Introduction to Chemistry Exam Materials - 2075 Verified Questions

Introduction to Chemistry

Exam Materials

Course Introduction

Introduction to Chemistry is a foundational course designed to provide students with a comprehensive overview of the basic principles and concepts of chemistry. The course covers key topics such as atomic structure, the periodic table, chemical bonding, stoichiometry, states of matter, chemical reactions, and the properties of acids and bases. Emphasis is placed on developing analytical and problem-solving skills through laboratory experiments and real-world applications. This course serves as a prerequisite for advanced studies in science and health-related fields, and it aims to build a solid understanding of how chemical processes impact everyday life.

Recommended Textbook Chemistry and Chemical Reactivity 9th Edition by John C. Kotz\New folder

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Chapter 1: Basic Concepts of Chemistry

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Q1) Which one of the following statements is \(\underline{\text{ correct? }}\)

A) A pure substance may be separated by filtration or distillation into two or more components.

B) A heterogeneous mixture is also known as a solution.

C) A heterogeneous mixture is composed of two or more substances in the same phase.

D) The composition is uniform throughout a homogeneous mixture.

E) The combination of a liquid and a solid always results in a heterogeneous mixture.

Answer: D

Q2) A \(\underline{\text{ theory }}\) is a ________.

A) mathematical formula that models a pattern of behavior

B) set of quantitative data

C) well-tested unifying principle that explains a body of facts

D) tentative explanation or predication based upon experimental observations

E) set of experiments designed to test a theory

Answer: C

Q3) A mass of 10 g of table salt dissolves in water to form a(n)________ mixture (i.e.,a mixture that is uniform throughout).

Answer: homogeneous

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3

Chapter 2: Mathlets Review: The Tools of Quantitative Chemistry

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Q1) What length of a cylindrical piece of tungsten wire having a radius of 2.35 mm has a mass of 92.3 g? The density of tungsten is 19.25 g/cm³ and Volume = \(\pi\)r²h.

A) 2.76 \(\times\) 10^-3 m

B) 3.08 \(\times\) 10² m

C) 2.76 \(\times\) 10^-1 m

D) 3.62 \(\times\) 10^-2 m

E) 3.62 \(\times\) 10^-4 m

Answer: C

Q2) Assuming the density of water is 1.00 g/cm³,the mass of 1.0 cubic meter (m³) of water is ________ grams.

Answer: 1.0 \(\times\) 10⁶

Q3) Express 0.00560 in exponential notation.

A) 5.60 \(\times\) 10³

B) 5.6 \(\times\) 10^-3

C) 5.60 \(\times\) 10^-3

D) 5.6 \(\times\) 10³

E) 5.600 \(\times\) 10³

Answer: C

Page 4

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Chapter 3: Atoms, molecules, and Ions

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Q1) In which group of the following groups of the periodic table are all the elements nonmetals?

A) 2A

B) 3A

C) 5A

D) 6A

E) 7A

Answer: E

Q2) Elements that have the same number of protons,but differ in their number of neutrons are called ________.

Answer: isotopes

Q3) What is the correct name for CCl₄?

A) carbon chlorine

B) tetracarbon chloride

C) carbon tetrachloride

D) carbon(IV)chloride

E) tetrachlorocarbide

Answer: C

Q4) Oxygen and ________ are the two most abundant elements in the Earth's crust. Answer: silicon

Page 5

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Chapter 4: Chemical Reactions

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Q1) Which of the following statements concerning electrolytes and nonelectrolytes is/are true?

1)Some molecular substances are electrolytes.

2)All electrolytes are ionic substances.

3)Strong electrolytes partially ionize in solution.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 2 and 3

Q2) If an aqueous solution of ____ is added to a mixture of F^- and SO₄^2-,the fluoride ion will precipitate,but the sulfate ion will remain in solution.

A) LiBr

B) HNO₃

C) Pb(ClO₄)₂

D) MgNO₃

E) AlCl₃

Q3) Ionic and molecular compounds that form ions in aqueous solution are called

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Chapter 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Q1) The combustion of 0.0272 mole of a hydrocarbon produces 1.9609 g H₂O and 3.5927 g CO₂.What is the molar mass of the hydrocarbon?

A) 16.0 g/mol

B) 30.1 g/mol

C) 44.1 g/mol

D) 72.2 g/mol

E) 92.1 g/mol

Q2) If the complete combustion of an unknown mass of ethylene produces 16.0 g CO₂,what mass of ethylene is combusted?

C₂H₄(g)+ 3 O₂(g)\(\to\) 2 CO₂(g)+

2 H₂O(g)

A) 0.182 g

B) 0.364 g

C) 5.10 g

D) 8.00 g

E) 12.6 g

Q3) The pH of purified water (or of a neutral solution)is _____.

Q4) The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.

Page 7

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Chapter 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

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Q1) Acetylene,C₂H₂,is a gas used in welding.The molar enthalpy of combustion for acetylene is -2599 kJ.A mass of 0.338 g C₂H₂(g)is combusted in a bomb calorimeter.If the heat capacity of the calorimeter is 729 J/K and it contains 1.150 kg of water,what is the temperature increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J/g.K and the molar mass of acetylene is 26.04 g/mol.

A) 1.59 K

B) 6.09 K

C) 7.01 K

D) 12.3 K

E) 18.0 K

Q2) When 0.236 mol of a weak base (A^-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is \(\Delta\)H for this reaction per mole of A^- consumed?

A) -34.2 kJ/mol

B) -59.4 kJ/mol

C) -29.3 kJ/mol

D) 34.2 kJ/mol

E) 29.3 kJ/mol

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Chapter 7: The Structure of Atoms

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Q1) Which of the following is/are correct postulates of Bohr's theory of the hydrogen atom ?

1)The energy of an electron in an atom is quantized (i.e.only specific energy values are possible).

2)The principal quantum number (n),specifies each unique energy level.

3)An electron transition from a lower energy level to a higher energy level results in an emission of a photon of light.

A) 1 only

B) 2 only

C) 3 only

D) 1 and 2

E) 1,2,and 3

Q2) For which of the following transitions would a hydrogen atom absorb a photon with the longest wavelength?

A) n = 1 to n = 2

B) n = 4 to n = 6

C) n = 5 to n = 4

D) n = 7 to n = 6

E) n = 6 to n = 7

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9

Chapter 8: The Structure of Atoms and Periodic Trends

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Q1) If the ground state electron configuration of an element is [Ar]3d¹⁰4s²4p⁵,what is the typical charge on the monatomic anion of the element?

A) 4+

B) 2+

C) 1-

D) 2-

E) 3-

Q2) What is the ground state electron configuration for Cr³⁺?

A) [Ar]

B) [Ar]3d⁷4s²

C) [Ar]3d¹4s²

D) [Ar]3d²4s¹

E) [Ar]3d³

Q3) What is the maximum number of electrons that can occupy the n = 1 shell?

A) 2

B) 8

C) 18

D) 32

E) 50

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Chapter 9: Bonding and Molecular Structure

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Q1) In the Lewis formula for sulfur dioxide,SO₂,the number of lone pairs of electrons around the sulfur atom is

A) 0.

B) 1.

C) 2.

D) 3.

E) 4.

Q2) Use VSEPR theory to predict the molecular geometry of BrF₅.

A) tetrahedral

B) see-saw

C) trigonal-bipyramidal

D) square-pyramidal

E) octahedral

Q3) The Lewis structure of which of the following formula violates the octet rule?

A) SF₆

B) NF₃

C) OF₂

D) HF

E) SiF₄

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Chapter 10: Bonding and Molecular Structure: Orbital

Hybridization and Molecular Orbitals

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Q1) Refer to Diagram 9-1.Assuming that the molecular orbital energy diagram for a homonuclear diatomic molecule applies to a heteronuclear diatomic molecule,determine which of the following species is paramagnetic.

A) NO⁺

B) CO

C) CN^-

D) OF^-

E) NO

Q2) Which of the following characteristics apply to NCl₃?

1)polar bonds

2)nonpolar molecule

3)triangular-planar molecular shape

4)sp² hybridized N atom

A) 1 only

B) 1 and 2

C) 3 and 4

D) 1,2,and 3

E) 1,2,3,and 4

Q3) The hybridization of the carbon atom in CF₃⁺ is

Page 12

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Chapter 11: Gases and Their Properties

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Q1) Equal volumes of propane,C₃H₈,and carbon monoxide,CO,at the same temperature and pressure have the same ____.

A) chemical properties.

B) number of atoms.

C) average molecular speed.

D) density.

E) number of molecules.

Q2) Into a 2.22-liter container at 25°C are placed 1.23 moles of O₂gas and 3.20 moles of solid C (graphite).If the carbon and oxygen react completely to form CO(g),what will be the final pressure in the container at 25°C?

A) 27.1 atm

B) 13.5 atm

C) 2.27 atm

D) 35.2 atm

E) none of these

Q3) The gas constant,R,expressed in SI units has a value of 8.314.The units of the constant are ________.

Q4) What are two ways in which real gases differ from ideal gases?

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Page 13

Chapter 12: Intermolecular Forces and Liquids

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Q1) A molecule will \(\underline{\text{always }}\) be polar if it ___.

A) has polar bonds

B) contains both carbon and chlorine

C) consists of more than three atoms

D) is diatomic with different electronegativities

E) contains atoms with different electronegativities

Q2) If 3.21 g of water is sealed in an evacuated 2.52 L flask and heated to the normal boiling point of 373 K,what is the pressure in the flask? (R = 0.08206 L.atm/mol.K)

A) 0.231 atm

B) 0.462 atm

C) 1.00 atm

D) 2.16 atm

E) 39.0 atm

Q3) Arrange HF,HCl,and HBr in order from lowest to highest boiling point.

A) HF < HCl < HBr

B) HF < HBr < HCl

C) HBr < HF < HCl

D) HBr < HCl < HF

E) HCl < HBr < HF

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Chapter 13: The Chemistry of Solids

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Q1) Lithium chloride crystallizes in a face-centered cubic unit cell with chloride ions occupying the lattice points and lithium ions occupying octahedral holes.How many chloride ions surround each lithium ion in LiCl?

A) 1

B) 4

C) 6

D) 8

E) 12

Q2) The lattice energy of NaBr is -752 kJ/mol.This energy corresponds to which reaction below?

A) Na(s)+ 1/2 Br₂(g)\(\to\) NaBr(s)

B) Na(g)+ Br(g)\(\to\) NaBr(s)

C) Na(g) + Br(g)\(\to\) NaBr(s)

D) Na⁺(g)+ Br^-(g)\(\to\) NaBr(s)

E) Na⁺(aq)+ Br^-(aq)\(\to\) NaBr(s)

Q3) A salt with a 1:1 ratio of anions to cations may pack in a face-centered cubic unit cell with the anions at the lattice points and the cations occupying one-half of the ________ holes.Zinc sulfide is an example of this structure.

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Chapter 14: Solutions and Their Behavior

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Q1) What mass of ethylene glycol,when mixed with 225 g H₂O,will reduce the equilibrium vapor pressure of H₂O from 1.00 atm to 0.800 atm at 100 S1U1P1\(\circ\)S1S1P0C? The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol,respectively.Assume ideal behavior for the solution.

A) 15.6 g

B) 49.9 g

C) 194 g

D) 969 g

E) 3.10 \(\times\) 10³ g

Q2) The solubility of 1-hexanol in water is 0.60 g per 100 g of water at 25°C.What is the maximum amount of 1-hexanol that will dissolve in 5.3 g of water at 25°C?

A) 0.032 g

B) 0.11 g

C) 0.60 g

D) 3.2 g

E) 0.0011 g

Q3) ________ are colloidal dispersions of one liquid in another liquid.

Q4) A surfactant used for cleaning is called a(n)________.

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Page 16

Chapter 15: Chemical Kinetics: the Rates of Chemical Reactions

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Q1) If a catalyst is present in a different phase from the reactants and products,it is referred to as a(n)________ catalyst.

Q2) The pre-exponential,A,in the Arrhenius equation is called the ________ factor.

Q3) Draw the reaction coordinate diagram for an exothermic reaction involving three mechanistic steps.

Q4) The reaction A \(\to\) B follows first-order kinetics with a half-life of 21.7 hours.If the concentration of A is 0.023 M after 48.0 hours,what is the initial concentration of A?

A) 0.0050 M

B) 0.051 M

C) 0.51 M

D) 0.11 M

E) 2.0 \(\times\) 10² M

Q5) Termolecular elementary steps are rare.Why?

Q6) The ________ of an elementary step is defined as the number of reactant molecules that come together in the reaction.

Q7) Radioactive isotopes decay by ________-order kinetics.

Page 17

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Chapter 16: Principles of Reactivity: Chemical Equilibria

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Q1) In 1913,the Haber-Bosch process was patented.The product of the Haber-Bosch process is ________.

Q2) If the reaction quotient,Q,is greater than K in a gas phase reaction,then

A) the chemical system has reached equilibrium.

B) the temperature must be increased for the reaction to proceed in the forward direction.

C) the reaction will proceed in the forward direction until equilibrium is established.

D) the reaction will proceed in the backward direction until equilibrium is established.

E) the reaction will proceed in the direction that increases the number of gas phase particles.

Q3) Which of the following statements about the reaction quotient,Q,is false?

A) The value of Q can be used to predict equilibrium concentrations.

B) It has the same expression as K_c.

C) Its value is calculated using nonequilibrium concentrations.

D) If Q > K_c,the reaction must move to equilibrium by forming more reactants.

E) If Q < K_c,the reaction must move to equilibrium by forming more products.

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Chapter 17: The Chemistry of Acids and Bases

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Q1) Write a net ionic equation for the neutralization reaction of hydrochloric acid and potassium hydroxide.Identify the spectator ion(s).

Q2) What is the pH of the solution which results from mixing 75 mL of 0.50 M NH₃(aq)and 75 mL of 0.50 HCl(aq)at 25 S1U1P1\(\circ\)S1S1P0C?

(K_b for NH₃ = 1.8 \(\times\) 10^-5)

A) 0.60

B) 2.67

C) 4.74

D) 4.93

E) 9.26

Q3) What is the hydronium-ion concentration of a 0.25 M solution of HCN (K_a = 4.9 \(\times\) 10^-10)at 25°C?

A) 1.6 \(\times\) 10^-4 M

B) 3.3 \(\times\) 10^-6 M

C) 2.1 \(\times\) 10^-6 M

D) 1.1 \(\times\) 10^-5 M

E) 4.4 \(\times\) 10^-5 M

Q4) A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

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Chapter 18: Principles of Reactivity: Other Aspects of Aqueous Equilibria

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Q1) To make a buffer with a pH of 8.00,you should use a weak acid with a K_a close to _______.

Q2) What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 \(\times\) 10^-3,K_a2 = 6.2 \(\times\) 10^-8,and K_a3 = 3.6 \(\times\) 10^-13)

A) 1.82

B) 2.12

C) 6.91

D) 7.21

E) 12.44

Q3) Calculate the pH of a solution made by mixing 100.0 mL of 0.635 M NH₃ with 100.0 mL of 0.100 M HCl.(K_b for NH₃ = 1.8 \(\times\) 10^-5)

A) 9.98

B) 4.02

C) 8.53

D) 9.26

E) none of these

Page 20

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Chapter 19: Entropy and Free Energy

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Q1) For a certain reversible process q = 57.40 kJ at 36.6S1U1P1\(\circ\)S1S1P0C.What is \(\Delta\)S for the process?

A) 0.185 J/K

B) 185 J/K

C) 1.57 J/K

D) (-0.185) J/K

E) 2130 J/K

Q2) Arrange the following reactions in order of increasing \(\Delta\)_rS° value.

1.H₂(g)+ F₂(g)\(\to\) 2HF(g)

2)NH₄NO₃(s)\(\to\) N₂O(g)+ 2H₂O(l)

3)(NH₄)₂Cr₂O₇(s)\(\to\) Cr₂O₃(s)+ 4H₂O(l)+ N₂(g)

A) 1 < 2 < 3

B) 2 < 3 < 1

C) 3 < 1 < 2

D) 1 < 3 < 2

E) 2 < 1 < 3

Q3) At what temperature (in kelvin units)is the entropy of a pure crystal 0.0 J/K.

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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 cell in which the hydrogen electrode is the anode and the cathode half-reaction is Pb⁴⁺(aq)+ 2e^- Pb²⁺(aq).

A) Pt(s)| H₂(g)| H⁺(aq)|| Pb⁴⁺(aq),Pb²⁺(aq)| Pt(s)

B) Pt(s)| H₂(g)| H⁺(aq)|| Pb⁴⁺(aq),Pb²⁺(aq)

C) Pb²⁺(aq),Pb⁴⁺(aq)|| H⁺(aq)| H₂(g)| Pt(s)

D) Pt(s)| Pb²⁺(aq),Pb⁴⁺(aq)|| H⁺(aq)| H₂(g)| Pt(s)

E) H₂(g)| H⁺(aq)|| Pb²⁺(aq),Pb⁴⁺(aq)

Q2) All of the following statements concerning voltaic cells are true EXCEPT

A) a salt bridge allows cations and anions to move between the half-cells.

B) electrons flow from the cathode to the anode in the external circuit.

C) oxidation occurs at the anode.

D) a voltaic cell can be used as a source of energy.

E) a voltaic cell consists of two-half cells.

Q3) Explain the function of a salt bridge in a voltaic cell.

Page 22

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Chapter 21: Environmental Chemistry Earths

Environment,energy,and Sustainability

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Q1) Which of the following is not a greenhouse gas?

A) CO₂

B) CH₄

C) H₂O

D) N₂O

E) N₂

Q2) The largest known source of tar sands is found in

A) the United States of America.

B) United Arab Emirates.

C) Venezuela.

D) Saudi Arabia.

E) Canada.

Q3) Helium and argon are added continuously to the atmosphere.What is the primary source of these gases?

A) the solar wind

B) mining operations

C) burning of fossil fuels

D) radioactive decay

E) volcanic eruptions

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) The Ostwald process is an industrial method of producing ____ from the oxidation of ____.

A) nitric acid,ammonia

B) ammonia,nitric acid

C) ammonia,nitrogen

D) nitric acid,nitrogen

E) dinitrogen monoxide,nitrogen

Q2) Which list contains the three most abundant elements in the Earth's crust?

A) hydrogen,helium,and lithium

B) sodium,calcium,and iron

C) oxygen,nitrogen,and iron

D) carbon,nitrogen,and oxygen

E) oxygen,aluminum,and silicon

Q3) The oxidation state per each nitrogen,given in parentheses,is correct in all the following cases except

A) HN₃ (-3).

B) N₂O₃ (+3).

C) HNO₃ (+5).

D) NH₄⁺ (-3).

E) N₂O (+2).

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Chapter 23: The Chemistry of the Transition Elements

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Q1) EDTA^4-,a hexadentate ligand,is most effective at chelating metal ions when the pH is greater than 12.Explain why low pH decreases the chelating ability of the ligand.

Q2) Geometric isomers with a cis or trans configuration are possible for which of the following geometries?

1)octahedral

2)tetrahedral

3)square planar

A) 1 only

B) 2 only

C) 3 only

D) 1 and 3

E) 1,2,and 3

Q3) The calcium silicate formed in the blast furnace reduction of iron ore is called ____.

A) charge

B) gangue

C) pig iron

D) flux

E) slag

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Page 25

Chapter 24: Carbon: Not Just Another Element

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Q1) The process by which long chain hydrocarbons in petroleum are shortened is called

Q2) Which of the following compounds might be used to oxidize an aldehyde to a carboxylic acid?

A) H₂

B) Na

C) LiAlH₄

D) KMnO₄

E) NaBH₄

Q3) What are the two types of stereoisomers?

A) geometrical and optical

B) optical and positional

C) geometrical and positional

D) geometrical and functional group

E) chiral and optical

Q4) Draw Lewis structures for all possible isomers of C₃H₆O.

Q5) In vulcanized rubber,the polymer chains of natural rubber are cross-linked with sulfur atoms.The polymer chains stretch when stressed,but they return to their original shape when the stress is removed.Substances that behave this way are called

Page 26

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Chapter 25: Biochemistry

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Q1) How many five membered rings are found in a steroid molecule?

A) < 3

B) 3

C) 4

D) 5

E) > 5

Q2) When a drop of the fatty acid oleic acid (CH₃(CH₂)₇CH=CH(CH₂)<sub>7</sub >CO₂H)is added to water it forms a molecule thick layer on the surface of the water.What is the likely orientation of the acid on the water surface?

Q3) Which of the following functional groups is not found in carbohydrates (sugars)?

A) carboxylic acid

B) alcohol

C) ketone

D) aldehyde

E) ether

Q4) The oxygen that bridges two sugars in a disaccharide is known as a ___ bond.

Q5) What is the role of tRNA in protein synthesis?

Q6) The amide linkages in a protein and also called ___ bonds.

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Q7) A compound which contains both a positive and negative charge is called a ____.

Chapter 26: Nuclear Chemistry

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Sample Questions

Q1) The half-life of ⁴²K is 12.5 h.How much will remain after 83 h if the original sample contained 256 g of ⁴²K?

A) 22 g

B) 2.6 g

C) 15 g

D) 20 g

E) 14 g

Q2) Explain the treatment named boron neutron capture therapy (BNCT).

Q3) Which particle has the same mass as a beta particle?

A) a neutron

B) a proton

C) a gamma ray

D) an alpha particle

E) a positron

Q4) All isotopes with atomic number greater than ____ are radioactive.

A) 43

B) 80

C) 86

D) 83

E) 90

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