General Chemistry I Exam Solutions
Course Introduction
General Chemistry I provides a comprehensive introduction to the fundamental principles of chemistry. The course covers essential topics such as atomic and molecular structure, periodic trends, chemical bonding, stoichiometry, states of matter, thermochemistry, and basic concepts in chemical reactions. Through a combination of lectures, laboratory experiments, and problem-solving exercises, students develop a solid foundation in chemical concepts and analytical techniques, preparing them for advanced study in chemistry and related scientific fields.
Recommended Textbook
Principles of General Chemistry 2nd Edition by Martin Silberberg
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23 Chapters
1830 Verified Questions
1830 Flashcards
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Chapter 1: Keys to the Study of Chemistry
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Sample Questions
Q1) Express 96,342 m using 2 significant figures.
A)9.60 \(\times\) 10<sup>4</sup> m
B)9.6 \(\times\) 10<sup>4</sup> m
C)9.60 \(\times\) 10<sup>-4</sup> m
D)9.6 \(\times\) 10<sup>-4</sup> m
E)96,000.m
Answer: B
Q2) You prepare 1000.mL of tea and transfer it to a 1.00 quart pitcher for storage.Which of the following statements is true?
A)The pitcher will be filled to 100% of its capacity with no tea spilled.
B)The pitcher will be filled to about 95% of its capacity.
C)The pitcher will be filled to about 50% of its capacity.
D)The pitcher will be completely filled and a small amount of tea will overflow.
E)The pitcher will be completely filled and most of the tea will overflow.
Answer: D
Q3) When applying the scientific method,it is important to avoid any form of hypothesis.
A)True
B)False
Answer: False
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Page 3
Chapter 2: The Components of Matter
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Sample Questions
Q1) The compound,BaO,absorbs water and carbon dioxide readily and is used to dry gases and organic solvents.What is its name?
A)barium oxide
B)barium(II)oxide
C)barium monoxide
D)baric oxide
E)barium peroxide
Answer: A
Q2) Who is credited with measuring the mass/charge ratio of the electron?
A)Dalton
B)Gay-Lussac
C)Thomson
D)Millikan
E)Rutherford
Answer: C
Q3) Modern studies have shown that the Law of Multiple Proportions is not valid.
A)True
B)False
Answer: False
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Page 4
Chapter 3: Stoichiometry of Formulas and Equations
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Sample Questions
Q1) In combustion analysis,the oxygen content of a substance is equal to the total oxygen in the CO<sub>2</sub> and H<sub>2</sub>O collected in the absorbers.
A)True
B)False
Answer: False
Q2) Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides)and dichlorine oxide (used as a bleach for wood,pulp and textiles).
SO<sub>2</sub>(g)+ 2Cl<sub>2</sub>(g) \(\to\)SOCl<sub>2</sub>(g)+
Cl<sub>2</sub>O(g)
If 0.400 mol of Cl<sub>2</sub> reacts with excess SO<sub>2</sub>,how many moles of Cl<sub>2</sub>O are formed?
A)0.800 mol
B)0.400 mol
C)0.200 mol
D)0.100 mol
E)0.0500 mol
Answer: C
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Page 5
Chapter 4: Three Major Classes of Chemical Reactions
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Sample Questions
Q1) A 0.00100 mol sample of Ca(OH)<sub>2</sub> requires 25.00 mL of aqueous HCl for neutralization according to the reaction below.What is the concentration of the HCl?
Equation: Ca(OH)<sub>2</sub>(s)+ 2HCl(aq) \(\to\) CaCl<sub>2</sub>(aq)+ H<sub>2</sub>O(l)
A)0.0200 M
B)0.0400 M
C)0.0800 M
D)4.00 \(\times\) 10<sup>-5</sup> M
E)None of these choices is correct.
Q2) In both of the following reactions,a precipitate is formed.Complete and balance the equations,showing the phases of the products.
a.BaCl<sub>2</sub>(aq)+ Na<sub>2</sub>SO<sub>4</sub>(aq) \(\to\)
b.Mg(NO<sub>3</sub>)<sub>2</sub>(aq)+ KOH(aq) \(\to\)
Q3) Which of the following is a strong base?
A)NH<sub>3</sub>
B)Ca(OH)<sub>2</sub>
C)Al(OH)<sub>3</sub>
D)B(OH)<sub>3</sub>
E)CH<sub>3</sub>OH
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Page 6
Chapter 5: Gases and the Kinetic-Molecular Theory
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Sample Questions
Q1) The rate of diffusion of a gas is inversely proportional to its molar mass.
A)True
B)False
Q2) A sample of an ideal gas has its volume doubled while its temperature remains constant.If the original pressure was 100 torr,what is the new pressure?
A)10 torr
B)50 torr
C)100 torr
D)200 torr
E)1000 torr
Q3) For a gas obeying Boyle's Law,a plot of V versus 1/P will give a straight line passing through the origin.
A)True
B)False
Q4) From the postulates of kinetic-molecular theory,it follows that the molecules of all gases at a given temperature have the same average kinetic energy.
A)True
B)False
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Chapter 6: Thermochemistry: Energy Flow and Chemical Change
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Sample Questions
Q1) a.Write a balanced equation for the combustion of benzene,C<sub>6</sub>H<sub>6</sub>(l)in oxygen.
b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation,\(\Delta\)H°<sub>f</sub> ,given the data: \(\Delta\)H°<sub>f</sub> [CO<sub>2</sub>(g)] = -394 kJ;\(\Delta\)H°<sub>f</sub> [H<sub>2</sub>O(l)] = -286 kJ
Q2) The reaction
2NaOH(aq)+ H<sub>2</sub>SO<sub>4</sub>(aq) \(\to\) Na<sub>2</sub>SO<sub>4</sub>(aq)+ 2H<sub>2</sub>O(l) was studied in a coffee cup calorimeter.100.mL portions of 1.00 M aqueous NaOH and H<sub>2</sub>SO<sub>4</sub>,each at 24.0°C,were mixed.The maximum temperature achieved was 30.6°C.Neglect the heat capacity of the cup and the thermometer,and assume that the solution of products has a density of exactly 1 g/mL and a specific heat capacity of 4.18 J/(g·K).
a.Calculate the heat of reaction,q,in J.
b.Calculate \(\Delta\)H,the heat (enthalpy)of reaction,in kJ/mol of Na<sub>2</sub>SO<sub>4</sub> produced.
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Page 8
Chapter 7: Quantum Theory and Atomic Structure
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Sample Questions
Q1) Who proposed the principle which states that one cannot simultaneously know the exact position and velocity of a particle?
A)Einstein
B)Planck
C)Heisenberg
D)Compton
E)de Broglie
Q2) Atomic orbitals developed using quantum mechanics
A)describe regions of space in which one is most likely to find an electron.
B)describe exact paths for electron motion.
C)give a description of the atomic structure which is essentially the same as the Bohr model.
D)allow scientists to calculate an exact volume for the hydrogen atom.
E)are in conflict with the Heisenberg Uncertainty Principle.
Q3) Line spectra are characteristic of atoms in the gas phase.
A)True
B)False
Q4) 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?
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Chapter 8: Electron Configuration and Chemical Periodicity
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Sample Questions
Q1) Which one of the following statements about orbital energies is incorrect?
A)In the hydrogen atom,the energy of an orbital depends only on the value of the quantum number n.
B)In many-electron atoms the energy of an orbital depends on both n and l.
C)Inner electrons shield outer electrons more effectively than do electrons in the same orbital.
D)The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect.
E)The energy of a given orbital increases as the nuclear charge Z increases.
Q2) "Each electron in an atom must have its own unique set of quantum numbers" is a statement of
A)the aufbau principle.
B)the Pauli exclusion principle.
C)Hund's rule.
D)the periodic law.
E)Heisenberg's principle.
Q3) State Hund's rule,and show how it applies to the ground state of phosphorus atoms.
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Chapter 9: Models of Chemical Bonding
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Sample Questions
Q1) Give a clear and concise definition of the term "electronegativity";i.e. ,what does it measure?
Q2) Ionic bonding typically occurs when a ______________ bonds with a
Q3) Describe in brief how electronegativity values can be used to predict the percent ionic character of a bond between two atoms.
Q4) Analysis of an unknown substance showed that it has a high boiling point and is brittle.It is an insulator as a solid but conducts electricity when melted.Which of the following substances would have those characteristics?
A)HCl
B)Al
C)KBr
D)SiF<sub>4</sub>
E)I<sub>2</sub>
Q5) The electrostatic energy of two charged particles is inversely proportional to the distance between them.
A)True
B)False
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Chapter 10: The Shapes of Molecules
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Sample Questions
Q1) Use VSEPR theory to predict the electron group arrangement around iodine,the central atom in the ion IF<sub>2</sub><sup>-</sup>.
A)octahedral
B)trigonal bipyramidal
C)tetrahedral
D)trigonal planar
E)bent
Q2) All possible resonance structures contribute equally to the resonance hybrid.
A)True
B)False
Q3) 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.
Q4) Boron never achieves an octet in any of its compounds.
A)True
B)False
Page 12
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Chapter 11: Theories of Covalent Bonding
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Sample Questions
Q1) In applying molecular orbital theory,the bond order is calculated in the same way as with Lewis structures.
A)True
B)False
Q2) The angles between sp<sup>2</sup> hybrid orbitals are 109.5°.
A)True
B)False
Q3) According to valence bond theory,which of the following molecules involves sp<sup>2</sup> hybridization of orbitals on the central atom? (central atom is bold)
A)C<sub>2</sub>H<sub>2</sub>
B)C<sub>2</sub>H<sub>4</sub>
C)C<sub>2</sub>H<sub>6</sub>
D)CO<sub>2</sub>
E)H<sub>2</sub>O
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) In one sentence state how molecular orbitals are usually obtained.
Q6) In one sentence state the basic principle of valence bond theory.
Page 13
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Chapter 12: Intermolecular Forces: Liquids,solids,and Phase Changes
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Sample Questions
Q1) Which of the following atoms should have the greatest polarizability?
A)F
B)Br
C)Po
D)Pb
E)He
Q2) The strongest intermolecular interactions between hydrogen fluoride (HF)molecules arise from
A)dipole-dipole forces.
B)London dispersion forces.
C)hydrogen bonding.
D)ion-dipole interactions.
E)ionic bonds.
Q3) Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first.
A)C<sub>7</sub>H<sub>16</sub>,C<sub>5</sub>H<sub>12</sub>
B)CCl<sub>4</sub>,CBr<sub>4</sub>
C)H<sub>2</sub>O,H<sub>2</sub>S
D)CH<sub>3</sub>CH<sub>2</sub>OH,CH<sub>3</sub>-O-CH<sub>3</sub>
E)Xe,Kr
Page 14
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Chapter 13: The Properties of Solutions
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Sample Questions
Q1) Calculate the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L.
A)0.28 M
B)0.91 M
C)1.1 M
D)3.1 M
E)3.9 M
Q2) Aqueous ammonia is commercially available in a solution that is 28% (w/w)ammonia.What is the mole fraction of ammonia in such a solution?
A)0.017
B)0.023
C)0.012
D)0.24
E)0.29
Q3) The solubility of gases in water increases with increase in the pressure of the gas.
A)True
B)False
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15
Chapter 14: The Main-Group Elements: Applying Principles of Bonding
and Structure
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Sample Questions
Q1) What are the products of the reaction of strontium hydride and water?
SrH<sub>2</sub>(s)+ H<sub>2</sub>O(l) \(\to\)
A)Sr<sup>2+</sup>(aq)+ H<sub>2</sub>(g)+ O<sub>2</sub>(g)
B)Sr<sup>2+</sup>(aq)+ H<sub>2</sub>(g)+ OH<sup>-</sup>(aq)
C)Sr(s)+ H<sub>2</sub>(g)+ OH<sup>-</sup>(aq)
D)Sr(s)+ H<sub>3</sub>O<sup>+</sup>(aq)
E)None of these choices is correct.
Q2) Predict the products for the following set of reactants.
Cs(s)+ Br<sub>2</sub>(l) \(\to\)
A)CsBr(s)
B)CsBr<sub>2</sub>(s)
C)CsBr(l)
D)CsBr<sub>2</sub>(l)
E)Cs<sub>2</sub>Br(s)
Q3) Which of the following oxides will be the most acidic?
A)Al<sub>2</sub>O<sub>3</sub>
B)Ga<sub>2</sub>O<sub>3</sub>
C)In<sub>2</sub>O<sub>3</sub>
D)Tl<sub>2</sub>O<sub>3</sub>
E)None of these oxides is acidic.
Page 16
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Chapter 15: Organic Compounds and the Atomic Properties of Carbon
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Sample Questions
Q1) A characteristic reaction of alkenes is addition.
A)True
B)False
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) Ethane (C<sub>2</sub>H<sub>6</sub>)is much more reactive than disilane (Si<sub>2</sub>H<sub>6</sub>).
A)True
B)False
Q4) The carbon atoms in a molecule of cyclohexane lie in the same plane.
A)True
B)False
Q5) The backbone of protein molecules consists of repeating N-C-C-O units.
A)True
B)False
Page 17
Q6) Given that each 3-base sequence in DNA is a "code word" for a particular amino acid,how many different code words are possible using a 3-base sequence and the bases available in DNA?
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Page 18
Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions
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Sample Questions
Q1) Is a bimolecular reaction necessarily second-order? Is a second-order reaction necessarily bimolecular? Answer,with explanations and clarifications.
Q2) What is the molecularity of the following elementary reaction? NH<sub>2</sub>Cl(aq)+ OH<sup>-</sup>(aq) \(\to\)NHCl<sup>-</sup>(aq)+ H<sub>2</sub>O(l)
A)unimolecular
B)bimolecular
C)termolecular
D)tetramolecular
E)The reaction order must be known before molecularity can be determined.
Q3) An elementary reaction is a simple,one-step process. A)True
B)False
Q4) A transition state is a species (or state)corresponding to an energy maximum on a reaction energy diagram.
A)True
B)False
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Chapter 17: Equilibrium: the Extent of Chemical Reactions
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Sample Questions
Q1) For some gas-phase reactions,K<sub>p</sub> = K<sub>c</sub>.
A)True
B)False
Q2) 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
Q3) 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.
Q4) When a reaction system reaches equilibrium,the forward and reverse reactions stop.
A)True
B)False
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20
Chapter 18: Acid-Base Equilibria
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Q1) The substance H<sub>2</sub>SO<sub>3</sub> is considered
A)a weak Arrhenius base.
B)a strong Arrhenius acid.
C)a strong Arrhenius base.
D)a neutral compound.
E)a weak Arrhenius acid.
Q2) Ammonium chloride is used as an electrolyte in dry cells.Which of the following statements about a 0.10 M solution of NH<sub>4</sub>Cl,is correct?
A)The solution is weakly basic.
B)The solution is strongly basic.
C)The solution is neutral.
D)The solution is acidic.
E)The values for K<sub>a</sub> and K<sub>b</sub> for the species in solution must be known before a prediction can be made.
Q3) Define an acid according to the Lewis theory.Write a balanced equation in support of this definition,in which the acid is neither an Arrhenius acid nor a Brønsted-Lowry acid.
Q4) Define an acid according to the Arrhenius theory,and write a balanced equation to support this definition.
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Page 21
Chapter 19: Ionic Equilibria in Aqueous Systems
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Q1) What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which
[H<sub>2</sub>PO<sub>4</sub><sup>-</sup>] = [HPO<sub>4</sub><sup>2-</sup>] = 0.35 M?
A)The pH will increase slightly.
B)The pH will increase significantly.
C)The pH will decrease slightly.
D)The pH will decrease significantly.
E)Since it is a buffer solution,the pH will not be affected.
Q2) A solution is prepared by adding 100 mL of 0.2 M hydrochloric acid to 100 mL of 0.4 M sodium formate.Is this a buffer solution,and if so,what is its pH?
A)It is a buffer,pH > pK<sub>a</sub> of formic acid.
B)It is a buffer,pH < pK<sub>a</sub> of formic acid.
C)It is a buffer,pH = pK<sub>a</sub> of formic acid.
D)It is a buffer,pH = pK<sub>b</sub> of sodium formate.
E)Since hydrochloric acid is a strong acid,this is not a buffer.
Q3) What is the pH of 375 mL of solution containing 0.150 mol of propenoic acid (HA)and 0.250 mol of sodium propenoate (NaA)? (K<sub>a</sub> for propenoic acid is 5.52 \(\times\) 10<sup>-5</sup>. )
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Page 22
Chapter
Direction of Chemical Reactions
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Q1) 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.
Q2) Which relationship or statement best describes \(\Delta\)S° for the following reaction?
CaO(s)+ CO<sub>2</sub>(g) \(\to\) CaCO<sub>3</sub>(s)
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) A chemical reaction has \(\Delta\)H° = 42.8 kJ and \(\Delta\)S° = 92.5 J/K,at 25°C.Calculate the temperature at which \(\Delta\)G° = 0.State any approximation involved in your calculation.
Page 23
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Chapter 21: Electrochemistry: Chemical Change and Electrical Work
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Q1) Which one of the following statements about electrochemical cells is correct?
A)In a salt bridge,current is carried by cations moving toward the anode,and anions toward the cathode.
B)In the external wire,electrons travel from cathode to anode.
C)The anode of a voltaic cell is labeled minus (-).
D)Oxidation occurs at the cathode,in an electrolytic cell.
E)None of these statements is correct.
Q2) Which,if any,of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°<sub>Fe</sub> = -0.44 V;all E° values refer to the M<sup>2+</sup>/M half-cell reactions.
A)copper,Cu,E° = 0.15 V
B)cobalt,Co,E° = -0.28 V
C)chromium,Cr,E° = -0.74 V
D)tin,Sn,E° = -0.14 V
E)None of these metals would be capable of acting as a sacrificial anode with iron.
Q3) In the shorthand notation for cells,a single vertical line represents a salt bridge. A)True
B)False
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Chapter 22: The Transition Elements and Their Coordination Compounds
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Q1) a.How many unpaired 3d electrons will there be in (i)high and (ii)low-spin complexes of Co(II)?
b.How can high and low-spin complexes be recognized and distinguished experimentally?
Q2) In the compound K[Co(C<sub>2</sub>O<sub>4</sub>)<sub>2</sub>(H<sub>2</sub>O)<sub>2</sub>] (where C<sub>2</sub>O<sub>4</sub><sup>2-</sup> = oxalate)the oxidation number and coordination number of cobalt are,respectively:
A)-1 and 4
B)-1 and 6
C)3 and 4
D)3 and 6
E)1 and 6
Q3) Tetrahedral complexes can exhibit both optical and linkage isomerism.
A)True
B)False
Q4) The compound Rh(CO)(H)(PH<sub>3</sub>)<sub>2</sub> forms cis and trans isomers.Use this information to predict the geometry of this complex,and draw the geometric isomers.
Page 25
Q5) What geometry is particularly common for complexes of d<sup>10</sup> metal ions?
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Chapter 23: Nuclear Reactions and Their Applications
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Q1) A 9.52 \(\times\) 10<sup>-5</sup> mol sample of rubidium-86 emits 8.87 \(\times\) 10<sup>16</sup> \(\beta\) particles in one hour.What is the half-life of rubidium-86?
A)2.23 \(\times\) 10<sup>-3</sup> h
B)1.55 \(\times\) 10<sup>-3</sup> h
C)448 h
D)645 h
E)None of these choices is correct.
Q2) Write a complete,balanced equation to represent the electron capture decay of argon-37.
Q3) Write a complete,balanced equation to represent the formation of manganese-55 by the beta decay of another nuclide.
Q4) Most foodstuffs contain natural,radioactive isotopes.
A)True
B)False
Q5) Briefly explain the relationship between the rad and the rem as units of radiation dosage.
Q6) Radioactive decay follows zero-order kinetics.
A)True
B)False
Page 27
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