Introductory Chemistry Mock Exam - 3452 Verified Questions

Introductory Chemistry

Mock Exam

Course Introduction

Introductory Chemistry provides students with a foundational understanding of the principles and concepts central to the study of chemistry. Covering topics such as atomic structure, chemical bonding, stoichiometry, states of matter, the periodic table, and basic chemical reactions, this course equips learners with the essential knowledge needed to explore more advanced chemistry concepts. Emphasis is placed on developing problem-solving skills, safe laboratory practices, and the application of chemical principles to real-world scenarios. This course is tailored for students with minimal prior background in chemistry and serves as a prerequisite for higher-level chemistry courses.

Recommended Textbook Chemistry A Molecular Approach 4th Edition by Nivaldo J. Tro

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25 Chapters

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Chapter 1: Matter, measurement, and Problem Solving

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Sample Questions

Q1) What answer should be reported,with the correct number of significant figures,for the following calculation? (433.621 - 333.9)× 11.900

A) 1.19 × 10³

B) 1.187 × 10³

C) 1.1868 × 10³

D) 1.18680 × 10³

E) 1.186799 × 10³

Answer: A

Q2) A substance that can't be chemically broken down into simpler substances is

A) a homogeneous mixture.

B) an element.

C) a heterogeneous mixture.

D) a compound.

E) an electron.

Answer: B

Q3) Define an atom.

Answer: An atom is the submicroscopic particle that constitutes the fundamental building block of ordinary matter.

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3

Chapter 2: Atoms and Elements

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Sample Questions

Q1) Iodine belongs to the ________ group of the periodic table.

A) alkali metal

B) metal

C) halogen

D) noble gas

Answer: C

Q2) Which of the following elements is a liquid at room temperature?

A) radon

B) boron

C) mercury

D) lithium

E) calcium

Answer: C

Q3) Describe an atom and what it is made up of according to modern atomic theory.

Answer: An atom is made up of a nucleus surrounded by electrons.The nucleus contains protons (positively charged particles)and neutrons (neutral particles)and is where most of the mass of an atom comes from,but is a tiny fraction of an atom's volume.The nucleus is surrounded by negatively charged electrons,the same number as there are protons in the nucleus.An atom is therefore neutral overall.

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Chapter 3: Molecules,compounds,and Chemical Equations

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Sample Questions

Q1) What is the mass of a single iodine molecule,I₂?

A) 2.107 × 10^-²² g

B) 4.215 × 10^-²² g

C) 126.9 g

D) 253.8 g

Answer: B

Q2) Give the formula for potassium dichromate.

A) KCrO

B) K₂Cr₂O₇

C) K₂CrO₄

D) K₂Cr₂O₆

E) KCr₃O₇

Answer: B

Q3) Give the formula for calcium hydrogen sulfate.

A) CaHSO₃

B) Ca₂(HSO₃)₂

C) Ca₂HSO₂

D) Ca(HSO₄)₂

E) CaSO₃

Answer: D

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Chapter 4: Chemical Quantities and Aqueous Reactions

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Sample Questions

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

A) HBr(aq) + NaOH(aq) NaBr(aq) + H₂O(l)

B) NaI(aq) + AgNO₃(aq) AgI(s) + NaNO₃(aq)

C) Pb(C₂H₃O₂)₂(aq) + 2 LiBr(aq) PbBr₂(s) + 2 LiC₂H₃O₂(aq)

D) Ba(s) + 2 HCl(aq) BaCl₂(aq) + H₂(g)

E) All of the above are oxidation-reduction reactions.

Q2) Which of the following compounds is insoluble in water?

A) Hg₂Cl₂

B) Na₂SO₄

C) (NH₄)₂CO₃

D) BaS

E) All of these compounds are soluble in water.

Q3) Identify ammonia.

A) strong electrolyte, strong base

B) strong electrolyte, weak base

C) weak electrolyte, strong base

D) weak electrolyte, weak base

E) nonelectrolyte

Q4) Determine the oxidation state of Mn in KMnO₄.

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Chapter 5: Gases

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Sample Questions

Q1) Given the equation C₂H₆(g)+ O₂(g) CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 120.0 grams of C₂H₆ is burned in excess oxygen gas.

Q2) Which of the following gases has the highest average speed at 400K?

A) NO₂

B) O₂ 

C) F₂

D) Cl₂

Q3) In Lhasa,Tibet,the elevation is 12,000 feet.The altimeter reading in an airplane is 19.00 in Hg.This pressure is equal to ________ mm Hg.

A) 9.33

B) 483

C) 0.635

D) 1.57

E) 23.14

Q4) Define pressure.

Q5) Define effusion.

Q6) Why does the rate of effusion increase with a decrease in the molar mass?

Q7) Why does HOT air rise?

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Chapter 6: Thermochemistry

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Sample Questions

Q1) Explain the difference between H and DE.

Q2) Choose the thermochemical equation that illustrates H°_f for Li₂SO₄.

A) 2 Li⁺(aq) + SO₄^2-(aq) Li₂SO₄(aq)

B) 2 Li(s) + 1/8 S₈(s, rhombic) + 2 O₂(g)

Li₂SO₄(s)

C) Li₂SO₄(aq) 2 Li⁺(aq) + SO₄^2-(aq)

D) 8 Li₂SO₄(s) 16 Li(s) + S₈(s, rhombic) + 16 O₂(g)

E) 16 Li(s) + S₈(s, rhombic) + 16 O₂(g) 8 Li₂SO₄(s)

Q3) Identify a substance that is NOT in its standard state.

A) HCl

B) Li

C) N₂

D) F₂

E) Rn

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Page 8

Chapter 7: The Quantum-Mechanical Model of the Atom

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Sample Questions

Q1) When waves of equal amplitude from two sources are in phase when they interact,it is called

A) destructive interference.

B) diffraction.

C) constructive interference.

D) effusion.

E) amplitude.

Q2) Which of the following occurs as the wavelength of a photon increases?

A) The frequency decreases.

B) The energy increases.

C) The speed decreases.

D) Planck's constant increases.

E) None of the above occurs as the wavelength of a photon increases.

Q3) Food can be cooked by ________ radiation.

A) ultraviolet

B) gamma

C) microwave

D) x-ray

E) radio

Q4) Give an example of a p orbital.

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Chapter 8: Periodic Properties of the Elements

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Sample Questions

Q1) How many unpaired electrons are present in the ground state Xe atom?

A) 2

B) 3

C) 0

D) 5

E) 8

Q2) A cation of +2 indicates that an element has

A) lost two electrons.

B) lost two protons.

C) lost two neutrons.

D) gained two electrons.

E) gained two protons.

Q3) Identify the s-block element.

A) Cm

B) Ta

C) Na

D) F

E) None of the above

Q4) Give the number of valence electrons for Mg²⁺.

Q5) Define paramagnetic.

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Chapter 9: Chemical Bonding I: Lewis Theory

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Sample Questions

Q1) Place the following in order of decreasing magnitude of lattice energy. K₂O Rb₂S Li₂O

A) Li₂O > K₂O > Rb₂S

B) Li₂O > Rb₂S > K₂O

C) Rb₂S > K₂O > Li₂O

D) Rb₂S > Li₂O > K₂O

E) K₂O > Li₂O > Rb₂S

Q2) Using periodic trends,place the following bonds in order of decreasing ionic character. Sb-I P-I As-I

A) Sb-I > As-I > P-I

B) As-I > Sb-I > P-I

C) Sb-I > P-I > As-I

D) P-I > As-I > Sb-I

E) (Sb-I > P-I > As-I)

Q3) How are electron affinity and electronegativity different?

Q4) Which compound has the longest carbon-carbon bond length?

A) CH₃CH₃

B) CH₂CH₂

C) HCCH

D) All bond lengths are the same.

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Chapter 10: Chemical Bonding Ii: Molecular Shapes,valence

Bond Theory,

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Sample Questions

Q1) Determine the molecular geometry about each interior atom in the following structure.Sketch the three-dimensional structure and label the interior atoms with the corresponding molecular geometry.

CH₂CHCCCH₃

Q2) Using the VSEPR model,the electron-domain geometry of the central atom in NH₄⁺ is

A) linear.

B) trigonal planar.

C) tetrahedral.

D) trigonal bipyramidal.

E) octahedral.

Q3) Determine the hybridization about each interior atom in the following structure.Sketch the three-dimensional structure and label the interior atoms with their corresponding hybridization.

CH₂CHCCCH₃

Q4) According to molecular orbital theory,what is an antibonding orbital?

Q5) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Q6) Explain why oil and water do not mix.

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Chapter 11: Liquids,solids,and Intermolecular Forces

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Sample Questions

Q1) Identify the compound that has hydrogen bonding.

A) (CH₃)₃N

B) Cl₂

C) CH₃CH₃

D) HI

E) H₂O

Q2) Which of the following statements is TRUE?

A) Intermolecular forces are generally stronger than bonding forces.

B) The potential energy of molecules decreases as they get closer to one another.

C) Energy is given off when the attraction between two molecules is broken.

D) Increasing the pressure on a solid usually causes it to become a liquid.

E) None of the above is true.

Q3) Identify the compound with the highest dipole moment.

A) CH₃OCH₃

B) CH₃CH₂CH₃

C) CH₃CHO

D) (CH₃)₂O

E) CH₃CN

Q4) Define dynamic equilibrium.

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Give the coordination number for a face-centered cubic cell.

A) 2

B) 8

C) 12

D) 10

E) 6

Q2) When two waves interact with their crests and troughs in alignment is called

A) complimentary interference.

B) destructive interference.

C) opposing interference.

D) constructive interference.

E) alignment interference.

Q3) Which of the following is considered an atomic solid?

A) F₂

B) CsBr

C) N₂

D) Nb

E) None of these is an atomic solid.

Q4) Give the edge length in terms of r for a simple cubic cell.

Q5) Describe the difference between the conduction band and the valence band.

Page 14

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Chapter 13: Solutions

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Sample Questions

Q1) Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in 15.0 mL of water at 25°C.

Q2) An aqueous solution is 0.467 M in HCl.What is the molality of the solution if the density is 1.23 g/mL?

A) 0.115 m

B) 0.275 m

C) 0.374 m

D) 0.525 m

E) 0.318 m

Q3) A solution is prepared by dissolving 76.3 g NaI in 545 g of water.Determine the mole fraction of NaI if the final volume of the solution is 576 mL.

A) 6.04 × 10^-3

B) 1.65 × 10^-2

C) 1.40 × 10^-³

D) 1.32 × 10^-2

E) 8.84 × 10^-2

Q4) Define colloid.

Q5) Define osmosis.

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Chapter 14: Chemical Kinetics

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Sample Questions

Q1) What are the units of k in the following rate law? Rate = k[X]²

A) Ms^-2

B) Ms

C) M^-1s^-1

D) M^-2s^-2

E) M²s^-1

Q2) For a reaction,what generally happens if the temperature is increased?

A) A decrease in k occurs, which results in a faster rate.

B) A decrease in k occurs, which results in a slower rate.

C) An increase in k occurs, which results in a faster rate.

D) An increase in k occurs, which results in a slower rate.

E) There is no change with k or the rate.

Q3) Explain how the order of a reaction can be determined.

Q4) For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

A) decrease by a factor of 1/25.0.

B) decrease by a factor of 1/5.00.

C) increase by a factor of 5.00.

D) increase by a factor of 25.0.

Page 16

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) The reaction below has a K_c value of 1.0 × 10¹².What is the value of K_p for this reaction at 200 K? 2 SO₂(g)+ O₂(g) 2 SO₃(g)

A) 6.1 × 10^-14

B) 1.0 × 10¹²

C) 1.6 × 10^-11

D) 1.6 × 10¹³

E) 6.1 × 10¹⁰

Q2) In a reaction mixture containing only products,what is the value of Q?

A) -1

B) 1

C)

D) 0

E) It cannot be determined without concentrations.

Q3) Why aren't solids or liquids included in an equilibrium expression?

Q4) Explain dynamic equilibrium.Use the generic reaction A(g) B(g)to explain.

Q5) Can the K_p and K_c for a reaction ever have the same value? Why or why not?

Q6) Define Le Chatelier's Principle.

Q7) Why is an equilibrium constant unitless?

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Chapter 16: Acids and Bases

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Sample Questions

Q1) Determine the pH of a 0.232 M Mg(OH)₂ solution at 25°C.

A) 12.73

B) 13.37

C) 13.67

D) 0.333

E) 0.634

Q2) What is the pH of a 0.40 M H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

A) 2.14

B) 3.89

C) 4.28

D) 5.57

Q3) Identify the food that does NOT irritate the wall of the stomach.

A) orange juice

B) plum

C) egg white

D) lemon

E) wine

Q4) What is the difference between a strong and weak acid?

Page 18

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Chapter 17: Aqueous Ionic Equilibrium

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Sample Questions

Q1) Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

A) 1.83 × 10^-2 M

B) 1.23 × 10^-5 M

C) 2.90 × 10^-2 M

D) 4.95 × 10^-3 M

E) 6.13 × 10^-6 M

Q2) What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl to reach the equivalence point? K_a = 3.0 × 10^-8 for HOCl.

A) 0.30

B) 3.18

C) 3.76

D) 4.03

Q3) Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

Q4) Identify the compound that is in stalactites and stalagmites.

Q5) Explain the common ion effect with respect to molar solubility.

Q6) Define a buffer.

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Chapter 18: Free Energy and Thermodynamics

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Sample Questions

Q1) Consider the following reaction at constant P.Use the information here to determine the value of S_surrat 298 K.Predict whether or not this reaction will be spontaneous at this temperature. N₂(g)+ 2 O₂(g) 2 NO₂(g) H = +66.4 kJ

A) S_surr = +223 J/K, reaction is spontaneous

B) S_surr = -223 J/K, reaction is not spontaneous

C) S_surr = -66.4 J/K, reaction is not spontaneous

D) S_surr = +2656 kJ/K, reaction is not spontaneous

E) S_surr = -66.4 J/K, it is not possible to predict the spontaneity of this reaction without more information.

Q2) For a given reaction, H = +35.5 kJ/mol and S = +83.6 J/Kmol.The reaction is spontaneous ________.Assume that H and S do not vary with temperature.

A) at T < 425 K

B) at T > 425 K

C) at all temperatures

D) at T > 298 K

E) at T < 298 K

Q3) Define entropy.

Q4) How is a nonspontaneous process made spontaneous?

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Chapter 19: Electrochemistry

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Sample Questions

Q1) Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Crand Cl₂ in the balanced reaction? Cr(s)+ Cl₂(g) Cr³⁺(aq)+ Cl^-(aq)

A) Cr = 2, Cl₂ = 3

B) Cr = 2, Cl₂ = 4

C) Cr = 1, Cl₂ = 2

D) Cr = 2, Cl₂ = 1

E) Cr = 3, Cl₂ = 2

Q2) Using the following standard reduction potentials, Fe³⁺(aq)+ e Fe²⁺(aq)E° = +0.77 V

Ni²⁺(aq)+ 2 e^- Ni(s)E° = -0.23 V

Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions. Ni²⁺(aq)+ 2 Fe²⁺(aq) 2 Fe³⁺(aq)+ Ni(s)

A) E° = -1.00 V, nonspontaneous

B) E° = -1.00 V, spontaneous

C) E° = +1.00 V, nonspontaneous

D) E° = +1.00 V, spontaneous

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Chapter 20: Radioactivity and Nuclear Chemistry

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Sample Questions

Q1) Define chain reaction in terms of the fission of uranium nucleus.

Q2) Define radioactivity.

Q3) Calculate the mass defect in Fe-56 if the mass of an Fe-56 nucleus is 55.921 amu.The mass of a proton is 1.00728 amu and the mass of a neutron is 1.008665 amu.

A) 0.528 amu

B) 3.507 amu

C) 0.564 amu

D) 1.056 amu

E) 0.079 amu

Q4) Identify the elements used in radiometric dating.

A) carbon-14 to nitrogen-14

B) uranium-238 to lead-206

C) potassium-40 to argon-40

D) all of the above

E) none of the above

Q5) How does a dosimeter measure exposure to radioactivity?

Q6) Why is an alpha emitter much more harmful if is ingested than when applied to the skin?

Q7) Explain the concept of "magic numbers."

Page 22

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Chapter 21: Organic Chemistry

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Sample Questions

Q1) Which part of HCN,the hydrogen or the cyano group,adds to the O in a C=O bond and why?

Q2) Which of the following compounds is an alcohol?

A) CH₃CH₂CH₂CO₂H

B) CH₃OSH₃

C) CH₃CO₂CH₂CH₃

D) CH₃CH₂I

E) CH₃CH₂OH

Q3) Why are there so many more carbon compounds than the number of compounds made up of all the rest of the elements combined?

Q4) Molecules with the same formula in which the atoms have a different connectivity are called

A) structural isomers.

B) achiral.

C) diastereomers.

D) enantiomers.

E) racemic mixture.

Q5) What does the term "racemic mixture" mean?

Q6) Why doesn't benzene typically undergo addition reactions like the alkenes do?

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Chapter 22: Biochemistry

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Sample Questions

Q1) Which of the following bond monosaccharide units together into polysaccharides?

A) ester bonds

B) glycosidic linkages

C) disulfide linkages

D) amine bonds

E) ketone linkages

Q2) Identify a base that is NOT in RNA.

A) adenine

B) cytosine

C) thymine

D) guanine

E) uracil

Q3) The following is part of a DNA sequence.What is its complementary sequence? AGTTCGAGCCT

A) AGTTCGAGCCT

B) TCCGAGCTTGA

C) CAGTCCA

D) AGGCTCGAACT

E) TCAAGCTCGGA

Q4) Why are lipids well-suited as structural components of cell membranes?

Page 24

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Chapter 23: Chemistry of the Nonmetals

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Sample Questions

Q1) Determine the oxidation state of nitrogen in LiNO₂.

A) +1

B) -2

C) +5

D) 0

E) +3

Q2) Why are the chemical properties of nitrogen and phosphorus so different when they are in the same family?

Q3) Identify a characteristic of chlorine dioxide.

A) bleaches wood

B) powerful oxidizing agent

C) explosive

D) bleaches flour

E) all of the above

Q4) What is the oxidation number of oxygen in H₂O₂?

A) -4

B) +2

C) -3

D) -1

E) +1

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Chapter 24: Metals and Metallurgy

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Sample Questions

Q1) Identify the element with the highest thermal conductivity.

A) copper

B) vanadium

C) silver

D) iron

Q2) Which of the following describes slag?

A) a waste material that is the product of smelting a metal ore

B) an aqueous portion of the gangue separated from a metal ore

C) a low density waste product, formed from the reaction of gangue with another substance, that can be easily separated from the metal ore of interest

D) a substance that reacts with the gangue to make a low density liquid compound that can be easily separated from the metal of interest

E) None of the above describes slag.

Q3) Identify the normal crystal structure at room temperature for Cr.

A) body-centered cubic

B) trigonal pyramidal

C) octahedral

D) hexagonal

E) hexagonal closest packed

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Chapter 25: Transition Metals and Coordination Compounds

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Sample Questions

Q1) Determine the chemical formula for the compound,potassiumtrisethylenediamine chromate(III).

A)

K₃[Cr(NH₂CH₂CH₂NH₂)< sub>3</sub>]

B)

[K(NH₂CH₂CH₂NH₂)₃]Cr< sup>3+</sup>

C)

[KCr(NH₂CH₂CH₂NH₂)₃]< sup>3+</sup>

D)

K₂[Cr(NH₂CH₂CH₂NH₂)< sub>4</sub>]

E)

[Cr(NH₂CH₂CH₂NH₂)₂]K< sub>2</sub>

Q2) What type of hybridization (according to valence bond theory)does Fe exhibit in the complex ion,[Fe(H₂O)₄(Br)₂]⁺?

A) dsp³

B) sp3

C) d²sp²

D) d²sp³

E) d²sp

Page 27

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