Preparatory Chemistry Study Guide
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Course Introduction
Preparatory Chemistry is designed to provide students with a solid foundation in the fundamental concepts and principles of chemistry. Emphasizing basic atomic structure, chemical nomenclature, stoichiometry, the behavior of gases, solutions, and introductory chemical reactions, the course prepares students for higher-level chemistry courses. Through lectures, laboratory exercises, and problem-solving sessions, students will develop essential skills in scientific reasoning, data interpretation, and safe laboratory practices. This course is ideal for those who need to strengthen their chemistry background before enrolling in general or introductory chemistry courses required for science majors.
Recommended Textbook
Introductory Chemistry An Active Learning Approach 6th Edition by Mark S. Cracolice
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Chapter 2: Matter and Energy
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Q1) Which of the following is a chemical property?
A)Combustibility
B)Boiling point
C)Density
D)Color
E)Shape
Answer: A
Q2) Why do chemists use models of atoms and molecules?
A)Use of models is more convenient and less expensive than using photographs from microscopes
B)Matter at the particulate level is too small to be seen
C)Chemists follow the tradition established by Watson and Crick
D)High-powered electron microscopes create computerized models of atoms and molecules
E)To illustrate textbooks and scientific reports with more color than black-and-white photographs of the atoms and molecules
Answer: B
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Page 3
Chapter 3: Measurement and Chemical Calculations
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Q1) Which of the following numbers are correctly expressed in exponential notation?
i.43,200,000 = 4.32 × 10<sup>7</sup>
ii.0.000977 = 9.77 × 10<sup>4</sup>
iii.606,000 = 6.06 × 10<sup>-5</sup>
iv.0.00000175 = 1.75 × 10<sup>-6</sup>
A)i and iv
B)ii and iii
C)i and iii
D)ii and iv
E)All are incorrect
Answer: A
Q2) Convert 373 liters to milliliters,centiliters,and kiloliters.
A)0.373 mL, 373,000 cL, 37,300 kL
B)37,300 mL, 0.373 cL, 373,000 kL
C)373,000 mL, 37,300 cL, 0.373 kL
D)0.373 mL, 3.73 cL, 373,000 kL
E)3.73 mL, 0.373 cL, 373,000 kL
Answer: C
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Page 4
Chapter 4: Introduction to Gases
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Sample Questions
Q1) Which of the following statements is true?
A)The actual volume of ideal gas molecules is negligible compared to the space they occupy
B)In an ideal gas, the volume of the molecules is typically as low as 10% of the total container volume
C)The distances between ideal gas molecules are usually about the same as the diameter of the molecules
D)Given that there is no chemical reaction between two gases, the ability to mix the gases in a rigid container of fixed volume depends on the external atmospheric pressure
E)Ideal gas molecules usually touch one another in a small container with low pressure and high temperature
Q2) Which of the following correctly expresses Boyle's Law?
A)V 1/P
B)V P
C)V n
D)V 1/T
E)V T
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Page 5
Chapter 5: Atomic Theory: The Nuclear Model of the Atom
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Q1) One of the features of Dalton's atomic theory no longer considered to be correct is: All atoms of each element are identical in every respect.Which of the following is the best explanation of why this feature is no longer considered valid?
A)The existence of isotopes
B)The existence of ions
C)Natural variation in the mass of the proton
D)Natural variation in the mass of the neutron
E)Natural variation in the masses of the proton and the neutron
Q2) Which of the following statements is/are false?
i.Groups are arranged vertically in the periodic table
ii.Periods are arranged horizontally in the periodic table
iii.Periods are numbered from top to bottom
iv.There are eight elements in the first period of the periodic table
A)i only
B)ii and iii
C)i and ii
D)iv only
E)i, ii, and iv
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Chapter 6: Chemical Nomenclature
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Q1) For each of the following names,choose the correct formula.
i.Mercury(II)ion
ii.Nitride ion
iii.Zinc ion
I ii iii
A)Hg<sup>2+</sup> N<sup>3-</sup> Zn<sup>2+</sup>
B)Hg<sub>2</sub><sup>2+</sup> N<sup>3-</sup> Zn<sup>2+</sup>
C)Hg<sup>2+</sup> N<sup>3-</sup> Zn<sup>+</sup>
D)Hg<sub>2</sub><sup>2+</sup> N<sub>2</sub><sup>3-</sup> Zn<sup>+</sup> E)Hg<sup>2+</sup> N<sub>2</sub><sup>3-</sup> Zn<sup>+</sup>
Q2) Which of the following name-formula pairs is/are incorrect?
i.HCO<sub>3</sub><sup>-</sup> / hydrogen carbonate ion
ii.HTe<sup>-</sup> / hydrogen telluride ion (Z = 52)
iii.H<sub>2</sub>PO<sub>4</sub><sup>-</sup> / hydrogen phosphate ion
iv.HSO<sub>3</sub><sup>-</sup> / hydrogen sulfite ion
A)iii only
B)i and ii
C)ii and iii
D)ii and iv
E)ii, iii, and iv
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Page 7
Chapter 7: Chemical Formula Relationships
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Q1) Which of the following statements is/are correct?
i.A mole of sodium atoms (atomic mass = 23.0 u)contains fewer atoms than a mole of potassium atoms (atomic mass = 39.1 u)
ii.A mole of sodium atoms (atomic mass = 23.0 u)contains more atoms than a mole of potassium atoms (atomic mass = 39.1 u)
iii.In effect,the word mole represents the number 6.02 × 10<sup>23</sup>
iv.One mole of a substance contains as many particles as there are atoms in 12 grams of carbon-12
v.One mole of molecular nitrogen contains as many molecules as 24.0 u of carbon-12
A)i and iii
B)ii and iii
C)i and iv
D)iii and iv
E)ii, iii, iv, and v
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Chapter 8: Chemical Reactions
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Q1) Magnesium is placed into sulfuric acid.Write the balanced chemical equation for this reaction.What is the sum of the coefficients?
A)4 or less
B)5
C)6
D)7
E)8 or more
Q2) 12.09 g of A<sub>2</sub> reacts with 96.00 g of B<sub>2</sub> to form 108.09 g of A<sub>2</sub>B.What is the ratio of the molar mass of A to the molar mass of B?
A)1:8
B)8:1
C)1:4
D)16:1
E)1:16
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9
Chapter 9: Chemical Change
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Sample Questions
Q1) What appears on the product side in the net ionic equation for the reaction of HNO<sub>3</sub>(aq)with KOH(aq).KNO<sub>3</sub> is water soluble.
A)NO<sub>3</sub><sup>-</sup>(aq) + K<sup>+</sup>(aq)
B)H<sub>2</sub>O<sub>(l)</sub>
C)H<sup>+</sup>(aq) + K<sup>+</sup>(aq)
D)H<sub>2</sub>(g) + O<sub>2</sub>(g)
E)K<sup>+</sup>(aq) + NO<sub>3</sub><sup>-</sup>(aq)
Q2) Write the net ionic equation for the reaction that produces solid aluminum phosphate.What are the reactants?
A)Al<sup>3+</sup>(aq) + PO<sub>4</sub><sup>3-</sup>(aq)
B)Al<sup>3+</sup>(aq) + P<sup>3-</sup>(aq)
C)Al(s) + PO<sub>4</sub>(s)
D)Al(aq) + PO<sub>4</sub>(aq)
E)Al<sup>3+</sup>(aq) + HPO<sub>4</sub><sup>2-</sup>(aq)
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Chapter 10: Quantity Relationships in Chemical Reactions
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Q1) How many moles of C<sub>6</sub>H<sub>12</sub>O<sub>6</sub> are formed when 0.250 mole of CO<sub>2</sub> is consumed in the reaction 6 CO<sub>2</sub> + 6 H<sub>2</sub>O C<sub>6</sub>H<sub>12</sub>O<sub>6</sub> + 6 O<sub>2</sub>?
A)1.50 mol
B)1.00 mol
C)0.250 mol
D)0.167 mol
E)0.0417 mol
Q2) Formation of two moles of hydrogen chloride gas from the gases hydrogen and chlorine is a reaction for which H is -185 kJ.Which of the following statements is correct?
i.The reaction is exothermic.
ii.Enthalpy of the system decreases.
iii.Heat is a "product".
A)All are correct
B)All are incorrect
C)i only
D)ii only
E)iii only
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Page 11
Chapter 11: Atomic Theory: The Quantum Model of the Atom
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Q1) Which of the following is not a property of metals?
A)Tend to gain electrons to form anions
B)1, 2, or 3 valence electrons
C)Low ionization energies
D)High electrical conductivity
E)Malleable and ductile
Q2) How many orbitals are in the 3p sublevel?
A)1
B)3
C)5
D)7
E)9
Q3) The maximum number of electrons that can be held in the 5p sublevel is:
A)2
B)3
C)4
D)5
E)6
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12
Chapter 12: Chemical Bonding
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Q1) How is the bond in an F<sub>2</sub> molecule formed?
A)Overlap of the half-filled 1s orbitals of two fluorine atoms
B)Overlap of the half-filled 1s orbital from one fluorine atom with the half-filled 2p orbital from a second fluorine atom
C)Overlap of the half-filled 2p orbitals of two fluorine atoms
D)Transfer of an electron from one fluorine atom to the other
E)Transfer of an electron from one fluorine atom to third atom, followed by an electron from a neutral fluorine atom being shared with the electron-deficient fluorine atom to form the bond
Q2) Which bond is completely nonpolar?
A)F-F
B)H-F
C)C-N
D)H-O
E)C-H
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13
Chapter 13: Structure and Shape
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Q1) Which of the following best describes a polar molecule?
A)One with atoms having the same electronegativities
B)One with asymmetrical distribution of charge
C)A molecule without charge
D)One with a tetrahedral molecular geometry
E)One that has two or more hydrogen atoms
Q2) Which of the following has a trigonal planar molecular geometry?
A)CH<sub>3</sub>OH
B)CH<sub>2</sub>O
C)NH<sub>3</sub>
D)NO<sub>2</sub><sup>-</sup>
E)H<sub>2</sub>O
Q3) What is the molecular geometry surrounding the carbon atom in CH<sub>4</sub>?
A)Tetrahedral
B)Angular (bent)
C)Trigonal pyramid
D)Linear
E)Trigonal planar
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Chapter 14: The Ideal Gas Law and Its Applications
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Q1) 37.9 liters of NO at 725 torr and 146°C are decomposed by the reaction 2 NO N<sub>2</sub> + O<sub>2</sub>.What volume of nitrogen,measured at 755 torr and 22.0°C,will be produced?
A)13.9 L
B)51.2 L
C)12.8 L
D)25.8 L
E)0.0781 L
Q2) Calculate the number of moles in 3.13 L of dinitrogen monoxide at STP.
A)0.140 mol
B)7.16 mol
C)93.9 mol
D)70.1 mol
E)138 mol
Q3) The STP density of a gas is 1.46 grams per liter.Calculate its molar mass.
A)0.0306 g/mol
B)2.49 × 10<sup>4</sup> g/mol
C)3.00 g/mol
D)33.1 g/mol
E)35.7 g/mol
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Chapter 15: Gases, Liquids, and Solids
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Q1) Closed system A consists of liquid acetone in equilibrium with its own vapor at 30°C.System B is like System A,except that the volume of liquid,the area of the liquid surface,and the volume of the vapor space above the liquid are all twice as large as System A,and the temperature is only 15°C.Identify the statement among the following that is positively false.
A)Evaporation and condensation rates are equal in A
B)Evaporation and condensation rates are equal in B
C)Evaporation rate in A is greater than evaporation rate in B
D)Vapor pressure in B is greater than vapor pressure in A
E)Condensation rate in A is greater than condensation rate in B
Q2) Calculate the heat of vaporization of zinc if 393 kJ is required to vaporize a 223-gram sample.
A)1.14 × 10<sup>-5</sup> kJ/g
B)8.76 × 10<sup>4</sup> kJ/g
C)0.567 kJ/g
D)1.76 kJ/g
E)2.26 kJ/g
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Chapter 16: Solutions
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Q1) When a saturated solution is in equilibrium with undissolved solute:
A)the solution separates into layers
B)dissolving and crystallization stop
C)the quantity of dissolved solute equals the quantity of undissolved solute
D)the concentration of the solution remains constant
E)the temperature increases until more solute dissolves
Q2) Calculate the normality of an unknown acid if 21.8 mL is required to titrate a 25.0 mL sample of 1.02 N NaOH.
A)1.02 N
B)1.17 N
C)0.855 N
D)0.889 N
E)There is insufficient information to answer this question
Q3) You are required to prepare a 3.50% AgNO<sub>3</sub> solution,using 5.00 g of silver nitrate.What mass of water will be needed?
A)143 g
B)148 g
C)138 g
D)125 g
E)17.5 g
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Chapter 17: Acidbase Proton Transferreactions
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Q1) What is the hydroxide ion concentration in a solution with pH = 3?
A)10<sup>-3</sup> M
B)11 M
C)10<sup>-11</sup> M
D)3 M
E)10<sup>11</sup> M
Q2) Which of the following solutions is most acidic?
A)[H<sup>+</sup>] = 1 × 10<sup>-4</sup>
B)[H<sup>+</sup>] = 1 × 10<sup>-14</sup>
C)[OH<sup>-</sup>] = 1 × 10<sup>-3</sup>
D)pH = 10
E)pOH = 12
Q3) What is the conjugate base of ammonia?
A)NH<sub>3</sub>(g)
B)NH<sub>4</sub><sup>+</sup>(aq)
C)NH<sub>4</sub>OH(aq)
D)NH<sub>2</sub><sup>-</sup>(aq)
E)OH<sup>-</sup>(aq)
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Chapter 18: Chemical Equilibrium
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Q1) What is the pH of a 0.20 M solution of nitrous acid? K<sub>a</sub> = 4.5 × 10<sup>-4</sup>
A)9.02
B)4.66
C)4.05
D)2.02
E)0.70
Q2) Calculate the molar solubility of aluminum phosphate in water given that K<sub>sp</sub> = 1.3 × 10<sup>-20</sup>.
A)1.1 × 10<sup>-10</sup> M
B)1.5 × 10<sup>-7</sup> M
C)1.7 × 10<sup>-40</sup> M
D)5.9 × 10<sup>39</sup> M
E)7.7 × 10<sup>19</sup> M
Q3) If the position of equilibrium shifts to the left,what will happen?
A)The concentration of products will increase
B)The concentration of reactants will increase
C)The temperature will rise
D)The temperature will decrease
E)The concentrations of both products and reactants will increase
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Chapter 19: Oxidationreduction Electron Transferreactions
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Q1) Which among the following are the parts that comprise an electrolytic cell?
i.Two electrodes
ii.A molecular liquid
iii.A salt bridge
iv.An ionic solution
A)i and ii
B)i and iv
C)ii, iii, and iv
D)i, ii, and iii
E)i, iii, and iv
Q2) Silver metal will not react with hydrochloric acid.What does this suggest about silver and hydrochloric acid?
A)HCl is a weak acid
B)HCl is a strong acid
C)Ag is a weaker reducing agent than H<sup>+</sup> in HCl(aq)
D)Ag is a stronger oxidizing agent than HCl
E)No conclusion can be made based on this information
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Chapter 20: Nuclear Chemistry
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Q1) Which of the following is the estimated average annual exposure to naturally occurring radiation sources?
A)3,600 mrem/yr
B)3.6 mrem/yr
C)0.360 mrem/yr
D)360 mrem/yr
E)36 mrem/yr
Q2) Which of the following units is most commonly used to express radiation exposure?
A)rem
B)R
C)J
D)rad
E)All can be used to measure radiation exposure.
Q3) Which of the following is the best description of a positron?
A)Positively charged electromagnetic radiation
B)A proton
C)A positive electron
D)A particle accelerator
E)An artificial element
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Page 21
Chapter 21: Organic Chemistry
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Q1) What functional group is necessarily present in the monomers from which chain-growth polymers are formed?
A)Carboxylic acid
B)Ether
C)Ketone
D)Alkene
E)Alcohol
Q2) Which of the following compounds is/are (an)ether(s)?
i.CH<sub>3</sub>-CO-CH<sub>3</sub>
ii.CH<sub>3</sub>CH<sub>2</sub>-OH
iii.C<sub>2</sub>H<sub>5</sub>-O-C<sub>2</sub>H<sub>5</sub> iv.CH<sub>3</sub>(CH<sub>2</sub>)<sub>5</sub>-OH
v.CH<sub>3</sub>-CH<sub>3</sub>
A)i only
B)ii only
C)iii only
D)ii and iv
E)i, ii, iii, and iv
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Chapter 22: Biochemistry
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Q1) Which of the following is the best definition of the term lipid?
A)A molecule made of two or more simpler sugar molecules
B)A substance that is found in living organisms and is insoluble in water but soluble in nonpolar solvents
C)A nucleic acid monomer
D)A small molecule characterized by a carboxyl group at one end of the carbon chain and an amine group on the carbon next to the carboxyl group
E)A catalyst that controls chemical reactions in a living system
Q2) Which of the following is the best definition of the term protein?
A)The class of polymeric molecules with molar masses from about 5,000 g/mole on up
B)An amino acid polymer typically containing more than 40 amino acids
C)A chemical compound formed by bonding two or more monomers
D)A compound consisting of a carbonyl group bonded to a hydrogen on one side and a hydrogen, alkyl, or aryl group on the other
E)A carboxylic acid containing both an amine group and a variable alkyl group
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