General Chemistry II Practice Questions
Course Introduction
General Chemistry II builds on foundational concepts introduced in General Chemistry I, offering a deeper exploration of the principles and applications of chemistry. This course covers advanced topics such as chemical kinetics, chemical equilibrium, acid-base equilibria, thermodynamics, electrochemistry, and coordination chemistry. Students will also learn about the properties and reactions of solids, liquids, and gases, as well as the basics of nuclear and organic chemistry. Emphasis is placed on problem-solving, laboratory techniques, and real-world applications to prepare students for further study in the sciences and related fields.
Recommended Textbook
Foundations of College Chemistry 13th Edition by Morris Hein
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Chapter 1: An Introduction to Chemistry
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Sample Questions
Q1) Which is a pure substance?
A)table salt
B)bronze
C)air
D)soil
Answer: A
Q2) Which is a mixture?
A)copper wire
B)sugar
C)water
D)mud
Answer: D
Q3) In which phase do the particles possess the greatest amount of kinetic energy?
A)solid
B)liquid
C)gas
D)crystal
Answer: C
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Chapter 2: Standards for Measurement
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Sample Questions
Q1) Which SI prefix means 1000?
A)Milli
B)Centi
C)Deci
D)Kilo
Answer: D
Q2) How many significant figures are in the number 14.38?
A)1
B)2
C)3
D)4
Answer: D
Q3) A liquid has a mass of 40.24g and a volume of 50.0mL.What is its density?
A)0.805g/mL
B)1.24g/mL
C)9.76g/mL
D)90.2g/mL
Answer: A
Q4) The density of ethanol is 0.7893g/mL.What is the mass of one pint of ethanol?
Answer: The mass of one pint of ethanol is 373.4g
Page 4
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Chapter 3: Elements and Compounds
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Sample Questions
Q1) Which element is not a gas at normal temperature and pressure?<sup> </sup>
A)Xenon
B)Chlorine
C)Carbon
D)Neon
Answer: C
Q2) Which represents an element?
A)CO
B)NI
C)N<sub>2</sub>
D)OS
Answer: C
Q3) Which is an anion?
A)Cl<sup>-1</sup>
B)H<sub>2</sub>
C)Fe
D)Fe<sup>+2</sup>
Answer: A
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Chapter 4: Properties of Matter
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Sample Questions
Q1) The specific heat of gold is 0.131 J/g<sup>º</sup>C.A 400.0g sample of gold at 350.0<sup>º</sup>C<sup> </sup>is dropped into 180.0g of water at 22.0<sup>º</sup>C.Assume no heat is lost to the environment.
A.What will be the final temperature of the water?
B.What will be the final temperature of the gold?
Q2) The correct SI unit for energy is the joule.
A)True
B)False
Q3) Calcium chloride is 36.0% calcium by mass.A 5.00g sample of calcium chloride contains what mass of chlorine?
A)1.80g
B)1.40g
C)3.20g
D)5.00g
Q4) The change of liquid water into ice is a A)chemical change. B)physical change.
C)heterogeneous change.
D)homogeneous change.
Q5) Explain what happens at the molecular level when water freezes.
Page 6
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Chapter 5: Early Atomic Theory and Structure
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Sample Questions
Q1) Naturally occurring silicon exists as three isotopes.92.23% is Si-28 with a mass of 27.977 amu,4.67% is Si- 29 with a mass of 28.977 amu,and 3.10% is Si-30 with a mass of 29.974 amu.What is the atomic mass of silicon?
A)14.00 amu
B)28.09 amu
C)28.98 amu
D)86.93 amu
Q2) Atom A has 5 protons and 6 neutrons;atom B has 6 protons and 5 neutrons.These atoms are
A)isotopes of the same element.
B)isomers of the same element.
C)atoms of different elements.
D)identical in physical properties.
Q3) Which pair of formulas illustrates the Law of Multiple Proportions?
A)CH<sub>3</sub>Cl and CH<sub>3</sub>OH
B)H<sub>2</sub>O and HOH
C)CuCl<sub>2</sub> and CuBr
D)H<sub>2</sub>O and H<sub>2</sub>O<sub>2</sub>
Q4) Explain how Rutheford's gold foil experiment changed the model of the atom proposed by Thomson.
Page 7
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Chapter 6: Nomenclature of Inorganic Compounds
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Sample Questions
Q1) Which is dinitrogen tetroxide?
A)N<sub>4</sub>O<sub>2</sub>
B)NO<sub>2</sub>
C)N<sub>2</sub>O<sub> </sub>
D)N<sub>2</sub>O<sub>4</sub>
Q2) What is the formula of barium oxide?
A)BaO
B)BaO<sub>2</sub>
C)Ba<sub>2</sub>O
D)Ba<sub>2</sub>O<sub>3</sub>
Q3) The formula of an ionic compound is X<sub>2</sub>Y<sub>3</sub>.Which pair of atoms is most likely to be X and Y?
A)Na and S
B)Al and O
C)Ca and P
D)Cr and Cl
Q4) All chemical compounds have a charge of zero.
A)True
B)False
Q5) Identify four elements that can form more than one cation.
Page 8
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Chapter 7: Quantitative Composition of Compounds
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Sample Questions
Q1) You receive a gift of one mole of dollars,the only condition is that you spend it at the rate of one million dollars per second.How many years will it take you to spend the mole of dollars?
Q2) What is the empirical formula of a substance that consists of 85.60% carbon and 14.40% hydrogen?
A)CH
B)CH<sub>2</sub>
C)CH<sub>3</sub>
D)CH<sub>4</sub>
Q3) What is the empirical formula of a substance that consists of 32.86% potassium and 67.14% bromine?
A)KBr
B)K<sub>2</sub>Br
C)KBr<sub>2</sub>
D)K<sub>2</sub>Br<sub>3</sub>
Q4) Which of the following contains the greatest number of atoms?
A)1.0g of lithium
B)1.0g of sodium
C)1.0g of aluminum
D)1.0g of silver
Page 9
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Chapter 8: Chemical Equations
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Sample Questions
Q1) Given the reaction: 4NH<sub>3</sub> + 3O<sub>2</sub> \(\rarr\)2N<sub>2</sub> + 6H<sub>2</sub>O.How many moles of N<sub>2</sub> are produced when1.0 mole of NH<sub>3</sub> is consumed?
A)0.50
B)1.0
C)2.0
D)4.0
Q2) The reaction: N<sub>2</sub> + O<sub>2</sub> + 182.6 kJ \(\rarr\) 2NO,is
A)endothermic.
B)exothermic.
C)isothermic.
D)protothermic.<sub> </sub>
Q3) The following reaction: NaOH + HCl \(\rarr\) NaCl + H<sub>2</sub>O,is an example of A)combination.
B)decomposition.
C)single-displacement.
D)double-displacement.
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Chapter 9: Calculations From Chemical Equations
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Sample Questions
Q1) How many moles of Al will be consumed when 0.400 moles of Al<sub>2</sub>O<sub>3</sub> are produced in thefollowing equation? 4Al + 3O<sub>2</sub> \(\rarr\)2Al<sub>2</sub>O<sub>3</sub>
A)0.200
B)0.400
C)0.600
D)0.800
Q2) How many molecules of O<sub>2</sub> are produced when 0.500 moles of P<sub>4</sub>O<sub>10</sub> react completely in the following equation? P<sub>4</sub>O<sub>10</sub> \(\rarr\) 4P + 5O<sub>2</sub>
A)1.21 * 10<sup>24</sup>
B)1.51 *10<sup>24</sup>
C)6.02 * 10<sup>24</sup>
D)3.01 * 10<sup>24</sup>
Q3) In all chemical reactions,the reactants are always completely consumed.
A)True
B)False
Q4) The limiting reactant in a chemical reaction is the substance in excess. A)True
B)False
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Chapter 10: Modern Atomic Theory and the Periodic Table
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Sample Questions
Q1) Write orbital diagrams for the following elements in their ground states.
A.Fluorine
B.Oxygen
C.Carbon
Q2) All of the following are used to characterize electromagnetic radiation except A)charge
B)frequency
C)speed
D)wavelength
Q3) What is the maximum number of electrons that can occupy an orbital?
A)1
B)2
C)3
D)4
Q4) Small discrete packets of energy are known as A)excited state energy.
B)ground state energy.
C)spectra of energy.
D)quanta of energy.
Q5) In the designation 4p<sup>3</sup>;what is the significance of 4,p,and 3?
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Chapter 11: Chemical Bonds: the Formation of Compounds
From Atoms
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Sample Questions
Q1) The shape of a carbon tetrachloride molecule is A)pyramidal.
B)trigonal planar.
C)bent.
D)tetrahedral.
Q2) The element with the highest electronegativity is fluorine.
A)True
B)False
Q3) When potassium fluoride forms from a potassium atom and a fluorine atom
A)a proton is transferred from the potassium atom to the fluorine atom.
B)a proton is transferred from the fluorine atom to the potassium atom.
C)an electron is transferred from the potassium atom to the fluorine atom.
D)an electron is transferred from the fluorine atom to the potassium atom.
Q4) Explain how magnesium chloride forms from its elements.
Be sure to include the following: How the anion and cation form.
Ground state electron configuration for both atoms.
Ground state electron configuration for both ions.
Balanced chemical equation for the entire process.
Page 13
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Chapter 12: The Gaseous State of Matter
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Sample Questions
Q1) A sample of gas has a volume of 8.00 L at 20.0<sup> </sup><sup>°</sup><sup> </sup>C and 700.torr.What will be its volume atSTP?
A)1.20 L
B)9.32 L
C)53.2 L
D)6.87 L
Q2) What is the volume of 3.00 moles of neon gas at STP?
A)6.73 L
B)7.47 L
C)60.6 L
D)67.2 L
Q3) What volume of sulfur dioxide gas will be consumed when 12.0 L of oxygen is consumed in the following equation? 2 SO<sub>2</sub>(g)+ O<sub>2</sub>(g)\(\rarr\) 2 SO<sub>3</sub>(g)
A)6.00 L
B)12.0 L
C)24.0 L
D)60.0 L
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14
Chapter 13: Liquids
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Sample Questions
Q1) Which has the highest vapor pressure?
A)25 mL of water at 283 K
B)10 mL of water at 298 K
C)50 mL of water at 293 K
D)5 mL of water at 323 K
Q2) The low equilibrium vapor pressure of water is due to
A)polar covalent bonds.
B)nonpolar covalent bonds.
C)ionic bonds.
D)hydrogen bonds.
Q3) Hard water contains salts of
A)potassium and sodium.
B)calcium and magnesium.
C)barium and lithium.
D)barium and sodium.
Q4) Which substance contains molecules that will not form hydrogen bonds?
A)Hydrogen
B)Hydrogen fluoride
C)Water
D)Ammonia
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Chapter 14: Solutions
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Sample Questions
Q1) What is the boiling point of a 3.40 m aqueous solution of a nonvolatile nonelectrolyte? (The boiling point elevation constant for water is 0.512<sup>°</sup> C/m)
A)1.74<sup>°</sup> C
B)98.3<sup>°</sup> C
C)100.<sup>°</sup> C
D)102<sup>°</sup> C
Q2) An ethylene glycol,C<sub>2</sub>H<sub>4</sub>(OH)<sub>2</sub>,solution contains 500.g of ethylene glycol dissolved in 600.g of water.(The boiling point elevation constant for water is 0.512<sup>°</sup> C/m. )
A.What is the molality of the solution?
B.What is the boiling point of the solution?
Q3) A solution has a lower vapor pressure than the pure solvent,therefore,it will have a lower boiling point.
A)True
B)False
Q4) As pressure increases,the solubility of a gas in water
A)increases.
B)decreases.
C)remains the same.
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Chapter 15: Acids, Bases, and Salts
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Sample Questions
Q1) What is the concentration of calcium ion in a 2.0 M solution of calcium chloride?
A)1.0 M
B)2.0 M
C)3.0 M
D)4.0 M
Q2) Which is a strong electrolyte?
A)sulfuric acid
B)sulfurous acid
C)ammonia
D)acetic acid
Q3) What is the concentration of a HNO<sub>3</sub> solution if 10.0 mL of the solution is neutralized by 3.6 mL of a 0.20 M NaOH solution?
A)0.072 M
B)53.6 M
C)0.56 M
D)5.6 M
Q4) Boron trifluoride is a Lewis acid.
A)True
B)False
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Chapter 16: Chemical Equilibrium
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Sample Questions
Q1) The sodium salts of all anions listed below yield basic solutions when dissolved in water except<sup> </sup>
A)fluoride
B)chloride
C)cyanide
D)nitrite
Q2) Aqueous solutions of NaBr,K<sub>2</sub>SO<sub>4</sub>,and NaF will be neutral.
A)True
B)False
Q3) Calculate the percent ionization of a 0.050 M aqueous solution of HF having a pH of 3.15.
A)1.4%
B)4.9%
C)1.6%
D)6.3%
Q4) What is the pH of a 0.0010 M HCl solution?
A)1.0 X 10<sup>-3</sup>
B)3.0
C)11
D)4.0
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Chapter 17: Oxidationreduction
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Sample Questions
Q1) What always travels through the salt bridge in a voltaic cell?
A)Protons
B)Electrons
C)Neutrons
D)Ions
Q2) In the electrolysis of fused (molten)sodium chloride,the product at the anode is
A)Na
B)Na<sup>+1</sup>
C)Cl<sup>-1</sup>
D)Cl<sub>2</sub>
Q3) The products of the reaction between iron metal and calcium chloride are
A)FeCl<sub>2</sub>(aq)+ Ca(s)
B)No reaction takes place.
C)FeCl(aq)+ CaCl(aq)
D)CaFe(s)+ Cl<sub>2</sub>(g)
Q4) What is the oxidation number of oxygen in OF<sub>2</sub>?
A)0
B)+2
C)-1
D)-2
Page 19
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Chapter 18: Nuclear Chemistry
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Sample Questions
Q1) In a fusion reaction two nuclei of H-2 combine to form a nucleus of
A)H-4
B)He-4
C)He-2
D)Li-4
Q2) All nuclides of which element must be radioactive?
A)Strontium
B)Plutonium
C)Arsenic
D)Sulfur
Q3) The half-life of Sn-110 is 4 hours.If you have 20.g of this isotope,how much would remain 8 hours later?
A)40.g
B)5.0 g
C)10.g
D)80.g
Q4) Different radioisotopes of the same element have the same half-lives.
A)True
B)False
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Chapter 19: Introduction to Organic Chemistry Online Only
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Sample Questions
Q1) Write the balanced molecular formulas for the incomplete combustion of the first three members of the alkane series.The products are carbon monoxide and water.
Q2) Name the following compounds.
A.CH<sub>3</sub>CHClCHClCH<sub>2</sub>CH<sub>3</sub>
B.CH<sub>3</sub>CCl<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>CH<sub>3</sub>
C.CH<sub>2</sub>ClCH<sub>2</sub>CH<sub>2</sub>CHClCH<sub>3</sub>
D.CH<sub>3</sub>CHClCH<sub>2</sub>CH<sub>2</sub>CH<sub>2</sub>Cl
Q3) Which hydrocarbon can undergo a substitution reaction?
A)C<sub>2</sub>H<sub>2</sub>
B)C<sub>6</sub>H<sub>6</sub>
C)C<sub>3</sub>H<sub>6</sub>
D)C<sub>4</sub>H<sub>6</sub>
Q4) Which hydrocarbon series is saturated?
A)Alkenes
B)Alkynes
C)Alkanes
D)Aromatics
Q5) All the isomers of C<sub>3</sub>H<sub>8</sub>O have the same properties.
A)True
B)False
Page 21
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Chapter 20: Introduction to Biochemistry Online Only
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Sample Questions
Q1) Which is a component of DNA?
A)Deoxyribose
B)Dextrose
C)Dodecane
D)Doryl
Q2) Draw the structure of the dipeptide formed by serine and proline.
Q3) Which sugar is not a hexose?
A)Ribose
B)Glucose
C)Fructose
D)Galactose
Q4) What is meant by an essential amino acid?
Q5) Proteins are polymers of A)amino acids.
B)glucose.
C)glycerol.
D)amylase.
Q6) The open-chain form of glucose is an aldohexose.
A)True
B)False
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