Principles of Chemistry Exam Bank
Course Introduction
Principles of Chemistry offers a comprehensive introduction to the fundamental concepts of chemistry, including atomic structure, molecular bonding, stoichiometry, thermodynamics, chemical equilibria, and reaction kinetics. This course emphasizes the structure and properties of matter, the behavior of gases, solutions, and acids and bases, and the basic principles underlying chemical reactions. Through a combination of theoretical lectures and practical laboratory exercises, students develop the analytical skills and scientific reasoning necessary to understand and predict chemical phenomena in both laboratory and real-world contexts.
Recommended Textbook
Principles of General Chemistry 2nd Edition by Martin Silberberg
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23 Chapters
1830 Verified Questions
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Page 2
Chapter 1: Keys to the Study of Chemistry
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Sample Questions
Q1) The distance between carbon atoms in ethylene is 134 picometers.Which of the following expresses that distance in meters?
A)1.34 \(\times\) 10<sup>-13</sup> m
B)1.34 \(\times\) 10<sup>-12</sup> m
C)1.34 \(\times\) 10<sup>-10</sup> m
D)1.34 \(\times\) 10<sup>-7</sup> m
E)1.34 \(\times\) 10<sup>-6</sup> m
Answer: C
Q2) The ripening of fruit,once picked,is an example of physical change.
A)True
B)False
Answer: False
Q3) The mass of a sample is 550 milligrams.Which of the following expresses that mass in kilograms?
A)5.5 \(\times\) 10<sup>8</sup> kg
B)5.5 \(\times\) 10<sup>5</sup> kg
C)5.5 \(\times\) 10<sup>-4</sup> kg
D)5.5 \(\times\) 10<sup>-6</sup> kg
E)5.5 \(\times\) 10<sup>-1</sup> kg
Answer: C
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Chapter 2: The Components of Matter
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Sample Questions
Q1) Determine the molecular mass of iron (III)bromide hexahydrate,a substance used as a catalyst in organic reactions.
A)403.65 amu
B)355.54 amu
C)317.61 amu
D)313.57 amu
E)295.56 amu
Answer: A
Q2) What is the name of IF<sub>7</sub>?
A)iodine fluoride
B)iodic fluoride
C)iodine heptafluoride
D)heptafluoroiodide
E)heptafluorine iodide
Answer: C
Q3) Name the three important "laws" that were accounted for by Dalton's atomic theory. Answer: Laws of conservation of mass;definite composition;multiple proportions
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4
Chapter 3: Stoichiometry of Formulas and Equations
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Sample Questions
Q1) One mole of O<sub>2</sub> has a mass of 16.0 g.
A)True
B)False
Answer: False
Q2) A compound containing chromium and silicon contains 73.52 mass percent chromium.Determine its empirical formula.
A)CrSi<sub>3</sub>
B)Cr<sub>2</sub>Si<sub>3</sub>
C)Cr<sub>3</sub>Si
D)Cr<sub>3</sub>Si<sub>2</sub>
E)Cr<sub>2</sub>S
Answer: D
Q3) Aluminum metal dissolved in hydrochloric acid as follows: 2Al(s)+ 6HCl(aq) \(\to\) 2AlCl<sub>3</sub>(aq)+ 3H<sub>2</sub>(g)
a.What is the minimum volume of 6.0 M HCl(aq)needed to completely dissolve 3.20 g of aluminum in this reaction?
b.What mass of AlCl<sub>3</sub> would be produced by complete reaction of 3.20 g of aluminum?
Answer: a.59.3 mL
b.15.8 g
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Chapter 4: Three Major Classes of Chemical Reactions
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Sample Questions
Q1) Select the classification for the following reaction.
Fe<sup>2+</sup>(aq)+ 2OH<sup>-</sup>(aq) \(\to\) Fe(OH)<sub>2</sub>(s)
A)precipitation
B)acid-base
C)redox
D)decomposition
E)None of these choices is correct.
Q2) Identify the oxidizing agent in the following redox reaction.
Hg<sup>2+</sup>(aq)+ Cu(s) \(\to\) Cu<sup>2+</sup>(aq)+ Hg(l)
A)Hg<sup>2+</sup>(aq)
B)Cu(s)
C)Cu<sup>2+</sup>(aq)
D)Hg(l)
E)Hg<sup>2+</sup>(aq)and Cu<sup>2+</sup>(aq)
Q3) In a redox reaction,the reducing agent undergoes loss of electrons.
A)True
B)False
Q4) A combination reaction may also be a displacement reaction.
A)True
B)False
Page 6
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Chapter 5: Gases and the Kinetic-Molecular Theory
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Sample Questions
Q1) Dr.I.M.A.Brightguy adds 0.1727 g of an unknown gas to a 125-mL flask.If Dr.B finds the pressure to be 736 torr at 20.0°C,is the gas likely to be methane,CH<sub>4</sub>,nitrogen,N<sub>2</sub>,oxygen,O<sub>2</sub>,neon,Ne,or argon,Ar?
A)CH<sub>4</sub>
B)N<sub>2</sub>
C)Ne
D)Ar
E)O<sub>2</sub>
Q2) "The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ Law.
A)Charles'
B)Boyle's
C)Amontons'
D)Avogadro's
E)Gay-Lussac's
Q3) A 255-mL gas sample weighing 0.292 g is at 52,810 Pa and 127°C.
a.How many moles of gas are present?
b.What is the molar mass of the gas?
Q4) State Avogadro's Law.
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Chapter 6: Thermochemistry: Energy Flow and Chemical Change
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Sample Questions
Q1) When Karl Kaveman adds chilled grog to his new granite mug,he removes 10.9 kJ of energy from the mug.If it has a mass of 625 g and was at 25°C,what is its new temperature? Specific heat capacity of granite = 0.79 J/(g·K)
A)3°C
B)14°C
C)22°C
D)47°C
E)None of these choices is correct.
Q2) Which one of the following statements about standard states is incorrect?
A)The standard state of a solid compound is the pure solid.
B)The standard state of a liquid compound is the pure liquid.
C)The standard state of a gaseous compound is the gas at a pressure of 1 atmosphere.
D)The standard state of an aqueous solute is a saturated solution in water.
E)The standard state of an element is the form in which it is stable at 1 atm and a specified temperature,usually 25°C.
Q3) Although internal energy (E)is more fundamental and conceptually easier than enthalpy (H),in most chemical applications \(\Delta\)H is more relevant and useful than \(\Delta\)E.Why?
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Chapter 7: Quantum Theory and Atomic Structure
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Sample Questions
Q1) a.What is the frequency of microwave radiation which has a wavelength of 10.7 cm?
b.What is the energy of one photon of this radiation?
Q2) For the following orbitals,state the values of n,l and m<sub>l</sub> which apply,and draw a sketch showing the shape and orientation of the orbital.
a.3s
b.2p<sub>x </sub>
Q3) Platinum,which is widely used as a catalyst,has a work function \(\phi\) (the minimum energy needed to eject an electron from the metal surface)of 9.05 \(\times\) 10<sup>-19</sup> J.What is the longest wavelength of light which will cause electrons to be emitted?
A)2.196 \(\times\) 10<sup>-7</sup> m
B)4.553 \(\times\) 10<sup>-6</sup> m
C)5.654 \(\times\) 10<sup>2</sup> m
D)1.370 \(\times\) 10<sup>15</sup> m
E)> 10<sup>6</sup> m
Q4) Line spectra are characteristic of atoms in the gas phase.
A)True
B)False
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Chapter 8: Electron Configuration and Chemical Periodicity
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Sample Questions
Q1) Select the element with the least metallic character.
A)Sn
B)Sr
C)Tl
D)Ge
E)Ga
Q2) The maximum number of electrons in an atom with the same value of n is 2n<sup>2</sup>.
A)True
B)False
Q3) The ____________________ quantum numbers are associated with the energy of an electron in a many-electron atom.
A)n and l
B)n and m<sub>l</sub>
C)l and m<sub>l</sub>
D)n and m<sub>s</sub>
E)n,l and m<sub>l</sub>
Q4) Define what is meant by electron affinity,and write a balanced chemical equation to represent the relevant process for element Y.
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Chapter 9: Models of Chemical Bonding
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Sample Questions
Q1) Describe in brief how electronegativity values can be used to predict the percent ionic character of a bond between two atoms.
Q2) Arrange aluminum,nitrogen,phosphorus and indium in order of increasing electronegativity.
A)Al < In < N < P
B)Al < In < P < N
C)In < Al < P < N
D)In < P < Al < N
E)None of these orders is correct.
Q3) Which of the following contains ionic bonding?
A)CO
B)SrF<sub>2</sub>
C)Al
D)OCl<sub>2</sub>
E)HCl
Q4) The more C-O and O-H bonds there are in a substance,the greater will be the amount of heat released when a fixed mass of the substance is burned.
A)True
B)False
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Chapter 10: The Shapes of Molecules
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Sample Questions
Q1) Draw all important resonance structures of the nitrate ion,NO<sub>3</sub><sup></sup>
Q2) What is the molecular shape of ClCN as predicted by the VSEPR theory? (Carbon is the central atom. )
A)linear
B)bent
C)angular
D)trigonal
E)None of these choices is correct.
Q3) In which one of the following is the best Lewis structure a resonance structure?
A)SO<sub>3</sub>
B)BF<sub>3</sub>
C)I<sub>3</sub><sup>-</sup>
D)SCO (C = central atom)
E)SO<sub>3</sub><sup>2-</sup>
Q4) Name and outline the concept which is introduced when more than one valid Lewis structure can be drawn for a given molecule or ion.Use appropriate diagrams of the formate ion (HCO<sub>2</sub><sup>-</sup>,carbon is the central atom)to illustrate.
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Page 12
Chapter 11: Theories of Covalent Bonding
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Sample Questions
Q1) Explain what is meant by a node (or nodal plane)in a molecular orbital and draw sketches of the following orbitals,indicating at least one nodal plane in each one.
a.a \(\sigma\)* orbital b.a \(\pi\)* orbital
Q2) In not more than two sentences,explain when and why chemists make use of the concept of hybridization.
Q3) In applying molecular orbital theory,the bond order is calculated in the same way as with Lewis structures.
A)True
B)False
Q4) Sketch the shapes of the \(\sigma\)<sub>1</sub><sub>s</sub> and \(\sigma\)<sub>1</sub><sub>s</sub>* molecular orbitals formed by the overlap of two hydrogen 1s atomic orbitals.
Q5) Explain what is meant by the term "bond order" and describe how it can be calculated using the information in a molecular orbital energy level diagram.
Q6) What type of hybridization is needed to explain why ethyne (acetylene,C<sub>2</sub>H<sub>2</sub>),is linear?
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Page 13
Chapter 12: Intermolecular Forces: Liquids,solids,and Phase Changes
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Sample Questions
Q1) Which one of the following substances does not exist in the indicated solid type?
A)graphite - network
B)Na - metallic
C)SiO<sub>2</sub> - molecular
D)NaCl - ionic
E)diamond - network
Q2) The energy needed to increase the surface area of a liquid is
A)capillary action.
B)surface tension.
C)viscosity.
D)cohesion.
E)specific elasticity.
Q3) a.Explain what is meant by the term "unit cell".
b.Copper metal has a face-centered cubic unit cell.The edge length of the unit cell is 361 pm,and the atomic weight of copper is 63.55 amu.Calculate the density of the copper in g/cm<sup>3</sup>.
(1 amu = 1.661 \(\times\) 10<sup>-24</sup> g. )
c.From the data in (b),calculate the radius of a copper atom in pm.
Q4) How do the electrical properties of semiconductors differ from those of metals?
Page 14
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Chapter 13: The Properties of Solutions
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Sample Questions
Q1) Predict the van't Hoff factor (i)for each of the following solutes: a.CaCl<sub>2</sub> <sub> </sub>b.Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> <sub> </sub>c.NH<sub>4</sub>Cl
Q2) Octane and nonane are liquids which are components of gasoline.Their vapor pressures at 25°C are 13.9 torr and 4.7 torr,respectively.What is the vapor pressure of a mixture consisting of 1 mole of each of these compounds?
Q3) How many moles of solute particles are present in 100.0 mL of 2.50 M (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub>?
A)0.100 mol
B)0.250 mol
C)0.500 mol
D)0.750 mol
E)l.00 mol
Q4) Heats of solution may be either positive or negative. A)True
B)False
Q5) A 50.0 % (w/w)solution of sulfuric acid (H<sub>2</sub>SO<sub>4</sub>)in water has a density of 1.395 g/mL.What is its molarity?
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Chapter 14: The Main-Group Elements: Applying Principles of
Bonding and Structure
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Sample Questions
Q1) Predict the products for the reaction of the following set of reactants.
Ca(s)+ H<sub>2</sub>(g) \(\to\)
A)CaH(s)
B)CaH<sub>2</sub>(s)
C)Ca<sub>2</sub>H<sub>3</sub>(s)
D)Ca<sub>3</sub>H<sub>2</sub>(s)
E)None of these choices is correct.
Q2) Consider the oxides XO<sub>2</sub>,where X is one of the first 20 elements.Identify X in each of the following cases:
a.XO<sub>2</sub> is a natural component of the atmosphere,whose buildup is implicated in climate change.
b.XO<sub>2</sub> is a toxic,brown gas which is a serious air pollutant.
c.XO<sub>2</sub> is a colorless,toxic gas formed during the combustion of coal.
d.XO<sub>2</sub> is network solid;the element X itself is also a network solid.
Q3) The nitrate anion is
A)a strong acid.
B)a strong base.
C)amphoteric.
D)a strong reducing agent.
E)a strong oxidizing agent.
Page 16
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Chapter 15: Organic Compounds and the Atomic Properties of
Carbon
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Sample Questions
Q1) Draw and name two non-alkenes with the formula C<sub>4</sub>H<sub>8</sub>.
Q2) a.Draw two different structures with the molecular formula C<sub>2</sub>H<sub>6</sub>O.
b.Name the functional group in each structure.
c.Which one will have the higher boiling point,and why?
Q3) A characteristic reaction of alkenes is addition.
A)True
B)False
Q4) One characteristic of the monomers that form condensation polymers that is not common in monomers which form addition polymers is
A)the presence of pi bonds.
B)the presence of two functional groups.
C)the presence of alkyl side chains.
D)the ability to form free radicals.
E)the presence of sulfur atoms.
Q5) Carboxylic acids are weak acids.
A)True
B)False
Q6) Draw the structure of trans-5-methyl-3-heptene.
Q7) Draw and name all stable molecules with the formula Page 17
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Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions
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Sample Questions
Q1) An elementary reaction is a simple,one-step process.
A)True
B)False
Q2) A chemical reaction of the general type
A \(\to\) 2B is first-order,with a rate constant of 1.52 \(\times\) 10<sup>-4</sup> s<sup>-1</sup>.
a.Calculate the half-life of A.
b.Assuming the initial concentration of A is 0.067 mol L<sup>-1</sup>,calculate the time needed for the concentration to fall to 0.010 mol L<sup>-1</sup>.
Q3) Sucrose decomposes to fructose and glucose in acid solution.When ln [sucrose] is plotted vs.time,a straight line with slope of -0.208 hr<sup>-1</sup> results.What is the rate law for the reaction?
A)Rate = 0.208 hr<sup>-1</sup> [sucrose]<sup>2</sup>
B)Rate = 0.208 hr<sup>-1</sup> [sucrose]
C)Rate = 0.0433 hr [sucrose]<sup>2</sup>
D)Rate = 0.0433 hr [sucrose]
E)Rate = 0.208 mol L<sup>-1</sup>hr<sup>-1</sup> [sucrose]<sup>0</sup>
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Chapter 17: Equilibrium: the Extent of Chemical Reactions
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Q1) If Q > K,more products need to be formed as the reaction proceeds to equilibrium.
A)True
B)False
Q2) In order to write the correct mass-action expression for a reaction one must
A)know the kinetic rate law for the reaction.
B)know the mechanism for the reaction.
C)have a properly balanced chemical equation.
D)have values for the concentrations of the reactants.
E)know the limiting reactant.
Q3) Unless \(\Delta\)H°<sub>rxn</sub> = 0,a change in temperature will affect the value of the equilibrium constant K<sub>c</sub>.
A)True
B)False
Q4) Although a system may be at equilibrium,the rate constants of the forward and reverse reactions will in general be different.
A)True
B)False
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Chapter 18: Acid-Base Equilibria
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Q1) A 1.25 M solution of the weak acid HA is 9.2% dissociated.What is the pH of the solution?
A)0.64
B)0.94
C)1.13
D)2.16
E)None of these choices is correct.
Q2) A solution of sodium acetate (CH<sub>3</sub>COONa)in water is weakly basic.
A)True
B)False
Q3) Which of the following is the strongest acid?
A)CH<sub>3</sub>COOH
B)HF
C)H<sub>3</sub>PO<sub>4</sub>
D)H<sub>2</sub>SO<sub>3</sub>
E)HI
Q4) Consider the reaction:
BF<sub>3</sub> + F<sup>-</sup> \(\to\) BF<sub>4</sub><sup>-</sup> <sup> </sup>Can this ever be considered to be an acid-base reaction? Support your answer with appropriate arguments.
Page 21
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Chapter 19: Ionic Equilibria in Aqueous Systems
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Q1) When a strong acid is titrated with a strong base,the pH at the equivalence point
A)is greater than 7.0.
B)is equal to 7.0.
C)is less than 7.0,but is not 3.5.
D)is equal to the pK<sub>a</sub> of the acid.
E)is equal to 3.5.
Q2) Calculate the solubility of magnesium sulfate,MgSO<sub>4</sub>,when placed into a 0.10 M MgCl<sub>2</sub> solution.
K<sub>sp</sub> = 5.9 \(\times\) 10<sup>-3</sup>
A)4.2 \(\times\) 10<sup>-2</sup> M
B)5.9 \(\times\) 10<sup>-2</sup> M
C)7.7 \(\times\) 10<sup>-2</sup> M
D)3.5 \(\times\) 10<sup>-5</sup> M
E)3.5 \(\times\) 10<sup>-6</sup> M
Q3) Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.
A)True
B)False
Q4) Make a clear distinction between buffer range and buffer capacity.
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Chapter
Direction of Chemical Reactions
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Q1) For a chemical reaction to be spontaneous only at low temperatures,which of the following conditions must be met?
A)(\(\Delta\)S°·> 0,\(\Delta\)H° > 0)
B)(\(\Delta\)S° > 0,\(\Delta\)H° < 0)
C)(\(\Delta\)S° < 0,\(\Delta\)H° < 0)
D)(\(\Delta\)S° < 0,\(\Delta\)H° > 0)
E)(\(\Delta\)G° > 0)
Q2) Which relationship or statement best describes \(\Delta\)S° for the following reaction?
BaCl<sub>2</sub>(aq)+ Na<sub>2</sub>SO<sub>4</sub>(aq) \(\to\)
BaSO<sub>4</sub>(s)+ 2NaCl(aq)
A)(\(\Delta\)S° \(\approx\) 0)
B)(\(\Delta\)S° < 0)
C)(\(\Delta\)S° > 0)
D)(\(\Delta\)S° = \(\Delta\)H°/T)
E)More information is needed to make a reasonable prediction.
Q3) State the second and third laws of thermodynamics.
Q4) A chemical reaction has \(\Delta\)G° = 10.0 kJ and \(\Delta\)S° = 50.0 J/K
a.Calculate \(\Delta\)H° for this reaction at 25°C.
b.Could this reaction ever be spontaneous? Explain your answer.
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Chapter 21: Electrochemistry: Chemical Change and Electrical Work
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Q1) Consider the reaction
CuO(s)+ H<sub>2</sub>(g) \(\to\) Cu(s)+ H<sub>2</sub>O(l)
In this reaction,which substances are the oxidant and reductant,respectively?
A)CuO and H<sub>2</sub>
B)H<sub>2</sub> and CuO
C)CuO and Cu
D)H<sub>2</sub>O and H<sub>2</sub>
E)None of these choices is correct.
Q2) Oxidation occurs at the cathode of a galvanic cell,but at the anode of an electrolytic cell.
A)True
B)False
Q3) In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.
A)True
B)False
Q4) Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.
Page 24
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Chapter 22: The Transition Elements and Their Coordination Compounds
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Q1) Which of the following octahedral complexes should have the largest crystal field splitting energy,\(\Delta\)?
A)[Cr(H<sub>2</sub>O)<sub>6</sub>]<sup>3+</sup>
B)[Cr(SCN)<sub>6</sub>]<sup>3-</sup>
C)[Cr(NH<sub>3</sub>)<sub>6</sub>]<sup>3+</sup>
D)[Cr(CN)<sub>6</sub>]<sup>3-</sup>
E)[Cr(en)<sub>3</sub>]<sup>3+</sup> (en = ethylenediamine)
Q2) How many unpaired electrons will there be in a high-spin octahedral complex of Fe(II)?
A)0
B)2
C)4
D)6
E)None of these choices is correct.
Q3) All atoms of the first transition series of elements have the ground state electronic configuration [Ar]4s<sup>2</sup>3d<sup>x</sup>,where x is an integer from 1 to 10.
A)True
B)False
Q4) What is the difference between a coordination compound and a complex ion?
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Chapter 23: Nuclear Reactions and Their Applications
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Q1) Cesium-134 is a \(\beta\) emitter with a half-life of 2.0 years.How much of a 2.50-g sample of cesium-134 will remain after 10 years?
A)0.0024 g
B)0.078 g
C)0.25 g
D)0.50 g
E)None of these choices is correct.
Q2) Briefly explain the relationship between the rad and the rem as units of radiation dosage.
Q3) Write a complete,balanced equation to represent the beta decay of thallium-207.
Q4) A 7.85 \(\times\) 10<sup>-5</sup> mol sample of copper-61 emits 1.47 \(\times\) 10<sup>19</sup> positrons in 90.0 minutes.What is the decay constant for copper-61?
A)0.00230 h<sup>-1</sup>
B)0.00346 h<sup>-1</sup>
C)0.207 h<sup>-1</sup>
D)0.311 h<sup>-1</sup>
E)None of these choices is correct.
Q5) Write a complete,balanced equation to represent the alpha decay of radon-210.
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