Chemical Science Practice Questions - 2610 Verified Questions

Chemical Science

Practice Questions

Course Introduction

Chemical Science is an interdisciplinary field that explores the composition, structure, properties, and changes of matter at the molecular and atomic levels. This course provides a comprehensive overview of fundamental chemical principles including atomic theory, chemical bonding, thermodynamics, kinetics, and equilibrium. Students will investigate the behavior of gases, liquids, and solids, study the periodic table and its implications, and explore the essentials of organic and inorganic chemistry. Laboratory sessions reinforce theoretical concepts through hands-on experiments, fostering skills in observation, analysis, and scientific reasoning. The course lays a strong foundation for advanced study in chemistry, environmental science, materials science, and related fields.

Recommended Textbook

General Chemistry 11th Edition by Darrell D. Ebbing

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Chapter 1: Chemistry and Measurement

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Sample Questions

Q1) The boiling point of chlorine is 172 K.This temperature corresponds to A)-82°C.

B)101°C.

C)172°C.

D)-172°C.

E)-101°C.

Answer: E

Q2) A car averages 28.5 miles per gallon of gasoline.How many liters of gasoline will be needed for a trip of 415 km? Some conversion factors that may be helpful are the following:

1 qt = 0.946 L

1 mile = 1.609 km

4 qt = 1 gal (exact)

1 ft = 12 in (exact)

A)3 × 10¹ L

B)5 × 10³ L

C)2 × 10³ L

D)9 × 10¹ L

E)3 × 10⁴ L

Answer: A

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Page 3

Chapter 2: Atoms, molecules, and Ions

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Q1) Which one of the following lists gives the correct symbols for the elements phosphorus,potassium,silver,chlorine,and sulfur?

A)P,Po,Ag,Cl,S

B)K,Ag,Po,Cl,S

C)P,K,Ag,Cl,S

D)Ph,K,Ag,S,Cl

E)Ph,Po,Ag,Cl,S

Answer: C

Q2) The elements in a row of the periodic table are known as A)metals.

B)a period.

C)metalloids.

D)a family.

E)a group.

Answer: B

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Chapter 3: Calculations With Chemical Formulas and Equations

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Sample Questions

Q1) How many grams of potassium are present in 28.7 g of K₂Cr₂O₇?

A)7.63 g

B)1.468 g

C)3.81 g

D)78.2 g

E)14.4 g

Answer: A

Q2) How many molecules are there in 60 g of acetic acid,C₂H₄O₂?

A)(6.02 × 10²³)/ 60

B)60

C)6.02 × 10²³

D)30

E)60 × (6.02 × 10²³)

Answer: C

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Chapter 4: Chemical Reactions

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Sample Questions

Q1) Which of the following do you need to know to be able to calculate the molarity of a salt solution?

I.the mass of salt added

II.the molar mass of the salt

III.the volume of water added

IV.the total volume of the solution

A)II and III only

B)I,II,and IV only

C)I,II,and III only

D)I and III only

E)You need all of the information.

Q2) What is the balanced reduction half-reaction for the reaction

3Mg(s)+ N₂(g) Mg₃N₂(s)

A)Mg²⁺ + 2e Mg

B)Mg Mg²⁺ + 2e

C)Mg²⁺ Mg + 2e

D)N₂ + 6e 2N³

E)N₂ 2N³+ 6e

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Page 6

Chapter 5: The Gaseous State

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Sample Questions

Q1) What is the partial pressure of carbon dioxide in a container that contains 3.63 mol of oxygen,1.49 mol of nitrogen,and 4.49 mol of carbon dioxide when the total pressure is 871 mmHg?

A)329 mmHg

B)763 mmHg

C)135 mmHg

D)406 mmHg

E)871 mmHg

Q2) Absolute zero is the point at which

A)a straight-line graph of V versus T (°C)intersects the origin.

B)a straight-line graph of 1/V versus P at constant T intersects the origin.

C)gaseous helium liquefies.

D)a straight-line graph of V versus 1/P at constant T intersects the origin.

E)a straight-line graph of V versus T (K)intersects the origin.

Q3) At STP,as the molar mass of the molecules that make up a pure gas increases,the

A)root mean square speed of the molecules increases.

B)root mean square speed of the molecules decreases.

C)root mean square speed of the molecules remains constant.

D)root mean square speed increases to a maximum,then decreases.

E)none of the above.

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Chapter 6: Thermochemistry

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Sample Questions

Q1) What is H° for the following reaction?

2C₂H₂(g)+ 5O₂(g) 4CO₂(g)+ 2H₂O(l)

Substance

H°_f (kJ/mol)

C₂H₂(g)

+226.7

CO₂(g) -393.5

H₂O(l)

-285.8

A)+1692.2 kJ

B)-452.6 kJ

C)-1692.2 kJ

D)+2599.0 kJ

E)-2599.0 kJ

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Chapter 7: Quantum Theory of the Atom

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Sample Questions

Q1) The square of the wave function, ²,of an electron in an atom

A)is inversely proportional to the distance between the electron and the nucleus.

B)specifies the momentum of the electron.

C)describes the energy of the electron.

D)is proportional to the velocity of the electron.

E)gives the probability of finding the electron in a region of space.

Q2) What is the energy per mole of photons with a wavelength of 307.1 nm?

(c=3.00×10⁸ m/s,h=6.63×10^-34

J·s,N_A=6.02×10²³mol^-1)

A) 6.48×10^-19 kJ/mol

B)1.85×10¹⁴ kJ/mol

C)5.88×10³⁵ kJ/mol

D)9.77×10¹⁴ kJ/mol

E)3.9×10² kJ/mol

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Chapter 8: Electron Configurations and Periodicity

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Sample Questions

Q1) The change in energy for which of the following processes corresponds to the first ionization energy of beryllium?

A)Be(g) Be⁺(g)+ e^-

B)Be(s) Be⁺(s)+ e^-

C)Be(s) Be⁺(g)+ e^-

D)Be(g) Be²⁺(g)+ 2e^-

E)Be(s)+ e^- Be^-(s)

Q2) What is the ground-state electron configuration of sulfur (S)?

A)[Ne]3s³3p³

B)[Ar]3s²3p⁴

C)[Ar]3p⁶

D)[Ne]3s²3p⁴

E)[Ne]3p⁶

Q3) What is the valence-shell electron configuration for the fourth-period element in Group VA?

A)4s²5p⁵

B)5s²5p⁵

C)4s²4p³

D)5s²4p⁵

E)4s²3d³

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Chapter 9: Ionic and Covalent Bonding

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Sample Questions

Q1) What is the total number of valence electrons in N₂O?

A)16

B)17

C)34

D)11

E)22

Q2) The electronic structure of which of the following species cannot be adequately described by a single Lewis formula?

A)CS₂

B)POF₃

C)HNNH

D)NO₃^-

E)H₂NNH₂

Q3) All of the following species are isoelectronic except

A)S^2-

B)K⁺

C)Na⁺

D)Ar

E)Cl^-

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Chapter 10: Molecular Geometry and Chemical Bonding Theory

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Sample Questions

Q1) The configuration ( _2s)²( _2s*)²( _2py)¹( _2px)¹ is the molecular orbital description for the ground state of A)C₂.

B)B₂.

C)Be₂.

D)Li₂⁺.

E)B₂^2-.

Q2) The approximate H-C-H bond angle in CH₃⁺ is A)60°.

B)90°.

C)120°.

D)109°.

E)180°.

Q3) Which molecule or ion has a trigonal planar molecular geometry?

A)PCl₃

B)HCN

C)CO₃^2-

D)HCCH

E)AsF₃

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Chapter 11: States of Matter; Liquids and Solids

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Sample Questions

Q1) Which of the following indicates the existence of strong intermolecular forces of attraction in a liquid?

A)a very low critical temperature

B)a very low boiling point

C)a very low vapor pressure

D)a very low viscosity

E)a very low enthalpy of vaporization

Q2) Which of the following pure substances has the highest melting point?

A)CCl₄

B)AlCl₃

C)NCl₃

D)LiCl

E)MgCl₂

Q3) The strongest intermolecular forces present in a sample of pure I₂ are A)London forces.

B)dipole-dipole forces.

C)metallic bonds.

D)covalent network bonds.

E)covalent bonds.

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Page 13

Chapter 12: Solutions

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Sample Questions

Q1) Which of the following pure liquids is the best solvent for carbon disulfide?

A)C₆H₆(l)

B)NH₃(l)

C)CH₃OH(l)

D)H₂O(l)

E)HBr(l)

Q2) A suspension of silver particles in water is most likely to form what type of colloid?

A)aerosol

B)micelle

C)hydrophobic colloid

D)association colloid

E)hydrophilic colloid

Q3) A 3.140 molal solution of NaCl is prepared.How many grams of NaCl are present in a sample containing 2.692 kg of water?

A)299.7 g

B)494.0 g

C)144.6 g

D)845.3 g

E)none of these

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Page 14

Chapter 13: Rates of Reaction

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Sample Questions

Q1) Which of the following statements is incorrect?

A)The rates of most chemical reactions change with time.

B)The rate constant for a reaction can be changed by changing the temperature.

C)The rate constant is dependent on the reactant concentrations.

D)In a series of stepwise reactions,the rate-determining step is the slowest one.

E)The rate of a catalyzed reaction is dependent on the concentration of the catalyst.

Q2) When the concentrations of the reactants are increased,the rate of the reaction increases.This is best explained by

A)an increase in the fraction of molecules that have enough energy to react.

B)an increase in the rate constant.

C)an increase in the average potential energy of the molecules.

D)an increase in the frequency of the molecular collisions.

E)an increase in the kinetic energy of the molecules.

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) For which of the following values of the equilibrium constant does the reaction mixture contain mostly products?

A)10⁰

B)10¹

C)10⁹

D)10^-1

E)10^-9

Q2) For a specific reaction,which of the following statements can be made about the equilibrium constant?

A)It can be changed by the addition of a catalyst.

B)It increases when the concentration of one of the products is increased.

C)It increases when the concentration of one of the reactants is increased.

D)It always remains the same.

E)It changes with changes in the temperature.

Q3) Which of the following represents a dynamic equilibrium?

A)a stoppered flask half full of water

B)a coin spinning in mid-air

C)two people of equal mass balanced on the ends of a seesaw

D)an open pan of boiling water

E)an object traveling at a constant speed

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Chapter 15: Acids and Bases

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Sample Questions

Q1) What is the pOH of a solution prepared by dissolving 0.591 g of KOH(s)in 7.50 L of water?

A)11.148

B)2.852

C)1.977

D)12.023

E)7.000

Q2) What is the hydronium-ion concentration of a 0.0017 M Ba(OH)₂ solution?

A)3.4 × 10^-3 M

B)1.7 × 10^-3 M

C)2.9 × 10^-12 M

D)5.9 × 10^-12 M

E)1.0 × 10^-7 M

Q3) Which solution would cause blue litmus to turn red?

A)a solution of pH 10

B)a solution of 0.01 M NH₃

C)a solution of pOH 4

D)a solution of 0.005 M CH₃COOH

E)a solution of 0.10 M NaOH

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) In a 0.20 M solution of a diprotic acid H₂A (Ka₁ = 1.3 × 10^-5 and Ka₂ = 2.7 × 10^-10 at 25°C),what is the equilibrium concentration of A^2-?

A)7.3 × 10^-6 M

B)2.7 × 10^-10 M

C)1.6 × 10^-3 M

D)0.40 M

E)0.20 M

Q2) What is K_a for the anilinium cation,C₆H₅NH₃⁺,at 25°C? (K_b for C₆H₅NH₂ = 4.2 × 10^-10 at 25°C.)

A)1.0 × 10^-7

B)4.2 × 10⁴

C)4.2 × 10^-24

D)2.4 × 10^-5

E)4.2 × 10^-10

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Page 18

Chapter 17: Solubility and Complex-Ion Equilibria

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Q1) What is the molar solubility of nickel(II)sulfide in 0.091 M KCN? For NiS,K_sp = 3.0 × 10^-19; for Ni(CN)₄^2-,K_f = 1.0 × 10³¹.

A)5.5 × 10^-10 M

B)9.1 × 10^-2 M

C)1.5 × 10^-19 M

D)2.3 × 10^-2 M

E)2.9 × 10^-5 M

Q2) In which of these solutions would silver(I)carbonate have the lowest molar solubility? For silver(I)carbonate,K_sp = 8.5 × 10^-12.

A)0.03 M H₂CO₃

B)0.1 M AgNO₃

C)0.01 M AgNO₃

D)0.1 M Na₂CO₃

E)pure water

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19

Chapter 18: Thermodynamics and Equilibrium

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Q1) The reaction CaO(s)+ SO₃(g) CaSO₄(s)is nonspontaneous at 2200 K,whereas it is spontaneous at room temperature.Which of the following statements is false?

A)The change in enthalpy is the main driving force of the reaction.

B)Both H and S are negative for the reaction.

C) G is negative at room temperature.

D)The change in entropy is the main driving force of the reaction.

E) G becomes zero at a temperature between 300 and 2200 K.

Q2) For a reaction that has an equilibrium constant of 6 × 10⁹,which of the following statements must be true?

A) S° is positive.

B) G° is negative.

C) G° is positive.

D) H° is negative.

E) H° is positive.

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Chapter 19: Electrochemistry

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Q1) If the value of E°_cell is 2.10 V for the reaction F₂ (g)+ 2Fe²⁺ (aq) 2Fe³⁺ (aq)+ 2F^- (aq),

What is the value of E°_cell for F^- (aq)+ Fe³⁺ (aq) Fe²⁺(aq)+ 1/2 F₂(g)?

A)-4.20 V

B)-1.05 V

C)2.10V

D)1.05 V

E)-2.10V

Q2) In a table of standard reduction potentials,the strongest reducing agents are the _______ species in the half-reactions with the _______ E° values.

A)reduced,most negative

B)oxidized,most positive

C)reduced,most positive

D)oxidized,most negative

E)none of these

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21

Chapter 20: Nuclear Chemistry

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Sample Questions

Q1) For which of the following radioactive decay processes does the atomic number not change?

A)electron capture

B)positron emission

C)alpha emission

D)gamma emission

E)beta emission

Q2) Which of the following corresponds to the most rapid nuclear decay?

A)t_1/2 = 1.0 × 10³ min

B)t_1/2 = 1.0 × 10⁹ year

C)k = 1.0 × 10^-3/year

D)k = 1.0 × 10^-1/day

E)k = 1.0 × 10^-5/s

Q3) Which of the following nuclides will produce ²⁴³Am upon undergoing alpha decay?

A)(²⁴⁷Bk)

B)(²³⁹Np)

C)(²⁴³Pu)

D)(²⁴³Cm)

E)(²⁴⁴Am)

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Chapter 21: Chemistry of the Main-Group Metals

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Sample Questions

Q1) Which of the following compounds would not be expected to react with oxygen?

A)NH₃

B)N₂H₄

C)N₂O₅

D)N₂O₄

E)Li₃N

Q2) Which of the following reactions does not represent a commercial method for preparing hydrogen gas?

A)C₃H₈(g)+ 3H₂O(g) 3CO(g)+ 7H₂(g)

B)C(s)+ H₂O(g) CO(g)+ H₂(g)

C)2NH₃(g) N₂(g)+ 3H₂(g)

D)2H₂O(l) 2H₂(g)+ O₂(g)

E)CO(g)+ H₂O(g) CO₂(g)+ H₂(g)

Q3) Which element is found in the ore galena?

A)aluminum

B)lead

C)silicon

D)germanium

E)tin

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Chapter 22: The Transition Elements and Coordination Compounds

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Q1) Which of the following salts would not be expected to be colored in aqueous solution?

A)CrF₃

B)NiF₂

C)TiF₃

D)ScF₃

E)MnF₃

Q2) The spectrochemical series is an arrangement of

A)ligands in order of their tendency to split the d orbitals of a transition metal ion.

B)coordination compounds in order of increasing ligand field splitting ( ).

C)complex ions in order of the wavelength of light absorbed.

D)ligands in the order of electronegativity.

E)ligands in order of Lewis basicity.

Q3) Which of the following is not a characteristic of the transition metals?

A)variable oxidation state

B)the ability to form many colored compounds

C)valence electrons in a d subshell

D)high electronegativity

E)the ability to form complex ions

Page 24

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Chapter 23: Organic Chemistry

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Q1) What is the common name for the following compound?

CH₃CH₂OCH₂CH₂CH₃

A)2-pentanone

B)pentyl ether

C)2-pentanol

D)propoxyethane

E)ethyl propyl ether

Q2) What is the composition of crude oil?

A)mostly unsaturated hydrocarbons having 5-12 carbons per molecule

B)mostly hydrocarbons,but the precise composition varies widely depending on location

C)mostly aromatic hydrocarbons

D)mostly saturated hydrocarbons having 5-12 carbons per molecule

E)mostly saturated hydrocarbons having 12-20 carbons per molecule

Q3) Which of the following is the general formula for an alkane?

A)C_nH₂_n₊₂

B)C₂_nH₂_n_-2

C)C_nH_n

D)C_nH₂_n

E)none of these

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Chapter 24: Polymer Materials: Synthetic and Biological

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Sample Questions

Q1) What is the cell structure that contains the cell's DNA?

A)chromosome

B)codon

C)ribosome

D)gene

E)nucleus

Q2) Which of the following pairs of substances could form a polyester?

A)H₂NCH₂COOH +

H₂NCH₂CH₂COOH

B)HO(CH₂)₄COOH + HOCH₂CH=CHCH₃

C)HOCH₂CH₂OH + HOOCCOOH

D)H₂C=CHCH₃ + HOCH₂CH₂COOH

E)H₂C=CHCN + H₂C=CHCH₃

Q3) Which of the following combinations can produce a condensation polymer? (R and R' are alkyl groups)

A)R OH + HOOC R' COOH

B)HO R OH + R' COOH

C)H₂N R NH₂ + HOOC R' COOH

D)A and C

E)A,B,and C

Page 26

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