Introductory Chemistry Practice Exam - 3150 Verified Questions

Introductory Chemistry Practice Exam

Course Introduction

Introductory Chemistry is designed to provide students with a foundational understanding of the basic principles and concepts in chemistry. The course covers topics such as atomic and molecular structure, chemical bonding, stoichiometry, states of matter, solutions, and introductory thermochemistry. Students will also learn about chemical reactions, the periodic table, and the scientific method as it applies to chemical investigation. Emphasis is placed on problem-solving skills, conceptual understanding, and practical laboratory techniques to prepare students for more advanced studies in chemistry and related sciences.

Recommended Textbook Chemistry 12th Edition by Raymond Chang

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25 Chapters

3150 Verified Questions

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Page 2

Chapter 1: Chemistry: The Study of Change

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Sample Questions

Q1) Convert 6.4 mm³ to mL.

A) 6.4 x 10^-3 mL

B) 6.4 x 10^-1 mL

C) 6.4 x 10³ mL

D) 6.4 x 10^-2 mL

E) 6.4 mL

Answer: A

Q2) Which of the following is true of an element

A) An element is a substance composed of atoms of two or more elements

B)An element is a substance that cannot be separated into simpler substances by chemical means.

C)An element is combination of two or more substances in which the substances retain their distinct identities.

D) An element must be heterogeneous

E) An element must be a solid at room temperature

Answer: B

Q3) Antifreeze boiling out of a radiator is a physical change.

A)True

B)False

Answer: True

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Chapter 2: Atoms Molecules and Ions

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Sample Questions

Q1) What are the two different ions present in the compound Li₃N

A) Li⁺, N^3-

B) Li₃⁺, N^-

C) Li₃³⁺, N^3-

D) Li⁺, N^-

E) Li³⁺, N^3-

Answer: A

Q2) Name the compound CuSO₄.

A) Copper (I) sulfate

B) Copper (I) sulfite

C) Copper (II) sulfite

D) Copper (II) sulfate

E) Copper (IV) sulfate

Answer: D

Q3) The formula of nitrous acid is HNO₃.

A)True

B)False

Answer: False

Q4) What are the two different ions present in the compound FeCl₃

Answer: \(Fe^{2+}, Cl^-\)

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) The mineral manganosite is a compound of ⁵⁵Mn and ¹⁶O. If 77% of the mass of manganosite is due to manganese, what is the empirical formula of manganosite

A) MnO

B) Mn₂O

C) Mn₂O₂

D) MnO₂

E) none of these

Answer: A

Q2) A compound with a percent composition by mass of 87.5% N and 12.5% H was recently discovered. What is the empirical formula for this compound

A) NH₂

B) NH₄

C) N₃H₂

D) N₂H₃

E) None of the above

Answer: A

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) Which of the following compounds is a nonelectrolyte

A) NaF

B) HNO₃

C) CH₃COOH (acetic acid)

D) NaOH

E) C₆H₁₂O₆ (glucose)

Q2) The distinguishing characteristic of all electrolyte solutions is that they

A) contain molecules.

B) conduct electricity.

C) react with other solutions.

D) always contain acids.

E) conduct heat.

Q3) Determine the correct oxidation numbers for all three elements in Ca(ClO)₂ in the order that the elements are shown in the formula

A) +2, +1, -2.

B) +2, -2, +1.

C) +2, -3, +2

D) -2, +2, -1

E) -2, +3, -2

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Page 6

Chapter 5: Gases

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Sample Questions

Q1) Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm³ at 97^\(\circ\)C.

The pressure of the chloroform is 728 mmHg.

A) 8.28 * 10^-3 g/mol

B) 31.6 g/mol

C) 112 g/mol

D) 121g/mol

E) 187g/mol

Q2) 5.00 g of hydrogen gas and 50.0 g of oxygen gas are introduced into an otherwise empty 9.00 L steel cylinder, and the hydrogen is ignited by an electric spark. If the reaction product is gaseous water and the temperature of the cylinder is maintained at 35ºC, what is the final gas pressure inside the cylinder

A) 0.92 atm

B) 2.58 atm

C) 6.96 atm

D) 7.86 atm

E) 18.3 atm

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Page 7

Chapter 6: Thermochemistry

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Sample Questions

Q1) The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH₄NO₃ is added to 40.0 mL of water in a calorimeter at 23.5^\(\circ\)C, what is the minimum temperature reached by the solution (The specific heat of water = 4.18 J/g·^\(\circ\)C; the heat capacity of the calorimeter = 650. J/^\(\circ\)C.)

A) -7.7^\(\circ\)C

B) 14.3^\(\circ\)C

C) 20.8^\(\circ\)C

D) 21.4^\(\circ\)C

E) 25.6^\(\circ\)C

Q2) For which of these reactions will the difference between \(\Delta\)H^\(\circ\) and \(\Delta\)E^\(\circ\) be the smallest

A) N₂(g) + 3H₂(g) \(\rarr\) 2NH₃(g)

B) 4PH₃(g) \(\rarr\) P₄(g) + 6H₂(g)

C) H₂(g) + Cl₂(g) \(\rarr\) 2HCl(g)

D) CO₂(g) + 2H₂O(l) \(\rarr\) CH₄(g) + 2O₂(g)

E) P₄(s) + 10Cl₂(g) \(\rarr\) 4PCl₅(s)

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) Which one of the following sets of quantum numbers represents an electron with the highest energy

A) n = 3, l = 2, m_l = -2, m_s = +1/2

B) n = 4, l = 1, m_l = 0, m_s = -1/2

C) n = 4, l = 0, m_l = 0, m_s = +1/2

D) n = 5, l = 0, m_l = 0, m_s = +1/2

E) n = 4, l = 2, m_l = -1, m_s = -1/2

Q2) List the following sets of quantum numbers in order of increasing energy:

I. n = 4, l = 1, m_l = 1, m_s = +1/2

II. n = 3, l = 2, m_l = -1, m_s = +1/2

III. n = 4, l = 0, m_l = 0, m_s = +1/2

A) I < II < III

B) II < III < I

C) III < II < I

D) I < III < II

E) III < I < II

Q3) There is nothing wrong with the following set of quantum numbers:

n = 3, l = 1, m_l = 0, m_s = +1/2

A)True

B)False

Page 9

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) The electron affinity of fluorine is essentially equal to

A) the negative of the ionization energy F.

B) the ionization energy F-.

C) the negative of the ionization energy F-.

D) the ionization energy Ne.

E) the negative of the ionization energy Ne.

Q2) In general the effective nuclear charge felt by the outermost electrons of an element increases when moving across a period.

A)True

B)False

Q3) The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) \(\rarr\)Hg⁺(g) + e^- is therefore

A) 1006 kJ/mol.

B) greater than 1006 kJ/mol.

C) less than 1006 kJ/mol.

D) is equal to the electron affinity of mercury.

E) is equal to the second ionization energy of mercury.

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Page 10

Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) The Lewis structure reveals only single bonds in which of the following species

A) CO₂

B) CO

C) CO₃^2-

D) Cl₂CO

E) CCl₄

Q2) The properties and chemical reactivity of a molecule is best explained by analyzing all possible resonance structures for that molecule.

A)True

B)False

Q3) Which one of the following compounds does not follow the octet rule

A) NF₃

B) CO₂

C) CF₄

D) Br₂

E) NO

Q4) The polarity of covalent bonds increases as the percent ionic character increases.

A)True

B)False

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Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization

of Atomic

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Sample Questions

Q1) What is the bond order of Cl₂^-

A) 0

B) 0.5

C) 1

D) 1.5

E) 2

Q2) Give the number of lone pairs around the central atom and the molecular geometry of XeF₂.

A) 0 lone pairs, linear

B) 1 lone pair, bent

C) 2 lone pairs, bent

D) 3 lone pairs, bent

E) 3 lone pairs, linear

Q3) The number of pi bonds in the oxalate ion (C₂O₄^2-) is

A) 1

B) 2

C) 3

D) 4

E) 5

Page 12

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) Indicate all the types of intermolecular forces of attraction in HCl(g).

A) Dispersion and Dipole-dipole

B) Dipole-dipole and Ionic

C) Ion-dipole and Hydrogen bonding

D) Hydrogen bonding and Dispersion

E) Dispersion

Q2) The intermolecular forces present in CH₃NH₂ include which of the following

I. dipole-dipole

II. ion-dipole

III. dispersion

IV. hydrogen bonding

A) I, II, III, and IV

B) I and III

C) I, III, and IV

D) I and II

E) II and IV

Q3) At room temperature, honey is more viscous than mustard.

A)True

B)False

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Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) The solubility of gases in water always decreases with increasing temperature.

A)True

B)False

Q2) Which of the following concentration units will change with temperature

A) Percent mass

B) Mole fraction

C) Molality

D) Molarity

E) None of the above will change with temperature

Q3) Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true

A) The vapor pressure of the solution is always greater than the vapor pressure of the pure solvent.

B) The boiling point of the solution is always greater than the boiling point of the pure solvent.

C) The freezing point of the solution is always greater than the freezing point of the pure solvent.

Q4) Meat that is salted before cooking tends to dry out.

A)True

B)False

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) The activation energy for a certain reaction is 113 kJ/mol. By what factor (how many times) will the rate constant increase when the temperature is raised from 310 K to 325 K

A) 36

B) 5.6

C) 7.6

D) 9.6

E) None of the above

Q2) Which of the following elementary steps is termolecular

A)2A + B \(\rarr\) A₂B

B)B₃ \(\rarr\) 2B + B

C)A + B \(\rarr\) AB

D)A₃ + B₂ \(\rarr\) 2AB + A

E)A₃B \(\rarr\) 2A + AB

Q3) Appropriate units for a first-order rate constant are

A) M/s.

B) 1/M·s.

C) 1/s.

D) 1/M²·s.

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Page 15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) The K_c for the reaction CO₂(g) + H₂(g) H₂O(g) + CO(g) is 1.6 at about 990ºC. Calculate the number of moles of hydrogen gas in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

A) 0.42 mol

B) 0.62 mol

C) 0.82 mol

D) 1.02 mol

E) None of the above

Q2) Concerning the following reaction at equilibrium: 3Fe(s) + 4H₂O(g) Fe₃O₄(s) + 4H₂(g), increasing the volume of the container would:

A) Shift the equilibrium to the right

B) Shift the equilibrium to the left

C) Increase the value of the equilibrium constant, K

D) Decrease the value of the equilibrium constant, K

E) Cause no change

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Page 16

Chapter 15: Acids and Bases

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Sample Questions

Q1) The pH of coffee is approximately 5.0. How many times greater is the [H₃O⁺] in coffee than in tap water having a pH of 8.0

A) 0.62

B) 1.6

C) 30

D) 1,000

E) 1.0 * 10⁴

Q2) Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10^-4 M.

A) 2.34

B) 3.47

C) 6.01

D) 7.99

E) 10.53

Q3) H₃AsO₃ is a stronger acid than H₃AsO₄.

A)True

B)False

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. (For CrF₃ , K_sp = 6.6 * 10^-11.)

A) 0.023 M

B) 0.032 M

C) 7.7 * 10^-8 M

D) 2.9 * 10^-9 M

E) 6.9 * 10^-10 M

Q2) What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M propanoic acid (C₂H₅COOH) to obtain a solution with a pH of 5.25? [K_a(C₂H₅COOH) = 1.34 * 10^-5]

A) 32 mL

B) 210 mL

C) 160 mL

D) 65 mL

E) 13 mL

Q3) The solubility of a salt increases as its K_sp increases.

A)True

B)False

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Page 18

Chapter 17: Entropy Free Energy and Equilibrium

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Sample Questions

Q1) Using the thermodynamic data provided below, calculate the standard change in entropy when one mole of sodium nitrate is dissolved in water. \(\begin{array}{|l|c|}

\hline & \mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol}) \\

\hline \mathrm{NaNO}_{3}(\mathrm{s}) & 116.3 \\

\hline \mathrm{Na}^{+}(a q) & 60.25 \\

\hline \mathrm{NO}_{3}^{-}(a q) & 146.4 \\

\hline

\end{array}\) Will the solubility of sodium nitrate increase or decrease if the temperature of the system is increased

A) -90.4 J/K·mol; solubility decreases with increasing temperature

B) -90.4 J/K·mol; solubility increases with increasing temperature

C) 90.4 J/K·mol; solubility decreases with increasing temperature

D) 90.4 J/K·mol; solubility increases with increasing temperature

E) None of the above

Q2) For a given substance the entropy always increases in the following order:

S (gas) < S (liq) < S (solid).

A)True

B)False

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Chapter 18: Electrochemistry

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Sample Questions

Q1) Under basic conditions, the correctly balanced redox reaction for CrO₄^2-(aq) + SO₃^2-(aq) \(\rarr\) Cr(OH)₃(s) + SO₄^2-(aq) is 2CrO₄^2-(aq) + 3SO₃^2-(aq) + 5H₂O(l) \(\rarr\)2Cr(OH)₃(s) + 3SO₄^2-(aq) + 2OH^-(aq)

A)True

B)False

Q2) Which of these metals will not reduce water to hydrogen in basic solution under standard conditions

A) Cd

B) Sr

C) Mg

D) Ba

E) K

Q3) When an aqueous solution of NaCl is electrolyzed, Na(l) is produced at the cathode, and Cl₂(g) is evolved at the anode.

A)True

B)False

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Page 20

Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) List the different types of nuclear radiation (alpha, beta, gamma) in order of increasing penetrating power.

A) alpha < beta < gamma

B) beta < alpha < gamma

C) gamma < alpha < beta

D) gamma < beta < alpha

E) alpha < gamma < beta

Q2) As opposed to chemical reaction, nuclear reactions have a significant (measureable) mass change relative to the mass of the reacting species.

A)True

B)False

Q3) Calculate the binding energy per nucleon of an Al-27 nucleus given the following masses: \({ }_{13}^{27} \mathrm{Al}\) : 26.981541 amu; : \({ }_{1}^{1} \mathrm{H}\) 1.007838 amu; : \({ }_{0}^{1} \mathrm{n}\) 1.008665 amu.

A) 1.14 * 10^-12 J/nucleon

B) 1.34 * 10^-12 J/nucleon

C) 1.54 * 10^-12 J/nucleon

D) 1.74 * 10^-12 J/nucleon

E) None of the above

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Page 21

Chapter 20: Chemistry in the Atmosphere

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Sample Questions

Q1) Which of the following sources does NOT contribute significantly to the greenhouse effect

A) Coal-fired power plants

B) Landfills

C) Automobile exhaust

D) Nuclear power plants

E) Chlorofluorocarbons

Q2) The steps in the mechanism by which ozone is formed in the stratosphere are shown here:

O₂(g) + O \(\rarr\) 2O(g)

O(g) + O₂(g) \(\rarr\) O₃(g)

A)True

B)False

Q3) In order for a gas to be a "greenhouse gas" it must

A) transmit visible light and absorb infrared radiation.

B) be radioactive.

C) transmit infrared light and absorb visible light.

D) be combustible.

E) absorb both visible light and infrared radiation.

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Page 22

Chapter 21: Metallurgy and the Chemistry of Metals

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Sample Questions

Q1) Write the chemical formula of pyrite.

A) FeS

B) Fe₂S₃

C) FeS₂

D) Fe₃S₂

E) None of the above

Q2) Metallic sodium is obtained commercially from molten sodium chloride by A) chemical reduction with magnesium.

B) flotation.

C) electrolysis.

D) zone refining.

E) roasting.

Q3) The following depicts a correctly balanced chemical equation illustrating roasting.2ZnS + 3O₂ \(\rarr\) 2ZnO + 2SO₂

A)True

B)False

Q4) Cast iron as it is prepared in a blast furnace is a product of high purity.

A)True

B)False

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Chapter 22: Nonmetallic Elements and Their Compounds

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Sample Questions

Q1) Which of the following choices is/are ionic oxides

I. SrO

II. SiO₂

III. SO₂

A) I only

B) II only

C) III only

D) I and II

E) II and III

Q2) Select acidic oxide from the choices given.

A) CaO

B) Na₂O

C) Na₂O₂

D) P₄O₆

E) KOH

Q3) Alkali metal hydrides are very reactive with water, forming H₂ gas.

A)True

B)False

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Chapter 23: Transition Metals Chemistry and Coordination Compounds

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Sample Questions

Q1) In the complex ion [ML₆]ⁿ⁺, Mⁿ⁺ has seven d electrons and L is a strong field ligand. According to crystal field theory, the magnetic properties of the complex ion correspond to how many unpaired electrons

A) 0

B) 1

C) 2

D) 3

E) 5

Q2) The total number of electrons in the 3d orbitals of Co³⁺ is A) 4.

B) 5.

C) 6.

D) 7.

E) 10.

Q3) The total number of electrons in the 3d orbitals of Cr³⁺ is

A) 1.

B) 2.

C) 3.

D) 4.

E) 5.

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Chapter 24: Organic Chemistry

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Sample Questions

Q1) The reaction of ethylene and water yields

A) an aldehyde.

B) an ester.

C) an alcohol.

D) an ether.

E) an organic acid.

Q2) The name for the compound with the formula CH₃CH₂CH₂CH₂OH is

A) propanol.

B) propane.

C) butanol.

D) pentane.

E) pentanol.

Q3) Which type of organic compound does not contain a carbonyl

A) carboxylic acid

B) ketone

C) aldehyde

D) ester

E) ether

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Page 26

Chapter 25: Synthetic and Natural Organic Polymers

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Sample Questions

Q1) Both DNA and RNA have double-helical structures.

A)True

B)False

Q2) Which of these molecules is a product of the hydrolysis of DNA

A) acetic acid

B) glucose

C) adenine

D) ribose

E) water

Q3) What structural feature is required to have an isotactic or syndiotactic carbon-based polymer

A) A repeating unit that contains an asymmetric carbon

B) A repeating unit that contains a double bond

C) A repeating unit that contains a triple bond

D) A repeating unit that contains an aromatic hydrocarbon

E) A repeating unit that contains an atom other than carbon

Q4) The primary structure of a protein refers to the unique amino acid sequence of the polypeptide chain.

A)True

B)False

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