General Chemistry I Mock Exam
Course Introduction
General Chemistry I is an introductory course that explores the fundamental principles and concepts of chemistry. The course covers atomic structure, chemical bonding, stoichiometry, periodic properties, chemical reactions, thermochemistry, and the properties of gases, liquids, and solids. Emphasis is placed on developing problem-solving skills and an understanding of the molecular basis of matter and its changes. Laboratory activities complement the lecture material by providing hands-on experience in basic chemical techniques and experimental data analysis. This course lays the groundwork for further studies in chemistry and related scientific fields.
Recommended Textbook
Introductory Chemistry An Atoms First Approach 1st Edition by Julia Burdge
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Chapter 1: Atoms and Elements
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Sample Questions
Q1) Lithium forms compounds which are used in dry cells, storage batteries, and in high-temperature lubricants.It has two naturally occurring isotopes, <sup>6</sup>Li (isotopic mass = 6.015123 amu) and <sup>7</sup>Li (isotopic mass = 7.016005 amu).Lithium has an atomic mass of 6.9412 amu.What is the percent abundance of lithium-6?
A)92.53%
B)86.65%
C)49.47%
D)7.47%
E)6.015%
Answer: D
Q2) The elements in a column of the periodic table are known as A)metalloids.
B)a period.
C)noble gases.
D)a group.
E)nonmetals.
Answer: D
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3
Chapter 2: Electrons and the Periodic Table
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Sample Questions
Q1) A sulfide ion, S<sup>2-</sup>, has
A)16 protons and 16 electrons.
B)32 protons and 16 electrons.
C)16 protons and 14 electrons.
D)16 protons and 18 electrons.
E)32 protons and 18 electrons.
Answer: D
Q2) List the following types of radiation from lowest frequency to highest frequency: microwave, X ray, ultraviolet, visible, and infrared
A)microwave < infrared < visible < ultraviolet < X ray
B)X ray < ultraviolet < visible < infrared < microwave
C)visible < ultraviolet < microwave < X ray < infrared
D)infrared < X ray < microwave < ultraviolet < visible
E)infrared < visible < microwave < ultraviolet < X ray
Answer: A
Q3) Each shell (principal energy level) of quantum number n contains n subshells.
A)True
B)False
Answer: True
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Chapter 3: Compounds and Chemical Bonds
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Sample Questions
Q1) Which of these is an example of a physical property?
A)Corrosiveness of sulfuric acid
B)Toxicity of cyanide
C)Flammability of gasoline
D)Neutralization of stomach acid with an antacid
E)Lead becomes a liquid when heated to 601°C.
Answer: E
Q2) What is the formula of iodous acid?
A)HI
B)HIO<sub>3</sub>
C)HIO
D)HIO<sub>4</sub>
E)HIO<sub>2</sub>
Answer: E
Q3) A scoop of vanilla ice cream is a pure substance.
A)True
B)False
Answer: False
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5
Chapter 4: How Chemists Use Numbers
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Sample Questions
Q1) Select the smallest unit.
A)mm
B) m
C)nm
D)km
E)dm
Q2) Convert the measurement 2.887 cL to units of mL.
A)2.887 × 10<sup>1</sup> mL
B)2.887 × 10<sup>4</sup> mL
C)2.887 × 10<sup>5</sup> mL
D)2.887 × 10<sup>8</sup> mL
E)2.887 × 10<sup> </sup><sup>8</sup> mL
Q3) What unit would be most appropriate when reporting the volume 1.94 × 10<sup> </sup><sup>3</sup> g?
A)mg
B) g
C)kg
D)dg
E)Mg
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Page 6
Chapter 5: The Mole and Chemical Formulas
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Sample Questions
Q1) How many grams are present in 0.885 moles of manganese?
A)62.1 g
B)48.6 g
C)21.5 g
D)27.5 g
E)0.016 g
Q2) Determine the mass of hydrogen (in grams) that contains 5.08 × 10<sup>15</sup> hydrogen atoms.
A)5.12 × 10<sup>15</sup> g
B)3.06 × 10<sup>39</sup> g
C)3.06 × 10<sup> </sup><sup>9</sup> g
D)8.50 × 10<sup> </sup><sup>9</sup> g
E)8.5 × 10<sup>15</sup> g
Q3) What is the molecular mass of acetaminophen, C<sub>8</sub>H<sub>9</sub>NO<sub>2</sub>?
A)43 amu
B)76 amu
C)151 amu
D)162 amu
E)125 amu
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Chapter 6: Molecular Shape
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Sample Questions
Q1) Which is the most reasonable prediction for the H-C-H bond angle in CH<sub>4</sub>?
A)90°
B)109.5°
C)120°
D)107°
E)105°
Q2) The strongest intermolecular interactions between ethyl alcohol (CH<sub>3</sub>CH<sub>2</sub>OH) molecules arise from
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)ion-dipole interactions.
E)carbon-oxygen bonds.
Q3) Which one of the following molecules is nonpolar?
A)NH<sub>3</sub>
B)OF<sub>2</sub>
C)CH<sub>3</sub>Cl
D)H<sub>2</sub>O
E)BeCl<sub>2</sub>
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Chapter 7: Solids, Liquids, and Phase Changes
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Sample Questions
Q1) Which of the substances would form an ionic solid?
A)NCl<sub>3</sub>
B)NH<sub>4</sub>Cl
C)Ag
D)He
E)OF<sub>2</sub>
Q2) Ammonia's unusually high melting point is the result of
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)covalent bonding.
E)ionic bonding.
Q3) How much heat is required to raise the temperature of 22.8 g of copper from 20.0°C to 875.0°C? The specific heat of copper is 0.385 J/g·°C.
A)14.4 J
B)176 J
C)7.51 kJ
D)7.68 kJ
E)9.90 kJ
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9
Chapter 8: Gases
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Sample Questions
Q1) What is the initial pressure of a gas having an initial temperature of 905 K, an initial volume of 14.3 L, a final pressure of 0.83 atm, a final temperature of 154 K and a final volume of 2.7 L?
A)26 atm
B)0.27 atm
C)0.75 atm
D)1.3 atm
E)0.92 atm
Q2) Gases are sold in large cylinders for laboratory use.What pressure is exerted by 2.500 kg of oxygen gas (O<sub>2</sub>) stored at 22°C in a 40.0-L cylinder? (R = 0.08206 L atm/K mol)
A)3.55 atm
B)1.51 ×10<sup>3</sup> atm
C)47.3 atm
D)7.56 × 10<sup>4</sup> atm
E)10.2 atm
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Chapter 9: Physical Properties of Solutions
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Sample Questions
Q1) Determine the molality of a solution formed by dissolving 0.0257 moles of Li<sub>3</sub>PO<sub>4</sub> in 735 grams of water.The density of the solution is 1.74 g/mL.
A)0.0189 m
B)0.0498 m
C)0.0201 m
D)0.0350 m
E)0.0286 m
Q2) Based on the solubility rules, which one of these compounds is soluble in water?
A)CaSO<sub>4</sub>
B)BaSO<sub>4</sub>
C)PbSO<sub>4</sub>
D)K<sub>2</sub>SO<sub>4</sub>
E)Ag<sub>2</sub>SO<sub>4</sub>
Q3) Based on the solubility rules, which one of these compounds is soluble in water?
A)AgBr
B)AgCl
C)Ag<sub>2</sub>CO<sub>3</sub>
D)AgNO<sub>3</sub>
E)Ag<sub>2</sub>S
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Chapter 10: Chemical Reactions and Chemical Equations
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Sample Questions
Q1) In the reaction 5H<sub>2</sub>O<sub>2</sub> + 2MnO<sub>4</sub><sup> </sup> + 6H<sup>+</sup> 2Mn<sup>2+</sup> + 8H<sub>2</sub>O + 5O<sub>2</sub>, what is the oxidizing agent?
A)H<sub>2</sub>O<sub>2</sub>
B)MnO<sub>4</sub><sup> </sup>
C)H<sup>+</sup>
D)Mn<sup>2+</sup>
E)O<sub>2</sub>
Q2) What is the oxidizing agent in the following reaction? 5Fe<sup>2</sup><sup>+</sup>(aq) + MnO<sub>4</sub><sup> </sup>(aq) + 8H<sup>+</sup>(aq) 5Fe<sup>3+</sup>(aq) + Mn<sup>2+</sup>(aq) + 4H<sub>2</sub>O(l)
A)Fe<sup>2+</sup>
B)MnO<sub>4</sub><sup> </sup>
C)H<sup>+</sup>
D)Mn<sup>2+</sup>
E)Fe<sup>3+</sup>
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12
Chapter 11: Using Balanced Chemical Equations
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Sample Questions
Q1) What is the volume of NH<sub>3</sub> produced in the following reaction when 3.0 L of N<sub>2</sub> reacts with 4.0 L of H<sub>2</sub> ? N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g)
A)1.5 L
B)2.7 L
C)6.0 L
D)7.5 L
E)12 L
Q2) Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions.A mixture of 82.49 g of aluminum and 117.65 g of oxygen is allowed to react.Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.
A)Oxygen is the limiting reactant; 19.81 g of aluminum remain.
B)Oxygen is the limiting reactant; 35.16 g of aluminum remain.
C)Aluminum is the limiting reactant; 16.70 g of oxygen remain.
D)Aluminum is the limiting reactant; 35.16 g of oxygen remain.
E)Aluminum is the limiting reactant; 44.27 g of oxygen remain.
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Chapter 12: Acids and Bases
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Sample Questions
Q1) What is the concentration of H<sup>+</sup> in a 0.025 M HCl solution?
A)0
B)0.013 M
C)0.025 M
D)0.050 M
E)0.010 M
Q2) Which solution is the most acidic?
A)pH = 1.00
B)pH = 10.00
C)pH = 5.00
D)pH = 3.00
E)pH = 4.00
Q3) Which pair of substances is capable of forming a buffer in aqueous solution?
A)H<sub>3</sub>PO<sub>4</sub>, Na<sub>3</sub>PO<sub>3</sub>
B)HNO<sub>3</sub>, NaNO<sub>3</sub>
C)HCl, NaCl
D)H<sub>2</sub>CO<sub>3</sub>, NaNO<sub>2</sub>
E)CH<sub>3</sub>COOH, CH<sub>3</sub>COONa
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Page 14
Chapter 13: Equilibrium
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Sample Questions
Q1) At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.
A)True
B)False
Q2) Which substances are included in the equilibrium constant expression, K<sub>c</sub>?
A)Only pure solids
B)Only pure liquids
C)Only pure solids and liquids
D)Only gases and dissolved substances
E)All participating substances
Q3) What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?
A)Reversibility expression
B)Reaction expression
C)Equilibrium expression
D)Product quotient
E)Mass action
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Chapter 14: Organic Chemistry
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Sample Questions
Q1) What label is given to an alkyl group?
A)Alk
B)A
C)K
D)R
E)AG
Q2) What name is given to a compound containing a COOH group?
A)Aldehyde
B)Ketone
C)Alcohol
D)Carboxylic acid
E)Ester
Q3) Which class or family of compounds contains both the carbonyl group and the amine group?
A)Alcohols
B)Esters
C)Amide
D)Carbohydrates
E)Ketones
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Page 16
Chapter 15: Biochemistry
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Sample Questions
Q1) Which of the following describes a lipid?
A)A group of molecules that contain both a carboxylic acid and amine functional group.
B)A relatively small, water-soluble molecule that contains either a ketone or an aldehyde functional group.
C)A group of small organic molecules that are insoluble in water.
D)And ester of phosphoric acid where one or more of the ionizable hydrogen atoms has been replaced by an R group.
E)A molecule that contains C, H, and N and exhibits Brønsted base behavior
Q2) The backbone of a strand of nucleic acid consists of
A)phosphate units only.
B)phosphate and sugar units.
C)polyester.
D)phosphate, sugar, and nitrogen base units.
E)sugar units only.
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Chapter 16: Nuclear Chemistry
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Sample Questions
Q1) Which of the following is used to image the liver?
A)(<sup>18</sup>O)
B)(<sup>131</sup>I)
C)(<sup>123</sup>I)
D)(<sup>24</sup>Na)
E)(<sup>99</sup>Tc)
Q2) What is the nuclear process called where small nuclei are combined into larger ones?
A)Photonuclear reactions
B)Nuclear fission
C)Thermal conductivity
D)Nuclear combination
E)Nuclear fusion
Q3) Which type of nuclear process requires an extremely high temperature (millions of degrees)?
A)Beta decay
B)Fission reaction
C)Fusion reaction
D)Alpha decay
E)Positron emission
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Chapter 17: Electrochemistry
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Sample Questions
Q1) Which is the correct cell notation for the following reaction? Au<sup>3</sup><sup>+</sup>(aq) + Al(s) Al<sup>3+</sup>(aq) + Au(s)
A)Al<sup>3</sup><sup>+</sup>(aq)|Al(s)||Au<sup>3+</sup>(aq)|Au(s) B)Al(s)|Al<sup>3+</sup>(aq)||Au<sup>3+</sup>(aq)|Au(s) C)Al<sup>3</sup><sup>+</sup>(aq)|Au<sup>3+</sup>(aq)||Al(s)|Au(s) D)Al<sup>3</sup><sup>+</sup>(aq)|Au(s)||Au<sup>3+</sup>(aq)|Al(s) E)Au(s)|Al(s)||Au<sup>3+</sup>(aq)|Al<sup>3+</sup>(aq)
Q2) A voltaic cell is prepared using copper and silver.Its cell notation is shown below.Cu(s) | Cu<sup>2</sup><sup>+</sup>(aq) || Ag<sup>+</sup>(aq) | Ag(s) Which reaction occurs at the cathode?
A)Cu(s) Cu<sup>2</sup><sup>+</sup>(aq) + 2e<sup> </sup> B)Cu<sup>2</sup><sup>+</sup>(aq) + 2e<sup> </sup> Cu(s)
C)Ag(s) Ag<sup>+</sup>(aq) + e<sup> </sup>
D)Ag<sup>+</sup>(aq) + e<sup> </sup> Ag(s) E)Cu(s) + 2Ag<sup>+</sup>(aq) Cu<sup>2+</sup>(aq) + 2Ag(s)
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