalent bond,the valence electrons from atoms are:

A)shared

B)transferred to the less metallic element

C)transferred to the more metallic element

D)gained by the anion

E)gained by the cation

Q2) Which bond is completely nonpolar?

A)F-F

B)H-F

C)C-N

D)H-O

E)C-H

Q3) What is the electron configuration of an ion that is isoelectronic with neon?

A)[Ne]3s23p6

B)[Ar]3s23p6

C)[Ar]4s2

D)1s22s22p6

E)1s22s22p2

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Page 13

Chapter 13: Structure and Shape

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Sample Questions

Q1) Which of the following best describes a polar molecule?

A)One with atoms having the same electronegativities

B)One with asymmetrical distribution of charge

C)A molecule without charge

D)One with a tetrahedral molecular geometry

E)One that has two or more hydrogen atoms

Q2) Which of the following has a linear electron pair geometry?

i.IO2-

ii.H2S

iii.BeF2

iv.ICl2+

A)i only

B)ii only

C)iii only

D)i and iv

E)ii and iii

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Chapter 14: The Ideal Gas Law and Its Applications

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Sample Questions

Q1) A gas has a density of 1.19 g/L at STP.Which of the following could be this gas?

A)C4H10

B)C3H6

C)HCN

D)HI

E)OF2

Q2) How many liters of hydrogen,measured at 20°C and 750 torr,are required to react with 55.2 grams of aluminum oxide in the reaction Al2O3 + 3 H2 2 Al + 3 H2O?

A)36.6 L

B)1.62 L

C)2.70 L

D)0.0253 L

E)0.0520 L

Q3) Calculate the molar volume of a gas at 21°C and 3.73 atm.

A)0.462 L/mol

B)0.155 L/mol

C)351 L/mol

D)4.92 × 103 L/mol

E)6.47 L/mol

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Chapter 15: Gases, Liquids, and Solids

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Sample Questions

Q1) Which of the following statements is correct?

A)Intermolecular forces are weaker in liquids than in gases because the particles are closer to each other

B)Smaller intermolecular distances in liquids result in stronger intermolecular forces, when compared to intermolecular distances and forces in gases

C)Compared to liquids, large distances between gaseous molecules yield large intermolecular attractions

D)The smaller the distance between molecules the smaller the intermolecular attractions, therefore attractions are weaker in liquids than gases

E)All statements are correct

Q2) The main reason equilibrium vapor pressure is greater at higher temperatures is that...

A)A larger fraction of the molecules in the sample has sufficient kinetic energy to move from the liquid phase to the vapor phase

B)The average kinetic energy is greater

C)Intermolecular attractions are weaker

D)The particles are moving at higher speeds

E)The escape energy is decreased

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Chapter 16: Solutions

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Sample Questions

Q1) Calculate the normality of a potassium hydroxide solution if 27.7 mL of the solution is needed to neutralize 0.477 g of sulfamic acid in the reaction NH2SO3H + KOH NH2SO3K + H2O.

A)3.57 × 10-4 N

B)1.77 × 10-4 N

C)4.38 × 103 N

D)5.64 N

E)0.177 N

Q2) Which of the following correctly applies to the term "solution"?

A)heterogeneous mixture

B)variable composition

C)constant properties

D)dissolved particles can are usually larger than about 10-7 cm

E)exist only in the liquid and gas state

Q3) When a saturated solution is in equilibrium with undissolved solute:

A)the solution separates into layers

B)dissolving and crystallization stop

C)the quantity of dissolved solute equals the quantity of undissolved solute

D)the concentration of the solution remains constant

E)the temperature increases until more solute dissolves

Page 17

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Chapter 17: Acidbase Proton Transferreactions

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Sample Questions

Q1) A water solution is considered acidic when what is true?

A)[H+] = [OH-]

B)[H+] < [OH-]

C)[OH- ] > [H+]

D)[H+] > [OH-]

E)[H+] = Kw

Q2) Which of the following is a Lewis acid but not a Brønsted-Lowry acid?

A)OH-

B)HPO42-

C)HCl

D)NH4+

E)Fe3+

Q3) Which of the following is a Brønsted-Lowry base but not an Arrhenius base?

A)HSO3-(aq)

B)NaOH(s)

C)NH4+(aq)

D)Al(OH)3(s)

E)NH4OH(aq)

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Chapter 18: Chemical Equilibrium

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Sample Questions

Q1) Which of the following statements is/are incorrect?

i.Undissolved sugar in contact with a saturated sugar solution in an open beaker cannot reach equilibrium

ii.A liquid and its vapor enclosed in two one-liter containers connected by an open glass tube cannot reach equilibrium

iii.A solution of a weak acid,hydronium ion,and the conjugate base of the weak acid cannot reach equilibrium

A)i only

B)ii only

C)i and ii

D)ii and iii

E)i, ii, and iii

Q2) What is the pH of a 0.20 M solution of nitrous acid? Ka = 4.5 × 10-4

A)9.02

B)4.66

C)4.05

D)2.02

E)0.70

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Chapter 19: Oxidationreduction Electron Transferreactions

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Sample Questions

Q1) Which of the following statements is correct for an electrolytic cell?

A)Electrons flow through the external circuit from the anode to the cathode

B)The electrode at which oxidation occurs is the cathode

C)The reaction occurring in the cell can be used to generate an electric current.

D)Charge is carried through the solution by electrons in one direction and by protons in the other direction

E)None of the statements above is correct

Q2) What is the oxidation number of sulfur in sulfite ion,SO32-?

A)+6

B)+4

C)-2

D)+2

E)-4

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Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) Which of the following is the best definition of the term nuclear fission?

A)A nuclear reaction in which two small nuclei combine to form a larger nucleus

B)A nuclear reaction in which a large nucleus splits into two smaller nuclei

C)The combination of a nucleus and an electron to produce an element with an atomic number one less than the original element

D)The combination of a nucleus and a positron to produce an element with an atomic number one more than the original element

E)The ejection of an electron from a nucleus to produce an element with an atomic number one more than the original element

Q2) Which of the following is not a source of radiation?

i.medical X rays

ii.tobacco smoke

iii.nuclear medicine

A)i only

B)i and ii

C)i and iii

D)ii and iii

E)All are sources of radiation

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Chapter 21: Organic Chemistry

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Sample Questions

Q1) Which of the following compounds are classified as alkenes? Assume that none of the compounds listed is a cycloalkane.

i.C5H10

ii.C7H16

iii.C4H8

iv.C10H22

v.CH4

A)i and iii

B)ii and iv

C)ii, iv, and v

D)iii, iv, and v

E)All are alkenes

Q2) What is the product of the hydrogenation of trans-2-pentene?

A)isopentane

B)neopentane

C)cis-2-pentane

D)trans-2-pentane

E)n-pentane

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Chapter 22: Biochemistry

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Sample Questions

Q1) Which of the following statements is correct?

i.The shape and polarity of the active site of an enzyme allows only a few dozen substrate molecules to bind reversibly to the enzyme at a time.

ii.If a substrate remains bound to an enzyme,that enzyme molecule can no longer function as a catalyst.

iii.Military nerve gases are examples of irreversible inhibitors.

A)i only

B)ii only

C)iii only

D)i and ii

E)ii and iii

Q2) In simple sugars,every carbon but one contains a hydroxyl group; the remaining carbon is double bonded to an oxygen atom as a carbonyl group.What type of sugar has the carbonyl at the end of the carbon chain?

A)Cretose

B)Polysaccharide

C)Disaccharide

D)Aldose

E)Ketose

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