General Chemistry I Study Guide Questions - 3323 Verified Questions

General Chemistry I Study Guide Questions

Course Introduction

General Chemistry I introduces students to the fundamental principles of chemistry, providing a comprehensive foundation for further study in the field. The course covers essential topics such as atomic and molecular structure, chemical bonding, stoichiometry, states of matter, thermochemistry, and the properties of gases, liquids, and solids. Emphasis is placed on developing problem-solving skills and an understanding of the scientific method through lectures, laboratory experiments, and practical applications. Students learn to analyze chemical reactions, interpret data, and understand the role of chemistry in everyday life and various scientific disciplines.

Recommended Textbook

General Chemistry Principles and Modern Applications 11th Edition by Ralph H. Petrucci

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3323 Verified Questions

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Chapter 1: Matter: Its Properties and Measurement

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Sample Questions

Q1) The temperature in the core of the warp drive of the starship Enterprise is supposedly 3 million (3.00 × 10⁶)degrees Celsius.What is this in degrees Fahrenheit?

A)5.40 × 10⁶ °F

B)2.99 × 10⁶ °F

C)1.67 × 10⁶ °F

D)3.27 × 10⁶ °F

E)8.13 × 10⁶ °F

Answer: A

Q2) The result of addition can have more significant figures than any of the numbers added.

A)True

B)False

Answer: True

Q3) Convert 4 m to metres.

A)4 × 10^-9 m

B)4 × 10^-6 m

C)4 × 10^-3 m

D)4 × 10⁶ m

Answer: B

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Page 3

Chapter 2: Atoms and the Atomic Theory

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Sample Questions

Q1) How many arsenic atoms are in 5.21 g of arsenic?

A)0.0695 atoms

B)9.51 × 10²² atoms

C)3.14 × 10²⁴atoms

D)2.10 × 10²²atoms

E)4.19 × 10²²atoms

Answer: E

Q2) An isotope with mass number 81 has eleven more neutrons than protons.This is an isotope of what element?

A)Tl

B)Yb

C)Zr

D)Br

E)Nb

Answer: D

Q3) Different ratios of atoms produce different compounds.

A)True

B)False

Answer: True

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Page 4

Chapter 3: Chemical Compounds

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Sample Questions

Q1) Hydrates are:

A)moisture sensitive hygroscopic inorganic salts

B)compounds in which each formula unit has one or more water molecules associated with it

C)readily soluble in water and release energy

D)organic compounds that contain oxygen together with usual carbon and hydrogen

E)concentrated solutions of salts in water

Answer: B

Q2) An unknown organic compound contains carbon,hydrogen,and bromine only.The mass percentages of C and H are 12.77% C and 1.60% H.Bromine from 1.87 g of this compound has been completely converted into 3.70 g of AgBr.The molar mass of unknown organic compound is 188 u.Determine the molecular formula of the unknown.

A)CH₃Br

B)C₂H₃Br₂

C)C₂H₂Br₂

D)C₂H₂Br₄

E)C₄H₆Br₄

Answer: B

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Page 5

Chapter 4: Chemical Reactions

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Q1) What is the concentration of NO₃^- ions in a solution prepared by dissolving 25.0 g of Ca(NO₃)₂ in enough water to produce 300 mL of solution?

A)0.254 mol L^-1

B)0.508 mol L^-1

C)0.672 mol L^-1

D)1.02 mol L^-1

Q2) Calcium phosphate reacts with sulfuric acid to form calcium sulfate and phosphoric acid.What is the coefficient for sulfuric acid when the equation is balanced using the lowest,whole-number coefficients?

A)1

B)2

C)3

D)none of the above

Q3) A chemical equation is a shorthand way of representing a chemical reaction. A)True B)False

Q4) A formula is a shorthand way of representing a chemical reaction. A)True B)False

Page 6

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Chapter 5: Introduction to Reactions in Aqueous Solutions

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Q1) A solution is 0.660 M in HNO₃(aq)and 1.02 M in Ca(NO₃)₂(aq).What is the molarity of NO₃^-(aq)in the solution?

A)2.70 M

B)1.68 M

C)1.02 M

D)0.660 M

E)0.360 M

Q2) The substance BaCl₂ is a:

A)salt

B)weak acid

C)strong base

D)weak base

E)strong acid

Q3) Which of the following compounds is an Arrhenius base?

A)C₆H₁₂O₆

B)HOCl

C)H₂SO₄

D)C₆H₅NH₂

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Page 7

Chapter 6: Gases

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Sample Questions

Q1) The volume of 350.mL of gas at 25 °C is decreased to 135 mL at constant pressure.What is the final temperature of the gas?

A)-158 °C

B)9.6 °C

C)65 °C

D)500 °C

Q2) How many liters of gas is 23.4 grams of nitrogen at 750 mmHg and 28.0 °C?

A)586 L

B)20.9 L

C)0.771 L

D)20.4 L

E)1.94 L

Q3) Under conditions for which chlorine gas has an effusion rate of 2.4 × 10^-6 mol/sec,what would be the effusion rate for bromine gas,in mol/sec?

A)1.1 × 10^-6mol/sec

B)1.6 × 10^-6mol/sec

C)2.3 × 10^-6mol/sec

D)3.6 × 10^-6mol/sec

E)5.4 × 10^-6mol/sec

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Page 8

Chapter 7: Thermochemistry

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Sample Questions

Q1) 246 g of hot coffee at 86.0 °C are placed in a 137 g mug at 20.0 °C.The specific heat of coffee is 4.00 J/g °C,while that of the mug is 0.752 J/g °C.Assuming no heat is lost to the surroundings,what is the final temperature of the system: mug + coffee?

A)79.7 °C

B)93.7 °C

C)98.4 °C

D)76.0 °C

E)53.0 °C

Q2) To have a standard enthalpy of formation referenced to 0 J/mol,the substance must:

I.be a simple substance (chemical element)

II.be in its most stable form

III.be under 1 bar of pressure

IV.have a concentration of 1.0000 M

A)I,III,IV

B)I,II,III

C)II,IV

D)I,III

E)II,III,IV

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Page 9

Chapter 8: Electrons in Atoms

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Sample Questions

Q1) Which of the following is not possible?

A)2p

B)4d

C)5p

D)3f

E)2s

Q2) The fact that we cannot simultaneously measure the exact position and precise momentum of an electron is referred to as:

A)Pauli Exclusion Principle

B)The Aufbau Principle

C)Hund's Rule

D)The DeBroglie Relationship

E)Heisenberg Uncertainty Principle

Q3) Calculate the deBroglie wavelength of a ball of mass 125 grams and velocity 90 m/s.

A)0.59 m

B)5.9 × 10^-31 m

C)5.9 × 10^-35 m

D)590 m

E)1.7 × 10³⁴ m

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Page 10

Chapter 9: The Periodic Table and Some Atomic Properties

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Sample Questions

Q1) The similar chemical behavior of the elements in a given group in the periodic table is best accounted for by the fact that atoms of these elements have:

A)the same number of isotopes

B)the same number of electrons

C)the same number of electrons in the outermost (valence)shell

D)similar nuclear structures

E)the same number of protons

Q2) The number of valence electrons for atomic potassium is ________.

A)1

B)5

C)6

D)15

E)19

Q3) Which of the following represents the change in electronic configuration that is associated with the first ionization energy of strontium?

A)[Kr]5s¹5p¹ [Kr]5s¹ + e^-

B)[Kr]5s² [Kr]5s¹5p¹

C)[Kr]5s² [Kr]5s¹ + e^-

D)[Kr]5s² + e^- [Kr]5s²5p¹

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Page 11

Chapter 10: Chemical Bonding I: Basic Concepts

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Sample Questions

Q1) Which of the following is diamagnetic?

A)ClO₂

B)NO

C)CO

D)NO₂

E)CH₃

Q2) Which of the following molecules has both an electron group geometry and a molecular geometry described as trigonal planar?

A)SiH₄

B)PF₃

C)OF₂

D)CHF₃

E)BF₃

Q3) Which of the following exhibits covalent bonding?

A)NaF

B)SrO

C)LiH

D)OF₂

E)K₂S

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Page 12

Chapter 11: Chemical Bonding Ii: Valence Bond and

Molecular Orbital Theories

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Q1) According to principles of VSEPR theory applied on AsCl₅^2-,which of the following is INCORRECT?

A)VSEPR formula = AX₅E

B)molecular geometry = square planar

C)electron-group geometry = octahedral

D)hybridization = sp³^d²

E)one lone pair and 5 bonding pairs

Q2) Which of the following does NOT involve any delocalized bonds?

A)acetate ion

B)carbonate ion

C)nitric acid

D)nitrous acid

E)ozone

Q3) According to MO theory,all of the following have a bond order of 2 EXCEPT:

A)NO

B)CN⁺

C)C₂

D)O₂

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Chapter 12: Intermolecular Forces: Liquids and Solids

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Sample Questions

Q1) When a liquid is in dynamic equilibrium with its vapor at a given temperature,the following conditions could exist:

I.There is no transfer of molecules between liquid and vapor.

II.The vapor pressure has a unique value.

III.The opposing processes, (liquid to vapor)and (vapor to liquid),proceed at equal rates.

IV.The concentration of vapor is dependent on time. Which of the above choices are applicable?

A)I

B)II and III

C)I,II,and III

D)II and IV

E)II,III and IV

Q2) Which type of bonding does Sr form upon solidification?

A)covalent network

B)ionic

C)metallic

D)molecular

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Chapter 13: Spontaneous Change: Entropy and Gibbs Energy

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Sample Questions

Q1) An increase in entropy is observed when a liquid forms from a gas.

A)True

B)False

Q2) Which of the following has the largest molar entropy?

A)I₂(g)

B)Xe(g)

C)H₂(g)

D)He(g)

E)O₂(g)

Q3) Ethyl chloride,C₂H₅Cl,is used as a local anesthetic.It works by cooling tissue as it vaporizes;its heat of vaporization is 26.4 kJ mol^-1.How much heat could be removed by 20.0 g of ethyl chloride?

A)8.19 kJ

B)341 kJ

C)528 kJ

D)3410 kJ

Q4) A microstate is a specific microscopic configuration describing how particles of a system are distributed among the available energy levels.

A)True

B)False

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Chapter 14: Solutions and Their Physical Properties

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Sample Questions

Q1) A solution that can dissolve no more solute is called:

A)unsaturated B)saturated C)concentrated

D)supersaturated E)oversaturated

Q2) What is the expected freezing point of a 0.50 mol kg^-1 solution of Li₂SO₄ in water? K_f for water is 1.86 °C m^-1.

A)-0.93 °C

B)-1.9 °C

C)-2.8 °C

D)-6.5 °C

Q3) Henry's Law states that:

A)a supersaturated solution is unstable

B)the solubility of a gas increases as the gas pressure is increased

C)the solubility of a gas decreases as the gas pressure is increased

D)a concentrated solution lowers the freezing point of a solution

E)a concentrated solution increases the boiling point of a solution

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Page 16

Chapter 15: Principles of Chemical Equilibrium

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Sample Questions

Q1) For the reaction: CH₄(g)+ 2 H₂O(g) CO₂(g)+ 4 H₂(g), _rH° = +190 kJ,when CH₄ is added:

A)the reaction shifts to the right

B)the reaction shifts to the left

C)the _rH° increases

D)the temperature increases E)there is no change in equilibrium position

Q2) For the production of NO₂,K_c = [NO₂]²/[NO]²[O₂].At equilibrium in a 2.50 L container,there are 3.00 mol NO,4.00 mol O₂ and 22.0 mol NO₂.The value of K_c is ________.

A)13.4

B)33.6

C)5.38

D)0.0116

E)3.75

Q3) Changes in temperature cause change in the equilibrium position.

A)True

B)False

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Page 17

Chapter 16: Acids and Bases

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Sample Questions

Q1) Choose the strongest acid.

A)HF

B)H₂CO₃

C)HCN

D)HC₂H₃O₂

E)HClO₄

Q2) A certain acid,HA,has a K_a given by: HA + H₂O H₃O⁺ + A^- K_a = 6.80 × 10^-6

What is the pH of a 0.247 M aqueous solution of the acid's potassium salt,KA,which undergoes the hydrolysis reaction?

A^- + H₂O OH^- + HA

A)4.72

B)9.28

C)4.11

D)9.89

E)9.44

Q3) The term pH = -ln [H⁺].

A)True

B)False

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Chapter 17: Additional Aspects of Acidbase Equilibria

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Q1) Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0.State what color the indicator will assume in the following solution: 0.10 M NaCN(aq).

A)red

B)yellow

C)red-yellow mixture

D)The indicator is its original color.

E)There is not enough information to answer this question.

Q2) If 30.0 mmol HCl(g)is added to 1.00 L of a buffer that is 0.340 M NH₃(aq)and 0.290 M NH₄Cl(aq),what are the final concentrations of NH₃(aq)and NH₄Cl(aq),respectively?

Assume no volume change.

A)0.310 M and 0.320 M

B)0.310 M and 0.290 M

C)0.370 M and 0.290 M

D)0.370 M and 0.320 M

Q3) A salt of a polyprotic acid such as NaHCO₃ cannot act as a source of an acid.

A)True

B)False

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Page 19

Chapter 18: Solubility and Complex-Ion Equilibria

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Sample Questions

Q1) The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is

A)K_sp = 9[Ag⁺]³

B)K_sp = 27[Ag⁺]⁴

C)K_sp = [Ag⁺]^1/3

D)K_sp = 0.125[Ag⁺]

E)K_sp = 0.333[Ag⁺]⁴

Q2) Write the solubility product constant expression for the following salt:

Ca(OH)₂(s).

A)[Ca²⁺][OH^-]

B)[Ca²⁺]²[OH^-]

C)[Ca²⁺]³[OH^-]

D)[Ca²⁺]²[OH^-]²

E)[Ca²⁺][OH^-]²

Q3) If Q_sp is larger than K_sp,precipitation should occur.

A)True

B)False

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20

Chapter 19: Electrochemistry

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Q1) Determine E°_cell for the reaction: 2 Ag(s)+ Mg²⁺(aq) 2 Ag⁺(aq)+ Mg.(s)The half reactions are: Mg²⁺(aq)+ 2 e^- Mg(s)E° = -2.356 V Ag⁺(aq)+ e^- Ag(s)E° = 0.800 V

A)0.756 V

B)-0.756 V

C)3.156 V

D)-3.156 V

E)1.556 V

Q2) A galvanic cell consists of a Ni²⁺(aq)/Ni(s)half-cell and a standard hydrogen electrode.If the Ni²⁺/Ni half-cell standard cell functions as the anode,and the standard cell potential is 0.26 V,what is the standard reduction potential for the Ni²⁺(aq)/Ni(s)half-cell?

A)-0.26 V

B)-0.13 V

C)+0.13 V

D)+0.26 V

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Chapter 20: Chemical Kinetics

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Sample Questions

Q1) If the half-life of a reactant is independent of its initial concentration,the reaction order is 0.

A)True

B)False

Q2) What is the rate constant at 305 K for the reaction: 2 N₂O₅ 2 N₂O₄ + O₂,

If k = 3.46 × 10^-5 s^-1 at 298 K and E_a = 106 kJ/mol?

A)2.4 × 10^-5 s^-1

B)4.8 × 10^-5 s^-1

C)6.0 × 10^-5 s^-1

D)1.2 × 10^-5 s^-1

E)9.2 × 10^-5 s^-1

Q3) In the Arrhenius equation,ln k = ^-^E_a/RT + ln

A,the symbol A denotes the initial concentration of A.

A)True

B)False

Q4) A heterogeneous catalyst is a catalyst that is in two phases of matter.

A)True

B)False

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Chapter 21: Chemistry of the Main-Group Elements I:

Groups 1,2,13,and 14

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Q1) The first ionization energy of calcium is smaller than that of strontium.

A)True

B)False

Q2) Choose the INCORRECT statement about silicon.

A)Silicon forms on stable oxide.

B)Silicon exhibits more catenation than carbon.

C)Sand and quartz are SiO₂.

D)The central feature of silicates is the SiO₄^4- tetrahedron.

E)A silicone is a compound with an alternating silicon and oxygen chain as a backbone with carbon containing groups as sidechains.

Q3) Write the equation for the electrolysis of molten NaCl.

A)2 NaCl(s) 2 Na(s)+ Cl₂(g)

B)2 NaCl(l) 2 Na(l)+ Cl₂(g)

C)2 NaCl(l) Na₂Cl₂(s)

D)2 NaCl(l) Na(s)+ NaCl₂(s)

E)There is no reaction.

Q4) Hydrogen peroxide may act only as an oxidizing agent.

A)True

B)False

Page 23

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Chapter 22: Chemistry of the Main-Group Elements Ii:

Groups 18,17,16,15,and Hydrogen

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Q1) HI(g)has a G_f° that is small and positive,so HI should dissociate to some extent but its activation energy is high.HI(g)is stable at room temperature.Chemists would describe the reason for the very slow dissociation reaction as:

A)thermodynamically controlled

B)the G_f° is wrong

C)the reaction is not slow

D)the reaction is kinetically controlled

E)the molecules can collide with each other

Q2) Which of the following is found in Teflon,Freon-12,and in the acid commonly used to etch glass?

A)carbon

B)chlorine

C)fluorine

D)hydrogen

E)oxygen

Q3) Hydrogen compounds are called hybrids.

A)True

B)False

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Chapter 23: The Transition Elements

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Q1) Which of the following definitions is INCORRECT?

A)amalgam: a solid solution or alloy containing mercury

B)coinage metals: the transition elements of Group 11 (1B)

C)galvanized iron: iron which has been electroplated with tin

D)lanthanides: elements of atomic number 58 through 71

E)pig iron: slightly impure iron as obtained directly from the blast furnace

Q2) What is the ground-state electron configuration for the element chromium (Z = 24)?

A)[Ne] 4s²3d⁴

B)[Ar] 4s²3d⁴

C)[Ar] 4s¹3d⁵

D)[Ar] 3d⁶

Q3) Choose the INCORRECT statement.

A)The electron configuration of Fe²⁺ is [Ar]3d⁶.

B)The electron configuration of Co²⁺ is [Ar]3d⁷.

C)The electron configuration of Fe³⁺ is [Ar]3d⁵.

D)The electron configuration of Ni²⁺ is [Ar]3d⁵.

E)A metal carbonyl is a compound formed from a metal and carbon monoxide.

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25

Chapter 24: Complex Ions and Coordination Compounds

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Q1) What is the correct name of the following ion: [Zn(CN)₄]^2-

A)zinc quadracyanide

B)tetracyanozincate(II)

C)zinc cyanide

D)tetracyanozinc(II)

E)cyanozinc(IV)

Q2) Choose the INCORRECT formula/name combination for ligands.

A)O^2- / hydroxo

B)NO / nitrosyl

C)I^- / iodo

D)CN^- / cyano

E)SO₄^2- / sulfato

Q3) Give the correct name for [AuF₄]^-.

A)gold fluoride

B)tetrafluoroaurate(III)

C)gold tetrafluoride

D)tetrafluorogold(III)

E)tetrafluoride gold

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Chapter 25: Nuclear Chemistry

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Q1) The unit of radiation which is equivalent to 0.010 J/kg of matter is the:

A)curie

B)roentgen

C)rad

D)rem

E)MeV

Q2) The most highly charged particle is:

A)alpha

B)beta

C)gamma

D)positron

E)neutron

Q3) Carbon-11 is used in medical imaging.The half-life of this radioisotope is 20.4 min.What percentage of a sample remains after 60.0 min?

A)71.2

B)5.28

C)13.0

D)34.0

E)2.94

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Page 27

Chapter 26: Structures of Organic Compounds

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Q1) How many primary,secondary,tertiary and quaternary carbon atoms are there in the structure of 2,4,6-trimetylheptane?

A)5 primary,2 secondary,2 tertiary and 1 quaternary carbon atoms

B)5 primary,3 secondary,2 tertiary and 0 quaternary carbon atoms

C)4 primary,4 secondary,2 tertiary and 0 quaternary carbon atoms

D)4 primary,2 secondary,2 tertiary and 2 quaternary carbon atoms

E)5 primary,2 secondary,3 tertiary and 0 quaternary carbon atoms

Q2) What are the possible positions for hydrogen on the chair conformation of cyclohexane?

A)staggered and eclipsed

B)axial and equatorial

C)equatorial and apical

D)longitudinal and latitudinal

E)chair and boat

Q3) A conformation is a set of all possible optical isomers of an organic compound of a given molecular formula.

A)True

B)False

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Chapter 27: Reactions of Organic Compounds

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Q1) Which of the following statements correctly describe the step-reaction polymerization?

I.It is also called condensation polymerization.

II.It produces polymers of moderately high molecular masses.

III.It requires that monomers have functional groups that can join together.

IV.This type of polymerization is fast.

V.It is accompanied with the addition of a small molecule.

A)I ,II and III

B)I ,and II

C)II ,III and IV

D)III ,IV and V

E)II ,IV and V

Q2) Predict the major product for the reaction: 1-butene + HI

A)CH₂ICH₂CH₂CH₃

B)CH₂ICH=CHCH₃

C)CH₂=CICH₂CH₃

D)CH₃CHICH₂CH₃

E)CH₃CI₂CH₂CH₃

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Chapter 28: Chemistry of the Living State

Available Study Resources on Quizplus for this Chatper

104 Verified Questions

104 Flashcards

Source URL: https://quizplus.com/quiz/64257

Sample Questions

Q1) In DNA,guanine always pairs with cytosine.

A)True

B)False

Q2) Apart from bringing the reactants close together,how does the binding of substrates in the active site of the enzyme serve to catalyze a reaction?

A)Binding lowers the activation energy of the reaction.

B)Enzymes provide energy upon substrate binding to drive the reaction.

C)Binding of the substrate maintains the optimal temperature for the reaction.

D)Binding maintains the optimal pH for enzyme activity.

E)Binding lowers the energy of the products increasing the reaction rate.

Q3) Living cells are unable to convert glucose-6P into which of the following?

A)glycogen

B)glucose

C)coenzyme A

D)polysaccharide stored in liver

E)it may be metabolized

Q4) Enantiomers are non-superimposable mirror images.

A)True

B)False

Q5) The hydrolysis of tristearin produces the soap potassium stearate and ________.

Page 30

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