Fundamentals of Chemistry Exam Bank - 3150 Verified Questions

Fundamentals of Chemistry Exam Bank

Course Introduction

Fundamentals of Chemistry is an introductory course designed to provide a comprehensive understanding of the core principles of chemistry. This course covers essential topics such as atomic structure, periodic trends, chemical bonding, stoichiometry, states of matter, thermochemistry, and the basics of chemical reactions. Students will also gain foundational laboratory skills, engage in experiments that demonstrate theoretical concepts, and develop problem-solving abilities critical for progression in scientific studies. Through lectures, laboratory work, and collaborative activities, students will build a solid base for more advanced studies in chemistry and related scientific fields.

Recommended Textbook Chemistry 12th Edition by Raymond Chang

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25 Chapters

3150 Verified Questions

3150 Flashcards

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Chapter 1: Chemistry: The Study of Change

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Sample Questions

Q1) A tentative explanation for a set of observations that can be tested by further experimentation is referred to as

A) a hypothesis.

B) a law.

C) a theory.

D) none of the above.

Answer: A

Q2) A long course triathlon entails a 2.0 mile swim, an 85.5 mile bike ride and a 15.0 mile run. What is the total distance in kilometers for the triathlon

A) 160 km

B) 165 km

C) 103 km

D) 164.9 km

E) 102.5 km

Answer: D

Q3) The number 0.07010 contains four significant figures.

A)True

B)False

Answer: True

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Page 3

Chapter 2: Atoms Molecules and Ions

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Sample Questions

Q1) Give the formula of magnesium nitrate.

A) MnNO₃

B) Mg(NO₃)₂

C) Mg(NO₂)₂

D) Mn(NO₃)₂

E) MgNO

Answer: B

Q2) What is the empirical formula for C₁₀H₂₂O₂

A) C₁₀H₂₂O₂

B) C₅H₁₁O

C) C₂₀H₄₄O₄

D) C₂H₁₁O

E) C₅H₁₁O₂

Answer: B

Q3) The formula of sulfuric acid is H₂SO₄.

A)True

B)False

Answer: True

Q4) What are the two different ions present in the compound FeCl₃

Answer: \(Fe^{2+}, Cl^-\)

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) Butane is reacted with oxygen gas to form carbon dioxide and water. Write the balanced reaction (omit state symbols (s), (l), (g), (aq), etc.).

A) 2C₄H₁₀ + 12O₂ \(\rarr\) 8CO₂ + 10H₂O

B) 2C₄H₁₀ + 13O₂ \(\rarr\) 8CO₂ + 10H₂O

C) 2C₄H₁₀ + 13O₂ \(\rarr\) 8CO₂ + 8H₂O

D) 2C₄H₁₀ + 10O₂ \(\rarr\) 8CO₂ + 10H₂O

E) None of the above are balanced

Answer: B

Q2) How many moles of iron are present in an iron cylinder that weighs 25 g

A) 0.33 mole

B) 0.45 mole

C) 0.67 mole

D) 0.71 mole

E) None of the above

Answer: B

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) Identify the major ionic species present in an aqueous solution of FeCl₃.

A) Fe⁺, Cl₃^-

B) Fe³⁺, Cl₃^3-

C) Fe³⁺, 3 Cl^-

D) Fe²⁺, 3 Cl^-

E) Fe⁺, 3 Cl^-

Q2) Identify the precipitate(s) formed when solutions of Pb(NO₃)₂(aq), Mg(ClO₄)₂(aq), and (NH₄)₂SO₄(aq) are mixed.

A) PbSO₄

B) MgSO₄

C) NH₄ClO₄

D) NH₄NO₃ and NH₄ClO₄

E) PbSO₄ and MgSO₄

Q3) Hydrogen is oxidized in the following chemical reaction.H₂ + Cl₂ \(\rarr\) 2HCl

A)True

B)False

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6

Chapter 5: Gases

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Sample Questions

Q1) Calculate the volume occupied by 35.2 g of methane gas (CH₄) at 25^\(\circ\)C and 1.0 atm. R = 0.08206 L.atm/K.mol.

A) 0.0186 L

B) 4.5 L

C) 11.2 L

D) 49.2 L E) 53.7 L

Q2) A 2.50-L flask contains a mixture of methane (CH₄) and propane (C₃H₈) at a pressure of 1.45 atm and 20^\(\circ\)C. When this gas mixture is then burned in excess oxygen, 8.60 g of carbon dioxide is formed. (The other product is water.) What is the mole fraction of methane in the original gas mixture

A) 0.145

B) 0.341

C) 0.659

D) 0.855

E) 1.00

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Page 7

Chapter 6: Thermochemistry

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Sample Questions

Q1) Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is -40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21^\(\circ\)C was observed. What is the heat capacity of the bomb calorimeter excluding the water

A) 1.76 kJ/^\(\circ\)C

B) 3.64 kJ/^\(\circ\)C

C) 7.8 kJ/^\(\circ\)C

D) 15.3 kJ/^\(\circ\)C

E) 32.9 kJ/^\(\circ\)C

Q2) When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60^\(\circ\)C was observed. What is the heat capacity of the bomb calorimeter, excluding the water The heat of combustion of benzoic acid is -26.42 kJ/g.

A) 1.34 kJ/^\(\circ\)C

B) 4.18 kJ/^\(\circ\)C

C) 5.52 kJ/^\(\circ\)C

D) 15.87 kJ/^\(\circ\)C

E) 752.1 kJ/^\(\circ\)C

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) An electron loses energy in the transition from a 4f subshell to a 6s subshell.

A)True

B)False

Q2) What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120 nm

A) 2.50 x 10⁹ J

B) 1.66 x 10^-24 J

C) 1.66 x 10^-33 J

D) 2.50 x 10¹⁸J

E) 1.66 x 10^-15J

Q3) Each shell (principal energy level) of quantum number n contains n subshells.

A)True

B)False

Q4) 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.

Page 9

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) Which of the following ground-state ions has the largest number of unpaired electrons

A) Cr²⁺

B) Mn²⁺

C) Ni²⁺

D) Cu⁺

E) Co²⁺

Q2) Which of the following elements is found as a monatomic species in its most stable form

A) sulfur

B) oxygen

C) hydrogen

D) argon

E) phosphorus

Q3) Which of the following is the electron configuration for the bromide ion

A) [Ar]

B) [Ar]4s²3d¹⁰4p⁷

C) [Kr]

D) [Kr]5s²4d¹⁰5p⁷

E) [Xe]

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which of the following is a useful guideline for the application of formal charges in neutral molecules

A) A Lewis structure in which there are no formal charges is preferred.

B) Lewis structures with large formal charges are preferred.

C) The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms.

Q2) How many covalent bonds will be drawn to bromine in BrO₃^- for the dot structure that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s)

A) 3

B) 4

C) 5

D) 6

E) 7

Q3) Covalent bonding is the only type of bonding present in the ClO₂^- ion.

A)True

B)False

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Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization

of Atomic

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Sample Questions

Q1) Valence Bond Theory alone can be used to determine that O₂ is paramagnetic.

A)True

B)False

Q2) The geometry of the ClF₃ molecule is best described as:

A) distorted tetrahedron

B) trigonal planar

C) tetrahedral

D) T-shaped

E) trigonal pyramidal

Q3) According to VSEPR theory, which one of the following molecules is trigonal bipyramidal

A) SF₄

B) XeF₄

C) NF₃

D) SF₆

E) PF₅

Q4) There is one \(\pi\)-bond in N₂H₂.

A)True

B)False

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) A phase change from the gas phase directly to the solid phase is called:

A) Sublimation

B) Condensation

C) Freezing

D) Melting

E) Deposition

Q2) The intermolecular forces present in CO include which of the following

I. dipole-dipole

II. ion-dipole

III. dispersion

IV. hydrogen bonding

A) I, II, III, and IV

B) I and III

C) I, III, and IV

D) I and II

E) II and IV

Q3) C₈H₁₈ has a higher vapor pressure than C₄H₁₀.

A)True

B)False

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Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) What is the osmotic pressure of a solution prepared from 13.7 g of the electrolyte HCl and enough water to make 0.500 L of solution at 18^\(\circ\)C

A) 0.55 atm

B) 1.10 atm

C) 8.95 atm

D) 17.9 atm

E) 35.9 atm

Q2) A 20.0 % by mass solution of phosphoric acid (H₃PO₄) in water has a density of 1.114 g/mL at 20^\(\circ\)C. What is the molarity of this solution

A) 0.0114 M

B) 0.0568 M

C) 0.114 M

D) 2.27 M

E) 11.4 M

Q3) The vapor pressure of a solution depends on the chemical nature of the non-volatile solute.

A)True

B)False

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Page 14

Chapter 13: Chemical Kinetics

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Sample Questions

Q1) The half life for a first order reaction is 45 min. What is the rate constant in units of s^-1

A) 0.015 s^-1

B) 65 s^-1

C) 2.6 x 10^-4 s^-1

D) 3.9 x 10³ s^-1

E) 1.9 x 10³ s^-1

Q2) The isomerization of methyl isocyanide, CH₃NC \(\rarr\) CH₃CN, follows first-order kinetics. The half-lives were found to be 161 min at 199^\(\circ\)C and 12.5 min at 230^\(\circ\)C. Calculate the activation energy for this reaction.

A) 6.17 * 10^-3 kJ/mol

B) 31.4 kJ/mol

C) 78.2 kJ/mol

D) 124 kJ/mol

E) 163 kJ/mol

Q3) The rate determining step must be the first step of a reaction mechanism in all cases.

A)True B)False

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) Consider the following equilibrium: 4NH₃(g) + 3O₂(g) 2N₂(g) + 6H₂O(g) + 1531 kJ

The concentrations the reactants would increase after nitrogen gas was removed from the system.

A)True

B)False

Q2) Hydrogen iodide decomposes according to the equation 2HI(g) \(\rightleftharpoons\) H₂(g) + I₂(g), for which K_c

= 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium.

A) 0.138 M

B) 0.220 M

C) 0.550 M

D) 0.275 M

E) 0.0275 M

Q3) For the reaction H₂(g) + I₂(g) 2HI(g), K_P = K_c.

A)True B)False

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Chapter 15: Acids and Bases

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Sample Questions

Q1) Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

A) 0.85

B) 1.70

C) 2.10

D) 11.90

E) 13.10

Q2) Which one of these salts will form a basic solution upon dissolving in water

A) NaCl

B) NaNO₂

C) NH₄NO₃

D) KBr

E) AlCl₃

Q3) The oxides CO₂ and SO₃ will form the following acids in water, respectively.

A) H₂CO₃(aq) and H₂SO₃(aq)

B) H₂CO₃(aq) and H₂SO₄(aq)

C) H₂CO₂(aq) and H₂SO₃(aq)

D) H₂CO₂(aq) and H₂SO₄(aq)

E) HCOO^-(aq) and H₂SO₃(aq)

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Page 17

Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) Acid dissociation constants for phosphoric acid are given below.

\(\begin{array}{|l|l|l|l|}

\hline & \mathrm{K}_{\mathrm{a} 1} & \mathrm{~K}_{\mathrm{a} 2} & \mathrm{~K}_{\mathrm{a} 3} \\

\hline \mathrm{H}_{3} \mathrm{PO}_{4} & 7.5 \times 10^{-3} & 6.2 \times 10^{-8} & 4.8 \times 10^{-13} \\ \hline

\end{array}\) A buffer with a pH = 7.4 can best be made by using

A) H₃PO₄ and NaH₂PO₄.

B) NaH₂PO₄ and Na₂HPO₄.

C) Na₂HPO₄ and Na₃PO₄.

D) only NaH₂PO₄.

E) only Na₂HPO₄.

Q2) Which of the following would decrease the K_sp for PbI₂

A) Lowering the pH of the solution

B) Adding a solution of Pb(NO₃)₂

C) Adding a solution of KI

D) None of the above-the K_sp of a compound is constant at constant temperature.

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Page 18

Chapter 17: Entropy Free Energy and Equilibrium

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Sample Questions

Q1) Consider the reaction CO(g) + 2H₂(g) \(\leftrightharpoons\)

CH₃OH(l) at 25^\(\circ\)C.

\(\Delta\)G^\(\circ\)_f (CO) = -137.3 kJ/mol

\(\Delta\)G^\(\circ\)_f (CH₃OH) = -166.3 kJ/mol

\(\Delta\)H^\(\circ\)_f (CO) = -110.5 kJ/mol

\(\Delta\)H^\(\circ\)_f (CH₃OH) = -238.7 kJ/mol

S^\(\circ\)(CO) = 197.9 J/K·mol

S^\(\circ\)(CH₃OH) = 126.8 J/K·mol

Calculate \(\Delta\)G^\(\circ\) at 25^\(\circ\)C.

A) -29.0 kJ/mol

B) -31.0 kJ/mol

C) -33.0 kJ/mol

D) -35.0 kJ/mol

E) None of the above

Q2) For a given substance the entropy always increases in the following order:

S (gas) < S (liq) < S (solid).

A)True

B)False

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Page 19

Chapter 18: Electrochemistry

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Sample Questions

Q1) How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl₃

A) 6.50 * 10⁴ C

B) 2.16 * 10⁴ C

C) 6.40 * 10⁴ C

D) 1.95 * 10⁵ C

E) 1.01 * 10⁷ C

Q2) Under acidic conditions, the correctly balanced equation for the redox reaction Cr₂O₇^2-(aq) + I^-(aq) \(\rarr\) Cr³⁺(aq) + IO₃^-(aq) Is:

Cr₂O₇^2-(aq) + I^-(aq) + 8H⁺(aq) \(\rarr\) 2Cr³⁺(aq) + IO₃^-(aq) + 4H₂O(l)

A)True

B)False

Q3) H₂(g) will form when Fe is placed in 1.0 M HCl.

A)True

B)False

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Page 20

Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) How old is a bottle of wine if the tritium (³H) content is 25% that of a new wine? The half-life of tritium is 12.5 years.

A) 0.25 yr

B) 3.1 yr

C) 25 yr

D) 38 yr

E) 50. yr

Q2) The half-life of ¹⁴C is 5,730 yr. Assuming some charcoal from a campfire 29,000 years old was found, what fraction of the original C-14 would remain today

A) 3.0 * 10^-2

B) 0.197

C) 3.51

D) 33.3

E) None of these.

Q3) Both H₂O and D₂O can be used as moderators to slow neutrons in nuclear reactors.

A)True

B)False

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Chapter 20: Chemistry in the Atmosphere

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Sample Questions

Q1) Which one of the following reactions is an example of nitrogen fixation

A)N₂O₅(g) \(\rarr\)NO₃(g) + NO₂(g)

B)N₂(g) + O₂(g) \(\rarr\) 2NO(g)

C)3NO₂(g) + H₂O(l) \(\rarr\)2HNO₃(aq) + NO(g)

D)2NO(g) + O₂(g) \(\rarr\) 2NO₂(g)

E)2NH₃(g) \(\rarr\)3H₂(aq) + N₂(g)

Q2) Which statement about ozone and the ozone layer is true

A) Ozone is found in a band of almost pure ozone several kilometers thick encircling the Earth.

B) The ozone in the ozone layer absorbs UV light between 200 and 300 nm.

C) Ozone is a compound with the chemical formula CO₂.

D) In the Earth's atmosphere, ozone exists only in the ozone layer.

E) Ozone is used as a coolant in refrigerators and air conditioners.

Q3) Determine two effects expected from the depletion of the ozone layer.1) asthma 2) lung cancer 3) skin cancer 4) genetic mutations 5) emphysema

A) 1 and 5

B) 2 and 3

C) 3 and 5

D) 3 and 4

E) 4 and 5

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Chapter 21: Metallurgy and the Chemistry of Metals

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Q1) Write the chemical formula of dolomite that provides a source for both magnesium and calcium.

A)CaCO₃ \(\times\)Mg(OH)₂ B)Ca(OH)₂ \(\times\)MgCO₃ C)Ca(OH)₂ \(\times\) Mg(OH)₂

D)CaCO₃ \(\times\) MgCO₃

E) None of the above

Q2) The following reaction is used to produce chromium metal at high temperature.Cr₂O₃(s) + 2Al(s) \(\rarr\) 2Cr(l) + Al₂O₃(s)

Which element is oxidized and which is reduced

A) Both chromium and aluminum are oxidized

B) Chromium is oxidized and aluminum is reduced

C) Chromium is reduced and aluminum is oxidized

D) Neither chromium or aluminum are oxidized

E) None of the above

Q3) The chemical formula of magnetite can be expressed as either Fe₃O₄ or FeO \(\times\) Fe₂O₃

A)True

B)False

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Chapter 22: Nonmetallic Elements and Their Compounds

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Q1) Hydrogen plays an important role in many industrial processes. The following correctly represents a balanced chemical equation for its production by the water gas reaction.C(s) + H₂O(g) \(\rarr\) CO(g) + H₂(g)

A)True

B)False

Q2) Based on the following options, select the compound with hydrogen in the - 1 oxidation state.

A) NaH

B) B₂H₆

C) H₂SO₄

D) H₂S

E) PH₃

Q3) Select basic oxide from the choices given.

A) CaO

B) SiO₂

C) CO₂

D) P₄O₆

E) H₂O₂

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Page 24

Chapter 23: Transition Metals Chemistry and Coordination Compounds

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Q1) What is the coordination number of cobalt in [Co(NHS1U1B13S1U1B0)S1U1B16S1U1B0]ClS1U1B13S1U1B0

A) 2

B) 4

C) 6

D) 8

E) None of the above

Q2) The correct name for [Fe(CO)₆]Br₃ is:

A) hexacarbonyliron(II) bromide

B) hexacarbonyliron(III) bromide

C) hexacarbonyltribromoiron(III)

D) hexacarbonyltribromoiron(II)

E) hexacarbonyliron(III) tribromide

Q3) Which of these ligands produces the strongest crystal field

A) Cl^-

B) CO

C) OH^-

D) H₂O

E) NH₃

Page 25

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Chapter 24: Organic Chemistry

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Q1) Which type of organic compound contains a hydroxyl functional group

A) ester

B) ether

C) carboxylic acid

D) aldehyde

E) ketone

Q2) The group of atoms that is responsible for the characteristic properties of a family of organic compounds is called a/an

A) reaction center.

B) functional group.

C) binding site.

D) enzyme.

E) polyatomic ion.

Q3) The oxidation product of 1-propanol when using Cr₂O₇^2- as the oxidizing agent is acetone.

A)True

B)False

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Chapter 25: Synthetic and Natural Organic Polymers

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Q1) Which choice lists both the sugar and the nitrogen base that are a part of RNA but are not part of DNA

A) deoxyribose and thymine

B) ribose and deoxyribose

C) ribose and uracil

D) uracil and thymine

E) ribose and thymine

Q2) The backbone of a strand of nucleic acid consists of

A) phosphate units only.

B) phosphate and sugar units.

C) polyester.

D) phosphate, sugar, and nitrogen base units.

E) sugar units only.

Q3) Cysteine and methionine are unique among the twenty essential amino acids in that they

A) are chiral.

B) contain an aromatic ring.

C) do not form dipolar ions.

D) contain sulfur.

E) cannot join with other amino acids to form peptides.

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