General Chemistry I Final Exam Questions - 2734 Verified Questions

General Chemistry I Final Exam Questions

Course Introduction

General Chemistry I introduces the foundational concepts of chemistry, focusing on the structure and properties of matter, atomic theory, periodic trends, chemical bonding, stoichiometry, chemical reactions, and an introduction to thermochemistry and gas laws. This course emphasizes the development of problem-solving skills and laboratory techniques necessary for further study in the physical and biological sciences. Through lectures and hands-on experiments, students gain a comprehensive understanding of the principles governing chemical behavior and their applications in real-world contexts.

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) The city of Los Angeles is now approximately 2400 miles south of Alaska. It is moving slowly northward as the San Andreas fault slides along. If Los Angeles is to arrive near Anchorage, Alaska, in 76 million years, at what average rate will it have to move in mm per month?

A)2.0 * 10^-10 mm/mo.

B)6.6 * 10^-6 mm/mo.

C)4.2 mm/mo.

D)9.5 mm/mo.

E)51 mm/mo.

Answer: C

Q2) If a car has an EPA mileage rating of 30 miles per gallon, what is this rating in kilometers per liter? (1 L = 1.06 qt)

A)200 km/L

B)180 km/L

C)70 km/L

D)13 km/L

E)11 km/L

Answer: D

Q3) Classify the following as an element, a compound, or a mixture: Air.

Answer: Mixture

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Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) The formula for isopropyl alcohol is sometimes written as (CH₃)₂CHOH to better indicate how the atoms are connected.How many hydrogen atoms would be contained in 3 dozen isopropyl alcohol molecules?

Answer: 288

Q2) Use the periodic table above to show where the alkali metals are located.

Answer: Group 1A

Q3) How many protons are there in one atom of uranium? Answer: 92

Q4) Give the formula for calcium chloride. Answer: CaCl₂

Q5) Give the number of protons (p), electrons (e), and neutrons (n)in one atom of nickel-62.

A)28 p, 28 e, 28 n

B)28 p, 28 e, 34 n

C)62 p, 28 e, 28 n

D)62 p, 62 e, 28 n

Answer: B

Q6) Write the formula for the acid formed from the nitrite anion, and then name the acid. Answer: HNO₂, nitrous acid

Page 4

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) Calculate the percent composition by mass of oxygen in Na₂CO₃.

Answer: 45.3%

Q2) Which one of the following does not represent 1.00 mol of the indicated substance?

A)6.02 * 10²³ C atoms

B)26.0 g Fe

C)12.01 g C

D)65.4 g Zn

E)6.02* 10²³ Fe atoms

Answer: B

Q3) Which of the following samples contains the greatest number of atoms?

A)100 g of Pb

B)2.0 mole of Ar

C)0.1 mole of Fe

D)5 g of He

E)20 million O₂ molecules

Answer: B

Q4) Calculate the molecular mass, in g/mol, of H₂SO₄.

Answer: 98.09 g/mol

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Chapter 4: Reactions in Aqueous Solution

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Sample Questions

Q1) Identify the following compound as a strong electrolyte, weak electrolyte, or nonelectrolyte: CH₃COOH.

Q2) Based on the solubility rules, which one of the following should be soluble in water?

A)(NH₄)₃PO₄

B)Ca₃(PO₄)₂

C)AlPO₄

D)Ag₃PO₄

E)Mg₃(PO₄)₂

Q3) The following experiments were carried out and observations recorded.

Expt.#1: copper metal was added to an aqueous solution of silver nitrate

Observation: The copper become coated with a substance.

Expt.#2: lead metal was added to an aqueous solution of copper(II)nitrate

Observation: The lead turned black and crumbled.

Expt.#3: zinc metal was added to an aqueous solution of lead(II)nitrate

Observation: The zinc appeared to fall apart.

Rank the metals from most active to least active.

Q4) Give an example of a triprotic acid.

Q5) Identify the following compound as an electrolyte or nonelectrolyte: MgCl₂.

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Chapter 5: Gases

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Q1) Many automobiles produce about 5 grams of NO for each mile they are driven. How many liters of NO gas at STP would be produced on a 100-mile trip?

Q2) Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100.cm³ at 95°C, and 1,000.mmHg.

A)0.19 g/mol

B)35.3 g/mol

C)70.9 g/mol

D)137 g/mol

E)384 g/mol

Q3) Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water. What volume of oxygen at STP is necessary to react with 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL.1 gal = 3.78 L)

Q4) In a weather forecast on a Seattle radio station the barometric pressure was reported to be 29.4 inches.What is this pressure in SI units? (1 inch = 25.4 mm, 1 atm = 760 mmHg)

Q5) How many grams of N₂O, nitrous oxide, are contained in 500.mL of the gas at STP?

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Chapter 6: Thermo-Chemistry

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Sample Questions

Q1) At body temperature 2,404 joules of energy are required to evaporate 1.00 g of water.After vigorous exercise, a person feels chilly because the body is giving up heat to evaporate the perspiration.A typical person perspires 25 mL of water after 20.minutes of exercise.How much body heat is this person using to evaporate this water?

Q2) Radiant energy is

A)the energy stored within the structural units of chemical substances.

B)the energy associated with the random motion of atoms and molecules.

C)solar energy, i.e.energy that comes from the sun.

D)energy available by virtue of an object's position.

Q3) Chemical energy is

A)the energy stored within the structural units of chemical substances.

B)the energy associated with the random motion of atoms and molecules.

C)solar energy, i.e.energy that comes from the sun.

D)energy available by virtue of an object's position.

Q4) A feverish student weighing 75 kilograms was immersed in 400.kg of water at 4.0°C to try to reduce the fever.The student's body temperature dropped from 40.0°C to 37.0°C.Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

Q5) Define specific heat.

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Chapter 7: Quantum Theory and the Electronic Structure of Atoms

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Sample Questions

Q1) An FM radio station broadcasts at a frequency of 101.7 MHz.Calculate the wavelength of the broadcast signal in meters.(c = 2.9979 * 10⁸ m/s)

Q2) Which element has the following ground-state electron configuration? [Kr]5s²4d¹⁰5p²

A)Sn

B)Sb

C)Pb

D)Ge

E)Te

Q3) What is the wavelength, in meters, of an alpha particle with a kinetic energy of 8.0 * 10^-13 J.[mass of an alpha particle = 4.00150 amu; 1 amu = 1.67 *10^-27 kg]

Q4) Write the ground state electron configuration for Ni.

Q5) What is the wavelength, in meters, of an alpha particle with a kinetic energy of 8.0 * 10^-13 J.(mass of an alpha particle = 4.00150 amu; 1 amu = 1.67 * 10^-27 kg)

Q6) Write the ground state electron configuration for the phosphorus atom.

Q7) What is the ground-state electron configuration for chlorine?

Q8) Write the ground state electron configuration for a lead atom. Page 9

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Chapter 8: Periodic Relationships Among the Elements

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Sample Questions

Q1) How many electrons are in the 4p orbitals of vanadium?

A)0

B)2

C)4

D)5

E)6

Q2) How many electrons are in the 4p orbitals of selenium?

A)0

B)2

C)4

D)5

E)6

Q3) Since zirconium is a metal, ZrO₂ is expected to be a/an _____ oxide.

A)acidic

B)ionic

C)amphoteric

D)neutral

E)basic

Q4) Write the ground-state electron configuration for Mg²⁺.

Q5) Write the ground-state electron configuration for Al³⁺.

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Chapter 9: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which one of these polar covalent bonds would have the greatest percent ionic character?

A)H -Br

B)H - Cl

C)H - F

D)H- I

Q2) Use the bond enthalpy data given to estimate the heat released when 25.0 g of acetylene gas, C₂H₂, burns in excess oxygen to yield carbon dioxide and water vapor at 25°C. BE(C-C)= 347 kJ/mol

BE(C\(\equiv\)C)= 812 kJ/mol

BE(C=O in CO₂)= 799 kJ/mol

BE(C-H)= 414 kJ/mol

BE(O-H)= 460 kJ/mol

BE(O=O)= 498.7 kJ/mol

A)1180 kJ

B)447 kJ

C)364 kJ

D)1230 kJ

E)16.8 kJ

Q3) 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) Indicate the type of hybrid orbitals used by the central atom in PCl₃.

A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Q2) The number of pi bonds in the oxalate ion

(C₂O₄^2-)is

A)1

B)2

C)3

D)4

E)5

Q3) The hybridization of the central nitrogen atom in the molecule N₂O is A)sp

B)sp²

C)sp³

D)sp³d

E)sp³d²

Page 13

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Chapter 11: Intermolecular Forces and Liquids and Solids

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Sample Questions

Q1) The zincblende structure of ZnS has the relatively large sulfide ions arranged at the lattice points of a face-centered cubic structure. The edge length of this cubic unit cell is 540.9 pm.Determine the density of zincblende.

A)3.081 g/cm³

B)1.023 g/cm³

C)4.091 g/cm³

D)2.046 g/cm³

E)2.032 g/cm³

Q2) Indicate all the types of intermolecular forces of attraction in F₂(l).

Q3) Which of the following properties indicates the presence of weak intermolecular forces in a liquid?

A)a high heat of vaporization

B)a high critical temperature

C)a high vapor pressure

D)a high boiling point

E)None of the above.

Q4) Methane has a heat of fusion of 0.84 kJ/mol and a heat of vaporization of 9.2 kJ/mol.Estimate the value for the heat of sublimation.

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Chapter 12: Physical Properties of Solutions

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Q1) How many grams of water are needed to dissolve 27.8 g of ammonium nitrate

NH₄NO₃ in order to prepare a 0.452 m solution?

A)769 g

B)36.2 g

C)100.g

D)0.157 g

E)157 g

Q2) Which of the following has the greater molal concentration (molality)?

A)1.0 m KNO₃

B)1.0 M KNO₃

C)Both have same molality.

Q3) What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

A)17.6°C

B)-176°C

C)-1.50°C

D)1.50°C

E)-17.6°C

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) Benzoyl chloride, C₆H₅COCl, reacts with water to form benzoic acid, C₆H₅COOH, and hydrochloric acid. This first-order reaction is 25% complete after 26 s. How much longer would one have to wait in order to obtain 99% conversion of benzoyl chloride to benzoic acid?

A)393 s

B)419 s

C)183 s

D)293 s

E)209 s

Q2) A nuclear stress test utilizes a gamma-emitting radioisotope such as thallium-201 to follow the flow of blood through the heart - first at rest, and then under stress.The first-order rate constant for the decay of thallium-201 is 9.5 x 10^-3 hr^-1.Calculate how long it takes for the amount of thallium-201 to fall to 5.0% of its original value.

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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Chapter 14: Chemical Equilibrium

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Q1) 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?

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) 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.

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Chapter 15: Acids and Bases

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Q1) A 8.0 M solution of formic acid (HCOOH)is 0.47% ionized.What is the K_a of formic acid?

Q2) What is the pH of a solution prepared by mixing 100.mL of 0.0500 M HCl with 300.mL of 0.500 M HF? [K_a(HF)= 7.1 * 10^-4]

A)1.47

B)1.90

C)1.30

D)1.63

E)2.82

Q3) Calculate the pH of a carbonated beverage in which the hydrogen ion concentration is 3.4 * 10^-4 M.

A)2.34

B)3.47

C)6.01

D)7.99

E)10.53

Q4) If the pH of seawater is 8.0, what is the hydroxide ion concentration in seawater?

Q5) Write the chemical formula for perchloric acid.

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Chapter 16: Acid-Base Equilibria and Solubility Equilibria

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Q1) Calculate the silver ion concentration in a saturated solution of silver(I)sulfate (K_sp = 1.4 * 10^-5).

A)1.5 * 10^-2 M

B)2.4 * 10^-2 M

C)3.0 * 10^-2 M

D)1.4 * 10^-5 M

E)None of the above.

Q2) 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

Q3) Bromothymol blue is a common acid-base indicator. It has a K_a equal to 1.6 * 10^-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

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Chapter 17: Chemistry in the Atmosphere

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

A)N₂O₅(g)\(\to\) NO₃(g)+ NO₂(g)

B)N₂(g)+ O₂(g)\(\to\) 2NO(g)

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

D)2NO(g)+ O₂(g)\(\to\) 2NO₂(g)

E)2NH₃(g)\(\to\) 3H₂(aq)+ N₂(g)

Q2) Write out the steps in the mechanism of ozone destruction by chlorine atoms.

Q3) Acid rain is precipitation having a pH that is

A)above 7.

B)below 5.5.

C)below 7.

D)above 8.6.

E)above 10.

Q4) Ozone is formed in the atmosphere by the combination of oxygen molecules with A)chlorofluorocarbons

B)hydrocarbons

C)oxygen atoms

D)CO₂

E)ClO

Q5) Name four "greenhouse gases" besides carbon dioxide.

Page 20

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Chapter 18: Entropy, Free Energy, and Equilibrium

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Q1) The heat of vaporization of water is 2.27 kJ/g. What is \(\Delta\)S_vap per mole at the normal boiling point?

Q2) The entropy change on vaporization (\(\Delta\)S_vap)of a compound or element is A)always negative. B)always positive.

C)sometimes is positive and sometimes is negative.

Q3) The following reaction is nonspontaneous at 25°C: Cu₂O(s)\(\to\) 2Cu(s)+ ¹/₂O₂(g), \(\Delta\)G° = 141 kJ/mol

If \(\Delta\)S° = 75.8 J/K·mol, what is the lowest temperature at which the reaction will be spontaneous?

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

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Chapter 19: Electrochemistry

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Q1) Consider the reaction Fe + Sn²⁺(1 \(\times\) 10^-3 M)\(\to\) Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

Q2) Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s)+ Cl^-\(\to\) Pb²⁺ + Cl₂(g)(acidic solution)

A)2

B)4

C)5 D)9

E)11

Q3) Calculate the cell voltage for the following reaction: Cu²⁺ (0.010 M)+ H₂(1 atm)\(\to\) Cu(s)+ 2H⁺( pH = 7.0)

A)0.19 V

B)-0.01 V

C)0.34 V

D)0.69 V

E)0.49 V

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Chapter 20: Metallurgy and the Chemistry of Metals

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Q1) In the Mond process, nickel is purified by

A)dissolving the crude ore in sulfuric acid, and precipitating the nickel(II)ion as the sulfate salt.

B)dissolving the crude ore in a lye (NaOH)solution, and precipitating the nickel(II)ion as the hydroxide salt.

C)heating the crude ore to its melting point and electrolytically reducing the nickel(II)ions to form the metal.

D)passing sodium gas over the crude ore at high temperatures, chemically reducing the nickel(II)to nickel metal.

E)passing carbon monoxide over the impure metal at high temperature, forming the volatile Ni(CO)₄ which is removed as a gas.

Q2) Write a balanced chemical equation illustrating chemical reduction.

Q3) Why is cryolite, Na₃AlF₆, mixed with alumina prior to electrolysis in the production of Al?

Q4) Write a balanced chemical equation illustrating roasting.

Q5) Write the chemical formula of dolomite that provides a source for both magnesium and calcium.

Q6) Write the chemical formula of epsomite (sold in pharmacies as Epsom salts).

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Chapter 21: Nonmetallic Elements and Their Compounds

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Q1) Write a balanced chemical equation to show the production of chlorine by the chlor-alkali process.

Q2) Why is it especially dangerous to mix cyanide salts with acids? Write a chemical equation to illustrate your answer.

Q3) Write the formula for the binary hydride you would expect calcium to form.

Q4) Which of these aqueous solutions has the highest pH?

A)0.100 M NaOH

B)0.100 M Na₂O

C)0.100 M Na₃N

D)all of these solutions have the same pH due to the leveling effect

E)these all are solutions of weak bases, so K_b values are needed in order to decide

Q5) When phosphate rock, Ca₃(PO₄)₂(s), is converted to phosphorus,

A)one of the products of the reaction is water.

B)sulfuric acid is added to generate insoluble calcium sulfate.

C)hydrogen is used to reduce the phosphate to phosphorus.

D)silica is added to form a calcium silicate slag.

E)oxygen must be added to prevent reaction of P₄.

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Chapter 22: Transition Metal Chemistry and Coordination Compounds

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Q1) What is the coodination number of silver in [Ag(NH₃)₂]Cl?

Q2) Predict the number of unpaired electrons in the [Fe(CN)₆]^4- ion.

Q3) Predict the number of unpaired electrons in the [Fe(CN)₆]^3- ion.

Q4) What terms describe the geometric isomers that are possible for the complex [CrF₂Cl₄]^3-?

Q5) Write the chemical formula of diamminedichloroplatinum(II).

Q6) The neutral monodentate ligand L forms the complex ion [CrL₆]²⁺, and the magnetic properties of this complex correspond to 2 unpaired electrons.Is L a strong-field or weak-field ligand? Explain your reasoning.

Q7) In K₄[Fe(CN)₆], how many 3d electrons does the iron atom have?

Page 25

Q8) Name the complex ion [Ni(CN)₄]^2-.

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Chapter 23: Nuclear Chemistry

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Q1) Tritium is a radioisotope of hydrogen having a half-life of 12.3 years.If you initially had 1.0 \(\times\) 10^-7 mole of tritium, calculate the decay rate of the sample.

Q2) Decay of silicon-27 by positron emission yields

A)magnesium-23.

B)sulfur-31.

C)phosphorus-27.

D)silicon-26.

E)aluminum-27.

Q3) Carbon-11 is a radioactive isotope of carbon. Its half-life is 20.3 minutes. What fraction of the initial number of carbon-11 atoms in a sample will remain after 81 minutes?

A)1/16

B)1/4

C)1/2

D)1/32

E)1/8

Q4) What nuclear fuel is produced in a breeder reactor?

Q5) 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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Chapter 24: Organic Chemistry

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Q1) Acetylene, C₂H₂, the simplest alkyne, can be prepared from "inorganic" materials. Which of these reactions is used to prepare acetylene in this way?

A)2C + H₂ \(\to\) C₂H₂ B)C₂H₄ \(\to\) C₂H₂ + H₂

C)2CO + 2H₂O \(\to\) C₂H₂ + H₂O₂

D)CaC₂ + 2H₂O \(\to\) C₂H₂ + Ca(OH)₂

Q2) How many structural isomers are there of C₄H₁₀?

A)4

B)6

C)2

D)8

E)10

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) The intermolecular force between bases on the opposite strands of DNA responsible for its double-helical structure is

A)hydrogen bonding.

B)dispersion force.

C)covalent bonding.

D)ionic force.

E)dipole-dipole force.

Q2) A peptide bond (also called an amide bond)joins two amino acids together. What atoms are linked by this bond?

A)C - O

B)C - H

C)C - N

D)N - S

E)S - C

Q3) Both DNA and RNA have double-helical structures.

A)True

B)False

Q4) The monomer used to prepare polyvinyl chloride (PVC)is CHCl=CHCl.

A)True

B)False

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