Introductory Chemistry Final
Exam
Course Introduction
Introductory Chemistry provides a foundational understanding of the principles and concepts of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, solutions, and basic thermochemistry. This course emphasizes the development of problem-solving skills through laboratory experiments, real-world applications, and conceptual discussions. Designed for students with limited background in chemistry, it prepares them for more advanced courses by covering both theoretical and practical aspects essential for further study in chemistry and related fields.
Recommended Textbook
Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder
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Page 2
Chapter 1: Basic Concepts of Chemistry
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Q1) Which one of the following statements is not a comparison of physical properties?
A) Mercury and gallium are both liquids at 50\(^{\circ}\)C.
B) Oxygen is more soluble in water than helium.
C) Silver and gold are malleable metals.
D) Oxygen and nitrogen are both liquids at -200\(^{\circ}\)C.
E) Calcium dissolves more quickly than iron in acids.
Answer: E
Q2) Which of the following statements concerning the kinetic-molecular theory of matter is/are CORRECT?
1)Particles in a gas move faster as the temperature increases.
2)Particles in a liquid are packed closely together,but are not confined to specific positions.
3)Particles in a gas vibrate back and forth about an average position.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
Answer: D
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Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry
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Q1) How many joules are equivalent to 450 calories?
A) 0.45 J
B) 4.5 \(\times\) 10<sup>2</sup> J
C) 9.3\(\times\) 10<sup>-3</sup> J
D) 1.9 \(\times\) 10<sup>3</sup> J
E) 4.5 \(\times\) 10<sup>5</sup> J
Answer: D
Q2) The SI base unit of length is the ____.
A) Newton
B) liter
C) meter
D) cm<sup>3</sup>
E) Ångstrom
Answer: C
Q3) Assuming the density of water is 1.00 g/cm<sup>3</sup>,the mass of 1.0 cubic meter (m<sup>3</sup>) of water is ________ grams.
Answer: 1.0 \(\times\) 10<sup>6</sup>
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Page 4
Chapter 3: Atoms, molecules, and Ions
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Q1) What is the mass number of an argon atom with 22 neutrons?
A) 2
B) 18
C) 22
D) 40
E) 39.95
Answer: D
Q2) Which of the following elements is not a metalloid?
A) boron
B) selenium
C) germanium
D) arsenic
E) silicon
Answer: B
Q3) Pure oxygen can exist as O<sub>2</sub> or O<sub>3</sub>.Elements that exist in more than one distinct form are called ________.
Answer: allotropes
Q4) Elements that have the same number of protons,but differ in their number of neutrons are called ________.
Answer: isotopes
Page 5
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Chapter 4: Chemical Reactions
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Q1) Which of the following statements is/are CORRECT?
1)A solution is a homogeneous mixture of two or more substances.
2)A solute is a mixture of a solvent and a soluble compound.
3)Aqueous solutions are solutions in which water is a solvent.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1 and 3
Q2) Write a balanced chemical equation for the reaction of aqueous solutions of sodium sulfide and zinc(II)chloride.
A) Na<sub>2</sub>S(aq)+ ZnCl<sub>2</sub>(aq)\(\to\) ZnS(s)+ 2 NaCl(aq)
B) Na<sub>2</sub>S(aq)+ ZnCl<sub>2</sub>(aq)\(\to\) ZnS(s)+ 2 NaCl(s)
C) Na<sub>2</sub>S(aq)+ ZnCl<sub>2</sub>(aq)\(\to\) Na<sub>2</sub>Zn(s)+ SCl<sub>2</sub>(aq)
D) Na<sub>2</sub>S(aq)+ ZnCl<sub>2</sub>(aq)\(\to\) Na<sub>2</sub>Zn(aq)+ SCl<sub>2</sub>(g)
E) No reaction occurs.
Q3) A(n)________ agent gains electrons in an oxidation-reduction reaction.
Q4) _____-oxides produce acids when reacted with water.
Page 6
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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions
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Q1) What volume of 2.52 M HCl is required to prepare 176.5 mL of 0.449 M HCl?
A) 9.91 \(\times\) 10<sup>2</sup> mL
B) 1.56 \(\times\) 10<sup>2</sup> mL
C) 31.4 mL
D) 0.0318 mL
E) 2.00 \(\times\) 10<sup>2</sup> mL
Q2) An impure sample of benzoic acid (C<sub>6</sub>H<sub>5</sub>COOH,122.12 g/mol)is titrated with 0.8067 M NaOH.A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint.What is the percent by mass of benzoic acid in the sample?
C<sub>6</sub>H<sub>5</sub>COOH(aq)+
NaOH(aq)\(\to\)NaC<sub>6</sub>H<sub>5</sub>COO(aq)+ H<sub>2</sub>O(l)
A) 0.02442 %
B) 2.982 %
C) 100.0 %
D) 24.42 %
E) 71.29 %
Q3) The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.
Page 7
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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions
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Q1) In thermodynamics,a(n)________ is defined as the object,or collection of objects,being studied.The surroundings include everything else.
Q2) At constant pressure and 25S1U1P1\(\circ\)S1S1P0C,what is \(\Delta\)<sub>r</sub>HS1U1P1\(\circ\)S1S1P0 for the following reaction
2C<sub>2</sub>H<sub>6</sub>(g)+ 7O<sub>2</sub>(g)\(\to\) 4CO<sub>2</sub>(g)+ H<sub>2</sub>O(l)
If the complete consumption of 89.4 g of C<sub>2</sub>H<sub>6</sub> liberates -4638
kJ of heat energy?
A) -3120 kJ/mol-rxn
B) -1560 kJ/mol-rxn
C) -27600 kJ/mol-rxn
D) -13800 kJ/mol-rxn
E) -787 kJ/mol-rxn
Q3) The energy stored in a fuel is called _____.
A) heat
B) internal energy
C) temperature
D) kinetic energy
E) potential energy
Page 8
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Chapter 7: The Structure of Atoms
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Q1) For which of the following transitions would a hydrogen atom emit the lowest energy photon?
A) n = 4 to n = 5
B) n = 5 to n = 2
C) n = 4 to n = 3
D) n = 3 to n = 1
E) n = 3 to n = 2
Q2) If a hydrogen atom in the excited n = 4 state relaxes to the ground state,what is the maximum number of possible emission lines?
A) 1
B) 3
C) 6
D) 8
E) infinite
Q3) What is the total number of orbitals found in the n = 4 shell?
A) 16
B) 4
C) 20
D) 24
E) 15
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Chapter 8: The Structure of Atoms and Periodic Trends
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Q1) Which 1+ ion has the ground state electron configuration [Kr]4d<sup>10</sup>?
A) Ru
B) Au
C) Ag
D) In
E) Cd
Q2) According to the general trend in electron affinities,which group (or family)of elements tend to form the most stable anions in the gas phase?
A) noble gases
B) halogens
C) transition metals
D) alkaline earth metals
E) alkali metals
Q3) How many electrons can be described by the quantum numbers n= 3 and l= 1?
A) 10
B) 2
C) 14
D) 18
E) 6
Q4) The f-block elements are also referred to as the ________ and actinides.
Page 10
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Chapter 9: Bonding and Molecular Structure
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Q1) Which of the following molecules or ions are likely to be free radicals: N<sub>2</sub>O,NO,and NO<sub>2</sub>?
A) N<sub>2</sub>O only
B) NO only
C) NO<sub>2</sub> only
D) N<sub>2</sub>O and NO
E) NO and NO<sub>2</sub>
Q2) What is the molecular geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and four single bonds.
A) tetrahedral
B) linear
C) bent
D) trigonal pyramidal
E) trigonal planar
Q3) In benzene,C<sub>6</sub>H<sub>6</sub>,the six carbon atoms are arranged in a ring.Two equivalent Lewis structures can be drawn for benzene.In both structures,the carbon atoms have a trigonal planar geometry.These two equivalent structures are referred to as ________ structures.
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Chapter 10: Bonding and Molecular Structure: Orbital
Hybridization and Molecular Orbitals
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Q1) What is the maximum number of hybridized orbitals that can be formed by a fluorine atom?
A) 1
B) 2
C) 3
D) 4
E) 6
Q2) In valence bond theory,each sigma bond in CH<sub>4</sub> is formed from the overlap of a hydrogen atom's 1s orbital with a(n)________ hybridized orbital on the carbon atom.
Q3) What is the molecular geometry around a central atom that is sp<sup>2</sup> hybridized,has three sigma bonds,and one pi bond?
A) trigonal-planar
B) trigonal-pyramidal
C) bent
D) T-shaped
E) tetrahedral
Q4) In molecular orbital theory,the bond order is defined as 1/2 \(\times\) (the number of electrons in ________ orbitals minus the number of electrons in antibonding orbitals).
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Chapter 11: Gases and Their Properties
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Q1) What volume of oxygen will react with 21 mL of ethanol,assuming the gases are present at the same temperature and pressure?
2 CH<sub>3</sub>CH<sub>2</sub>OH(g)+ 6 O<sub>2</sub>(g)\(\to\) 4 CO<sub>2</sub>(g)+ 6 H<sub>2</sub>O(g)
A) 7.0 mL
B) 14 mL
C) 21 mL
D) 42 mL
E) 63 mL
Q2) When 0.5000 grams of an unknown hydrocarbon,C<sub>x</sub>H<sub>y</sub>,is completely combusted with excess oxygen,1.037 L CO<sub>2</sub> gas and is produced at 98.3 S1U1P1\(\circ\)S1S1P0C and 1.000 atm.What is the empirical formula of the hydrocarbon? (R = 0.08206 L.atm/mol.K)
A) CH
B) CH<sub>2</sub>
C) C<sub>2</sub>H<sub>3</sub>
D) C<sub>3</sub>H<sub>5</sub>
E) C<sub>3</sub>H<sub>8</sub>
Q3) What are two ways in which real gases differ from ideal gases?
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Chapter 12: Intermolecular Forces and Liquids
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Q1) Which of the following liquids has the\(\underline{\text{ lowest }}\) enthalpy of vaporization?
A) C<sub>2</sub>H<sub>6</sub>
B) C<sub>3</sub>H<sub>8</sub>
C) C<sub>4</sub>H<sub>10</sub>
D) C<sub>5</sub>H<sub>12</sub>
E) C<sub>6</sub>H<sub>14</sub>
Q2) Arrange Cl<sub>2</sub>,ICl,and Br<sub>2</sub> in order from lowest to highest boiling point.
A) Cl<sub>2</sub> < Br<sub>2</sub> < ICl
B) Cl<sub>2</sub> < ICl < Br<sub>2</sub>
C) ICl < Cl<sub>2</sub> < Br<sub>2</sub>
D) Br<sub>2</sub> < Cl<sub>2</sub> < ICl
E) Br<sub>2</sub> < ICl < Cl<sub>2</sub>
Q3) What is responsible for capillary action,a property of liquids?
A) cohesive forces
B) adhesive forces
C) viscosity
D) A and B
E) A,B,and C
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Chapter 13: The Chemistry of Solids
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Q1) Which of the following compounds is expected to have the strongest ionic bonds?
A) RbI
B) KCl
C) NaBr
D) CsF
E) LiF
Q2) Silver chloride crystallizes with the sodium chloride (rock salt)structure.The length of a unit cell edge is 555 pm.What is the density of AgCl?
A) 5.57 g/cm<sup>3</sup>
B) 4.19 g/cm<sup>3</sup>
C) 2.79 g/cm<sup>3</sup>
D) 2.10 g/cm<sup>3</sup>
E) 1.39 g/cm<sup>3</sup>
Q3) Which of the following ionic compounds is expected to have the lowest enthalpy of fusion?
A) RbF
B) RbCl
C) RbBr
D) RbI
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Chapter 14: Solutions and Their Behavior
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Q1) Which of the following statements concerning solubility is/are CORRECT?
1)Ionic compounds composed of Group 1A metal ions and halide ions,such as NaCl,are insoluble in nonpolar solvents.
2)The solubility of the halogens (Cl<sub>2</sub>,Br<sub>2</sub>,and I<sub>2</sub>)in polar solvents is greater than their solubility in nonpolar solvents.
3)The solubility of polar molecules,such as sugar,in polar solvents is generally greater than their solubility in nonpolar solvents.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3
Q2) What type of colloid is formed when a solid is dispersed in a liquid?
A) foam
B) aerosol
C) sol
D) emulsion
E) gel
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Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions
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Q1) A second-order reaction starts with an initial concentration of 0.100 mol/L of the reactant.If the rate constant is 1.4 \(\times\) 10<sup>-2</sup> L/mol·s,what is the time required to decrease the initial concentration to 0.050 mol/L?
2A \(\to\) B \(~~~~~~~~\)rate = k[A]<sup>2</sup>
A) 710 s
B) 1100 s
C) 49.5 s
D) 3.57 s
E) 2100 s
Q2) In general,as temperature increases,the rate of a chemical reaction
A) decreases due to fewer collisions with proper molecular orientation.
B) increases for exothermic reactions,but decreases for endothermic reactions. C) increases due to a greater number of effective collisions. D) remains unchanged.
E) decreases due to an increase in the activation energy.
Q3) Termolecular elementary steps are rare.Why?
Q4) The pre-exponential,A,in the Arrhenius equation is called the ________ factor.
Q5) Draw the reaction coordinate diagram for an exothermic reaction involving three mechanistic steps.
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Chapter 16: Principles of Reactivity: Chemical Equilibria
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Q1) If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.
Q2) Which of the following statements is/are CORRECT?
1)For a chemical system,if the reaction quotient (Q)is greater than K,reactant must be converted to products to reach equilibrium.
2)For a chemical system at equilibrium,the forward and reverse rates of reaction are equal.
3)For a chemical system at equilibrium,the concentrations of products divided by the concentrations of reactants equals one.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
Q3) The symbol Q is called the ________.
Q4) In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.
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18
Chapter 17: The Chemistry of Acids and Bases
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Q1) What is the pH of a 0.11 M solution of methylamine (CH<sub>3</sub>NH<sub>2</sub>,K<sub>b</sub> = 4.4 \(\times\) 10<sup>-4</sup>)at 25<sup>o</sup>C? (K<sub>w</sub> = 1.01 \(\times\) 10<sup>-14</sup>)
A) 5.80
B) 0.96
C) 11.83
D) 13.04
E) 2.17
Q2) What is the equilibrium pH of a 0.835 M solution of H<sub>3</sub>PO<sub>4</sub>(aq)? (K<sub>a1</sub> = 7.5 \(\times\) 10<sup>-3</sup>,K<sub>a2</sub> = 6.2 \(\times\) 10<sup>-8</sup>,K<sub>a3</sub> = 4.8 \(\times\) 10<sup>-13</sup>)
A) 1.12
B) 3.64
C) 12.32
D) 6.20
E) 7.21
Q3) Which is the stronger Brønsted-Lowry acid,Fe(H<sub>2</sub>O)<sub>6</sub><sup>2+</sup> or Fe(H<sub>2</sub>O)<sub>6</sub><sup>3+</sup>? Explain.
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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria
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Q1) A 25.00-mL sample of propionic acid,HC<sub>3</sub>H<sub>5</sub>O<sub>2</sub>,of unknown concentration was titrated with 0.143 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What was the original concentration of the propionic acid?
A) 0.295 M
B) 0.125 M
C) 0.082 M
D) 0.143 M
E) 0.250 M
Q2) What is the pH of the buffer that results when 12.0 g of NaH<sub>2</sub>PO<sub>4</sub> and 8.00 g of Na<sub>2</sub>HPO<sub>4</sub> are diluted with water to a volume of 0.50 L? (K<sub>a</sub> of H<sub>2</sub>PO<sub>4</sub><sup>-</sup> = 6.2 \(\times\) 10<sup>-8</sup>,the molar masses of NaH<sub>2</sub>PO<sub>4</sub> and Na<sub>2</sub>HPO<sub>4</sub> are 120.0 g/mol and 142.0 mol,respectively)
A) 4.10
B) 6.96
C) 7.21
D) 7.46
E) 9.90
Page 20
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Chapter 19: Entropy and Free Energy
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Q1) The change in entropy for any process is not dependent upon the pathway by which the process occurs.In other words,the change in entropy for any process is a(n)________ function.
Q2) Which of the following changes lead to a \(\underline{\text{ decrease }}\) in entropy?
A) the sublimation (vaporization)of dry ice (solid carbon dioxide)
B) sugar dissolving in coffee
C) evaporation of water from a lake
D) diffusion of perfume throughout a room
E) halving the volume of a gas
Q3) When a chemical process occurs under standard conditions,which of the following conditions always apply?
1)Gaseous species are at a pressure of 1 bar.
2)Solution concentrations species are 1 molal.
3)The temperature is 298.15 K.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
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Chapter 20: Principles of Reactivity: Electron Transfer Reactions
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Q1) What is the correct cell notation for a voltaic cell based on the reaction below? Cu<sup>2+</sup>(aq)+ Fe(s)\(\to\) Cu(s)+ Fe<sup>2+</sup>(aq)
A) Cu(s)| Cu<sup>2+</sup>(aq)|| Fe<sup>2+</sup>(aq)| Fe(s)
B) Fe(s)|| Fe<sup>2+</sup>(aq),Cu<sup>2+</sup>(aq)| Cu(s)
C) Cu(s)|| Cu<sup>2+</sup>(aq),Fe<sup>2+</sup>(aq)|| Fe(s)
D) Cu(s)| Fe<sup>2+</sup>(aq)|| Cu<sup>2+</sup>(aq)| Fe(s)
E) Fe(s)| Fe<sup>2+</sup>(aq)|| Cu<sup>2+</sup>(aq)| Cu(s)
Q2) Which of the following statements concerning a voltaic cell is/are correct?
1)Reduction occurs at the cathode.
2)A spontaneous reaction generates an electric current in a voltaic cell.
3)Without a salt bridge charge buildup will cause the cell reaction to stop.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3
Q3) Gold and platinum are commonly used as inert electrodes in laboratory experiments.In commercial applications,such as batteries,________ is more commonly used for inert electrodes because it is far less expensive.
Page 22
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Chapter 21: Environmental Chemistry Earths
Environment,energy,and Sustainability
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Q1) The majority of electricity generated in the United States is produced from ___.
A) wind and solar
B) moving water
C) nuclear fission
D) natural gas
E) coal
Q2) Which of the following water disinfectants persist in water pipes even after the initial disinfection process?
A) Cl<sub>2</sub>
B) NaOCl
C) O<sub>3</sub>
D) A and B
E) A,B,and C
Q3) Which ion occurs in the highest concentration in seawater?
A) Cl<sup>-</sup>
B) Na<sup>+</sup>
C) HCO<sub>3</sub><sup>-</sup>CO<sub>3</sub><sup>2-</sup>
D) Mg<sup>2+</sup>
E) Ca<sup>2+</sup>
Q4) Explain why the melting of Arctic sea ice will not raise the sea level.
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Chapter 22: The Chemistry of the Main Group Elements
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Q1) What is the molecular formula of chlorous acid?
A) HClO
B) HClO<sub>2</sub>
C) HClO<sub>3</sub>
D) HClO<sub>4</sub>
E) HCl
Q2) Which of the following statements is INCORRECT?
A) Quartz is a form of silicon dioxide that is used for controlling the frequency of radio and television transmissions.
B) Silica gel,a noncrystalline for of SiO<sub>2</sub>,is used to keep electronics dry.
C) Passing beer through a bed of silica gel removes small particles that cause cloudiness.
D) Gaseous SiO<sub>2</sub> is a linear molecule with silicon-oxygen double bonds and a boiling point slight below 0 S1U1P1\(\circ\)S1S1P0C.
E) Silicon dioxide is resistant to attack from all acids except HF.
Q3) Silicon is purified in a process called ________,where a narrow segment of a silicon rod is melted and allowed to slowly recrystallize.
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Chapter 23: The Chemistry of the Transition Elements
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Q1) The complex ion [NiCl<sub>4</sub>]<sup>2-</sup> is paramagnetic,but the complex ion [Ni(NH<sub>3</sub>)<sub>4</sub>]<sup>2+</sup> is diamagnetic.Why do the magnetic properties of these two nickel complexes differ?
Q2) Determine the number of unpaired electrons in an octahedral,high-spin Cr(II)complex.
A) 1
B) 2
C) 3
D) 4
E) 5
Q3) All of the following metals are generally found in nature as either oxides or sulfides,EXCEPT ____.
A) Fe
B) Au
C) Ni
D) Cr
E) Hg
Q4) One method of recovering metals from their ores involves aqueous solutions; a second method involves heat.The method involving heat is called ________.
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Chapter 24: Carbon: Not Just Another Element
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Q1) Which of the following compounds might be used to oxidize an aldehyde to a carboxylic acid?
A) H<sub>2</sub>
B) Na
C) LiAlH<sub>4</sub>
D) KMnO<sub>4</sub>
E) NaBH<sub>4</sub>
Q2) Which of the following statements concerning methanol is/are CORRECT?
1)Methanol is used as a fuel in high-powered racing cars.
2)Human consumption of methanol can lead to blindness.
3)Methanol is converted by the human body to formaldehyde and formic acid.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3
Q3) The molecule 2-chloro-4-methylhexane is made by addition of HCl to an alkene.Write a balanced chemical equation for this reaction.
Q4) The process by which long chain hydrocarbons in petroleum are shortened is called
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Chapter 25: Biochemistry
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Sample Questions
Q1) The sequence of the amino acids in a protein is termed the ____ structure.
A) isomeric
B) primary
C) secondary
D) tertiary
E) quaternary
Q2) The oxygen that bridges two sugars in a disaccharide is known as a ___ bond.
Q3) The glycosidic bonds that form the link between sugars in disaccharides are formed by
A) an alkylation reaction.
B) a condensation reaction.
C) a hydrolysis reaction.
D) an addition reaction.
E) a substitution reaction.
Q4) Which of the following is \(\underline{\text{ not }}\) a component of RNA?
A) cytosine
B) phosphodiester groups
C) (\(\beta\))-D-ribose
D) guanine
E) thymine
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Chapter 26: Nuclear Chemistry
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Sample Questions
Q1) If a nucleus undergoes positron particle emission
A) its atomic number decreases by four and its mass number decreases by two.
B) its atomic number decreases by two and its mass number decreases by four.
C) its atomic number increases by one and its mass number is unchanged.
D) its atomic number decreases by one and its mass number is unchanged.
E) its atomic number is unchanged and its mass number decreases by one.
Q2) The rate constant for the decay of a radioactive isotope is 4.231 \(\times\)
10<sup>-3 </sup>/ day.What is the half-life of this isotope?
A) 327.6 days
B) 409.5 days
C) 81.90 days
D) 163.8 days
E) none of these
Q3) When a nucleus undergoes radioactive decay,its new mass number is
A) always less than its original mass number.
B) never more than its original mass number.
C) never less than its original mass number.
D) always the same as its original mass number.
E) always more than its original mass number.
Q4) A unit used to quantify biological damage is called the ________ or rem.
Page 28
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