Chemical Science
Exam Solutions
Course Introduction
Chemical Science is the study of matter, its properties, composition, structure, and the changes it undergoes during chemical reactions. This course explores foundational concepts such as atomic and molecular theory, chemical bonding, thermodynamics, kinetics, and equilibrium, as well as the behavior and interaction of elements and compounds. Students will gain an understanding of laboratory techniques, analytical methods, and real-world applications in fields such as industry, medicine, and environmental science. Through lectures, laboratory experiments, and problem-solving exercises, students develop critical-thinking skills and a solid grounding in the principles and practices of modern chemistry.
Recommended Textbook Chemistry 10th Edition by Raymond Chang
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Chapter 1: Chemistry: The Study of Change
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Sample Questions
Q1) How many cubic centimeters of an ore containing only 0.22% gold (by mass)must be processed to obtain $100 worth of gold? The density of the ore is 8.0 g/cm<sup>3</sup> and the price of gold is $818 per troy ounce.(14.6 troy oz = 1.0 ordinary pound, called an avoirdupois pound; 1 lb = 454 g)
A)0.48 cm<sup>3</sup>
B)220 cm<sup>3</sup>
C)1.4 * 10<sup>3</sup> cm<sup>3</sup>
D)1.7 * 10<sup>3</sup> cm<sup>3</sup>
E)1.8 * 10<sup>4</sup> cm<sup>3</sup>
Answer: B
Q2) Many home freezers maintain a temperature of 0<sup>\(\circ\)</sup>F. Express this temperature in <sup>\(\circ\)</sup>C.
A)-32<sup>\(\circ\)</sup>C
B)-18<sup>\(\circ\)</sup>C
C)0<sup>\(\circ\)</sup>C
D)18<sup>\(\circ\)</sup>C
E)57.6<sup>\(\circ\)</sup>C
Answer: B
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Chapter 2: Atoms, Molecules, and Ions
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Sample Questions
Q1) Which of the following scientists developed the nuclear model of the atom?
A)John Dalton
B)Robert Millikan
C)J.J.Thomson
D)Henry Moseley
E)Ernest Rutherford
Answer: E
Q2) The formula for isopropyl alcohol is sometimes written as (CH<sub>3</sub>)<sub>2</sub>CHOH to better indicate how the atoms are connected.How many hydrogen atoms would be contained in 3 dozen isopropyl alcohol molecules?
Answer: 288
Q3) When J.J.Thomson discovered the electron, what physical property of the electron did he measure?
A)its charge, e
B)its charge-to-mass ratio, e/m
C)its temperature, T
D)its mass, m
E)its atomic number, Z
Answer: B
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Chapter 3: Mass Relationships in Chemical Reactions
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Sample Questions
Q1) Calculate the molecular mass of menthol, C<sub>10</sub>H<sub>20</sub>O.
A)156 amu
B)140 amu
C)29 amu
D)146 amu
E)136 amu
Answer: A
Q2) One nanogram does not seem like a very large number. How many magnesium atoms are there in 1.00 ng of magnesium?
A)4.11 * 10<sup>-11</sup> atoms
B)2.48 * 10<sup>13</sup> atoms
C)6.83 * 10<sup>-35</sup> atoms
D)6.02 * 10<sup>14</sup> atoms
E)1.46 * 10<sup>34</sup> atoms
Answer: B
Q3) A compound with a percent composition by mass of 87.5% N and 12.5% H was recently discovered.What is the empirical formula for this compound?
Answer: NH<sub>2</sub>
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Chapter 4: Reactions in Aqueous Solution
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Sample Questions
Q1) The following reaction is a redox reaction.
CaC<sub>2</sub>(s)+ H<sub>2</sub>O(l)\(\rarr\) HCCH(g)+ CaO(s)
A)True
B)False
Q2) What is the chemical formula of the salt produced by the complete neutralization of sodium hydroxide with sulfuric acid?
A)Na<sub>2</sub>SO<sub>4</sub>
B)Na<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>
C)Na(SO<sub>4</sub>)<sub>2</sub>
D)NaSO<sub>3</sub>
E)Na<sub>3</sub>SO<sub>4</sub>
Q3) What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide?
A)CaO
B)CaCl<sub>2</sub>
C)CaH<sub>2</sub>
D)CaCl
E)CaClH
Q4) Determine the oxidation number of each of the elements BaNaPO<sub>4</sub>?
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Chapter 5: Gases
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Sample Questions
Q1) Deviations from the ideal gas law are greater at
A)low temperatures and low pressures.
B)low temperatures and high pressures.
C)high temperatures and high pressures.
D)high temperatures and low pressures.
Q2) A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm.Calculate the final volume of the bubble if its initial volume was 2.1 mL.
A)0.72 mL
B)6.2 mL
C)41.4 mL
D)22.4 mL
E)7.1 mL
Q3) Which gas has molecules with the greatest average molecular speed at 25°C?
A)CH<sub>4</sub>
B)Kr
C)N<sub>2</sub>
D)CO<sub>2</sub>
E)Ar
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Chapter 6: Thermo-Chemistry
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Sample Questions
Q1) Calculate the enthalpy of reaction for H<sub>2</sub>(g)+ C<sub>2</sub>H<sub>4</sub>(g)\(\rarr\) C<sub>2</sub>H<sub>6</sub>(g). [\(\Delta\)H°<sub>f</sub>(C<sub>2</sub>H<sub>4</sub>(g))= 52.3 kJ/mol; \(\Delta\)H°<sub>f</sub>(C<sub>2</sub>H<sub>6</sub>(g))= -84.7 kJ/mol]
Q2) Which of the following processes always results in an increase in the energy of a system?
A)The system loses heat and does work on the surroundings.
B)The system gains heat and does work on the surroundings.
C)The system loses heat and has work done on it by the surroundings.
D)The system gains heat and has work done on it by the surroundings.
E)None of these is always true.
Q3) The heat of hydration (\(\Delta\)H<sub>hydr</sub>)of ions is always endothermic. A)True B)False
Q4) How many grams of ethylene (C<sub>2</sub>H<sub>4</sub>)would have to be burned to produce 450 kJ of heat? C<sub>2</sub>H<sub>4</sub>(g)+ 3O<sub>2</sub>(g)\(\rarr\)2CO<sub>2</sub>(g)+ H<sub>2</sub>O(l)\(\Delta\)H°<sub>rxn</sub> = -1411 kJ/mol
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Chapter 7: Quantum Theory and the Electronic Structure of Atoms
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Sample Questions
Q1) What is the wavelength of radiation that has a frequency of 2.10 *10<sup>14</sup> s<sup> -1</sup>?
A)6.30 * 10<sup>22</sup> m
B)7.00 * 10<sup>2</sup> nm
C)7.00 * 10<sup>5</sup> m
D)1.43 * 10<sup>-6</sup> m
E)3.00 * 10<sup>8</sup> m
Q2) How many unpaired electrons does a ground-state atom of sulfur have?
A)0
B)1
C)2
D)3
E)4
Q3) Lanthanide (or rare earth elements)have atoms or ions with partially filled A)s subshells. B)p subshells.
C)d subshells. D)f subshells. E)g subshells.
Q4) Write the ground state electron configuration for an iodine atom.
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Chapter 8: Periodic Relationships Among the Elements
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Sample Questions
Q1) Which one of the following does not have [Xe] as its electronic configuration?
A)Te<sup>2-</sup>
B)I<sup>-</sup>
C)Cs<sup>+</sup>
D)Ba<sup>2+</sup>
E)Sn<sup>4+</sup>
Q2) Write the ground-state electron configuration for I<sup>-</sup>.
Q3) Which ion is isoelectronic with Ar?
A)Fe<sup>2+</sup>
B)F<sup>-</sup>
C)Br<sup>-</sup>
D)Ga<sup>3+</sup>
E)Ca<sup>2+</sup>
Q4) The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l)\(\rarr\) Hg<sup>+</sup>(g)+ e<sup>-</sup> is therefore
A)1006 kJ/mol.
B)greater than 1006 kJ/mol.
C)less than 1006 kJ/mol.
D)is equal to the electron affinity of mercury.
E)is equal to the second ionization energy of mercury.
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Chapter 9: Chemical Bonding I: Basic Concepts
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Sample Questions
Q1) Write the Lewis dot symbol for the chloride ion.
Q2) Which of the following solids would have the highest melting point?
A)NaI
B)NaF
C)MgO
D)MgCl<sub>2</sub>
E)KF
Q3) In the Lewis structure of the iodate ion, IO<sub>3</sub><sup>-</sup>, that satisfies the octet rule, the formal charge on the central iodine atom is A)+2
B)+1
C)0
D)-1
E)-2
Q4) The Si - Cl bond has less ionic character than the C - Cl bond.
A)True
B)False
Q5) Write a Lewis structure for OF<sub>2</sub>.
Q6) Write the Lewis structure of boron trifluoride.
Q7) Write the Lewis dot symbol for the sulfide ion.
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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization
of Atomic Orbitals
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Sample Questions
Q1) According to the VSEPR theory, the molecular geometry of beryllium chloride is A)linear
B)trigonal planar
C)bent
D)tetrahedral
E)trigonal pyramidal
Q2) The geometry of the SF<sub>4</sub> molecule is
A)tetrahedral.
B)trigonal pyramidal.
C)trigonal planar.
D)square planar.
E)distorted tetrahedron (seesaw).
Q3) The geometry of the CS<sub>2</sub> molecule is best described as A)linear.
B)trigonal planar.
C)tetrahedral.
D)bent.
E)trigonal pyramidal.
Q4) Indicate the number of \(\pi\)-bonds in C<sub>2</sub>H<sub>6</sub>.
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Q5) Which should have the longer bond, B<sub>2</sub> or B<sub>2</sub><sup>-</sup>?
Chapter 11: Intermolecular Forces and Liquids and Solids
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Sample Questions
Q1) Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point?
A)ethanol, bp = 78°C
B)methanol, bp = 65°C
C)water, bp = 100°C
D)benzene, bp = 80°C
E)The vapor pressure of each of the liquids at its normal boiling point would be the same.
Q2) What mass of water would need to evaporate from your skin in order to dissipate 1.7 * 10<sup>5</sup> J of heat from your body?
H<sub>2</sub>O(l)\(\rarr\)H<sub>2</sub>O(g)\(\Delta\)H<sub>vap</sub> = 40.7 kJ/mol
A)7.52 * 10<sup>4</sup> g
B)418 g
C)75.2 g
D)58.4 g
E)6.92 * 10<sup>6</sup> g
Q3) Of the given pair of compounds, which would have the higher boiling point? H<sub>2</sub>Se or H<sub>2</sub>O
Q4) Indicate all the types of intermolecular forces of attraction in HCl(g).
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Chapter 12: Physical Properties of Solutions
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Sample Questions
Q1) What is the mass percent CH<sub>3</sub>OH of a 0.256 m CH<sub>3</sub>OH(aq)solution.
A)0.814 %
B)0.992 %
C)1.23 %
D)1.29 %
E)1.51 %
Q2) Automobile radiators usually carry a sticker that indicates that they must contain an antifreeze solution for proper operation, winter or summer.Why should you not use ordinary water during the summer?
Q3) Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.
Q4) Define solvation.
Q5) Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C<sub>12</sub>H<sub>22</sub>O<sub>11</sub>.
Q6) What is the concentration of O<sub>2</sub>(g)in water at 25°C exposed to a partial pressure of oxygen of 325 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10<sup>-3</sup> mol/L·atm.
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Chapter 13: Chemical Kinetics
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Sample Questions
Q1) In the reaction, 2N<sub>2</sub>O F1F1F1S1 F1F1F10 2N<sub>2</sub> + O<sub>2</sub>, oxygen and nitrogen gases are formed at the same rate (mol/L·s).
A)True
B)False
Q2) At a particular temperature the first-order gas-phase reaction 2N<sub>2</sub>O<sub>5</sub> F1F1F1S1 F1F1F10 2N<sub>2</sub>O<sub>4</sub> + O<sub>2</sub> has a half-life for the disappearance of dinitrogen pentoxide of 3240 s. If 1.00 atm of N<sub>2</sub>O<sub>5</sub> is introduced into an evacuated 5.00 L flask, what will be the total pressure of the gases in the flask after 1.50 hours?
A)0.685 atm
B)1.00 atm
C)0.315 atm
D)1.68 atm
E)1.34 atm
Q3) For the first-order reaction, A F1F1F1S1 F1F1F10 products, if half of the initial concentration of A reacts in 20 min, then the remaining half will completely react in the next 20 min.
A)True
B)False
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Chapter 14: Chemical Equilibrium
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Sample Questions
Q1) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.
Q2) The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10<sup>-18</sup>.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?
Q3) What conditions are used in the Haber process to enhance the yield of ammonia? Explain why each condition affects the yield in terms of the Le Châtelier principle.
Q4) Which of these statements is true about chemical equilibria in general?
A)At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants].
B)Equilibrium is the result of the cessation of all chemical change.
C)There is only one set of equilibrium concentrations that equals the K<sub>c</sub> value.
D)At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction.
E)At equilibrium, the rate of the forward reaction is equal to as the rate of the reverse reaction.
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Chapter 15: Acids and Bases
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Sample Questions
Q1) What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO<sub>3</sub>? [K<sub>a</sub>(HIO<sub>3</sub>)= 1.6 * 10<sup>-1</sup>]
A)1.52
B)0.80
C)0.72
D)0.89
E)0.66
Q2) What mass of sodium nitrite must be added to 350.mL of water to give a solution with pH = 8.40? [K<sub>a</sub>(HNO<sub>2</sub>)= 5.6 * 10<sup>-4</sup>]
A)68 g
B)1.7 * 10<sup>-4</sup> g
C)0.039 g
D)8.3 g
E)24 g
Q3) Which of these acids is stronger, H<sub>3</sub>PO<sub>4</sub> or H<sub>3</sub>AsO<sub>4</sub>?
Q4) Which of these acids is stronger, H<sub>2</sub>SO<sub>4</sub> or HSO<sub>4</sub><sup>-</sup>?
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Chapter 16: Acid-Base Equilibria and Solubility Equilibria
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Sample Questions
Q1) What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?
A)1.0
B)6.0
C)7.0
D)8.0
E)13.0
Q2) A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K<sub>a</sub>(HOCl)= 3.2 * 10<sup>-8</sup>]
A)4.10
B)7.00
C)7.19
D)7.49
E)7.80
Q3) At 25 °C, the base ionization constant for NH<sub>3</sub> is 1.8 * 10<sup>-5</sup>. Determine the percentage ionization of a 0.150 M solution of ammonia at 25 °C.
Q4) Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH)buffer that has a pH of 4.77.
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Chapter 17: Chemistry in the Atmosphere
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Sample Questions
Q1) Write out the steps in the reaction scheme for nitrogen fixation by lightening.
Q2) The rate constant of the reaction O + O<sub>3</sub> \(\to\) 2O<sub>2</sub> is 7.0 \(\times\) 10<sup>5</sup> M<sup>-1</sup> s<sup>-1</sup> at -40°C and 4.8 \(\times\) 10<sup>6</sup> M<sup>-</sup><sup>1</sup>s<sup>-1</sup> at 25°C.
Calculate the activation energy of this reaction.
A)2.0 kJ/mol
B)17 kJ/mol
C)1100 kJ/mol
D)25.kJ/mol
E)0.13 kJ/mol
Q3) Which region of the atmosphere contains the ozone layer?
A)thermosphere
B)mesosphere
C)stratosphere
D)troposphere
Q4) The average person breathes about 20 m<sup>3</sup> of air a day.What mass of particulates would a person breathe in a day if the particulate level were 400 micrograms per cubic meter?
Q5) Name four "greenhouse gases" besides carbon dioxide.
Q6) Write out the steps in the mechanism of ozone destruction by chlorine atoms.
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Chapter 18: Entropy, Free Energy, and Equilibrium
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Sample Questions
Q1) Which species will have the greatest absolute entropy at 25°C?
A)Ne(g)
B)C<sub>2</sub>H<sub>2</sub>(g)
C)H<sub>2</sub>O(l)
D)C<sub>2</sub>H<sub>5</sub>OH(l)
E)C<sub>4</sub>H<sub>10</sub>(g)
Q2) Assuming \(\Delta\)S° and \(\Delta\)H° do not vary with temperature, at what temperature will the reaction shown below become spontaneous?
C(s)+ H<sub>2</sub>O(g)\(\to\) H<sub>2</sub>(g)+ CO(s)(\(\Delta\)S° = 133.6 J/K·mol; \(\Delta\)H° = 131.3 kJ/mol)
Q3) For the reaction H<sub>2</sub>O<sub>2</sub>(g)\(\to\) H<sub>2</sub>O(g)+ <sup>1</sup>/<sub>2</sub>O<sub>2</sub>(g), \(\Delta\)H° = -106 kJ/mol and \(\Delta\)S° = 58 J/K·mol at 25°C. Calculate \(\Delta\)G° for this reaction at this temperature.
Q4) How does the entropy change when a molecular solid is dissolved in water?
Q5) For the reaction H<sub>2</sub>O<sub>2</sub>(g)\(\to\) H<sub>2</sub>O(g)+ <sup>1</sup>/<sub>2</sub>O<sub>2</sub>(g), \(\Delta\)H° = -106 kJ/mol and \(\Delta\)S° = 58 J/K·mol at 25°C. Is H<sub>2</sub>O<sub>2</sub>(g)stable with respect to dissociation into water vapor and oxygen gas at 25°C?
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Chapter 19: Electrochemistry
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Q1) The half-reaction that should occur at the anode during electrolysis of an aqueous potassium bromide solution is
A)Br<sub>2</sub> + 2e<sup>-</sup> \(\to\) 2Br<sup>-</sup>.
B)Na \(\to\) Na<sup>+</sup> + e<sup>-</sup>.
C)Na<sup>+</sup> + e<sup>-</sup> \(\to\) Na.
D)2Br<sup>-</sup> \(\to\) Br<sub>2</sub> + 2e<sup>-</sup>.
E)2H<sub>2</sub>O \(\to\)O<sub>2</sub> + 4H<sup>+</sup> + 4e<sup>-</sup>.
Q2) The reduction of 1.00 mole of Cr<sup>3+</sup> to Cr requires 9.65 \(\times\) 10<sup>4</sup> C of electrical charge.
A)True
B)False
Q3) How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO<sub>4</sub> for 90.0 min?
A)0.20 g
B)0.40 g
C)12 g
D)24 g
E)47 g
Q4) Will H<sub>2</sub>(g)form when Ag is placed in 1.0 M HCl?
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Chapter 20: Metallurgy and the Chemistry of Metals
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Q1) Why is cryolite, Na<sub>3</sub>AlF<sub>6</sub>, mixed with alumina prior to electrolysis in the production of Al?
Q2) In Al<sub>2</sub>Cl<sub>6</sub>, the geometry of the molecule at each aluminum atom is
A)trigonal planar
B)tetrahedral
C)trigonal pyramidal
D)square planar
E)octahedral
Q3) The flotation process used in metallurgy involves A)the roasting of sulfides.
B)separation of gangue from ore.
C)electrolytic reduction..
D)chemical reduction of a metal.
E)zone refining.
Q4) The following reaction is used to produce titanium metal at high temperature. TiCl<sub>4</sub>(g)+ 2Mg(l)\(\to\) Ti(s)+ 2MgCl<sub>2</sub>(l)
Which element is oxidized and which is reduced?
Q5) Write the chemical formula of halite.
Q6) Write the chemical formula of calcite.
Page 22
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Chapter 21: Nonmetallic Elements and Their Compounds
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Q1) Phosphoric acid is the most important of the phosphorus oxoacids. Industrially, phosphoric acid is prepared by
A)the Ostwald process.
B)the Haber process.
C)the reaction of phosphate rock with sulfuric acid.
D)the reaction of P<sub>4</sub>O<sub>10</sub> with water.
E)the Frasch process.
Q2) Which of these substances is the active ingredient in ordinary household bleach?
A)HCl
B)Cl<sub>2</sub>
C)NaCl
D)NaClO
E)NaClO<sub>4</sub>
Q3) Write an equation for a laboratory preparation of nitrogen gas.
Q4) Which of these hydrides is the most ionic?
A)LiH
B)NaH
C)CH<sub>4</sub>
D)NH<sub>3</sub>
E)RbH
Page 23
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Chapter 22: Transition Metal Chemistry and Coordination Compounds
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Q1) Predict the number of unpaired electrons in the [Fe(CN)<sub>6</sub>]<sup>4-</sup> ion.
Q2) How many geometric isomers are possible for the complex [CrF<sub>3</sub>Br<sub>3</sub>]<sup>3-</sup>? Draw these isomers.
Q3) In the coordination compound [Cr(NH<sub>3</sub>)(en)<sub>2</sub>Cl]Br<sub>2</sub>, the coordination number (C.N.)and oxidation number (O.N.)of the metal atom are, respectively,
A)C.N.= 6; O.N.= +4.
B)C.N.= 6; O.N.= +3.
C)C.N.= 5; O.N.= +2.
D)C.N.= 4; O.N.= +2.
E)C.N.= 4; O.N.= +3.
Q4) The correct formula for the dibromobis(oxalato)cobaltate(III)ion is [Co(C<sub>2</sub>O<sub>4</sub>)Br<sub>2</sub>]<sup>3+</sup>.
A)True
B)False
Q5) A molecule or atom that accepts an electron pair to form a coordinate covalent bond is called a Lewis _______.
Q6) Write the chemical formula of diamminedichloroplatinum(II).
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Chapter 23: Nuclear Chemistry
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Sample Questions
Q1) The rates of radioactive decay processes, like the rates of chemical reactions, are sensitive to temperature changes.
A)True
B)False
Q2) Find the nuclear binding enrgy of potassium-40 (atomic mass = 39.9632591 amu)in units of joules per nucleon.[Data: neutron mass = 1.674928 \(\times\) 10<sup>-24</sup> g; proton mass = 1.672623 \(\times\) 10<sup>-24</sup>g; electron mass = 9.109387 \(\times\) 10<sup>-28</sup> g; N<sub>A</sub> = 6.0221367 \(\times\) 10<sup>23</sup> /mol; c = 2.99792458 \(\times\) 10<sup>8</sup> m/s]
A)1.37 \(\times\) 10<sup>-12</sup> J/nucleon
B)5.48 \(\times\) 10<sup>-11</sup> J/nucleon
C)5.64 \(\times\) 10<sup>-11</sup> J/nucleon
D)1.41 \(\times\) 10<sup>-12</sup> J/nucleon
E)2.97 \(\times\) 10<sup>-12</sup> J/nucleon
Q3) The isotope of iodine with mass number 128 undergoes beta decay with a half-life of 25.00 minutes. Write a balanced nuclear reaction for this process.
Q4) Strontium-90 has a half-life of 28.8 years.How much strontium-90 was present initially, if after 144 years 10.0 g remain?
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Page 25
Chapter 24: Organic Chemistry
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Sample Questions
Q1) Which of these statements describes a condensation reaction?
A)addition of H<sub>2</sub>O to a double bond
B)linking an acid and an alcohol to make an ester and water
C)addition of H<sub>2</sub> to an alkene
D)oxidation of ethanol to acetaldehyde
E)hydrolysis of an ester
Q2) The reaction of ethylene and water yields
A)an aldehyde.
B)an ester.
C)an alcohol.
D)an ether.
E)an organic acid.
Q3) The octane rating of gasoline refers to its
A)percentage C<sub>8</sub>H<sub>18</sub> by volume.
B)radiation dose.
C)alcohol level.
D)ability to resist engine knocking.
E)percentage of unsaturated hydrocarbons.
Q4) A compound with the formula C<sub>6</sub>H<sub>12</sub> may or may not be a saturated hydrocarbon.Explain.
Page 26
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Chapter 25: Synthetic and Natural Organic Polymers
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Q1) Proteins occurring in the \(\beta\)-pleated sheet structure
A)are relatively inelastic.
B)never occur in nature.
C)produce structurally weak materials.
D)contain no peptide bonds.
E)are not involved in hydrogen bonds.
Q2) Which nitrogen base is found in RNA but not in DNA?
A)adenine
B)cytosine
C)guanine
D)thymine
E)uracil
Q3) A protein that has been reversibly denatured has
A)temporarily lost part or all of its secondary or tertiary structure.
B)temporarily lost part or all of its primary structure.
C)been genetically modified due to errors in the nucleotides in the parent DNA.
D)temporarily lost its amino acid residues.
E)temporarily lost the hydrogen bonding between nitrogenous bases.
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