General Chemistry II Review
Questions
Course Introduction
General Chemistry II builds upon the foundational principles introduced in General Chemistry I, delving deeper into topics such as chemical thermodynamics, kinetics, equilibrium, acids and bases, electrochemistry, and coordination chemistry. The course emphasizes problem-solving skills and the application of chemistry concepts to real-world scenarios. Through lectures, laboratory experiments, and collaborative learning, students will further develop their understanding of the behavior of matter, chemical reactions, and the properties of solutions. This course is essential for students pursuing studies in science, engineering, health professions, and related fields.
Recommended Textbook
Introductory Chemistry 4th Edition by Nivaldo J. Tro
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19 Chapters
1962 Verified Questions
1962 Flashcards
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Page 2
Chapter 1: The Chemical World
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54 Verified Questions
54 Flashcards
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Sample Questions
Q1) Charcoal was burned in a barbecue grill.The ashes that remained weighed considerably less than the charcoal that was burned.Does this mean that the law of conservation of mass is wrong? Explain.
Answer: No.The gaseous products formed during the combustion of charcoal escaped into the air and are not accounted for.If all those products could have been collected and weighed along with the ashes,the total mass of the products would have been equal to the mass of the charcoal.
Q2) An established theory is the pinnacle of scientific understanding.
A)True
B)False
Answer: True
Q3) A hypothesis can never be proven as wrong.
A)True
B)False
Answer: False
Q4) Lavoisier developed the law of conservation of mass.
A)True
B)False Answer: False
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Chapter 2: Measurement and Problem Solving
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Sample Questions
Q1) How many inches are in 2.80 ft?
A)34
B)33.6
C)0.233
D)4.29
E)none of the above
Answer: B
Q2) When the number 2.35 is rounded to contain 2 significant figures it becomes 2.4.
A)True
B)False
Answer: True
Q3) How many cm<sup>3</sup> are there in 2.5 m<sup>3</sup>?
A)2.5 × 10<sup>6</sup>
B)2.5 × 10<sup>-</sup><sup>2</sup>
C)2.5 × 10<sup>2</sup>
D)2.5 × 10<sup>-</sup><sup>6</sup>
E)none of the above
Answer: A
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4
Chapter 3: Matter and Energy
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Sample Questions
Q1) Which type of energy is associated with position?
A)chemical
B)electrical
C)potential
D)kinetic
E)none of the above
Answer: C
Q2) How many kilojoules are there in 95.0 Calories?
A)2.27 × 10<sup>7</sup>
B)3.97 × 10<sup>-</sup><sup>4</sup>
C)397
D)22.7
E)none of the above
Answer: C
Q3) Mixtures of miscible liquids that differ in their boiling points may be separated by distillation.
A)True
B)False
Answer: True
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Page 5
Chapter 4: Atoms and Elements
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Sample Questions
Q1) Which statement reflects the results of Rutherford's gold foil experiments?
A)Almost all of the alpha particles were deflected back in the direction from which they came.
B)Almost all of the alpha particles sputtered gold atoms off of the surface of the foil.
C)Almost all of the alpha particles were deflected while passing through the foil.
D)Almost all of the alpha particles passed directly through the foil.
E)none of the above
Q2) Group 8A elements are also called:
A)noble gases.
B)halogens.
C)alkaline earth metals.
D)alkali metals.
E)none of the above
Q3) If two atoms each contain different numbers of protons,the atoms must be from different elements.
A)True
B)False
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6
Chapter 5: Molecules and Compounds
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Sample Questions
Q1) The correct formula for calcium fluoride is CaF<sub>3</sub>.
A)True
B)False
Q2) Which of the following is a molecular compound?
A)barium sulfide
B)calcium acetate
C)potassium hydroxide
D)nitrogen monoxide
E)none of the above
Q3) The formula of a compound comprised of two nitrogen atoms and one oxygen atom should be written properly as ON<sub>2</sub>.
A)True
B)False
Q4) Which formula shows the proper use of parentheses?
A)Ca(F)<sub>2</sub>
B)Ca(SO<sub>4</sub>)
C)(NH<sub>4</sub>)<sub>3</sub>(PO<sub>4</sub>)
D)Ca(NO<sub>3</sub>)<sub>2</sub>
E)none of the above
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Chapter 6: Chemical Composition
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Sample Questions
Q1) If 3.011 ×<sup> </sup>10<sup>23</sup> molecules have a mass of 20.04 grams,what is the molar mass of this substance?
A)40.08 g/mol
B)10.02 g/mol
C)20.04 g/mol
D)6.658 × 10<sup>-23</sup> g/mol
E)none of the above
Q2) How many moles of fluorine are in 3.2 moles of xenon hexafluoride?
A)22.4
B)12.8
C)19.2
D)16
E)none of the above
Q3) What is the mass of 3.09 × 10<sup>24</sup> atoms of sulfur in grams?
A)9.64 × 10<sup>22</sup>
B)9.91 × 10<sup>25</sup>
C)165
D)0.160
E)none of the above
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Page 8
Chapter 7: Chemical Reactions
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Sample Questions
Q1) Which of the following compounds is INSOLUBLE?
A)potassium acetate
B)lithium carbonate
C)magnesium bromide
D)aluminum sulfide
E)none of the above
Q2) The formation of either a solid or a gas is evidence of a chemical reaction.
A)True
B)False
Q3) Which of the following is NOT evidence that a chemical reaction has occurred?
A)color change when chemicals are contacted with each other
B)solid formation when chemicals are contacted with each other
C)gas formation when chemicals are contacted with each other
D)emission of light when chemicals are contact with each other
E)All of the above are evidence of a chemical reaction.
Q4) Mixing two aqueous solutions will always result in formation of a precipitate.
A)True
B)False
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9
Chapter 8: Quantities in Chemical Reactions
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Sample Questions
Q1) Consider the following generic chemical equation: 2A + 5B C + 3D
If you react 4 units of A with 10 units of B,which statement is TRUE?
A)Substance A will be the limiting reactant.
B)Substance B will be the limiting reactant.
C)There is just enough of A and B so that everything reacts completely.
D)Substance C cannot be formed from this reaction.
E)none of the above
Q2) The primary cause of increasing greenhouse gases is:
A)the burning of vast amounts of rain forests.
B)the production of CO<sub>2</sub> by respiration.
C)the increased use of natural gas,petroleum and coal.
D)the release of CO<sub>2</sub> by decreasing solubility in the ocean.
E)none of the above
Q3) The conversion factor between mass and moles for a compound is the molar mass.
A)True
B)False
Q4) Given the recipe: 2 cups flour + 1 egg + 3 oz blueberries 4 muffins.
You can make 1 dozen muffins from 3 eggs.
A)True
B)False
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Chapter 9: Electrons in Atoms and the Periodic Table
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Sample Questions
Q1) The number of cycles of a wave that passes a stationary point in one second is called its
A)wavelength.
B)frequency.
C)crest.
D)trough.
E)none of the above
Q2) Electrons behave like particles and we can describe their exact paths.
A)True
B)False
Q3) Light is a type of matter.
A)True
B)False
Q4) The atomic size of lithium is larger than the atomic size of nitrogen.
A)True
B)False
Q5) The orbital diagram for fluorine shows 1 unpaired electron in a p orbital.
A)True
B)False
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Chapter 10: Chemical Bonding
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Sample Questions
Q1) What is the molecular geometry of SCl<sub>2</sub>?
A)bent
B)linear
C)tetrahedral
D)trigonal pyramidal
E)not enough information
Q2) What is the angle between electron groups in the linear electron geometry?
A)90°
B)109.5°
C)120°
D)180°
E)not enough information
Q3) Bonding theories are used to predict how atoms bond together to form molecules.
A)True
B)False
Q4) The triple bond present in diatomic nitrogen,N<sub>2</sub>,is what makes this molecule so reactive.
A)True
B)False
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Chapter 11: Gases
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Sample Questions
Q1) Gas particles act independently of each other.
A)True
B)False
Q2) STP conditions are 273 K and 760 mm Hg.
A)True
B)False
Q3) The vapor pressure of water at 20.0°C is 17.5 mm Hg.If the pressure of a gas collected over water was measured to be 453.0 mm Hg.What is the pressure of the pure gas?
A)0.0230 atm
B)0.619 atm
C)0.573 atm
D)0.596 atm
E)none of the above
Q4) What problem could happen if deep sea divers used pure oxygen in their tanks?
A)hypoxia
B)oxygen toxicity
C)nitrogen narcosis
D)rapture of oxygen
E)none of the above
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Chapter 12: Liquids,solids,and Intermolecular Forces
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Sample Questions
Q1) The shapes of protein molecules are determined by intermolecular forces.
A)True
B)False
Q2) Which state of matter has a high density and an indefinite shape?
A)solids
B)liquids
C)gases
D)both solids and liquids
E)none of the above
Q3) How many kJ of heat are needed to completely melt 1.70 moles of H<sub>2</sub>O,given that the water is at its melting point? The heat of fusion for water is 6.02 kJ/mole.
A)30.6
B)10.2
C)3.54
D)63.7
E)none of the above
Q4) Dipole-dipole forces are weaker than dispersion forces.
A)True
B)False
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Chapter 13: Solutions
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Sample Questions
Q1) Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink composed of water.What is the solute in this type of martini?
A)water
B)alcohol
C)ice
D)olive
E)none of the above
Q2) A 90.0 g sample of NaOH is dissolved in water and the solution is diluted to give a final volume of 3.00 liters.The molarity of the final solution is ________.
A)0.500 M
B)0.750 M
C)1.00 M
D)2.25 M
E)none of the above
Q3) The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.
A)True
B)False
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15
Chapter 14: Acids and Bases
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Sample Questions
Q1) The equation HCl (aq)+ H<sub>2</sub>O (l) H<sub>3</sub>O<sup>+</sup> (aq)+ Cl<sup>-</sup><sup> </sup>(aq)properly depicts the behavior of hydrochloric acid in water.
A)True
B)False
Q2) If the pH of an aqueous solution changed from 9.10 to 4.67,what happened to the hydronium ion concentration?
A)It decreased.
B)It became zero.
C)It became less than zero.
D)It increased.
E)none of the above
Q3) The Bronsted-Lowry definition of a base is:
A)a proton donor.
B)a proton acceptor.
C)produces H in solution.
D)produces OH in solution.
E)none of the above
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16
Chapter 15: Chemical Equilibrium
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Sample Questions
Q1) For a given chemical equation,the coefficients for each substance become the exponents for each substance in the written equilibrium expression.
A)True
B)False
Q2) What is the concentration of the Mg<sup>2+</sup> ion in solution when [CO<sub>3</sub><sup>2-</sup>] = 0.25 M given that the K<sub>sp</sub> = 6.82 × 10<sup>-6</sup> for the following reaction: MgCO3(s) Mg<sup>2+</sup> (aq)+ CO<sub>3</sub><sup>2-</sup> (aq)?
A)5.2 × 10<sup>-2</sup>
B)3.7 × 10<sup>4</sup>
C)2.7 × 10<sup>-5</sup>
D)19.2
E)none of the above
Q3) What must be TRUE for a reaction possessing a large equilibrium constant?
A)The reaction rate is fast.
B)The reaction rate is slow.
C)The forward reaction is favored.
D)The reverse reaction is favored.
E)none of the above
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Page 17
Chapter 16: Oxidation and Reduction
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Sample Questions
Q1) A spontaneous redox reaction can be used to produce electrical current.
A)True
B)False
Q2) If you properly balance the following half reaction in acid solution,how many electrons would appear on the product side of the equation? NO (g) NO<sub>3</sub><sup>1</sup><sup>-</sup> (aq)
A)1
B)2
C)3
D)5
E)none of the above
Q3) Fuel cells are based on the tendency of some elements to gain electrons from gasoline.
A)True
B)False
Q4) Rusting of iron requires the presence of both oxygen and water.
A)True
B)False
Q5) Distinguish between a galvanic (voltaic)cell and an electrolytic cell.
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Chapter 17: Radioactivity and Nuclear Chemistry
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Sample Questions
Q1) Nuclear fusion:
A)requires intense temperatures that make it impossible to harness as an energy source with our current technology.
B)is the basis of the hydrogen bomb.
C)can be done but requires the detonation of a traditional fission bomb.
D)is a possible energy source of the future.
E)all of the above
Q2) The energy of the sun comes from fusion reactions.
A)True
B)False
Q3) Nuclear fusion:
A)is the formation of heavier elements from lighter ones.
B)releases a larger amount of heat than nuclear fission.
C)is the energy source of the sun and stars.
D)produces non-radioactive elements.
E)all of the above
Q4) The combination of two light nuclei to form a heavier one is known as nuclear fission.
A)True
B)False
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Chapter 18: Organic Chemistry
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Sample Questions
Q1) Which formula represents butane?
A)C<sub>4</sub>H<sub>10</sub>
B)C<sub>3</sub>H<sub>8</sub>
C)C<sub>7</sub>H<sub>16</sub>
D)C<sub>2</sub>H<sub>6</sub>
E)all of the above
Q2) Hydrocarbons are commonly used for:
A)fuel.
B)wax.
C)fabrics.
D)plastics.
E)all of the above
Q3) Which of the following compounds is an alkyne?
A)C<sub>2</sub>H<sub>6</sub>
B)C<sub>3</sub>H<sub>6</sub>
C)C<sub>2</sub>H<sub>2</sub>
D)C<sub>5</sub>H<sub>12</sub>
E)none of the above
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Chapter 19: Biochemistry
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Sample Questions
Q1) The structure of DNA is:
A)the pleated sheet.
B)the alpha helix.
C)the beta helix.
D)the double helix.
E)none of the above
Q2) Which protein structure provides the large-scale bends and folds in the protein?
A)Primary Structure
B)Secondary Structure
C)Tertiary Structure
D)Quaternary Structure
E)Pental Structure
Q3) Which type of structure is maintained by interaction between R-groups on amino acids that are separated by long distances on the same chain?
A)Primary Structure
B)Secondary Structure
C)Tertiary Structure
D)Quaternary Structure
E)Pental Structure
Q4) What is the difference between saturated and unsaturated fatty acids?
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