Foundations of Chemistry Solved
Exam Questions
Course Introduction
Foundations of Chemistry provides a comprehensive introduction to the fundamental principles of chemistry, including the structure of atoms and molecules, periodic properties, chemical bonding, stoichiometry, states of matter, chemical reactions, and thermochemistry. Emphasis is placed on developing a conceptual understanding and applying quantitative problem-solving skills to real-world chemical phenomena, preparing students for advanced study in chemistry and related scientific fields.
Recommended Textbook
Principles of Chemistry A Molecular Approach 3rd Edition by Nivaldo J. Tro
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Chapter 1: Matter, Measurement, and Problem Solving
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Sample Questions
Q1) Which of the following is an example of physical change?
A)Sugar is dissolved in water.
B)Coffee is brewed.
C)Dry ice sublimes.
D)Ice (solid water)melts.
E)All of these are examples of physical change.
Answer: E
Q2) A student performs an experiment to determine the density of a sugar solution.She obtains the following results: 4.11 g/mL,4.81 g/mL,4.95 g/mL,3.75 g/mL.If the actual value for the density of the sugar solution is 4.75 g/mL,which statement below best describes her results?
A)Her results are precise,but not accurate.
B)Her results are accurate,but not precise.
C)Her results are both precise and accurate
D)Her results are neither precise nor accurate.
E)It isn't possible to determine with the information given. Answer: D
Q3) Define matter.
Answer: Matter is anything that occupies space and has mass.
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Chapter 2: Atoms and Elements
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Sample Questions
Q1) The mass number is equal to
A)the sum of the sum of the electrons and protons.
B)the sum of the sum of the neutrons and electrons.
C)the sum of the number of protons,neutrons,and electrons.
D)the sum of the number of protons and neutrons.
Answer: D
Q2) Which of the following statements is false according to Dalton's Atomic Theory?
A)Atoms combine in simple whole number ratios to form compounds.
B)All atoms of chlorine have identical properties that distinguish them from other elements.
C)One carbon atom will combine with one oxygen atom to form a molecule of carbon monoxide.
D)Atoms of sodium do not change into another element during chemical reaction with chlorine.
E)An atom of nitrogen can be broken down into smaller particles that will still have the unique properties of nitrogen.
Answer: E
Q3) Give the name of the element whose symbol is Na. Answer: sodium
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Chapter 3: Molecules, Compounds and Chemical
Equations
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Sample Questions
Q1) Determine the volume of hexane that contains 5.33 × 10<sup>22</sup> molecules of hexane.The density of hexane is 0.6548 g/mL and its molar mass is 86.17 g/mol.
A)8.59 mL
B)13.5 mL
C)7.40 mL
D)12.4 mL
E)11.6 mL
Answer: E
Q2) calcium
A)I(s)
B)Cl(g)
C)O(g)
D)Cl2(g)
E)Ne2(g)
F)Ne(g)
G)Ca(s)
H)Q<sub>2</sub>(g)
I)I2(s)
J)Ca2(s)
Answer: G
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Chapter 4: Chemical Quantities and Aqueous Reactions
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Sample Questions
Q1) According to the following balanced reaction,how many moles of NO are formed from 8.44 moles of NO<sub>2 </sub>if there is plenty of water present?
3 NO<sub>2</sub>(g)+ H<sub>2</sub>O(l) 2 HNO<sub>3</sub>(aq)+ NO(g)
A)2.81 moles NO
B)25.3 moles NO
C)8.44 moles NO
D)5.50 moles NO
E)1.83 moles NO
Q2) How many grams of AgNO<sub>3</sub> are needed to make 250.mL of a solution that is 0.135 M?
A)0.0917 g
B)0.174 g
C)5.73 g
D)91.7 g
Q3) How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution?
A)58.40 g
B)175.3 g
C)14.60 g
D)43.83 g
Q4) How can you tell if a reaction is an oxidation-reduction reaction?
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Chapter 5: Gases
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Sample Questions
Q1) How many molecules of N<sub>2</sub> are in a 400.0 mL container at 780 mm Hg and 135°C?
A)7.01 × 10<sup>21</sup><sup> molecules</sup>
B)7.38 × 10<sup>21</sup><sup> molecules</sup>
C)2.12 × 10<sup>22</sup> molecules
D)2.23 × 10<sup>22</sup> molecules
Q2) What is the total pressure in a 6.00-L flask which contains 0.127 mol of H<sub>2</sub>(g)and 0.288 mol of N<sub>2</sub>(g)at 20.0°C?
A)0.510 atm
B)0.681 atm
C)1.16 atm
D)1.66 atm
Q3) A sample of air from a home is found to contain 6.2 ppm of carbon monoxide.This means that if the total pressure is 695 torr,then the partial pressure of CO is ________ torr.
A)4.3 × 10<sup>3</sup>
B)4.3 × 10<sup>-</sup><sup>3</sup>
C)4.3
D)8.9 × 10<sup>3</sup>
E)1.1 × 10<sup>8</sup>
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Chapter 6: Thermochemistry
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Sample Questions
Q1) Use the H°<sub>f</sub> and H°<sub>rxn </sub>information provided to calculate H°<sub>f</sub> for SO<sub>3</sub>(g):
H°<sub>f (kJ/mol)</sub> 2 SO<sub>2</sub>(g)+ O<sub>2</sub>(g) 2
SO<sub>3</sub>(g) H°<sub>rxn </sub>= -198 kJ
SO<sub>2</sub>(g)-297
A)-792 kJ/mol
B)-248 kJ/mol
C)-495 kJ/mol
D)-578 kJ/mol
E)-396 kJ/mol
Q2) Calculate the work done by the system when 2 moles of hydrogen gas is produced by the following reaction in a flask fitted with an inflatable balloon.
Zn(s)+2HCl(aq)= ZnCl<sub>2</sub>(aq)+ H<sub>2</sub>(g)
A)+4.8 kJ
B)-4.8 kJ
C)0 kJ
D)2.0kJ
Q3) Explain the difference between H and E.
Q4) Give the equation to calculate the enthalpy of a system.
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Chapter 7: The Quantum-Mechanical Model of the Atom
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Sample Questions
Q1) What are the possible values of l if n = 6?
A)6
B)0,1,2,3,4,or 5
C)-4,-3,-2,-1,0,+1,+2,+3,or +4
D)-5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5
Q2) n = 3 to n = 2
A)103 nm
B)657 nm
C)7460 nm
D)122 nm
E)1280 nm
Q3) For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?
A)2s 3p
B)2p 6d
C)6p 4s
D)7f 5d
Q4) Why don't we observe the wavelength of everyday macroscopic objects?
Q5) What is the photoelectric effect?
Q6) Define constructive interference.
Page 9
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Chapter 8: Periodic Properties of the Elements
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Sample Questions
Q1) Write out the orbital diagram that represents the ground state of As.How many unpaired electrons are there?
A)0
B)4
C)3
D)2
E)1
Q2) Which has the largest atomic radius?
A)K
B)Na
C)Li
D)Cs
Q3) Below is a list of successive ionization energies (in kJ/mol)for a period 3 element.Identify the element and explain how you came to that conclusion. IE<sub>2</sub> = 2250 IE<sub>3</sub> = 3360 IE<sub>4</sub>= 4560 IE<sub>5</sub>= 7010 IE<sub>6</sub>= 8500 IE<sub>7 </sub>= 27,100
Q4) Define ionization energy.
Q5) List the noble gas that has the highest ionization energy.
Q6) Define electron affinity.
Page 10
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Chapter 9: Chemical Bonding I: Lewis Theory
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Sample Questions
Q1) Identify an ionic bond.
A)Electrons are pooled.
B)Electrons are shared.
C)Electrons are transferred.
D)Protons are gained.
E)Electrons are lost.
Q2) Sr-Sr
A)weakest ionic bond
B)strongest covalent bond
C)metallic bond
D)highest melting point
E)longest covalent bond
F)Na-Br
G)C-F
Q3) Choose the bond below that is the weakest.
A)Na-Cl
B)I-I
C)C=N
D)Li-F
E)C=O
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Chapter 10: Chemical Bonding II: Molecular Shapes,
Valence Bond Theory, and
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Sample Questions
Q1) Determine the electron geometry (eg)and molecular geometry (mg)of CH<sub>3</sub><sup>1</sup><sup>+</sup>.
A)eg = tetrahedral,mg = tetrahedral
B)eg = tetrahedral,mg = trigonal pyramidal
C)eg = trigonal planar,mg = bent
D)eg = trigonal planar,mg = trigonal planar
E)eg = tetrahedral,mg = trigonal planar
Q2) Using the VSEPR model,the molecular geometry of the central atom in SO<sub>2</sub> is ________.
A)linear
B)trigonal planar
C)tetrahedral
D)bent
E)trigonal pyramidal
Q3) Give the approximate bond angle for a molecule with a tetrahedral shape.
A)109.5°
B)180°
C)120°
D)105°
Q4) Explain why oil and water do not mix.
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Chapter 11: Liquids, Solids, and Intermolecular Forces
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Sample Questions
Q1) Place the following substances in order of decreasing vapor pressure at a given temperature.
PF<sub>5</sub> BrF<sub>3</sub> CF<sub>4</sub>
A)BrF<sub>3</sub> > PF<sub>5</sub> > CF<sub>4</sub>
B)BrF<sub>3</sub> > CF<sub>4 </sub>> PF<sub>5</sub>
C)PF<sub>5</sub> > BrF<sub>3 </sub>> CF<sub>4</sub>
D)CF<sub>4</sub> > BrF<sub>3</sub> > PF<sub>5</sub>
E)CF<sub>4</sub> > PF<sub>5</sub> > BrF<sub>3</sub>
Q2) Which is expected to have the largest dispersion forces?
A)C<sub>3</sub>H<sub>8</sub>
B)C<sub>12</sub>H<sub>26</sub>
C)F<sub>2</sub>
D)Be<sub> </sub>Cl<sub>2</sub>
Q3) Why does the temperature of a substance stay constant during a phase change such as vaporization?
Q4) Which is expected to have the largest dispersion forces?
A)C<sub>3</sub>H<sub>8</sub>
B)C<sub>12</sub>H<sub>26</sub>
C)F<sub>2</sub>
D)Be<sub> </sub>Cl<sub>2</sub>
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Chapter 12: Solutions
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Q1) Which of the following statements is true?
A)The solubility of a solid is not dependent on either temperature or pressure.
B)The solubility of a solid is highly dependent on pressure.
C)The solubility of a solid is highly dependent on both pressure and temperature.
D)The solubility of a solid is highly dependent on temperature.
E)None of the above.
Q2) 0.0050 m CO<sub>2</sub>
A)largest van't Hoff factor
B)solution of ionic compound with highest freezing point
C)solution with T<sub>b</sub> = 0.026°C
D)highest boiling point
E)solution that is most strongly dependent upon pressure
Q3) Which of the following ions should have the most exothermic H<sub>hydration</sub>?
A)Na<sup> </sup>
B)Mg<sup>2 </sup>
C)Al<sup>3 </sup>
D)Ca<sup>2 </sup>
E)Sr<sup>2 </sup>
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Chapter 13: Chemical Kinetics
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Sample Questions
Q1) What data should be plotted to show that experimental concentration data fits a first-order reaction?
A)1/[reactant] vs.time
B)[reactant] vs.time
C)ln[reactant] vs.time
D)ln(k)vs.1/T
E)ln(k)vs.E<sub>a</sub>
Q2) Which of the following reactions would you predict to have the largest orientation factor?
A)NOF(g)+ NOF(g) 2NO(g)+ F<sub>2</sub>(g)
B)Br<sub>2</sub>(g)+ H<sub>2</sub>C=CH<sub>2</sub>(g)
H<sub>2</sub>BrC-CBrH<sub>2</sub>(g)
C)NH<sub>3</sub>(g)+ BCl<sub>3</sub>(g) H<sub>3</sub>N-BCl<sub>3</sub>(g)
D)H(g)+ Cl(g) HCl(g)
E)All of these reactions should have nearly identical orientation factors.
Q3) What is a catalyst and what function does it serve?
Q4) Define half-life.
Q5) Explain what the exponential factor in the Arrhenius equation represents.
Q6) What function do enzymes serve?
Page 15
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Consider the following reaction:
CO<sub>2</sub>(g)+ C(graphite) 2 CO(g)
A reaction mixture initially contains 0.56 atm CO<sub>2</sub> and 0.32 atm CO.Determine the equilibrium pressure of CO if K<sub>p</sub> for the reaction at this temperature is 2.25.
A)0.83 atm
B)0.31 atm
C)0.26 atm
D)0.58 atm
E)0.42 atm
Q2) At equilibrium in a 10.0 L vessel,there are 7.6 × 10<sup>-2</sup> moles of SO<sub>2</sub>,8.6 × 10<sup>-2</sup> moles of O<sub>2</sub>,and 8.2 × 10<sup>-2</sup> moles of SO<sub>3</sub>.What is the equilibrium constant (K<sub>c)</sub>for the reaction: 2SO<sub>2</sub>(g)+ O<sub>2</sub>(g) 2SO<sub>3</sub>(g)
A)7.4 × 10<sup>-3</sup>
B)12.5
C)135
D)13.5
Q3) Define reaction quotient.
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Chapter 15: Acids and Bases
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Q1) Which Br nsted-Lowry acid is not considered to be a strong acid in water?
A)HI
B)HBr<sub> </sub>
C)H<sub>2</sub>SO<sub>3</sub>
D)H<sub> </sub>NO<sub>3</sub>
Q2) What is the concentration of hydroxide ions in pure water at 30.0<sup> </sup>C,if K<sub>w</sub> at this temperature is 1.47 × 10<sup>-14</sup>?
A)1.00 × 10<sup>-7</sup> M
B)1.30 × 10<sup>-7</sup> M
C)1.47 × 10<sup>-7</sup> M
D)8.93 × 10<sup>-8</sup> M
E)1.21 × 10<sup>-7</sup> M
Q3) Calculate the pH of a solution that contains 7.8 × 10<sup>-6</sup> M OH<sup> </sup> at 25°C.
A)1.28
B)5.11
C)12.72
D)8.89
E)9.64
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Chapter 16: Aqueous Ionic Equilibrium
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Q1) Which one of the following statements is true?
A)A buffer is an aqueous solution composed of two weak acids.
B)A buffer can absorb an unlimited amount of acid or base.
C)A buffer resists pH change by neutralizing added acids and bases.
D)A buffer does not change pH when strong acid or base is added.
E)None of the above are true.
Q2) If the pK<sub>a</sub> of HCHO<sub>2</sub> is 3.74 and the pH of an HCHO<sub>2</sub>/NaCHO<sub>2 </sub>solution is 3.89,which of the following is true?
A)[HCHO<sub>2</sub>] < [NaCHO<sub>2</sub>]
B)[HCHO<sub>2</sub>] = [NaCHO<sub>2</sub>]
C)[HCHO<sub>2</sub>] > [NaCHO<sub>2</sub>]
D)[HCHO<sub>2</sub>] >> [NaCHO<sub>2</sub>]
E)It is not possible to make a buffer of this pH from HCHO<sub>2</sub> and NaCHO<sub>2</sub>.
Q3) Which metal hydroxide is most soluble in water?
A)Fe(OH)<sub>2</sub>;K<sub>sp</sub> = 4.87 × 10<sup>-17</sup>
B)Mg(OH)<sub>2</sub>;K<sub>sp</sub> = 2.06 × 10<sup>-13</sup>
C)Ca(OH)<sub>2</sub>;K<sub>sp</sub> = 4.68 × 10<sup>-6</sup>
D)Ba(OH)<sub>2</sub>;K<sub>sp</sub> = 5.0 × 10<sup>-3</sup>
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Chapter 17: Free Energy and Thermodynamics
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Q1) Calculate the G°<sub>rxn</sub> using the following information.
2 HNO<sub>3</sub>(aq)+ NO(g) 3 NO<sub>2</sub>(g)+ H<sub>2</sub>O(l) G°<sub>rxn </sub>= ?
H°<sub>f</sub> (kJ/mol)-207.0 91.3 33.2 -285.8
S°(J/mol<sup></sup>K)46.0 210.8 240.1 70.0
A)-151 kJ
B)-85.5 kJ
C)+50.8 kJ
D)+222 kJ
E)-186 kJ
Q2) Choose the statement below that is true.
A)If K < 1,the reaction is spontaneous in the reverse direction.
B)If K < 1,the reaction is spontaneous in the forward direction.
C)If K < 1,the reaction is at equilibrium.
D)Not enough information is given.
Q3) What is "free" energy? Give a fictitious example.
Q4) Define the third law of thermodynamics.
Q5) Give the standard states for a gas,liquid,solid,and solution.
Q6) Define the second law of thermodynamics.
Q7) Define allotrope.
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Chapter 18: Electrochemistry
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Q1) Q = 1
A)E<sub>cell</sub> = E°<sub>cell</sub>
B)E<sub>cell</sub> = 0
C)E°<sub>cell</sub> < 0
D)E<sub>cell </sub>< 0
E)E°<sub>cell</sub> > 0
F)E<sub>cell </sub>> 0
Q2) G° > 0
A)E<sub>cell</sub> = E°<sub>cell</sub>
B)E<sub>cell</sub> = 0
C)E°<sub>cell</sub> < 0
D)E<sub>cell </sub>< 0
E)E°<sub>cell</sub> > 0
F)E<sub>cell </sub>> 0
Q3) Which of the following metal cations is the best oxidizing agent?
A)Co<sup>2+</sup>
B)Fe<sup>2+</sup>
C)Fe<sup>3+</sup>
D)Zn<sup>2+</sup>
Q4) Why,if we multiply a reaction by 2,don't we multiply its E°<sub>red</sub> by 2?
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Chapter 19: Radioactivity and Nuclear Chemistry
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Q1) Describe what changes occur during electron capture.
A)The mass number and atomic number decrease.
B)The mass number and atomic number increase.
C)The mass number is unchanged and the atomic number decreases.
D)The mass number is unchanged and the atomic number increases.
E)The mass number and atomic number do not change.
Q2) Neptunium-239 has a half-life of 2.35 days.How many days must elapse for a sample of <sup>239</sup>Np to decay to 0.100% of its original quantity?
A)0.0427 days
B)1.491 days
C)2.04 days
D)23.4 days
Q3) Explain how radiation increases cancer risk.
Q4) Stable isotopes,with low atomic numbers,have a N/Z ratio of 1.What does that imply?
A)The number of neutrons equals the number of protons.
B)The number of neutrons equals the number of electrons plus protons.
C)The number of electrons equals the number of neutrons plus protons.
D)The atomic number equals the atomic mass.
E)The number of protons equals the number of electrons plus neutrons.
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