General Chemistry II Review Questions
Course Introduction
General Chemistry II is a continuation of introductory chemistry that delves deeper into fundamental chemical concepts. This course covers topics such as chemical kinetics, chemical equilibrium, acids and bases, thermodynamics, electrochemistry, and coordination chemistry. Students will also explore aspects of descriptive inorganic chemistry, including the properties of metals and nonmetals, and gain exposure to laboratory techniques that reinforce theoretical knowledge. Emphasis is placed on quantitative problem-solving, critical thinking, and the application of chemistry in real-world scenarios, providing a solid foundation for advanced study in chemistry 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) Name four different ways in which you could classify or organize twenty different types of fasteners such as nails or screws.
Answer: Any four properties of the fasteners,such as: length of the fasteners,color of the fasteners,composition of the fasteners,thickness of the fasteners,shape of the fasteners,Are the fasteners threaded? Are the fasteners curved or straight?
Q2) Which has neither a definite shape nor a definite volume?
A)crystal
B)solid
C)gas
D)liquid
Answer: C
Q3) Which is a scientific observation?
A)Freezing and boiling are called physical changes
B)Water freezes at zero degrees C
C)If a substance has a density of 1.00g/mL it must be water.
D)When a substance freezes its molecules lose potential energy.
Answer: B
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Chapter 2: Standards for Measurement
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Sample Questions
Q1) Convert 3.00 inches into centimeters.
A)1.18cm
B)2.54cm
C)7.62cm
D)10.2cm
Answer: C
Q2) Convert 33.0 inch<sup>2</sup> to mm<sup>2</sup>.
A)2.13 x 10<sup>3</sup> mm<sup>2</sup>
B)8.38 x 10<sup>2</sup> mm<sup>2</sup>
C)2.13 x 10<sup>4</sup> mm<sup>2</sup>
D)5.12 x 10<sup>2</sup> mm<sup>2</sup>
Answer: C
Q3) How many zeroes are significant in the number 0.03003?
A)1
B)2
C)3
D)4
Answer: B
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 a liquid at room temperature?
A)fluorine.
B)chlorine.
C)bromine.
D)iodine.
Answer: C
Q2) At room temperature the majority of metals exist as A)vapors.
B)solids.
C)gases.
D)liquids. Answer: B
Q3) Which is a transition element?
A)Magnesium
B)Potassium
C)Manganese
D)Silicon
Answer: C
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Page 5
Chapter 4: Properties of Matter
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Sample Questions
Q1) Which is not a physical property?
A)Boiling point
B)Physical state
C)Color
D)Bleaching action
Q2) Explain what happens at the molecular level when water freezes.
Q3) Combining hydrogen and oxygen to form water is a
A)chemical change.
B)physical change.
C)conservation reaction.
D)none of these.
Q4) The specific heat of copper is 0.386 J/g<sup>º</sup>C.A 20.0g sample of copper is heated from 25.0<sup>º</sup>C to 35.0<sup>º</sup>C.How much heat did the copper absorb?
A)837 J
B)77.2 J
C)194 J
D)270 J
Q5) Compare a substance with a high specific heat to a substance with low specific heat with respect to ability to absorb or release heat.
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Chapter 5: Early Atomic Theory and Structure
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Sample Questions
Q1) An atom of silver-108 contains 47 protons,47 electrons,and 61 neutrons.
A)True
B)False
Q2) Which experiment led to the notion that the atom contains an extremely small,positively charged nucleus?
A)Millikan's oil drop experiment
B)Rutherford's gold foil experiment
C)Thomson's cathode ray experiment
D)Dalton's atomic experiment
Q3) What is the mass number of an atom that contains 23 protons,23 electrons,and 28 neutrons?
A)5
B)28
C)51
D)74
Q4) How many electrons are in a neutral atom of Ar-40?
A)18
B)22
C)40
D)58
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Chapter 6: Nomenclature of Inorganic Compounds
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Sample Questions
Q1) What is the correct name for K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>?
A)dipotassium chromate.
B)potassium dichromate.
C)potassium(II)chromate.
D)dipotassium dichromate.
Q2) Which ions combined to form the compound PbO<sub>2</sub>?
A)Pb<sup>2+</sup> and O<sup>-</sup>
B)Pb<sup>2+</sup> and O<sup>2-</sup>
C)Pb<sup>+</sup> and O<sup>2-</sup>
D)Pb<sup>4+</sup> and O<sup>2-</sup>
Q3) AgCl is a molecular compound.
A)True
B)False
Q4) 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>
Q5) Identify four elements that can form more than one cation.
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Chapter 7: Quantitative Composition of Compounds
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Sample Questions
Q1) One mole of magnesium and one mole of magnesium sulfate contain the same number of magnesium atoms.
A)True
B)False
Q2) A substance is known to contain 2.00 g of carbon for every 5.33 g of oxygen.How many grams of carbon will be present in 55.0 g of this substance?
A)15.0 g
B)27.5 g
C)20.6 g
D)10.3 g
Q3) What is the molar mass of carbon tetrachloride?
A)47.46g
B)82.91g
C)118.36g
D)153.81g
Q4) A 2.489 sample of a compound is found to contain water.When heated,the water is driven off.The mass of the remaining compound is 1.591g.
A.What is the mass of the water that was lost?
B.What is the percent by mass of the water in the original compound?
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Chapter 8: Chemical Equations
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Sample Questions
Q1) The products of the complete combustion of the hydrocarbon methane are
A)carbon monoxide and water.
B)carbon dioxide and water.
C)carbon monoxide and hydrogen.
D)carbon dioxide and hydrogen.
Q2) Absent-minded Joe prepared two colorless aqueous solutions but forgot to label the flasks! He knew that one solution was made with potassium sulfate and the other with zinc bromide.List three reactants that you may add to a small portion of the solutions in order to differentiate between them using the selective formation of a solid.
Q3) The amount of energy that must be supplied to start a chemical reaction is called the
A)heat of reaction.
B)heat of fusion.
C)heat of vaporization.
D)activation energy.
Q4) In a neutralization reaction,one of the reactants behaves as an acid and the other behaves as a base.
A)True
B)False
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Chapter 9: Calculations From Chemical Equations
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Sample Questions
Q1) How many moles of Zn are consumed when 1.60 * 10<sup>24</sup> molecules of HCl react completelyin the following equation? Zn + 2HCl \(\rarr\) ZnCl<sub>2</sub> + H<sub>2</sub>
A)1.33
B)2.66
C)3.99
D)5.32
Q2) Nitrogen gas to water
Q3) What mass of HCl is produced when 3.00 moles of H<sub>2</sub> react completely in the following equation? H<sub>2</sub> + Cl<sub>2</sub> \(\rarr\) 2HCl
A)54.7g
B)72.9g
C)109g
D)219g
Q4) In all chemical reactions,the reactants are always completely consumed.
A)True B)False
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Chapter 10: Modern Atomic Theory and the Periodic Table
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Sample Questions
Q1) Which element is in the d-block of the periodic table?
A)Cr
B)Am
C)Ca
D)As
Q2) In the designation 4p<sup>3</sup>;what is the significance of 4,p,and 3?
Q3) The characteristic bright line spectrum of an element is produced when electron(s)
A)move to higher energy levels.
B)fall back to lower energy levels.
C)are emitted as gamma radiation.
D)are absorbed into the nucleus.
Q4) What is the number of orbitals in an f sublevel?
A)2
B)3
C)5
D)7
Q5) The second principal energy level contains s and p orbitals.
A)True
B)False
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Chapter 11: Chemical Bonds: the Formation of Compounds
From Atoms
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Sample Questions
Q1) The series Cl,As,Sb,In is arranged by increasing ionization energy..
A)True
B)False
Q2) The shape of a carbon tetrachloride molecule is
A)pyramidal.
B)trigonal planar.
C)bent.
D)tetrahedral.
Q3) The element with the highest electronegativity is fluorine.
A)True
B)False
Q4) A nonpolar covalent bond will form between which two atoms?
A)Potassium and chlorine
B)Hydrogen and chlorine
C)Sodium and bromine
D)Chlorine and chlorine
Q5) The bond formed between one carbon atom and one oxygen atom is a polar covalent bond.
A)True
B)False
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Chapter 12: The Gaseous State of Matter
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Sample Questions
Q1) A sample of gas is in a cylinder of fixed volume.At 20.0<sup> </sup><sup>°</sup>C its internal pressure is 3.42 atm.What will be its pressure at 120.0<sup>°</sup>C?
A)2.55 atm
B)4.59 atm
C)0.570 atm
D)20.5 atm
Q2) A sample of gas is in a cylinder of fixed volume.As the temperature of the sampleincreases,its internal pressure will A)increase.
B)decrease.
C)remain the same.
Q3) Which gas has approximately the same density as carbon dioxide gas at STP?
A)CH<sub>4</sub>
B)C<sub>2</sub>H<sub>6</sub>
C)C<sub>3</sub>H<sub>8</sub>
D)C<sub>4</sub>H<sub>10</sub>
Q4) What is the molar mass of a gas if 36.4 g of the gas occupies 100.0 L at 32.0<sup> </sup><sup>°</sup><sup> </sup>C and 0.800 atm?
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Page 14
Chapter 13: Liquids
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Sample Questions
Q1) Evaporation is the change from the liquid phase to the vapor phase.
A)True
B)False
Q2) The formula for the anhydride of potassium hydroxide is K<sub>2</sub>O.
A)True
B)False
Q3) What quantity of heat is required to change the temperature of 30.0 g of water at 10.0<sup> </sup><sup>°</sup>C to 25.0<sup> </sup><sup>°</sup>C? The specific heat of liquid water is 4.184 J/g<sup> </sup><sup>°</sup>C.
A)62.8 J
B)126 J
C)107 J
D)1880 J
Q4) At pressures below one atmosphere,water will boil above 100.<sup> </sup><sup>°</sup>C.
A)True
B)False
Q5) Small amounts of water evaporate at room temperature.If one mole of water evaporates from a sample in one day,how many molecules are evaporating per second?
Page 15
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Chapter 14: Solutions
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Sample Questions
Q1) Which would most likely increase the solubility of a solid in water?
A)Stirring
B)Increase the surface area of the solid
C)Increase the pressure
D)Increase the temperature
Q2) Which of the following solutions would have the lowest boiling point?
A)1.0 g of NaCl in 100 g of water
B)1.0 g of KNO<sub>3</sub> in 100 g of water
C)1.0 g of NaC<sub>2</sub>H<sub>3</sub>O<sub>2</sub> in 100 g of water
D)All the solutions will have the same boiling point.
Q3) The solubility of ammonium chloride at 70.<sup> </sup><sup>°</sup> C is 60.g of solute per 100.g of water.Whichsolution would be unsaturated at 70.<sup> </sup><sup>°</sup><sup> </sup>C?
A)110.g of solute per 200.g of water
B)120.g of solute per 200.g of water
C)30.g of solute per 50.g of water
D)35g of solute per 50.g of water
Q4) What mass of ethanol,C<sub>2</sub>H<sub>5</sub>OH,is required to decrease the freezing point of 2.000 L of water to -10.00<sup>°</sup> C? (The freezing point depression constant for water is 1.86<sup>°</sup> C/m)
Page 16
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Chapter 15: Acids, Bases, and Salts
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Sample Questions
Q1) What is the concentration of a H<sub>2</sub>SO<sub>4</sub> solution if 15.0 mL of the solution is neutralized by 3.60 mL of a 0.65 M Ca(OH)<sub>2</sub> solution?
A)0.078 M
B)0.16 M
C)0.31 M
D)2.7 M
Q2) Combining potassium hydroxide and sulfuric acid will produce water and A)potassium sulfide.
B)potassium sulfate.
C)potassium sulfite.
D)potassium hypersulfate.
Q3) What is the conjugate base of HS<sup> -1</sup>?
A)H<sub>2</sub>S
B)S<sup> -2</sup>
C)H<sup> +1</sup>
D)OH<sup> -1</sup>
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 addition of a catalyst will change the value of K<sub>eq</sub> in an equilibrium system.
A)True
B)False
Q2) The magnitude of K<sub>eq</sub> depends on
A)initial concentration of reactants.
B)presence of a catalyst.
C)temperature.
D)volume of reaction vessel.
Q3) Which solution has the lowest pH?
A)0.1 M HNO<sub>2</sub>
B)0.1 M HCl<sup> </sup> <sup> </sup>
C)0.1 M KOH
D)0.1 M NH<sub>4</sub>OH
Q4) If HCl (aq)is added to a saturated NaCl solution,the [Na<sup>+1</sup>] will A)increase.
B)decrease.
C)remain the same.
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Chapter 17: Oxidationreduction
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Sample Questions
Q1) What is the oxidation number of chlorine in HClO<sub>4</sub>?
A)0
B)+7
C)-1
D)-3
Q2) Oxygen has the same oxidation number in ozone (O<sub>3</sub>)and in oxygen (O<sub>2</sub>).
A)True
B)False
Q3) Which is the correct oxidation half-reaction for the following equation?
2 Na + 2 H<sub>2</sub>O \(\rarr\) 2 NaOH + H<sub>2</sub>
A)Na<sup>+1</sup> + e<sup>-1</sup> \(\rarr\) Na
B)Na \(\rarr\) Na<sup>+1</sup> + e<sup>-1</sup>
C)2 H<sup>+1</sup> + 2 e<sup>-1</sup> \(\rarr\) H<sub>2</sub>
D)H<sub>2</sub> \(\rarr\) 2 H<sup>+1</sup> + 2 e<sup>-1</sup>
Q4) What always occurs at the anode in an electrolytic cell?
A)Protons are gained
B)Protons are lost
C)Electrons are gained
D)Electrons are lost
Page 19
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Chapter 18: Nuclear Chemistry
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Sample Questions
Q1) In an artificial transmutation process,a nucleus of Al-27 absorbs a neutron,emits an alpha particle,and is converted into a new nuclide.What is the new nuclide formed?
A)Mg-28
B)Na-24
C)P-30
D)Na-28
Q2) In a nuclear reactor,the purpose of the control rods is to A)convert steam into electricity.
B)capture neutrons to slow the rate of fission.
C)cool the steam generated by the reactor.
D)produce neutrons to increase the rate of fission.
Q3) In an artificial transmutation process,a nucleus of Al-27 is absorbs an alpha particle and emits a neutron.What is the new nuclide formed?
A)Na-30
B)Mg-23
C)P-29
D)P-30
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Chapter 19: Introduction to Organic Chemistry Online Only
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Sample Questions
Q1) C<sub>2</sub>H<sub>2</sub> is A)methane.
B)methyne.
C)ethane.
D)ethyne.
Q2) How many pairs of electrons are shared in a triple covalent bond?
A)One
B)Two
C)Three
D)Four
Q3) C<sub>n</sub>H<sub>2n-2</sub> is the general formula for the A)Alkynes
B)Alkanes
C)Alkenes
D)Aromatics
Q4) Which of these has no structural isomers?
A)C<sub>5</sub>H<sub>10</sub>
B)C<sub>4</sub>H<sub>10</sub>
C)C<sub>3</sub>H<sub>8</sub>
D)C<sub>6</sub>H<sub>12</sub>
Page 21
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Chapter 20: Introduction to Biochemistry Online Only
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Sample Questions
Q1) The two strands of the double stranded helix of DNA are held together by A)ionic bonds.
B)hydrogen bonds.
C)peptide bonds.
D)phosphate ester bonds.
Q2) The end product of the digestion of starch is A)cellulose.
B)glucose.
C)glycogen.
D)glucagon.
Q3) Draw the structure for the dipeptide formed by alanine and glycine.
Q4) The complete oxidation of glucose yields water and A)polysaccharides.
B)polypeptides.
C)dextrose.
D)carbon dioxide.
Q5) The bond connecting amino acids in a protein is called a peptide linkage. A)True
B)False
Q6) What is meant by an essential amino acid?
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