Principles of Chemistry
Exam Materials
Course Introduction
Principles of Chemistry provides a foundational understanding of the core concepts in chemistry that are essential for further study in the sciences. This course explores atomic and molecular structure, chemical bonding, stoichiometry, thermochemistry, chemical reactions, and properties of gases, liquids, and solids. Students will also develop problem-solving skills by applying theoretical concepts to laboratory experiments and real-world scenarios. Emphasis is placed on developing critical thinking and practical laboratory skills needed for success in more advanced chemistry and related courses.
Recommended Textbook
Chemistry The Central Science 14th Edition by Theodore E. Brown
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Page 2
Chapter 1: Introduction: Matter, energy, and Measurement
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Sample Questions
Q1) ________ is the abbreviation for the prefix milli-.
A)k
B)m
C)M
D)n
E)d
Answer: B
Q2) Express the temperature,275.18 K,in degrees Celsius.
A)548.33 °C
B)274.17 °C
C)2.03 °C
D)120.88 °C
E)22.78 °C
Answer: C
Q3) Sn is the symbol for the element ________. Answer: Tin
Q4) Cu is the symbol for the element ________. Answer: Copper
Q5) Gases do not have a fixed ________ as they are able to be ________. Answer: volume,compressed
3
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Chapter 2: Atoms, molecules, and Ions
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Sample Questions
Q1) The correct formula of iron (III)bromide is ________.
A)FeBr<sub>2</sub>
B)FeBr<sub>3</sub>
C)FeBr
D)Fe<sub>3</sub>Br<sub>3</sub>
E)Fe<sub>3</sub>Br
Answer: B
Q2) The name of the ionic compound (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub> is ________.
A)ammonium phosphate
B)nitrogen hydrogen phosphate
C)tetrammonium phosphate
D)ammonia phosphide
E)triammonium phosphate
Answer: A
Q3) What is the name of an alcohol derived from hexane?
Answer: hexanol
Q4) The formula for potassium sulfide is ________.
Answer: K<sub>2</sub>S
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Chapter 3: Chemical Reactions and Reaction Stoichiometry
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Q1) When the following equation is balanced,the coefficient of H<sub>3</sub>PO<sub>4</sub> is ________. H<sub>3</sub>PO<sub>4 </sub>(aq)+ NaOH (aq) Na<sub>3</sub>PO<sub>4 </sub>(aq)+ H<sub>2</sub>O (l)
E)0 Answer: A
Q2) Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N<sub>2</sub> (g)+ 3H<sub>2 </sub>(g) 2NH<sub>3 </sub>(g)
If the reaction yield is 81.4 %,how many moles of N<sub>2 </sub>are needed to produce 8.50 mol of NH<sub>3</sub>?
A)20.9
B)10.4
C)5.22
D)6.92
E)15.7
Answer: C
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Chapter 4: Reactions in Aqueous Solution
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Q1) The concentration of species in 100 mL of a 3.47 M solution of sodium iodide is ________ M sodium ion and ________ M iodide ion.
A)0.0347, 0.0347
B)0.347, 0.347
C)0.347, 0.694
D)0.694, 0.347
E)3.47, 3.47
Q2) Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl<sub>2</sub> and AgNO<sub>3</sub>?
A)Co<sup>2+ </sup>and NO<sub>3</sub><sup>-</sup>
B)NO<sub>3</sub><sup>-</sup> and Cl<sup>-</sup>
C)Co<sup>2+</sup> and Ag<sup>+</sup>
D)Cl<sup>-</sup>
E)NO<sub>3</sub><sup>-</sup>
Q3) How many grams of an unknown substance with a molar mass of 40.0 are there in 500.0 mL of a 0.175 M solution of the unknown?
Q4) The solvent in an aqueous solution is ________.
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Chapter 5: Thermochemistry
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Q1) The term Btu which stands for ________ is commonly used in engineering applications.
A)Best thermal unit
B)Bunsen thermal unit
C)British thermal unit
D)Bake thermal unit
E)Brush thermal unit
Q2) Fuel values of hydrocarbons increase as the ________ increases.
A)C atomic ratio
B)H/C atomic ratio
C)H atomic ratio
D)C/C atomic ratio
E)C/H atomic ratio
Q3) The internal energy of a system is always increased by ________.
A)adding heat to the system
B)having the system do work on the surroundings
C)withdrawing heat from the system
D)adding heat to the system and having the system do work on the surroundings
E)a volume decompression
Q4) ________ is defined as the energy used to move an object against a force.
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Chapter 6: Electronic Structure of Atoms
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Q1) How many different principal quantum numbers can be found in the ground-state electron configuration of nickel?
A)2
B)3
C)4
D)5
E)6
Q2) What is the maximum angular momentum quantum number in the ground state electron configuration of iodine?
A)3
B)6
C)7
D)4
E)5
Q3) In the de Broglie formula describing the movement of an electron about the nucleus,the quantity "mv" is called its ________.
Q4) The shape of an orbital is defined by the angular momentum quantum number which is represented as letter ________.
Q5) The ground state electron configuration of copper is ________.
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Chapter 7: Periodic Properties of the Elements
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Q1) Element M reacts with chlorine to form a compound with the formula MCl<sub>2</sub>.Element M is more reactive than magnesium and has a smaller radius than barium.This element is ________.
A)Sr
B)K
C)Na
D)Ra
E)Be
Q2) Oxides of the active metals combine with acid to form ________.
A)hydrogen gas
B)metal hydrides
C)water and a salt
D)oxygen gas
E)metal hydroxides
Q3) Which of the following correctly represents the electron affinity of bromine?
A)Br (g) Br<sup>+</sup> (g)+ e<sup>-</sup>
B)Br (g)+ e<sup>-</sup> Br<sup>-</sup> (g)
C)Br<sub>2</sub> (g)+ e<sup>-</sup> Br<sup>-</sup> (g)
D)Br<sub>2</sub> (g)+ 2e<sup>-</sup> 2Br<sup>-</sup> (g)
E)Br<sup>+</sup> (g)+ e<sup>-</sup> Br (g)
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Chapter 8: Basic Concepts of Chemical Bonding
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Q1) In the Lewis structure of HCO<sub>3</sub><sup>-</sup>,the formal charge on H is ________,and the formal charge on C is ________.
A)-1, -1
B)0, 0
C)0, -1
D)+1, -1
E)-1, +1
Q2) Determining lattice energy from Born-Haber cycle data requires the use of
A)the octet rule
B)Coulomb's law
C)Periodic law
D)Hess's law
E)Avogadro's number
Q3) What is the maximum number of double bonds that a carbon atom can form?
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Chapter 9: Molecular Geometry and Bonding Theories
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Q1) According to molecular orbital theory,the bond order in a Be<sub>2</sub> molecule is ________.
A)3
B)1/2
C)1
D)2
E)0
Q2) The molecular geometry of the CHCl<sub>3</sub> molecule is ________.
A)bent
B)trigonal planar
C)trigonal pyramidal
D)tetrahedral
E)T-shaped
Q3) For a molecule with the formula AB<sub>3</sub>,the molecular shape is ________.
A)linear, octahedral, or bent
B)linear, bent, or trigonal planar
C)linear, bent, or T-shaped
D)tetrahedral
E)trigonal planar, trigonal pyramidal, or T-shaped
Q4) The ________ hydrogen orbital overlaps with the ________ fluoride orbital in HF.
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Chapter 10: Gases
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Q1) The molecular weight of a gas is ________ g/mol if 6.7 g of the gas occupies 6.3 L at STP.
A)24
B)3.6 × 10<sup>3</sup>
C)27
D)3.0 × 10<sup>2</sup>
E)1.8 × 10<sup>-2</sup>
Q2) 0.7515 moles of nitrogen gas and 0.1135 moles of methane gas are placed in a 171.6 ml container at 20.8 °C.What is the partial pressure (atm)of methane gas?
A)1.14
B)0.473
C)16.0
D)106
E)226
Q3) The deviation from ideal behavior of a gas is most evident at ________ and/or low temperature.
Q4) The effusion rate of a gas is proportional to the square root of its molar mass.
A)True
B)False
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Chapter 11: Liquids and Intermolecular Forces
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Q1) On a phase diagram,the critical pressure is ________.
A)the pressure required to melt a solid
B)the pressure below which a substance is a solid at all temperatures
C)the pressure above which a substance is a liquid at all temperatures
D)the pressure at which a liquid changes to a gas
E)the pressure required to liquefy a gas at its critical temperature
Q2) Of the following substances,________ has the highest boiling point.
A)HOCH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>OH
B)CH<sub>3</sub>CH<sub>2</sub>OH
C)C<sub>4</sub>H<sub>10</sub>
D)N<sub>2</sub>
E)Cl<sub>2</sub>
Q3) Elemental iodine (I<sub>2</sub>)is a solid at room temperature.What is the major attractive force that exists among different I<sub>2</sub> molecules in the solid?
A)London dispersion forces
B)dipole-dipole interactions
C)ionic-dipole interactions
D)covalent-ionic interactions
E)dipole-dipole attractions
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Chapter 12: Solids and Modern Materials
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Q1) Which of the following lattices is one of the five two-dimensional lattices in which the lattice vectors a and b are equal and the angle between them is 90°?
A)hexagonal
B)rectangular
C)square
D)rhombic
E)oblique
Q2) Which statement best describes the classification of Sterling silver?
A)It is pure silver.
B)It is oxidized silver.
C)It is an alloy of silver.
D)It is a mixture of silver and gold.
E)It is a liquid at room temperature.
Q3) What is the percent gold in a 6 karat gold link?
A)94
B)6.0
C)75
D)25
E)1.0 × 10<sup>2</sup>
Q4) Define a face-centered cubic lattice.
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Chapter 13: Properties of Solutions
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Q1) The process of solute particles being surrounded by solvent particles is known as
A)salutation
B)agglomeration
C)solvation
D)agglutination
E)dehydration
Q2) Which of the following will have an ideal van't Hoff factor (i)value of 1?
A)sucrose
B)NaF
C)LiNO<sub>3</sub>
D)NH<sub>4</sub>NO<sub>3</sub>
E)Li<sub>2</sub>PO<sub>4</sub>
Q3) What is the molality of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL?
A)9.00
B)2.12
C)2.33
D)90.0
E)0.0900
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Chapter 14: Chemical Kinetics
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Q1) The rate law for a reaction is rate = k[A][B]
Which one of the following statements is false?
A)The reaction is first order overall.
B)The reaction is first order in [A].
C)The reaction is first order in [B].
D)k is the reaction rate constant
E)If [A] is doubled, the reaction rate will increase by a factor of 2.
Q2) Units of the rate constant of a reaction are independent of the overall reaction order.
A)True
B)False
Q3) Rates of reaction can be positive or negative.
A)True
B)False
Q4) What is the order of the reaction in B?
A)1
B)2
C)3
D)4
E)0
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Chapter 15: Chemical Equilibrium
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Q1) Le Châtelier's principle states that if a system at equilibrium is disturbed,then more reactants are produced.
A)True
B)False
Q2) If the reaction quotient Q for a reaction is greater than the value of the equilibrium constant K for that reaction at a given temperature,________ must be converted to ________ for the system to reach equilibrium.
Q3) If the reaction quotient Q for a reaction is equal to the value of the equilibrium constant K for that reaction at a given temperature,then the reaction is at ________.
Q4) Which of the following statements is true?
A)Q does not change with temperature.
B)K<sub>eq</sub> does not change with temperature, whereas Q is temperature dependent.
C)K does not depend on the concentrations or partial pressures of reaction components.
D)Q does not depend on the concentrations or partial pressures of reaction components.
E)Q is the same as K<sub>eq</sub> when a reaction is at equilibrium.
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Chapter 16: Acid-Base Equilibria
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Q1) An aqueous solution of NaF is prepared by dissolving 0.350 mol of NaF in sufficient water to yield 1.0 L of solution.The pH of the solution was 8.93 at 25.0 °C.The K<sub>b</sub> of F<sup>- </sup>is ________.
A)1.2 × 10<sup>-5</sup>
B)2.1 × 10<sup>-10</sup>
C)6.9 × 10<sup>-9</sup>
D)2.8 × 10<sup>-12</sup>
E)9.9 × 10<sup>-2</sup>
Q2) The molar concentration of hydronium ion in pure water at 25 °C is ________.
A)0.00
B)1.0 × 10<sup>-7</sup>
C)1.0 × 10<sup>-14</sup>
D)1.00
E)7.00
Q3) The conjugate base of CH<sub>3</sub>NH<sub>3</sub><sup>+</sup> is ________.
A)CH<sub>3</sub>NH<sub>2</sub><sup>+</sup>
B)CH<sub>3</sub>NH<sub>2</sub><sup>-</sup>
C)CH<sub>3</sub>NH<sup>+</sup>
D)CH<sub>3</sub>NH<sub>2</sub>
E)none of the above
Page 18
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Chapter 17: Additional Aspects of Aqueous Equilibria
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Q1) The addition of HCl and ________ to water produces a buffer solution.
A)NH<sub>3</sub>
B)HC<sub>6</sub>H<sub>5</sub>O
C)KOH
D)KNO<sub>3</sub>
E)HNO<sub>3</sub>
Q2) Which of the following could be added to a solution of sodium acetate to produce a buffer?
A)acetic acid only
B)acetic acid or hydrochloric acid
C)hydrochloric acid only
D)potassium acetate only
E)sodium chloride or potassium acetate
Q3) Which compound listed below has the smallest molar solubility in water?
A)ZnCO<sub>3</sub>
B)Cd(OH)<sub>2</sub>
C)CdCO<sub>3</sub>
D)AgI
E)CaF<sub>2</sub>
Q4) A complex ion is when a metal ion binds to a ________.
Page 19
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Chapter 18: Chemistry of the Environment
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Q1) Of the noble gases,________ is present in highest concentration in dry air at sea level.
A)Ne
B)He
C)Xe
D)Kr
E)Ar
Q2) Ozone is a necessary,protective component of the ________,but is considered a pollutant in the ________.
A)troposphere, upper atmosphere
B)troposphere, air
C)photochemical smog, air we breathe
D)upper atmosphere, troposphere
E)air we breathe, upper atmosphere
Q3) The layer of the atmosphere that contains our weather is called the ________.
A)mesosphere
B)heterosphere
C)stratosphere
D)thermosphere
E)troposphere
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Chapter 19: Chemical Thermodynamics
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Q1) A reversible change produces the maximum amount of ________ that can be achieved by the system on the surroundings.
Q2) The value of S° for the catalytic hydrogenation of acetylene to ethane, C<sub>2</sub>H<sub>2</sub> (g)+ 2H<sub>2</sub> (g) C<sub>2</sub>H<sub>6</sub> (g) Is ________ J/K mol.
A)-76.0
B)+440.9
C)-232.5
D)+232.5
E)+28.7
Q3) Calculate G°<sup> </sup>(in kJ/mol)for the following reaction at 1 atm and 25 °C: C<sub>2</sub>H<sub>6</sub> (g)+ O<sub>2</sub> (g) CO<sub>2</sub> (g)+ H<sub>2</sub>O (l)(unbalanced)
G<sub>f</sub>° C<sub>2</sub>H<sub>6</sub> (g)= -32.89 kJ/mol; G<sub>f</sub>°<sup> </sup>CO<sub>2</sub> (g)= -394.4 kJ/mol; G<sub>f</sub>° H<sub>2</sub>O (l)= -237.13 kJ/mol
Q4) At what temperature (in K)will a reaction become spontaneous? H is 115.0 kJ/mol and S is 75.00 J/K mol.
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Chapter 20: Electrochemistry
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Q1) What is the coefficient of the dichromate ion when the following equation is balanced?
Fe<sup>2+</sup> + Cr<sub>2</sub>O<sub>7</sub><sup>2-</sup>
Fe<sup>3+</sup> + Cr<sup>3+</sup> (acidic solution)
A)1
B)2
C)3
D)5
E)6
Q2) Based on standard reduction potentials,the most difficult species to reduce and the poorest oxidizing agent is ________.
Q3) In a lead-acid battery,the electrodes are consumed.In this battery,________.
A)the anode is Pb
B)the anode is PbSO<sub>4</sub>
C)the anode is PbO<sub>2</sub>
D)the cathode is PbSO<sub>4</sub>
E)the cathode is Pb
Q4) Define the Nernst equation.
Q5) Define a coulomb.
Q6) What is a galvanized iron nail?
Page 22
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Chapter 21: Nuclear Chemistry
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Q1) Radioactive seeds that are implanted into a tumor are coated with ________ to stop alpha and beta ray penetration.
Q2) What happens to the mass number and the atomic number of an element when it undergoes beta decay?
A)Neither the mass number nor the atomic number changes.
B)The mass number decreases by 4 and the atomic number decreases by 2.
C)The mass number does not change and the atomic number increases by 1.
D)The mass number does not change and the atomic number decreases by 2.
E)The mass number increases by 2 and the atomic number increases by 1.
Q3) Which type of radioactive decay results in no change in mass number and atomic number for the starting nucleus?
A)alpha
B)beta
C)positron emission
D)electron capture
E)gamma
Q4) Conversion of one nucleus into another was first demonstrated in 1919 by
Q5) The major type of cancer caused by radiation is ________.
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Chapter 22: Chemistry of the Nonmetals
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Q1) The primary commercial use of nitric acid is ________.
A)in the manufacture of plastics
B)in the manufacture of explosives
C)in pool water maintenance
D)in the manufacture of fertilizers
E)in the manufacture of anti-depressant drugs
Q2) A borane is a ________.
A)compound containing only boron and oxygen
B)compound containing only boron and aluminum
C)compound containing only boron and hydrogen
D)compound containing only boron and carbon
E)three-dimensional covalent network of boron atoms
Q3) What is the oxidation state of oxygen in the superoxide ion?
Q4) Why does calcium carbonate dissolve in water containing carbon dioxide?
Q5) Most mined phosphate rock is ________.
A)used as a strong acid
B)used as a reducing agent
C)used as a detergent
D)converted to fertilizer
E)discarded as a by-product
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Chapter 23: Transition Metals and Coordination Chemistry
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Q1) What is the charge on the complex ion in Ca<sub>2</sub>[Fe(CN)<sub>6</sub>]?
A)3-
B)2+
C)2-
D)1-
E)4-
Q2) A substance with unpaired electrons will be ________.
A)slightly attracted to a magnet
B)slightly repelled by a magnet
C)permanently magnetic
D)brightly colored
E)nonmetallic
Q3) How many d electrons are associated with the metal ion in [Cr(NH<sub>3</sub>)<sub>3</sub><sup>+</sup>?
A)1
B)2
C)3
D)4
E)5
Q4) The two more common oxidation states of lead are ________ and ________.
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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry
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Q1) The aromas of different fruit are due to the chemical compounds known as
Q2) The secondary structure of a protein is the result of ________ bonding.
A)covalent
B)peptide
C)ionic
D)hydrogen
E)none of the above
Q3) ________ could be the formula of an alkene.
A)C<sub>3</sub>H<sub>8</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>6</sub>H<sub>6</sub>
D)C<sub>17</sub>H<sub>36</sub>
E)CH<sub>8</sub>
Q4) The primary ingredient in vinegar is ________.
Q5) Living organisms must expend energy to counter any increase in ________.
Q6) In general,________ are the least reactive hydrocarbons.
A)alkenes
B)alkynes
C)alkanes
Page 26
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