Fundamentals of Chemistry Exam Review - 2734 Verified Questions

Fundamentals of Chemistry Exam Review

Course Introduction

Fundamentals of Chemistry provides a comprehensive introduction to the core principles and concepts of chemistry, including atomic and molecular structure, periodicity, chemical bonding, states of matter, and the basics of chemical reactions. The course explores the foundations of stoichiometry, thermochemistry, and the properties of solutions, alongside an introduction to acids, bases, and equilibrium processes. Emphasizing problem-solving and critical thinking, students develop an understanding of how chemical principles apply to everyday life, laboratory practices, and ongoing scientific advancements.

Recommended Textbook Chemistry 10th Edition by Raymond Chang

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Page 2

Chapter 1: Chemistry: The Study of Change

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Sample Questions

Q1) Classify the following as a physical or chemical change: Food spoils. Answer: Chemical

Q2) Classify the following as either a physical or a chemical property: Newspaper burns. Answer: Chemical

Q3) Express the fraction 1/23 as a decimal to 4 significant figures.

A)0.0434

B)0.0435

C)0.04347

D)0.04348

E)0.04350

Answer: D

Q4) The conversion of water into steam is an example of a chemical change. A)True

B)False

Answer: False

Q5) Give examples of three physical properties. Answer: (Answers will vary.)Melting point, boiling point, density, color

Q6) Classify the following as an element, a compound, or a mixture: Chicken broth. Answer: Mixture

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) Use the periodic table above to show where the metalloids are located.

Answer: Group 2A

Q2) Which one of the following elements is most likely to form a 2+ ion?

A)beryllium

B)carbon

C)fluorine

D)oxygen

E)sodium

Answer: A

Q3) The Stock system name for Mn₂O₇ is A)dimanganese heptaoxide.

B)magnesium oxide.

C)manganese(VII)oxide.

D)manganese(II)oxide.

E)manganese(III)oxide.

Answer: C

Q4) Give the formula of nitric acid.

Answer: HNO₃

Q5) Name the following binary compound: MnCl₂.

Answer: manganese(II)chloride

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) How many moles of HCl are represented by 1.0 * 10¹⁹ HCl molecules?

A)1.7 * 10^-5 mol

B)1.5 * 10^-3 mol

C)1.0 * 10¹⁹ mol

D)36.5 mol

E)6.02 * 10⁴ mol

Answer: A

Q2) Refer to the (unbalanced)equation CS₂ + CaO \(\rarr\) CO₂ + CaS. How many grams of CaS are produced if 53 g of CO₂ are produced?

Answer: 170 g

Q3) A 1.375 g sample of mannitol, a sugar found in seaweed, is burned completely in oxygen to give 1.993 g of carbon dioxide and 0.9519 g of water. The empirical formula of mannitol is A)CHO

B)CH₇O₃

C)C₃H₂O

D)C₃H₇O₃

E)CH₂O

Answer: D

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) What element is oxidized in the following chemical reaction? 3Cu + 8HNO₃ \(\rarr\)3Cu(NO₃)₂ + 2NO + 4H₂O

A)Cu

B)H

C)N

D)O

E)H₂O

Q2) Identify the reducing agent in the following reaction. 4Al + 3O₂\(\rarr\)2Al₂O₃

Q3) The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq)\(\rarr\) AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)

A)True

B)False

Q4) A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper and the solution turned a blue color characteristic of copper(II)ions. Write the balanced chemical equation for this reaction.

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Chapter 5: Gases

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Sample Questions

Q1) If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change?

A)8

B)2

C)1/2

D)1/4

E)1/8

Q2) Calculate the density of Br₂(g)at 59.0°C and 1.00 atm pressure.

A)27.2 g/L

B)5.83 g/L

C)769 g/L

D)22.4 g/L

E)3.45 g/L

Q3) At standard temperature and pressure, a given sample of water vapor occupies a volume of 2.80 L. How many moles of water vapor are present?

Q4) On a spring morning (20°C)you fill your tires to a pressure of 2.25 atmospheres.As you ride along, the tire heats up to 45°C from the friction on the road.What is the pressure in your tires now?

Q5) What is the definition of a "gas"?

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Chapter 6: Thermo-Chemistry

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Sample Questions

Q1) When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000.g of water, a temperature rise of 3.60°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)15.87 kJ/°C

B)4.18 kJ/°C

C)5.52 kJ/°C

D)1.34 kJ/°C

E)752.1 kJ/°C

Q2) A 26.2 g piece of copper metal is heated from 21.5°C to 201.6°C. Calculate the amount of heat absorbed by the metal. The specific heat of Cu is 0.385 J/g·°C.

Q3) Which of the following processes is endothermic?

A)O₂(g)+ 2H₂(g)\(\rarr\)2H₂O(g)

B)H₂O(g)\(\rarr\)H₂O(l)

C)3O₂(g)+ 2CH₃OH(g)\(\rarr\)2CO₂(g)+ 2H₂O(g)

D)H₂O(s)\(\rarr\)H₂O(l)

Q4) Define specific heat.

Q5) What is the standard enthalpy of formation of H₂(g)at 25°C?

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200.nm shines on a copper plate?

A)1.48 * 10⁶ m/s

B)6.22 * 10⁵ m/s

C)4.67 * 10⁴ m/s

D)1.97 * 10⁴ m/s

E)1.34 * 10⁶ m/s

Q2) When the electron in a hydrogen atom falls from its first excited energy level to the ground state energy level, a photon with wavelength \(\lambda\) is emitted. A proton having this same wavelength would have a velocity of

A)3.87 m/s

B)5990 m/s

C)1.21 * 10^-7 m/s

D)3.26 m/s

E)5.99 m/s

Q3) What is the total number of electrons possible in the 2p orbitals?

Q4) Write the ground state electron configuration for a lead atom.

Q5) What is the ground-state electron configuration for chlorine?

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) Arrange the following ions in order of decreasing ionic radius: Al³⁺, Mg²⁺, Na⁺, O^2-. decreasing radius \(\rarr\)

A)Al³⁺ > Mg²⁺ > O^2- > Na⁺

B)Al³⁺ > Mg²⁺ > Na⁺ > O^2-

C)Na⁺ > Mg²⁺ > Al³⁺ > O^2-

D)O^2- > Al³⁺ > Mg²⁺ > Na⁺

E)O^2- > Na⁺ > Mg²⁺ > Al³⁺

Q2) Which of the following is a basic oxide?

A)CO₂

B)MgO

C)As₂O₃

D)SO₂

E)Cl₂O₇

Q3) Sodium ions are more reactive than sodium atoms.

A)True

B)False

Q4) Amphoteric oxides exhibit both acidic and basic properties.

A)True

B)False

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which one of the following compounds does not follow the octet rule?

A)NF₃

B)CF₄

C)PF₅

D)AsH₃

E)HCl

Q2) Which of the bonds below would have the greatest polarity (i.e., highest percent ionic character)?

A)Si - P

B)Si - S

C)Si - Se

D)Si - Cl

E)Si - I

Q3) Write the Lewis structure for the product that forms when boron trifluoride combines with ammonia.

Q4) Write the Lewis dot symbol for the chloride ion.

Q5) Write a Lewis structure for SO₃ that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s).

Page 11

Q6) Write the Lewis structure of ammonia (nitrogen trihydride).

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Chapter 10: Chemical Bonding Ii: Molecular Geometry and Hybridization

of Atomic Orbitals

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Sample Questions

Q1) Which of the following correctly lists species in order of increasing bond order?

A)C₂ < Li₂ < Be₂ < N₂

B)Be₂ < Li₂ < C₂ < N₂

C)N₂ < Be₂ < Li₂ < C₂

D)N₂ < C₂ < Li₂ < Be₂

E)Be₂ < C₂ < N₂ < Li₂

Q2) According to the VSEPR theory, the geometry of the SO₃ molecule is A)pyramidal.

B)tetrahedral.

C)trigonal planar.

D)distorted tetrahedron (seesaw).

E)square planar.

Q3) Indicate the type of hybrid orbitals used by the central atom in BrF₃.

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) Given the following compound and its boiling point, identify whether it is polar or nonpolar: HCl, -84.9°C.

Q2) Find the temperature at which water boils on a day in the mountains when the barometric pressure is 593 mmHg.(Given: the heat of vaporization of water is 40.79 kJ/mol)

A)93.1°C

B)117°C

C)41.5°C

D)97.0°C

E)68.1°C

Q3) Helium atoms do not combine to form He₂ molecules, yet He atoms do attract one another weakly through

A)dipole-dipole forces.

B)ion-dipole forces.

C)dispersion forces.

D)dipole-induced dipole forces.

E)hydrogen bonding.

Q4) Of the given pair of compounds, which would have the higher boiling point? H₂Se or H₂O

Q5) Indicate all the types of intermolecular forces of attraction in HCl(g).

Page 13

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Chapter 12: Physical Properties of Solutions

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Sample Questions

Q1) In which of the following solvents would you expect KBr to be most soluble?

A)C₆H₁₄ (hexane)

B)CH₃CH₂OH (ethanol)

C)C₆H₆ (benzene)

D)CCl₄ (carbon tetrachloride)

E)C₆H₁₂ (cyclohexane)

Q2) Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

A)2.45 * 10^-4 m

B)5.80 * 10^-4 m

C)2.45 * 10^-1 m

D)103 m

E)5.80 m

Q3) Maple syrup is mostly a solution of sucrose in water.Calculate the molality of the syrup if a sample freezes at -0.50°C, assuming the solute is pure sucrose. [For water, K_f is 1.86°C/m.]

Q4) 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.

Q5) Define solvation.

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) Given that E_a for a certain biological reaction is 48 kJ/mol and that the rate constant is 2.5 F1F1F1S1 F1F1F10 10^-2 s^-1at 15°C, what is the rate constant at 37°C?

A)2.7 F1F1F1S1 F1F1F10 10^-2 s^-1

B)2.5 F1F1F1S1 F1F1F10 10^-1 s^-1

C)1.0 F1F1F1S1 F1F1F10 10^-1 s^-1

D)6.0 F1F1F1S1 F1F1F10 10^-3 s^-1

E)1.1 s^-1

Q2) The activation energy for the reaction CH₃CO F1F1F1S1 F1F1F10 CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

A)0.40

B)1.1

C)2.5

D)4.0

E)5.0

Q3) The rate constant for a certain first-order reaction is 0.40/min.What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

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15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) 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_c 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.

Q2) 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.

Q3) Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Q4) The dissociation of solid silver chloride in water to produce silver ions and chloride ions has an equilibrium constant of 1.8 * 10^-18.Based on the magnitude of the equilibrium constant, is silver chloride very soluble in water? Why?

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Chapter 15: Acids and Bases

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Sample Questions

Q1) In aqueous solutions at 25°C, the sum of the ion concentrations ([H⁺] + [OH^-])equals

1 * 10^{- 14}.

A)True

B)False

Q2) Acid strength decreases in the series HI > HSO₄^- > HF > HCN.

Which of these anions is the weakest base?

A)I^-

B)SO₄^2-

C)F^-

D)CN^-

Q3) Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized.

A)1.00

B)0.00070

C)3.15

D)5.15

E)7.00

Q4) If the pH of liquid bleach is 12.0, what is the hydroxide ion concentration in this solution?

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Sample Questions

Q1) At 25 °C, the base ionization constant for NH₃ is 1.8 * 10^-5.

Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Q2) Will a precipitate of magnesium fluoride form when 300.mL of 1.1 * 10^-3 M MgCl₂ are added to 500.mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

A)Yes, Q > K_sp

B)No, Q < K_sp

C)No, Q = K_sp

D)Yes, Q < K_sp

Q3) You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH₃COOH)and 0.20 M sodium acetate (CH₃COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a = 1.8 * 10^-5]

A)4.65

B)4.71

C)4.56

D)4.84

E)5.07

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Chapter 17: Chemistry in the Atmosphere

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Sample Questions

Q1) The most prevalent noble gas in our atmosphere is A)helium.

B)neon.

C)argon.

D)krypton.

E)xenon.

Q2) Ozone in the stratosphere protects animals and plants from A)infrared radiation.

B)acid rain.

C)visible sunlight.

D)radioactivity.

E)ultraviolet rays.

Q3) 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.

Q4) Write out the steps in the mechanism of ozone destruction by chlorine atoms.

Page 19

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Chapter 18: Entropy, Free Energy, and Equilibrium

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Q1) The entropy change \(\times\)S° for the reaction NH₄Cl(s)\(\to\) NH₃(g)+ HCl(g)will be negative.

A)True

B)False

Q2) Predict the sign of \(\Delta\)S for the process N₂(g, 10 atm)\(\to\) N₂(g, 1atm).

Q3) The heat of vaporization of water is 2.27 kJ/g. What is \(\Delta\)S_vap per mole at the normal boiling point?

Q4) Which species will have the greatest absolute entropy at 25°C?

A)Ne(g)

B)C₂H₂(g)

C)H₂O(l)

D)C₂H₅OH(l)

E)C₄H₁₀(g)

Q5) The following reaction is spontaneous under standard state conditions at 25°C: AgCl(s)\(\to\) Ag⁺(aq)+ Cl^-(aq)(\(\Delta\)G° = 55 kJ/mol)

A)True

B)False

Q6) How does the entropy change when a solid is melted?

Page 20

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Chapter 19: Electrochemistry

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Sample Questions

Q1) Which one of the following reagents is capable of transforming Cu²⁺(1 M)to Cu(s)?

A)I^-(1 M)

B)Ni(s)

C)Al³⁺(1 M)

D)F^-(1 M)

E)Ag(s)

Q2) In the following half equation, which is the oxidizing agent? NO₃^-(aq)+ 4H⁺(aq)+ 3e^- \(\to\)

NO(g)+ 2H₂O

A)NO₃^-

B)H⁺

C)e^-

D)NO

E)H₂O

Q3) Complete and balance the following redox reaction under basic conditions: CrO₄^2-(aq)+ SO₃^2-(aq)\(\to\) Cr(OH)₃(s)+ SO₄^2-(aq)

Q4) Will H₂(g)form when Ag is placed in 1.0 M HCl?

Q5) Will H₂(g)form when Fe is placed in 1.0 M HCl?

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Chapter 20: Metallurgy and the Chemistry of Metals

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Q1) The principal reducing agent in a blast furnace is

A)CaO(s)

B)CaSiO₃(l)

C)CO(g)

D)O₂(g)

E)CO₂(g)

Q2) Mercury, magnesium, and zinc have low enough boiling points that they can be purified by distillation.

A)True

B)False

Q3) Which of these ions is most likely to substitute for Ca²⁺ in the human body?

A)Cl^-

B)Sr²⁺

C)K⁺

D)S^2-

E)Pb²⁺

Q4) Write the chemical formula of pyrite.

Q5) Write a balanced chemical equation illustrating chemical reduction.

Q6) Write the chemical formula of fluorite.

Page 22

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Chapter 21: Nonmetallic Elements and Their Compounds

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Q1) Write the chemical formula of the oxide ion.

Q2) Alkali metal hydrides are very reactive with water, forming H₂ gas.

A)True

B)False

Q3) When in the liquid state, which one of these substances resembles water, insofar as it is a solvent for many electrolytes and even undergoes autoionization as water does?

A)N₂

B)Cl₂

C)NH₃

D)N₂O

E)Xe

Q4) Chlorine gas is prepared commercially by

A)electrolysis of carbon tetrachloride.

B)oxidation of chloride ion with F₂(g).

C)electrolysis of NaCl(aq).

D)oxidation of chloride ion with Br₂(aq).

E)electrolysis of AlCl₃(aq).

Q5) Write a balanced chemical equation to show the production of chlorine by the chlor-alkali process.

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Chapter 22: Transition Metal Chemistry and Coordination Compounds

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Q1) Name the complex ion [Co(H₂O)₄Cl₂]⁺.

Q2) A molecule or ion that provides an electron pair for coordinate covalent bond formation is called a Lewis ________.

Q3) How many unpaired electrons are there in the complex ion [Mn(CN)₆]^3-?

A)0

B)1

C)2

D)3

E)4

Q4) Draw and label the geometric isomers of [CrF₂Cl₄]^3-?

Q5) Which of these ligands produces the strongest crystal field?

A)Cl^-

B)CO

C)OH^-

D)H₂O

E)NH₃

Page 24

Q6) What is the coodination number of silver in [Ag(NH₃)₂]Cl?

Q7) What is the coordination number of chromium in Cr(en)₂Cl₂?

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Page 25

Chapter 23: Nuclear Chemistry

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Q1) Protactinium-234 has a half-life of 1 minute.How much of a 400.g sample protactinium would remain after 4 minutes?

Q2) If 12% of a certain radioisotope decays in 5.2 years, what is the half-life of this isotope?

A)0.59 yr

B)1.7 yr

C)22 yr

D)28 yr

E)32 yr

Q3) Which is the most penetrating of the three types of nuclear radiation?

A)alpha

B)beta

C)gamma

Q4) The rates of radioactive decay processes, like the rates of chemical reactions, are sensitive to temperature changes.

A)True

B)False

Q5) Protactinium-234 has a half-life of 1 minute.How much of a 400.g sample protactinium would remain after 2 minutes?

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Chapter 24: Organic Chemistry

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Q1) The formula CH₃CH₂CH₂CH=CH₂ represents

A)an alkane.

B)a cycloalkane.

C)an alkene.

D)an alkyne.

E)an aromatic compound.

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) A compound with the formula C₆H₁₂ may or may not be a saturated hydrocarbon.Explain.

Q4) 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) Amides are synthesized from two classes of organic compounds. Those two types of compounds are

A)carboxylic acids and alkenes.

B)amines and alcohols.

C)alcohols and carboxylic acids.

D)amines and carboxylic acids.

E)alkenes and amines.

Q2) An essential amino acid is one that A)must be included in the diet.

B)contains no sulfur.

C)occurs in all types of proteins.

D)is necessary for vitamin production.

E)the body can synthesize.

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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