Principles of Chemistry Final Test Solutions - 3674 Verified Questions

Course Introduction

Principles of Chemistry

Final Test Solutions

Principles of Chemistry provides a foundational understanding of the essential concepts and theories in chemistry, introducing students to atomic and molecular structure, chemical bonding, states of matter, stoichiometry, thermochemistry, and the periodic table. The course explores chemical reactions, equilibrium, acids and bases, and basic thermodynamics, emphasizing both the qualitative and quantitative aspects of chemical phenomena. Through lectures, laboratory experiments, and problem-solving sessions, students develop critical thinking and analytical skills necessary for further study in scientific disciplines.

Recommended Textbook

Chemistry The Central Science 14th Edition by Theodore E. Brown

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24 Chapters

3674 Verified Questions

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Page 2

Chapter 1: Introduction: Matter, energy, and Measurement

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Sample Questions

Q1) The density of silver is 10.5 g/cm³.A piece of silver with a mass of 61.3 g would occupy a volume of ________ cm³.

A)0.171

B)644

C)10.5

D)0.00155

E)5.84

Answer: E

Q2) The symbol for the element platinum is ________.

A)K

B)P

C)Pt

D)S

E)Ca

Answer: C

Q3) Temperature is a physical property that determines the direction of heat flow.

A)True

B)False

Answer: True

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Page 3

Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) How many total electrons are in the O^2- ion?

A)10

B)8

C)6

D)16

E)4

Answer: A

Q2) The charge on the manganese in the salt MnF₃ is ________.

A)1+

B)1-

C)2+

D)2-

E)3+

Answer: E

Q3) The possible oxidation numbers for iron are +1 and +2.

A)True

B)False

Answer: False

Q4) The formula for potassium sulfide is ________.

Answer: K₂S

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Chapter 3: Chemical Reactions and Reaction Stoichiometry

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Sample Questions

Q1) When a hydrocarbon burns in air,a component produced is ________.

A)oxygen

B)nitrogen

C)carbon

D)water

E)argon

Answer: D

Q2) Lithium and nitrogen react to produce lithium nitride: 6Li (s)+ N₂(g) 2Li₃N (s)

How many moles of lithium nitride are produced when 0.330 mol of lithium react in this fashion?

A)0.110

B)0.660

C)0.0550

D)0.990

E)0.165

Answer: A

Q3) What is the mass percent of C in carbonic acid (H₂CO₃).

Answer: 19.36

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag⁺(aq)+ Cl^- (aq) AgCl (s)

Silver chloride is virtually insoluble in water so that the reaction appears to go to completion.How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO₃ solution to completely precipitate the silver?

A)9.81

B)6.37 × 10^-5

C)0.218

D)0.102

E)0.633

Q2) Of the species below,only ________ is not an electrolyte.

A)HCl

B)Rb₂SO₄

C)Ar

D)KOH

E)NaCl

Q3) How many grams of an unknown substance with a molar mass of 40.0 are there in 500.0 mL of a 0.175 M solution of the unknown?

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Chapter 5: Thermochemistry

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Sample Questions

Q1) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________ J.

A)1900

B)77.8

C)145

D)1.43 × 10^-3

E)6.00

Q2) A 26.9 g rock rolls down the hill at a speed of 81.9 m/s .What is the kinetic energy of the rock?

A)90.2 J

B)145 J

C)0.950 J

D)90200 J

E)1450 J

Q3) Energy units include watts,volts,and newtons.

A)True

B)False

Q4) Coal contains hydrocarbons of high molecular weight as well as compounds containing ________,sulfur,or nitrogen.

Q5) ________ is defined as the energy used to move an object against a force.

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) A photon that has an energy of 8.63 × 10^-12 J would emit light at which wavelength (m)?

A)230

B)2.30 × 10^-14

C)2.30

D)3.48 × 10¹⁹

E)2.30 × 10^-5

Q2) In a hydrogen atom,an electron in a 1s orbital can ________ a photon,but cannot ________ a photon.

A)accept, absorb

B)absorb, accept

C)absorb, emit

D)emit, absorb

E)emit, accept

Q3) The wavelength of radio waves can be longer than a football field.

A)True

B)False

Q4) Which group is represented by a ns²np¹ valence shell electron configuration?

Q5) A line spectrum contains radiation of ________ wavelengths.

Page 8

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) ________ compounds in fireworks are responsible for the observed blue colors.

A)sodium

B)barium

C)calcium

D)copper

E)strontium

Q2) What is the coefficient of H₂O when the following equation is completed and balanced?

Ca (s)+ H₂O (l)

A)1

B)3

C)2

D)5

E)Ca(s)does not react with H₂O (l).

Q3) When electrons are removed from a lithium atom,they are removed first from which orbital?

Q4) Which element(s)in group VIIA are solids at room temperature?

Q5) Write a balanced equation for the reaction of sodium metal with water.

Q6) Write a balanced equation for the reaction of elemental chlorine with liquid water.

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) Based on the octet rule,iodine most likely forms an ________ ion.

A)I²⁺

B)I⁴⁺

C)I^4-

D)I⁺

E)I^-

Q2) Of the bonds below,________ is the least polar.

A)C-O

B)N-O

C)C-F

D)S-O

E)K-Br

Q3) Based on the octet rule,aluminum most likely forms an ________ ion.

A)Al³⁺

B)Al⁴⁺

C)Al^4-

D)Al⁺

E)Al^-

Q4) If more than one Lewis structure can be drawn then the molecule or ion is said to have ________ forms.

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) According to the Pauli exclusion principle,no more than ________ electrons with their spins paired can occupy a molecular orbital.

Q2) For a molecule with the formula AB₃,the molecular shape is ________.

A)linear, octahedral, or bent

B)linear, bent, or trigonal planar

C)linear, bent, or T-shaped

D)tetrahedral

E)trigonal planar, trigonal pyramidal, or T-shaped

Q3) What is the molecular shape of H₂O?

A)T-shaped

B)tetrahedral

C)linear

D)trigonal pyramidal

E)bent

Q4) Of the following molecules,only ________ is polar.

A)CCl₄

B)BCl₃

C)NCl₃

D)BeCl₂

E)Cl₂

Page 11

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Chapter 10: Gases

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Sample Questions

Q1) 760 torr is equivalent to ________ mm Hg.

A)380

B)4.78 × 10³

C)1

D)760

E)121

Q2) What volume (L)of NH₃ gas at STP is produced by the complete reaction of 7.5 g of H₂O according to the following reaction?

Mg₃N₂ (s)+ 6H₂O (l) 3Mg(OH)₂(aq)+

2NH₃ (g)

A)3.1

B)9.3

C)19

D)28

E)0.32

Q3) What is the rms speed (m/s)of oxygen molecules at 36.0 °C?

Q4) The ________ corrects the ideal gas law for the finite volume and attractive forces of gas molecules.

Q5) How many molecules are there in 4.00 L of oxygen gas at 500 °C and 50.0 torr?

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) Which of the following has London dispersion forces as its only intermolecular force?

A)NBr₃

B)CH₃COOH

C)SiCl₄

D)HBr

E)Cl₂O

Q2) Elemental iodine (I₂)is a solid at room temperature.What is the major attractive force that exists among different I₂ molecules in the solid?

A)London dispersion forces

B)dipole-dipole interactions

C)ionic-dipole interactions

D)covalent-ionic interactions

E)dipole-dipole attractions

Q3) In general,intramolecular forces determine the ________ properties of a substance and intermolecular forces determine its ________ properties.

Q4) The conversion of a solid to a liquid is called ________.

Q5) The initial discovery of a liquid crystal resulted from studies of a ________ derivative.

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) The process of ________ can produce an n-type semiconductor,which can greatly increase intrinsic conductivity.

A)melting

B)fusing

C)doping

D)mixing

E)infusing

Q2) The ________ for Ge shows it to be a semiconductor,because the gap between the filled lower and empty higher energy bands is relatively small.

A)molecular-orbital model

B)quantum mechanics model

C)atomic-orbital model

D)valence bond model

E)intermolecular model

Q3) Semiconductors are ________ conductive than metals because of a band gap.

Q4) Define a body-centered cubic lattice.

Q5) Polyethylene is formed by a condensation reaction.

A)True

B)False

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) What is the % by mass of sodium chloride in an aqueous solution that is 2.39 M and has a density of 1.01 g/mL?

A)2.36

B)13.8

C)7.83

D)140.

E)19.6

Q2) Which of the following statements is false?

A)Nonpolar liquids tend to be insoluble in polar liquids.

B)The weaker the attraction between the solute and solvent molecules, the greater the solubility.

C)Substances with similar intermolecular attractive forces tend to be soluble in one another.

D)The solubility of a gas increases in direct proportion to its partial pressure above the solution.

E)The solubility of gases in water decreases with increasing temperature.

Q3) What is the osmotic pressure (in atm)of a 0.015 M calcium chloride solution at 28 °C?

Q4) What is the osmotic pressure (in atm)of a 0.0255 M NaCl solution at 25.0 °C?

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Page 15

Chapter 14: Chemical Kinetics

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Sample Questions

Q1) What is the order of the reaction with respect to ClO₂? A)1

E)4

Q2) The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

A)True

B)False

Q3) Biological catalysts are referred to as ________.

Q4) Write the rate law for the reaction:

aA bB + cC.

Q5) The instantaneous rate of a reaction can be read directly from the graph of molarity versus time at any point on the graph.

A)True

B)False

Q6) According to the collision model,reaction rates are affected by reactant ________ and ________.

Page 16

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) If Reaction A + Reaction B = Reaction C,then K_c for Reaction C is

Q2) How is the reaction quotient used to determine whether a system is at equilibrium?

A)The reaction quotient must be satisfied for equilibrium to be achieved.

B)At equilibrium, the reaction quotient is undefined.

C)The reaction is at equilibrium when Q < K_eq.

D)The reaction is at equilibrium when Q > K_eq.

E)The reaction is at equilibrium when Q = K_eq.

Q3) If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature,________ must be converted to ________ for the system to reach equilibrium.

Q4) Define the reaction quotient.

Q5) Le Châtelier's principle states that if a system at equilibrium is disturbed,then more products are produced.

A)True

B)False

Q6) If the value for the equilibrium constant is much less than 1,then the equilibrium mixture contains mostly ________.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) An aqueous solution of a particular compound has pH = 7.46.The compound is

A)a weak base

B)a weak acid

C)a strong acid

D)a strong base

E)a salt

Q2) The conjugate base of H₂PO₄^- is ________.

A)H₃PO₄

B)HPO₄^2-

C)PO₄^3-

D)H₃O⁺

E)OH^-

Q3) Classify the following compounds as weak acids (W)or strong acids (S): benzoic acid nitric acid acetic acid

A)W W W

B)S S S

C)S W W

D)W S S

E)W S W

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Sample Questions

Q1) In which of the following aqueous solutions would you expect AgI to have the highest solubility?

A)pure water

B)0.050 M BaI₂

C)0.050 M NaI

D)0.050 M KI

E)0.010 M AgNO₃

Q2) A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution.The equivalence point is reached when 10.2 mL of the base is added.The concentration of acetic acid in the sample was ________ M.

A)0.365

B)0.175

C)0.119

D)0.0714

E)none of the above

Q3) CaCO₃ is very soluble in the presence of ________.

Q4) Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH? The K_a of HA is 1.77 × 10^-5.

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Chapter 18: Chemistry of the Environment

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Sample Questions

Q1) The most abundant component of air is ________.

Q2) The "scale" caused by hard water is ________.

A)calcium ions

B)sodium chloride

C)magnesium oxide

D)sodium ions

E)calcium carbonate

Q3) Ozone is a(n)________ of oxygen.

A)isomer

B)allotrope

C)isotope

D)resonance structure

E)atomic form

Q4) The majority of ozone that protects against the high energy radiation of the sun is found in the ________.

A)thermosphere

B)mesosphere

C)mesopause

D)stratosphere

E)troposphere

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Chapter 19: Chemical Thermodynamics

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Sample Questions

Q1) The value of G° at 25 °C for the decomposition of calcium chloride into its constituent elements, CaCl₂(s) Ca (s)+ Cl₂ (g) Is ________ kJ/mol.

A)-795.8

B)+795.8

C)+763.7

D)+748.1

E)-748.1

Q2) Of the following,only ________ is not a state function.

A)S

B)H

C)q

D)E

E)T

Q3) Which of the following has the largest entropy?

A)HI (g)

B)HBr (g)

C)HCl (g)

D)HCl (s)

E)HCl (l)

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Chapter 20: Electrochemistry

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Sample Questions

Q1) Which substance does not undergo oxidation or reduction in the reaction below?

Pb + PbO₂ + 2H₂SO₄ 2PbSO₄ + 2H₂O

A)Pb

B)H₂SO₄

C)PbO₂

D)PbSO₄

E)The reaction above is not a redox reaction

Q2) The half-reaction occurring at the anode in the balanced reaction shown below is ________. 3MnO₄^- (aq)+ 24H⁺ (aq)+ 5Fe (s) 3Mn²⁺ (aq)+ 5Fe³⁺ (aq)+ 12H₂O (l)

A)MnO₄^- (aq)+ 8H⁺ (aq)+ 5e^-

Mn²⁺ (aq)+ 4H₂O (l)

B)2MnO₄^- (aq)+ 12H⁺ (aq)+ 6e^- 2Mn²⁺ (aq)+ 3H₂O (l)

C)Fe (s) Fe³⁺ (aq)+ 3e^-

D)Fe (s) Fe²⁺ (aq)+ 2e^-

E)Fe²⁺ (aq) Fe³⁺ (aq)+ e^-

Q3) Define a coulomb.

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Page 22

Chapter 21: Nuclear Chemistry

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Sample Questions

Q1) The relative biological effectiveness (RBE)values of beta rays,gamma rays,and alpha rays are ________,respectively.

Q2) When ionizing radiation enters the body,what is the predominant free radical produced?

A)H

B)H₃O

C)protein

D)OH

E)H₂O

Q3) ⁴¹Ca decays by electron capture.The product of this reaction undergoes alpha decay.What is the product of this second decay reaction?

A)Ti

B)Ca

C)Ar

D)Cl

E)Sc

Q4) Carbon-11,fluorine-18,oxygen-15 and nitrogen-13 are all used in the clinical diagnostic technique known as ________.

Q5) What was the purpose of the Manhattan project?

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Chapter 22: Chemistry of the Nonmetals

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Sample Questions

Q1) Hydrogen can have oxidation states of ________.

A)+1 only

B)-1, 0, and +1

C)0 and +1 only

D)-1 and +1 only

E)0 only

Q2) The oxidation number of B in B₂O₃ is ________.

A)+3

B)+2

C)+1

D)+4

E)+5

Q3) Which one of the following is false concerning buckminsterfullerene?

A)It is the most recently discovered crystalline allotrope of carbon.

B)It consists of individual molecules like C₆₀and C₇₀.

C)It is a molecular form of carbon.

D)It is made up of Cl₂ molecules.

E)It is made up of molecules that resemble soccer balls.

Q4) Chains of silicate tetrahedra are called ________.

Q5) What noble gas is radioactive?

Page 24

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Chapter 23: Transition Metals and Coordination Chemistry

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Sample Questions

Q1) What is a siderophore?

Q2) Isomers whose ligands can bind directly to a metal or be outside the lattice are called ________.

A)linkage isomers

B)rotational isomers

C)coordination sphere isomers

D)geometric isomers

E)optical isomers

Q3) Name Na [Ru(H₂O)₂ (C₂O₄)₂].

Q4) The porphyrin compound that contains Mg (II)is called ________.

Q5) The transport of iron into bacteria is facilitated by the formation of the complex ________.

Q6) A compound that can occupy two coordination sites is a (an)________.

Q7) How many bonds can ethylenediamine form to a metal ion?

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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

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Sample Questions

Q1) How many chiral centers are there in CH₃CHCHCH₂CHBr₂?

A)0

B)1

C)2

D)3

E)4

Q2) Hydrocarbons containing only single bonds between the carbon atoms are called ________.

A)alkenes

B)alkynes

C)aromatics

D)alkanes

E)ketones

Q3) The aromas of different fruit are due to the chemical compounds known as ________.

Q4) Why is cyclopropane more reactive than propane?

Q5) Aldehydes are less reactive than ketones. A)True

B)False

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