Chemical Fundamentals for Science Majors
Textbook Exam Questions
Course Introduction
This course provides a comprehensive introduction to the fundamental principles of chemistry, tailored for students pursuing science-related majors. Topics include atomic and molecular structure, chemical bonding, stoichiometry, states of matter, chemical reactions, thermochemistry, and an overview of kinetics and equilibrium. Emphasis is placed on developing problem-solving skills, applying chemical concepts to real-world situations, and building a strong foundation for more advanced studies in the scientific disciplines. Laboratory exercises complement the lecture material, offering hands-on experience with essential techniques and reinforcing core theoretical concepts.
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) Identify a liquid.
A)definite volume and definite shape
B)definite volume and no definite shape
C)definite shape and no definite volume
D)no definite shape and no definite volume
Answer: B
Q2) What is the difference between a physical property and a chemical property? Give an example of each.
Answer: A physical property is one that a substance displays without changing its composition,whereas a chemical property is one that a substance displays only by changing its composition via a chemical change.Physical properties include color,appearance,melting point,boiling point,and density.Chemical properties include corrosiveness,flammability,acidity,and toxicity.
Q3) What decimal power does the abbreviation pico represent?
A)1 × 10<sup>6</sup>
B)1 × 10<sup>9 </sup>
C)1 × 10<sup>-1</sup>
D)1 × 10<sup>-12</sup>
E)1 × 10<sup>-15</sup>
Answer: D
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Chapter 2: Atoms and Elements
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Sample Questions
Q1) How many protons (p)and neutrons (n)are in an atom of barium-130?
A)56 p,74 n
B)56 p,130 n
C)74 p,56 n
D)130 p,56 n
Answer: A
Q2) What element is defined by the following information?
P<sup>+</sup> = 11 n° = 12 e<sup>-</sup> = 11
A)sodium
B)vanadium
C)magnesium
D)titanium
Answer: A
Q3) What mass,in mg,does 2.63 moles of nickel have?
A)44.8 mg
B)2.23 × 10<sup>4</sup> mg
C)129 mg
D)3.56 × 10<sup>5</sup> mg
E)1.54 × 10<sup>5 </sup>mg
Answer: E
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Chapter 3: Molecules, Compounds and Chemical Equations
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Sample Questions
Q1) Determine the empirical formula for a compound that is 36.86% N and 63.14% O by mass.
A)NO
B)N<sub>2</sub>O
C)NO<sub>2</sub>
D)N<sub>2</sub>O<sub>3</sub>
E)NO<sub>3</sub>
Answer: D
Q2) Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.
A)H<sub>2</sub>SO<sub>4</sub>(aq)+ LiOH(aq)
Li<sub>2</sub>SO<sub>4</sub>(aq)
B)H<sub>2</sub>SO<sub>3</sub>(aq)+ 2 LiOH(aq) 2
Li<sub>2</sub>SO<sub>3</sub>(aq)
H<sub>2</sub>O(l)+
H<sub>2</sub>O(l)+
C)HSO<sub>3</sub>(aq)+ LiOH(aq) H<sub>2</sub>O(l)+ LiSO<sub>3</sub>(aq)
D)HSO<sub>4</sub>(aq)+ LiOH(aq) H<sub>2</sub>O(l)+ LiSO<sub>4</sub>(aq)
E)H<sub>2</sub>S(aq)+ 2 LiOH(aq) 2 H<sub>2</sub>O(l)+ Li<sub>2</sub>S(aq)
Answer: B
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Chapter 4: Chemical Quantities and Aqueous Reactions
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Sample Questions
Q1) How many moles of BCl<sub>3</sub> are needed to produce 10.0 g of HCl(aq)in the following reaction?
BCl<sub>3</sub>(g)+ 3 H<sub>2</sub>O(l) 3 HCl(aq)+ B(OH)<sub>3</sub>(aq)
A)0.0914 mol
B)0.274 mol
C)0.823 mol
D)10.9 mol
Q2) How many milliliters of a 0.266 M NaNO<sub>3</sub> solution are required to make 150.0 mL of 0.075 M NaNO<sub>3</sub> solution?
A)53.2 mL
B)42.3 mL
C)18.8 mL
D)23.6 mL
E)35.1 mL
Q3) Which one of the following compounds is insoluble in water?
A)Ca<sub> </sub>Cl<sub>2</sub>
B)NaNO<sub>3</sub>
C)Pb<sub> </sub>Cl<sub>2</sub>
D)K<sub>2</sub>CO<sub>3</sub>
Q4) What causes a precipitation reaction to occur between two soluble compounds?
Page 6
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Chapter 5: Gases
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Sample Questions
Q1) A mixture of 0.220 moles CO,0.350 moles H<sub>2</sub> and 0.640 moles He has a total pressure of 2.95 atm.What is the pressure of H<sub>2</sub>?
A)1.17 atm
B)0.853 atm
C)1.03 atm
D)0.969 atm
E)0.649 atm
Q2) If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions,what volume will 0.66 moles occupy under the same conditions?
A)12 L
B)8.6 L
C)17 L
D)5.0 L
E)15 L
Q3) Why does the rate of effusion increase with a decrease in the molar mass?
Q4) Why doesn't Dalton's Law of Partial Pressures depend on the identity of the gases present?
Q5) Define diffusion.
Q6) Why does hot air rise?
Page 7
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Chapter 6: Thermochemistry
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Sample Questions
Q1) It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C.What is the specific heat of benzene?
A)1.14 J/(g °C)
B)1.72 J/(g °C)
C)3.48 J/(g °C)
D)5.25 J/(g °C)
Q2) The specific heat of copper is 0.385 J/(g °C).If 34.2 g of copper,initially at 24.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?
A)24.4°C
B)26.8°C
C)356°C
D)380°C
Q3) Which of the following processes is exothermic?
A)the ionization of a lithium atom
B)the breaking of a Cl-Cl bond
C)the sublimation of dry ice (CO<sub>2</sub>(s))
D)the reaction associated with H<sup> </sup><sub>f</sub> for an ionic compound
E)All of the above processes are exothermic.
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) Identify the location of the visible range of light.
A)between X-ray and ultraviolet
B)between microwave and radio
C)between gamma ray and ultraviolet
D)between X-ray and gamma ray
E)between ultraviolet and infrared
Q2) Place the following types of electromagnetic radiation in order of increasing wavelength.
Visible light gamma rays microwaves
A)gamma rays < microwaves < visible light
B)microwaves < visible light < gamma rays
C)microwaves < gamma rays < visible light
D)visible light < gamma rays < microwaves
E)gamma rays < visible light < microwaves
Q3) What is the photoelectric effect?
Q4) How many orbitals are there in the fourth shell?
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Chapter 8: Periodic Properties of the Elements
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Sample Questions
Q1) Which of the following statements is true?
A)An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
B)An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
C)It is possible for two electrons in the same atom to have identical values for all four quantum numbers.
D)Two electrons in the same orbital can have the same spin.
E)None of the above are true.
Q2) Which of the following represents the change in electronic configuration that is associated with the first ionization energy of strontium?
A)[Kr]5s<sup>1</sup>5p<sup>1</sup> [Kr]5s<sup>1</sup> + e<sup>-</sup>
B)[Kr]5s<sup>2</sup> [Kr]5s<sup>1</sup>5p<sup>1</sup>
C)[Kr]5s<sup>2</sup> [Kr]5s<sup>1</sup> + e<sup>-</sup>
D)[Kr]5s<sup>2</sup> + e<sup>-</sup> [Kr]5s<sup>2</sup>5p<sup>1</sup>
Q3) Give the ground state electron configuration for Cd<sup>+2</sup>.
Q4) Define ionization energy.
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Chapter 9: Chemical Bonding I: Lewis Theory
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Sample Questions
Q1) List the following compounds in decreasing electronegativity difference.
Cl<sub>2</sub> HCl NaCl
A)NaCl > Cl<sub>2</sub> > HCl
B)Cl<sub>2</sub> > HCl > NaCl
C)HCl > NaCl > Cl<sub>2</sub>
D)NaCl > HCl > Cl<sub>2</sub>
Q2) Place the following in order of increasing magnitude of lattice energy.
MgO LiI BaS
A)BaS < MgO < LiI
B)LiI < BaS < MgO
C)MgO < BaS < LiI
D)LiI < MgO < BaS
E)MgO < LiI < BaS
Q3) Which element can expand its valence shell to accommodate more than eight electrons?
A)N
B)O
C)Br
D)He
Q4) Define dipole moment.
Page 11
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Chapter 10: Chemical Bonding II: Molecular Shapes,
Valence Bond Theory, and
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Q1) How many of the following molecules have sp<sup>3</sup>d hybridization on the central atom?
SiCl<sub>4</sub> BrF<sub>5</sub> AsF<sub>5</sub> BrF<sub>3</sub>
A)2
B)0
C)4
D)1
E)3
Q2) Using the VSEPR model,the electron-domain geometry of the central atom in BrF<sub>4</sub><sup>-</sup> is ________.
A)linear
B)trigonal planar
C)tetrahedral
D)trigonal bipyramidal
E)octahedral
Q3) What is the molecular geometry of TeCl<sub>4</sub>?
A)seesaw
B)square planar
C)square pyramidal
D)tetrahedral
Page 12
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Chapter 11: Liquids, Solids, and Intermolecular Forces
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Sample Questions
Q1) Place the following compounds in order of decreasing strength of intermolecular forces.
HF O<sub>2 </sub>CO<sub>2</sub>
A)HF > CO<sub>2 </sub>> O<sub>2</sub>
B)HF > O<sub>2</sub> > CO<sub>2 </sub>
C)O<sub>2</sub> > CO<sub>2 </sub>> HF
D)CO<sub>2</sub> > HF > O<sub>2</sub>
E)CO<sub>2</sub> > O<sub>2</sub> > HF
Q2) Gold crystallizes in a face-centered cubic structure.What is the edge length of the unit cell if the atomic radius of gold is 144 pm?
A)204 pm
B)288 pm
C)333 pm
D)407 pm
Q3) Choose the substance with the lowest boiling point.
A)H<sub>2</sub>S
B)NBr<sub>3</sub>
C)F<sub>2</sub>
D)CF<sub>2</sub>H<sub>2</sub>
E)H<sub>2</sub>O<sub>2</sub>
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Chapter 12: Solutions
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Q1) The Henry's law constant for helium gas in water at 30°C is 3.70 × 10<sup>-</sup><sup>4</sup> M/atm.When the partial pressure of helium above a sample of water is 0.650 atm,the concentration of helium in the water is ________ M.
A)5.69 × 10<sup>-4</sup>
B)1.76 × 10<sup>3</sup>
C)1.30
D)2.41 × 10<sup>-</sup><sup>4</sup>
E)3.70 × 10<sup>-4</sup>
Q2) What mass (in g)of NH<sub>3</sub> must be dissolved in 475 g of methanol to make a 0.250 m solution?
A)2.02 g
B)4.94 g
C)1.19 g
D)8.42 g
E)1.90 g
Q3) Calculate the osmotic pressure,in torr,of a solution containing 3.00 mg of a sugar (342 g/mole)in 15.0 mL of water at 25°C.
Q4) Define molality.
Q5) What is a semipermeable membrane?
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Chapter 13: Chemical Kinetics
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Q1) The first-order reaction,SO<sub>2</sub>Cl<sub>2</sub> SO<sub>2</sub> + Cl<sub>2</sub>,has a rate constant equal to 2.20 × 10<sup>-5</sup> s<sup>-1</sup> at 593 K.What percentage of the initial amount of SO<sub>2</sub>Cl<sub>2</sub> will remain after 6.00 hours?
A)1.00%
B)37.8%
C)40.2%
D)62.2%
Q2) 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>
Q3) Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?
Q4) What is the difference between average reaction rate and instantaneous reaction rate?
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) The equilibrium constant,K<sub>p</sub>,equals 3.40 for the isomerization reaction: Cis-2-butene trans-2-butene.
If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene,what is the equilibrium pressure of each gas?
A)P(cis-2-butene)= 0.0426 atm and P(trans-2-butene)= 0.145 atm
B)P(cis-2-butene)= 0.0471 atm and P(trans-2-butene)= 0.160 atm
C)P(cis-2-butene)= 0.0735 atm and P(trans-2-butene)= 0.250 atm
D)P(cis-2-butene)= 0.0898 atm and P(trans-2-butene)= 0.305 atm
Q2) What will happen to the following exothermic reaction at equilibrium if the pressure is raised?
N<sub>2</sub>(g)+ 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g)
A)Less NH<sub>3 </sub>will be produced.
B)More N<sub>2</sub> and H<sub>2 </sub>will be produced.
C)There will be no change in concentrations.
D)More NH<sub>3 </sub>will be produced.
Q3) Define reaction quotient.
Q4) Why aren't solids or liquids included in an equilibrium expression?
Q5) How is the reaction quotient different from an equilibrium constant for a given reaction?
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Chapter 15: Acids and Bases
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Sample Questions
Q1) Which of the following is a Lewis base?
A)AlF<sub>3</sub>
B)H<sub>2</sub>O
C)SiF<sub>4</sub>
D)C<sub>5</sub>H<sub>12</sub>
E)None of the above are Lewis bases.
Q2) Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10<sup>-</sup><sup>4</sup> hydroxide ion.
A)4.65 × 10<sup>-11</sup>
B)2.15 × 10<sup>-4 </sup>
C)3.67
D)10.33
Q3) What is the conjugate base of H<sub>2</sub>PO<sub>4</sub><sup> </sup>?
A)HPO<sub>4</sub><sup>2-</sup>
B)PO<sub>4</sub><sup>3-</sup>
C)H<sub>3</sub>PO<sub>4</sub>
D)H<sub>3</sub>O<sup>+</sup>
E)OH<sup> </sup>
Q4) What is the autoionization of water?
Q5) What does the term amphoteric mean?
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Chapter 16: Aqueous Ionic Equilibrium
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Sample Questions
Q1) Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH<sub>4</sub>Cl with 100.0 mL of 0.20 M NH<sub>3</sub>.The K<sub>b</sub> for NH<sub>3</sub> is 1.8 × 10<sup>-5</sup>.
A)9.13
B)9.25
C)9.53
D)4.74
E)8.98
Q2) pH = pK<sub>a</sub>
A)half-way to equivalence point of a weak acid/strong base titration
B)equivalence point of a strong acid/strong base titration
C)equivalence point of a weak base/strong acid titration
D)equivalence point of a weak acid/strong base titration
Q3) Identify the indicator that can be used at the highest pH.
A)Alizarin
B)Thymol blue
C)Crystal violet
D)Phenolphthalein
E)Alizarin yellow R
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Chapter 17: Free Energy and Thermodynamics
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Q1) Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25°C?
A)C<sub>10</sub>H<sub>22</sub>(s)
B)C<sub>10</sub>H<sub>22</sub>(l)
C)C<sub>14</sub>H<sub>30</sub>(s)
D)C<sub>14</sub>H<sub>30</sub>OH(l)
Q2) Determine G°<sub>rxn</sub> using the following information. CaCO<sub>3</sub>(s) CaO(s)+ CO<sub>2</sub>(g) H° = +179.2 kJ; S° = +160.2 J/K
A)-607.0 kJ
B)+112 .0 kJ
C)-89.3 kJ
D)+131.4 kJ
E)+228.1 kJ
Q3) What is "free" energy? Give a fictitious example.
Q4) In which of the following processes do the molecules become more orderly?
A)water freezing
B)ice melting
C)water evaporating
D)salt dissolving in water
E)dry ice subliming
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Chapter 18: Electrochemistry
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Q1) What element is being oxidized in the following redox reaction?
Zn<sup>2+</sup>(aq)+ NH<sub>4</sub><sup>+</sup>(aq) Zn(s)+ NO<sub>3</sub> (aq)
A)Zn
B)N
C)H
D)O
Q2) A galvanic cell consists of a Mg<sup>2+</sup>/Mg half-cell and a standard hydrogen electrode.If the Mg<sup>2+</sup>/Mg half-cell standard cell functions as the anode,and the standard cell potential is 2.37 V,what is the standard reduction potential for the Mg<sup>2+</sup>/Mg half-cell?
A)-2.37 V
B)-1.18 V
C)+1.18 V
D)+2.37 V
Q3) What is the difference between a voltaic cell and an electrolytic cell?
Q4) Which of the following metals is the best reducing agent?
A)Al
B)Zn
C)Sn
D)Ni
Page 20
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Chapter 19: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Which particle has the highest penetrating power?
A)alpha particle
B)beta particle
C)gamma particle
D)positron emission
E)electron capture
Q2) A rock contains 0.167 mg of lead-206 for each milligram of uranium-238.The half-life for the decay of uranium-238 to lead-206 is 4.5 × 10<sup>9</sup> yr.The rock was formed ________ years ago.
A)7.52 × 10<sup>8</sup>
B)6.08 × 10<sup>8</sup>
C)7.95 × 10<sup>8</sup>
D)1.15 × 10<sup>9</sup>
E)8.77 × 10<sup>8</sup>
Q3) Identify the symptom that is not from radiation exposure.
A)measles
B)increased cancer risk
C)death
D)genetic effects
E)weaker immune systems
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