Chemical Science Chapter Exam Questions - 4331 Verified Questions

Chemical Science

Chapter Exam Questions

Course Introduction

Chemical Science is a multidisciplinary field that explores the composition, structure, properties, and changes of matter at the molecular and atomic levels. The course provides foundational knowledge in general, organic, inorganic, physical, and analytical chemistry, examining both theoretical concepts and practical laboratory techniques. Through the study of chemical reactions, bonding, energetics, and kinetics, students learn how chemical principles underpin a wide range of phenomena in natural and industrial processes. Emphasis is placed on scientific inquiry, problem-solving, and the real-world applications of chemistry in fields such as pharmaceuticals, materials science, environmental science, and biotechnology.

Recommended Textbook Chemistry 6th Edition by John E. McMurry

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Chapter 1: Chemistry: Matter and Measurement

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Sample Questions

Q1) Convert 1 m to meters.

A)1 × 10^-9 m

B)1 × 10^-6 m

C)1 × 10^-3 m

D)1 × 10⁶ m

Answer: B

Q2) A piece of metal ore weighs 8.25 g.When a student places it into a graduated cylinder containing water,the liquid level rises from 21.25 mL to 26.47 mL.What is the density of the ore?

A)0)312 g/mL

B)0)633 g/mL

C)1)58 g/mL

D)3)21 g/mL

Answer: C

Q3) Given that 2.54 cm = 1 in,350 in³ = ________ L.

Answer: 5.74

Q4) The quantity 3.00 cm³ is the same as ________ mL.

Answer: 3.00

Q5) Pb is the symbol for the element ________.

Answer: lead

Page 3

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Chapter 2: Atoms, molecules, and Ions

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Q1) What kind of decay process is occurring in the decay of isotope B to isotope C in the figure shown above?

A) emission

B) emission

C) emission

D)electron capture or positron emission

Answer: B

Q2) The ion,IO₂^-,is named

A)iodate ion.

B)iodite ion.

C)iodine dioxide ion.

D)iodine(II)oxide ion.

Answer: B

Q3) Which drawing represents the ionic compound Na₂CO₃?

A)drawing (a)

B)drawing (b)

C)drawing (c)

D)drawing (d)

Answer: B

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Chapter 3: Formulas, equations, and Moles

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Q1) Given the chemical equation: N₂ + 3 H₂ 2 NH₃.On a molecular level,what do the coefficients mean?

A)1 atom of nitrogen reacts with 3 atoms of hydrogen to give 2 atoms of ammonia.

B)28 g of nitrogen reacts with 6 grams of hydrogen to give 34 grams of ammonia.

C)1 mole of nitrogen reacts with 3 moles of hydrogen to give 2 moles of ammonia.

D)1 molecule of nitrogen reacts with 3 molecules of hydrogen to give 2 molecules of ammonia.

Answer: D

Q2) What is the molarity of a solution prepared by dissolving 0.80 g of NaOH in enough water to make 250 mL of solution?

Answer: 0.080 M

Q3) The balanced equation for the reaction of acetylene,C₂H₂,and oxygen in an acetylene torch is 2 C₂H₂ + 5 O₂ 4 CO₂ + 2 H₂O.

In this reaction the number of grams of oxygen required to react with 0.13 g of acetylene is ________.

Answer: 0.40 g

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) What is the oxidation number of the oxygen atom in H₂O₂?

A)-2

B)-1

C)+1

D)+2

Q2) Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq),is needed to completely react with 24.88 mL of 0.125 M KI₃(aq)?

2 S₂O₃^2-(aq)+ I₃^-(aq)

S₄O₆^2-(aq)+ 3 I^-(aq)

A)6)22 mL

B)12.4 mL

C)24.9 mL

D)99.5 mL

Q3) When NaOH(aq)is mixed with CuSO₄(aq)a precipitate forms.Based on solubility guidelines the formula of the precipitate is ________.

Q4) CH₃CO₂H is an example of a ________ electrolyte.

Q5) The oxidation number of hydrogen in CaH₂ is ________.

Q6) The best oxidizing agents are found at the ________ of the activity series.

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Chapter 5: Periodicity and the Atomic Structure of Atoms

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Sample Questions

Q1) According to the Balmer-Rydberg equation,which transition results in the emission of a photon in the ultraviolet region of the electromagnetic radiation spectrum?

A)m = 1 n = 2

B)m = 3 n = 4

C)m = 2 n = 1

D)m = 4 n = 3

Q2) What is the de Broglie wavelength of an electron (m = 9.11 × 10^-31

kg)moving at a velocity of 3)0 × 10⁷ m/s (10% of the speed of light)?

A)less than 3.9 × 10^-12 m

B)2)4 × 10^-11 m

C)3)3 × 10^-8 m

D)greater than 1.1 × 10^-4 m

Q3) What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals?

A)ns¹

B)ns²

C)1s²2s¹

D)1s²2s²

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Chapter 6: Ionic Bonds and Some Main-Group Chemistry

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Sample Questions

Q1) Which sphere most likely represents the K⁺ ion?

A)A

B)B

C)A or B

D)C or D

Q2) How many electrons are in the outermost shell of the In³⁺ ion in its ground state?

A)2

B)3

C)6

D)18

Q3) Which ion does not have a noble gas configuration in its ground state?

A)Sc³⁺

B)Al³⁺

C)Ga³⁺

D)As^3-

Q4) The element in group 7A with the least favorable (least negative)electron affinity is

Q5) The ion Q²⁺ contains 10 electrons.The identity of element Q is

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Chapter 7: Covalent Bonds and Molecular Structure

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Sample Questions

Q1) Which element can accommodate more than eight electrons in its valence shell?

A)C

B)O

C)P

D)He

Q2) Given that O₂ is paramagnetic and has a bond order of 2,and its highest occupied molecular orbital is antibonding,what would be the expected bond orders for O₂^2- and O₂²⁺?

A)1 for O₂^2- and 3 for O₂²⁺

B)3/2 for O₂^2- and 5/2 for O₂²⁺

C)5/2 for O₂^2- and 3/2 for O₂²⁺

D)3 for O₂^2- and 1 for O₂²⁺

Q3) The orbital hybridization on the carbon atom in HCN is A)sp.

B)sp².

C)sp³.

D)None of these

Q4) The Lewis electron-dot structure of N₂ has ________ nonbonding electrons pairs,________ bonding electron pairs,and a bond order of ________.

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Chapter 8: Thermochemistry: Chemical Energy

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Sample Questions

Q1) The first law of thermodynamics

A)defines chemical energy.

B)defines entropy.

C)is a statement of conservation of energy.

D)provides a criterion for the spontaneity of a reaction.

Q2) For the reaction I₂(g) I₂(s), H° = -62.4 kJ at 25°C.Based on these data,at 25°C

A) H°_vap = -62.4 kJ/mol.

B) H°_vap = 62.4 kJ/mol.

C) H°_sub = -62.4 kJ/mol.

D) H°_sub = 62.4 kJ/mol.

Q3) Which combination always results in a reaction being spontaneous?

A) H is negative and S is negative.

B) H is negative and S is positive.

C) H is positive and S is negative.

D) H is positive and S is positive.

Q4) Is chemical energy a form of kinetic or potential molecular energy?

Q5) A reaction for which E = -450 kJ is one in which products have 450 kJ ________ internal energy than the reactants,and products are ________ stable than the reactants.

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Chapter 9: Gases: Their Properties and Behavior

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Sample Questions

Q1) What is the average speed (actually the root-mean-square speed)of a neon atom at 27°C?

A)5)78 m/s

B)19.3 m/s

C)183 m/s

D)609 m/s

Q2) Which of the following regions of the earth's atmosphere contains the ozone layer?

A)mesosphere

B)stratosphere

C)thermosphere

D)troposphere

Q3) Some assumptions from the kinetic molecular theory are listed below.Which one is most frequently cited to explain Charles' law?

A)The average kinetic energy of gas particles is proportional to the Kelvin temperature.

B)Collisions of gas particles are elastic and total kinetic energy of the gas is constant.

C)A gas consists of tiny particles moving in random straight line motion.

D)The volume of the particles is negligible compared to the volume of the gas.

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Chapter 10: Liquids,solids,and Phase Changes

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Sample Questions

Q1) The critical temperature of a substance is the A)highest temperature at which the liquid phase can exist in equilibrium with the gas phase.

B)temperature above which the compound decomposes.

C)temperature at which all three phases can exist in equilibrium.

D)temperature at which sublimation occurs.

Q2) When a liquid is heated at its boiling point,the A)covalent bonds are broken,allowing vaporization to occur. B)temperature of the liquid increases.

C)temperature of the liquid remains the same as long as any liquid is present. D)temperature of the vapor phase increases.

Q3) Pt(NH₃)₂Cl₂ is square planar.The isomer of Pt(NH₃)₂Cl₂ that has a non-zero dipole moment has a Cl-Pt-Cl bond angle of ________ degrees.

Q4) Which of the following molecules does not have a dipole moment?

A)C₂H₂  

B)H₂O

C)CH₃CH₂OH D)H I

Q5) The coordination number of each atom in a simple cubic unit cell is ________.

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Chapter 11: Solutions and Their Properties

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Sample Questions

Q1) Which concentration becomes smaller as the temperature is increased from 20°C to 80°C?

A)mass %

B)molality

C)molarity

D)mole fraction

Q2) When 2.36 g of a nonvolatile solute is dissolved in 100 g of solvent,the largest change in freezing point will be achieved when the solvent is

A)benzene,K_f = 5.07.

B)camphor,K_f = 37.8.

C)chloroform,K_f = 4.70.

D)All are expected to have the same freezing point.

Q3) What is the molality of ethanol in a solution made by dissolving 14.6 g of ethanol,C₂H₅OH,in 53.6 g of water?

A)0)00591 m

B)0)272 m

C)5)91 m

D)272 m

Q4) Molarity is defined as ________,whereas molality is defined as ________.

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Chapter 12: Chemical Kinetics

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Sample Questions

Q1) The first-order reaction,SO₂Cl₂ SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

A)0)143 hr

B)2)28 hr

C)6)99 hr

D)22.7 hr

Q2) The first-order decomposition of hydrogen peroxide occurs according to the equation

2 H₂O₂(aq) 2 H₂O(l)+ O₂(g)

Using data from a concentration-time study of this reaction,which plot will produce a straight line?

A)[H₂O₂] versus time

B)[H₂O₂]² versus time

C)1/[H₂O₂] versus time

D)ln[H₂O₂] versus time

Q3) A reaction has a rate constant,k = 1.2 × 10^-12 s^-1 at 273 K and k = 5.1 × 10^-7 s^-1 at 373 K has an activation energy,E_a = ________ kJ/mol.

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Chapter 13: Chemical Equilibrium

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Sample Questions

Q1) A reaction reaches dynamic equilibrium at a given temperature when

A)the amount of products exceeds the amount of reactants.

B)k_fwd equals k_rev.

C)opposing reactions cease and the system is static.

D)the relative amounts of reactants and products are constant and rate_fwd = rate_rev.

Q2) A catalyst increases the rate of a chemical reaction by providing a lower-energy mechanism for the reaction.When this occurs,which one of the following is not affected?

A)activation energy for the forward reaction

B)activation energy for the reverse reaction

C)equilibrium constant

D)rate of the reverse reaction

Q3) Which nonequilibrium mixtures will react in the reverse direction to reach equilibrium?

A)reaction mixtures (1)and (2)

B)reaction mixtures (1)and (4)

C)reaction mixtures (2)and (3)

D)reaction mixtures (3)and (4)

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Chapter 14: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO₃,50.0 mL of 0.20 M HCl,and 100.0 mL of water? Assume that the volumes are additive.

A)0)30

B)0)82

C)1)00

D)1)10

Q2) Undersea flora prefer a maximum concentration of OH^- of 1.58 × 10^-5.The concentration of H₃O⁺ in the seawater is ________,and this solution is ________ (acidic,basic,neutral).

Q3) What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)₂ with 50.00 mL of 0.300 M NaOH? Assume that the volumes are additive.

A)13.05

B)13.10

C)13.28

D)13.58

Q4) A 0.10 M KNO₂ solution will have a pH ________ seven.

Q5) A proton hydrated by four water molecules has the formula ________.

Q6) The pH of a 0.025 M KOH solution is ________.

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Chapter 15: Applications of Aqueous Equilibria

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Sample Questions

Q1) What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

A)96%

B)10%

C)5%

D)1%

Q2) Which picture represents the system at the first equivalence point?

A)(1)

B)(2)

C)(3)

D)(4)

Q3) Addition of 0.0125 mol KOH to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________? The K_a of formic acid is 1.8 × 10^-4.

Q4) Which of the following combinations of chemicals could be used to make a buffer solution?

A)HCl/NaOH

B)HCl/NH₃

C)HCl/H₃PO₄

D)NaOH/NH₃

Page 17

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Chapter 16: Thermodynamics: Entropy, free Energy, and Equilibrium

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Sample Questions

Q1) Solid NaHCO₃ is heated to 90°C.At equilibrium the total pressure of the gases produced is 0.545 atm.Calculate G° at 90°C for the reaction 2 NaHCO₃(s) Na₂CO₃(s)+ H₂O(g)+ CO₂(g).

A)-7.85 kJ

B)-3.67 kJ

C)+3.67 kJ

D)+7.85 kJ

Q2) Which of the following statements must be true for the entropy of a pure solid to be zero?

I.The temperature must be 0 K.

II.The solid must be crystalline,not amorphous.

III).The solid must be perfectly ordered.

IV.The solid must be an element.

A)I

B)I and II

C)I,II,and III

D)I,II,III,and IV

Q3) The entropy of water at 25° is ________ than the entropy of water at 35°C.

Page 18

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Chapter 17: Electrochemistry

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Q1) Calculate the cell potential at 25°C for the cell Fe(s) (Fe²⁺(0.100 M) Pd²⁺(1.0 × 10^-5 M) Pd(s)

Given that the standard reduction potential for Fe²⁺/Fe is -0.45 V and for Pd²⁺/Pd is +0.95 V.

A)+1.16 V

B)+1.28 V

C)+1.52 V

D)+1.68 V

Q2) For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode?

Zn(s) Zn²⁺(aq) Ni²⁺(aq) Ni(s)

A)Zn(s) Zn²⁺(aq)+ 2 e^-

B)Zn²⁺(aq)+ 2 e^- Zn(s)

C)Ni(s) Ni²⁺(aq)+ 2 e^-

D)Ni²⁺(aq)+ 2 e^- Ni(s)

Q3) If a constant current of 1.50 × 10⁸ A is passed through a molten mixture of aluminum oxide and cryolite for 4.00 hour ________ kg of aluminum can be produced.

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Chapter 18: Hydrogen, oxygen, and Water

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Q1) Which isotope of diatomic hydrogen should have the highest heat of vaporization?

A)H₂

B)D₂

C)T₂

D)The values are equal.

Q2) What is the anhydrous form of nitric acid,HNO₃?

A)NO

B)NO₂

C)N₂O₃

D)N₂O₅

Q3) Which oxide is the most covalent?

A)A

B)B

C)C

D)D

Q4) Which is not an isotope of hydrogen?

A)hydrogen-1

B)hydrogen-2

C)hydrogen-3

D)hydrogen-4

Page 20

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Chapter 19: The Main-Group Elements

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Q1) As one traverses the periodic table from left to right,the effective nuclear charge

Z_eff increases.As a result of this the periodic properties of ________.

A)atomic size increases,IE increases,EA increases and electronegativity increases

B)atomic size decreases,IE increases,EA increases and electronegativity increases

C)atomic size decreases,IE decreases,EA increases and electronegativity increases

D)atomic size decreases,IE increases,EA decreases and electronegativity increases

Q2) What is the oxidation number of carbon in CaC₂?

A)+ 4

B)+ 1

C)- 1

D)- 2

Q3) When P₄O₁₀ is dissolved in water,the water will have a(n)________ (acidic,basic,neutral)pH due to the reaction ________.

Q4) The most acidic oxides of the group 5A elements are oxides of the element

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Chapter 20: Transition Elements and Coordination Chemistry

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Q1) A chromium(III)ion forms a complex ion with two ammonia molecules and four thiocyanate ions.What is the formula of the complex ion?

A)[Cr(NH₃)₂(NCS)₄]³⁺

B)[Cr(NH₄)₂(NCS)₄]⁺

C)[Cr(NH₃)₂(NCS)₄]^-

D)[Cr(NH₃)₂(NCS)₄]^4-

Q2) The complex [Ni(CN)₄]^2- is diamagnetic and the complex [NiCl₄]^2- is paramagnetic.What can you conclude about their molecular geometries?

A)Both complexes have square planar geometries.

B)Both complexes have tetrahedral geometries.

C)[NiCl₄]^2- has a square planar geometry while [Ni(CN)₄]^2- has a tetrahedral geometry.

D)[NiCl₄]^2- has a tetrahedral geometry while [Ni(CN)₄]^2- has a square planar geometry.

Q3) The number of unpaired electrons in square planar PtCl₄^2- is ________.

Q4) Mn²⁺ has ________ d electrons.

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Chapter

21: Metals and Solid-State Materials

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Q1) Steel is a mixture composed primarily of ________.

A)iron and carbon

B)iron and copper

C)iron and silicon

D)iron and sulfur

Q2) Silica (SiO₂)can be prepared from silicon ethoxide by the sol-gel process.Write a balanced equation for the hydrolysis of silicon ethoxide.

A)SiCl₄ + 4 HOCH₂CH₃ + 4 NH₃

Si(OCH₂CH₃)₄ + 4 NH₄Cl (in benzene)

B)Si(OCH₂CH₃)₄ + 4 H₂O Si(OH)₄ + 4 HOCH₂CH₃

C)Si(OCH₂CH₃)₄ + 4 HOCH₃

Si(OCH₃)₄ + 4 HOCH₂CH₃

D)Si(OCH₃)₄ + 4 H₂O Si(OH)₄ + 4 HOCH₃

Q3) Copper can be obtained from its copper(I)sulfide ore by roasting.What is the balanced equation for the roasting of copper(I)sulfide?

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Chapter 22: Nuclear Chemistry

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Q1) Carbon-14 has a half-life of 5715 years.Currently living organisms decay at a rate of 15.3 disintegrations/ min per gram of carbon.If an archeological artifact has a carbon-14 decay rate of 12.0 disintegrations/ min per gram of carbon,the approximate age of the artifact is ________ years old.

Q2) Which unit of radiation describes the amount of energy absorbed by a kilogram of tissue exposed to a radiation source?

A)becquerel

B)curie

C)rad

D)rem

Q3) A sievert is:

A)the amount of sample that undergoes 1 disintegration per second.

B)the amount of sample that undergoes 3.7 × 10¹⁰ disintegrations per second.

C)the amount of tissue damage done by radiation.

D)equal to 0.01 J of energy absorbed per kilogram of tissue.

Q4) ²⁰¹Tl is used in myocardial perfusion imaging.It undergoes beta decay with a half-life of 73 hours generating 80 keV X-rays.A typical dose is 2.5 mCi which is equal to ________ Bq.

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Chapter 23: Organic and Biological Chemistry

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Q1) How many isomers exist for C₅H₁₂? Of these isomers,how many are straight-chain isomers and how many are branched isomers?

Q2) What is the H-C-H bond angle?

A)90°

B)109.5°

C)120°

D)180°

Q3) Lactose,or milk sugar,when hydrolyzed will form ________.

A)amylose and glycogen

B)cellulose and starch

C)glucose and galactose

D)fructose and maltose

Q4) What hybrid orbitals are used by carbon to form covalent bonds with hydrogen?

A)sp

B)sp²

C)sp³

D)sp³^d

Q5) The molecule

CH₃CH₂CO₂CH₂CO₂H contains an ________ functional group and a ________ functional group.

Page 25

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