Course Introduction
Physical Science
Exam Solutions
Physical Science is an interdisciplinary course that explores the fundamental principles governing the natural world, focusing primarily on the areas of physics and chemistry. Students examine topics such as the structure of matter, energy, forces, motion, and the nature of chemical reactions. The course emphasizes scientific inquiry, laboratory investigation, and critical thinking to understand how physical laws explain everyday phenomena and technological advancements. Through a combination of theoretical concepts and practical experiments, students gain foundational knowledge that prepares them for further study in science and develops their appreciation for the role of physical science in society.
Recommended Textbook
Principles of Chemistry A Molecular Approach 3rd Edition by Nivaldo J. Tro
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Page 2
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)Dew forms on a blade of grass.
B)A Halloween light stick glows after shaking.
C)An egg solidifies during cooking.
D)A hydrogen balloon explodes when contacted with a flame.
E)An iron pipe rusts in the yard.
Answer: A
Q2) Convert 35 m<sup>3</sup> to liters.
A)3.5 × 10<sup>-2</sup> L
B)3.5 L
C)3.5 × 10<sup>2</sup> L
D)3.5 × 10<sup>4</sup> L
Answer: D
Q3) What symbol is used to represent the factor 10<sup>-1</sup>?
A)M
B)m
C)
D)d
Answer: D
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Chapter 2: Atoms and Elements
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Sample Questions
Q1) Which of the following statements is false?
A)Anions are usually larger than their corresponding atom.
B)Metals tend to form cations.
C)Atoms are usually larger than their corresponding cation.
D)The halogens tend to form 1+ ions.
E)Nonmetals tend to gain electrons.
Answer: D
Q2) Define atomic mass.
Answer: The atomic mass represents the average mass of the isotopes that compose that element weighted according to the natural abundance of each isotope.
Q3) Calculate the atomic mass of element "X",if it has 2 naturally occurring isotopes with the following masses and natural abundances: X-45 44.8776 amu 32.88%
X-47 46.9443 amu 67.12%
A)46.26 amu
B)45.91 amu
C)46.34 amu
D)46.84 amu
E)44.99 amu
Answer: A
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Page 4
Chapter 3: Molecules, Compounds and Chemical
Equations
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Sample Questions
Q1) A certain alcohol contains only three elements,carbon,hydrogen,and oxygen.Combustion of a 50.00 gram sample of the alcohol produced 95.50 grams of CO<sub>2</sub> and 58.70 grams of H<sub>2</sub>O.What is the empirical formula of the alcohol?
Answer: C<sub>2</sub>H<sub>6</sub>O
Q2) The chemical formula for lithium peroxide is A)LiOH.
B)LiO<sub>2</sub>.
C)Li<sub>2</sub>O.
D)Li<sub>2</sub>O<sub>2</sub>.
Answer: D
Q3) Determine the name for N<sub>2</sub>O<sub>5</sub>.
A)dinitrogen pentoxide
B)nitrogen oxide
C)nitrogen (IV)oxide
D)nitrogen (II)oxide
E)nitrogen tetroxide
Answer: A
Q4) Give the name for HNO<sub>2</sub>.
Answer: nitrous acid
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Chapter 4: Chemical Quantities and Aqueous Reactions
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Sample Questions
Q1) How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days.Why?
Q2) Calculate the concentration (M)of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.
Q3) What reagent could not be used to separate Br<sup>-</sup> from CO<sub>3</sub><sup>2-</sup> when added to an aqueous solution containing both?
A)AgNO<sub>3</sub>(aq)
B)Ca(NO<sub>3</sub>)<sub>2</sub>(aq)
C)Cu(NO<sub>3</sub>)<sub>2</sub>(aq)
D)Fe(NO<sub>3</sub>)<sub>2</sub>(aq)
Q4) Which of the following pairs of aqueous solutions will react to produce a precipitate?
A)NH<sub>4</sub>NO<sub>3</sub> + Li<sub>2</sub>CO<sub>3</sub>
B)Hg<sub>2</sub>(NO<sub>3</sub>)<sub>2</sub> + LiI
C)NaCl + Li<sub>3</sub>PO<sub>4</sub>
D)AgC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> + Cu(NO<sub>3</sub>)<sub>2</sub>
E)None of the above solution pairs will produce a precipitate.
Q5) What causes a precipitation reaction to occur between two soluble compounds?
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Chapter 5: Gases
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Sample Questions
Q1) Calculate the root mean square velocity of nitrogen molecules at 25°C.
A)729 m/s
B)515 m/s
C)149 m/s
D)297 m/s
Q2) A sample of N<sub>2</sub> effuses in 255 s.How long will the same size sample of Cl<sub>2</sub> take to effuse?
A)406 s
B)247 s
C)645 s
D)155 s
E)388 s
Q3) A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage.What is the pressure of the basketball outside where the temperature is -1.00°C?
A)1.74 atm
B)1.80 atm
C)2.00 atm
D)2.08 atm
Q4) Define diffusion.
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Chapter 6: Thermochemistry
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Sample Questions
Q1) Define chemical energy.
Q2) Calculate the change in internal energy ( E)for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 atm pressure.(Remember that 101.3 J = 1 L<sup></sup>atm)
A)+25.9 kJ
B)-16.0 kJ
C)-25.9 kJ
D)-24.1 kJ
E)937 kJ
Q3) When 1.50 g of Ba(s)is added to 100.00 g of water in a container open to the atmosphere,the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C.If the specific heat of the solution is 4.18 J/(g °C),calculate H for the reaction,as written.
Ba(s)+ 2 H<sub>2</sub>O(l) Ba(OH)<sub>2</sub>(aq)+ H<sub>2</sub>(g) H = ?
A)-431 kJ
B)-3.14 kJ
C)+3.14 kJ
D)+431 kJ
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 total energy (in kJ)is contained in 1.0 mol of photons,all with a frequency of 2.75 × 10<sup>14</sup> Hz?
A)182 kJ
B)219 kJ
C)457 kJ
D)326 kJ
E)110 kJ
Q2) Which of the following statements are true?
A)The principal quantum number (n)describes the shape of an orbital.
B)The angular momentum quantum number (l)describes the size and energy associated with an orbital.
C)The magnetic quantum number (m<sub>l</sub>)describes the orientation of the orbital.
D)An orbital is the path that an electron follows during its movement in an atom.
E)All of the above are true.
Q3) Describe how a neon light works.
Q4) How many orbitals are contained in the n = 2 level? Give the<sub> </sub>l and m<sub>l</sub> values of each of them.
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Chapter 8: Periodic Properties of the Elements
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Sample Questions
Q1) Give the ground state electron configuration for Cd.
A)[Kr] 5s<sup>2 </sup>5d<sup>10</sup>
B)[Kr] 5s<sup>2 </sup>4d<sup>10 </sup>5p<sup>2</sup>
C)[Kr] 4d<sup>10</sup>
D)[Kr] 5s<sup>2 </sup>4d<sup>8</sup>
E)[Kr] 5s<sup>2 </sup>4d<sup>10</sup>
Q2) Place the following elements in order of decreasing atomic radius. Xe Rb Ar
A)Ar > Xe > Rb
B)Xe > Rb > Ar
C)Ar > Rb > Xe
D)Rb > Xe > Ar
E)Rb > Ar > Xe
Q3) Give the ground state electron configuration for the ion of Ba.
A)[Kr] 5s<sup>2 </sup>5p<sup>6</sup>
B)[Kr] 5s<sup>2 </sup>4d<sup>10 </sup>5p<sup>6 </sup>6s<sup>2 </sup>6p<sup>2</sup>
C)[Kr] 5s<sup>2 </sup>4d<sup>10 </sup>5p<sup>6 </sup>6s<sup>1</sup>
D)[Kr] 5s<sup>2 </sup>4d<sup>10 </sup>5p<sup>6 </sup>6s<sup>2</sup>
E)[Kr] 5s<sup>2 </sup>4d<sup>10 </sup>5p<sup>6</sup>
Q4) Why do Li,Na,and K have similar chemical properties?
Page 10
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Chapter 9: Chemical Bonding I: Lewis Theory
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Sample Questions
Q1) Choose the bond below that is the strongest.
A)C-F
B)C=O
C)C-I
D)I-I
E)C N
Q2) Which molecule or compound below contains a pure covalent bond?
A)Li<sub>2</sub>CO<sub>3</sub>
B)SCl<sub>6</sub>
C)Cl<sub>2</sub>
D)PF<sub>3</sub>
E)NaCl
Q3) Place the following in order of decreasing bond length.
H-F H-I H-Br
A)H-F > H-Br > H-I
B)H-I > H-F > H-Br
C)H-I > H-Br > H-F
D)H-Br > H-F > H-I
E)H-F > H-I > H-Br
Q4) How are electron affinity and electronegativity different?
Page 11
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Chapter 10: Chemical Bonding II: Molecular Shapes,
Valence Bond Theory, and
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Sample Questions
Q1) Give the approximate bond angle for a molecule with a tetrahedral shape. A)109.5°
B)180°
C)120°
D)105°
Q2) According to molecular orbital theory,what is an antibonding orbital?
Q3) Determine the hybridization about each carbon atom in the following structure. CH<sub>2</sub>CHCCCH<sub>3</sub>
Q4) Which of the following best describes ClF<sub>2</sub><sup>-</sup>? It has a molecular geometry that is
A)linear with no lone pairs on the Cl atom.
B)linear with lone pairs on the Cl atom.
C)nonlinear with no lone pairs on the Cl atom.
D)nonlinear with lone pairs on the Cl atom.
Q5) How many electrons are present in the bonding MO orbital of H<sub>2</sub>?
A)2
B)0
C)1
D)4
Q6) Explain why oil and water do not mix.
Page 12
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Chapter 11: Liquids, Solids, and Intermolecular Forces
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Sample Questions
Q1) The fluorocarbon C<sub>2</sub>Cl<sub>3</sub>F<sub>3</sub> has a normal boiling point of 47.6°C.The specific heats of C<sub>2</sub>Cl<sub>3</sub>F<sub>3</sub>(l)and C<sub>2</sub>Cl<sub>3</sub>F<sub>3</sub>(g)are 0.91 J/gK and 0.67 J/gK,respectively.The heat of vaporization of the compound is 27.49 kJ/mol.The heat required to convert 50.0 g of the compound from the liquid at 50.0°C to the gas at 80.0°C is ________ kJ.
A)8.19
B)1454
C)30.51
D)3031
E)10.36
Q2) What is the strongest type of intermolecular force present in NH<sub>2</sub>CH<sub>3</sub>?
A)dispersion
B)dipole-dipole
C)hydrogen bonding
D)ion-dipole
E)None of the above
Q3) Define viscosity.
Q4) Define dynamic equilibrium as it relates to vapor pressure.
Page 14
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Chapter 12: Solutions
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Sample Questions
Q1) A solution is prepared by adding 1.43 mol of KCl to 889 g of water.The concentration of KCl is ________ molal.
A)1.61 × 10<sup>-3</sup>
B)622
C)0.622
D)1.27 × 10<sup>3</sup>
E)1.61
Q2) Define molality.
Q3) An intravenous solution (IV)contains 0.9% aqueous solution.This IV is injected into a patient ________.
A)to make the osmotic pressure equal to that of body fluids
B)to make the blood pressure equal to that of body fluids
C)to make the osmotic pressure higher than that of body fluids
D)to make the osmotic pressure lower than that of body fluids
Q4) Give the term for amount of solute in mole per mass of solvent in kg.
A)molality
B)molarity
C)mole fraction
D)mole percent
E)mass percent
Page 15
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Chapter 13: Chemical Kinetics
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Sample Questions
Q1) What is the overall order of the following reaction,given the rate law?
Rate = k[X]<sup>3</sup>[Y]<sup>2</sup> <sup> </sup>
A)3rd order
B)5th order
C)2nd order
D)1st order
E)6th order
Q2) Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled?
Rate = k [X][Y]
A)The rate of reaction will increase by a factor of 2.
B)The rate of reaction will increase by a factor of 4.
C)The rate of reaction will increase by a factor of 5.
D)The rate of reaction will decrease by a factor of 2.
E)The rate of reaction will remain unchanged.
Q3) Define half-life.
Q4) What is the difference between average reaction rate and instantaneous reaction rate?
Q5) What is a catalyst and what function does it serve?
Page 16
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) The equilibrium constant is given for one of the reactions below.Determine the value of the missing equilibrium constant.
2 SO<sub>2</sub>(g)+ O<sub>2</sub>(g) 2 SO<sub>3</sub>(g)K<sub>c</sub> = 1.7 × 10<sup>6</sup>
SO<sub>3</sub>(g) 1/2 O<sub>2</sub>(g)+ SO<sub>2</sub>(g)K<sub>c</sub> = ?
A)3.4 × 10<sup>2</sup>
B)8.5
C)1.3 × 10<sup>3</sup>
D)1.2 × 10<sup>-6</sup>
E)7.7 × 10<sup>-4</sup>
Q2) Determine the value of K<sub>c</sub> for the following reaction if the equilibrium concentrations are as follows: [HCl]<sub>eq</sub> = 0.13 M,[HI]<sub>eq</sub> = 5.6 × 10<sup>-16</sup> M,[Cl<sub>2</sub>]<sub>eq</sub> = 0.0019 M.
2 HCl(g)+ I<sub>2</sub>(s) 2 HI(g)+ Cl<sub>2</sub>(g)
A)8.2 × 10<sup>-18</sup>
B)2.9 × 10<sup>31</sup>
C)1.2 × 10<sup>17</sup>
D)1.4 × 10<sup>-19</sup>
E)3.5 × 10<sup>-32</sup>
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Chapter 15: Acids and Bases
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Sample Questions
Q1) Determine the [OH ] concentration in a 0.169 M Ca(OH)<sub>2</sub> solution.
A)0.338 M
B)0.169 M
C)5.92 × 10<sup>-14</sup> M
D)2.96 × 10<sup>-14</sup> M
E)0.298 M
Q2) Which of the following acids will have the strongest conjugate base?
A)HCl
B)HClO<sub>4</sub>
C)HNO<sub>3</sub>
D)HCN
E)HI
Q3) Which will be the most predominant species in a 0.1 CH<sub>3</sub>COOH solution in water? (K<sub>a</sub> = 1.8 × 10<sup>-5</sup>)
A)H<sub>3</sub>O<sup>+ </sup>ions
B)CH<sub>3</sub>COO<sup>- </sup>ions
C)CH<sub>3</sub>COOH molecules
D)all of the above
Q4) What is the difference between a strong and weak acid?
Q5) Define a Lewis acid.
18
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Chapter 16: Aqueous Ionic Equilibrium
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Q1) The molar solubility of ZnS is 1.6 × 10<sup>-12</sup> M in pure water.Calculate the K<sub>sp</sub> for ZnS.
A)8.0 × 10<sup>-13</sup>
B)3.2 × 10<sup>-12</sup>
C)1.6 × 10<sup>-35</sup>
D)2.6 × 10<sup>-24</sup>
E)6.80 × 10<sup>-5</sup>
Q2) What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH?
K<sub>a</sub> = 6.76 × 10<sup>-4</sup> for HF.
A)1.74
B)5.75
C)8.25
D)12.26
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) Under which of the following conditions would one mole of He have the highest entropy,S?
A)17°C and 15 L
B)127°C and 15 L
C)17°C and 25 L
D)127°C and 25 L
Q2) Estimate G°<sub>rxn</sub> for the following reaction at 387 K. HCN(g)+ 2 H<sub>2</sub>(g) CH<sub>3</sub>NH<sub>2</sub>(g) H° = -158.0 kJ; S° = -219.9 J/K
A)+243 kJ
B)-72.9 kJ
C)+84.9 kJ
D)-92.5 kJ
E)-188 kJ
Q3) Which of the following is not true for G<sub>rxn</sub>?
A)If G°<sub>rxn</sub> > 0,the reaction is spontaneous in the forward direction.
B)If Q = 1,then G<sub>rxn</sub> = G°<sub>rxn</sub>.
C)If G°<sub>rxn</sub> = 0,the reaction is spontaneous in the reverse direction.
D)If G°<sub>rxn</sub> > 0,the reaction is spontaneous in the reverse direction.
E)Under equilibrium conditions, G<sub>rxn</sub> = 0.
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Chapter 18: Electrochemistry
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Q1) Which of the following metals,if coated onto iron,would prevent the corrosion (oxidation)of iron?
A)Zn
B)Cu
C)Ag
D)Au
Q2) Give the criteria for a nonspontaneous reaction.
A) G° < 0,E°<sub>cell</sub> > 0,K > 1
B) G° > 0,E°<sub>cell</sub> > 0,K > 1
C) G° > 0,E°<sub>cell </sub>< 0,K > 1
D) G° < 0,E°<sub>cell</sub> > 0,K < 1
E) G° > 0,E°<sub>cell</sub> < 0,K < 1
Q3) Identify oxidation.
A)increase in oxidation number
B)loss of electrons
C)gain of electrons
D)decrease in oxidation number
E)both A and B
Q4) Why are iron nails coated with zinc?
Q5) Explain the use of a salt bridge.
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Chapter 19: Radioactivity and Nuclear Chemistry
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Q1) 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.
Q2) Beta decay of <sup>60</sup>Co produces a beta particle and ________.
A)(<sup>56</sup>Mn)
B)(<sup>59</sup>Co)
C)(<sup>60</sup>Fe)
D)(<sup>60</sup>Ni)
Q3) Which of the following nuclides are most likely to decay via positron emission?
A)Na-26
B)I-121
C)Ca-42
D)S-30
E)Sb-122
Q4) Explain how radiation increases cancer risk.
Q5) What is the "mass defect"?
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