Chemistry for Engineers Question Bank - 4358 Verified Questions

Course Introduction

Chemistry for Engineers Question

Bank

Chemistry for Engineers offers an introduction to the fundamental principles of chemistry with a focus on their application in engineering contexts. Students explore atomic and molecular structure, chemical bonding, thermodynamics, kinetics, equilibrium, and the properties of materials, all tailored to illustrate relevance in engineering problems and industrial processes. The course emphasizes problem-solving skills, laboratory techniques, and real-world applications such as materials selection, corrosion, energy production, and environmental considerations, equipping engineering students with the chemical knowledge necessary for successful practice in their respective fields.

Recommended Textbook Chemistry 7th Edition by John E. McMurry

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23 Chapters

4358 Verified Questions

4358 Flashcards

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Page 2

Chapter 1: Chemical Tools: Experimentation and Measurement

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Sample Questions

Q1) Calculate the kinetic energy of a 150-g baseball moving at a speed of 38.m/s (85 mph).

A)5.7 J

B)1.1 × 10²J

C)5.7 × 10³ J

D)1.1 × 10⁵ J

Answer: B

Q2) The nutritionist unit Calorie is equal to ________ calories. Answer: 1000

Q3) The factor 10^-2 corresponds to which prefix?

A)deka

B)deci

C)centi

D)milli

Answer: C

Q4) A preliminary explanation of the results of many experiments that can be used to make predictions and suggest further experimentations is a ________.

Answer: hypothesis

Q5) Stored energy is ________ energy,and energy of motion is ________ energy.

Answer: potential,kinetic

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Chapter 2: Atoms, molecules, and Ions

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Sample Questions

Q1) If shaded and unshaded spheres represent atoms of different elements,which of the above drawings most likely represents a molecular compound at room temperature and a pressure of 1 atm?

A)drawing (a)

B)drawing (b)

C)drawing (c)

D)drawing (d)

Answer: B

Q2) Pb is the symbol for the element ________.

Answer: lead

Q3) The subatomic particles contained in the nucleus of an atom are ________ and ________.

Answer: protons,neutrons

Q4) The chemical formula for magnesium nitride is

A)Mg(NO₃)₂.

B)Mg(NO₂)₂.

C)Mg₃N₂.

D)MgN₂.

Answer: C

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Chapter 3: Mass Relationships in Chemical Reactions

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Sample Questions

Q1) Which of the following statements is false concerning the formula of a compound?

A)The empirical formula is the simplest whole numbered ratio of atoms in a compound.

B)The molecular formula is the true ratio of atoms in a compound.

C)The molecular formula and empirical formula can be identical.

D)The number of atoms in a molecular formula is always greater than the number of atoms in an empirical formula.

Answer: D

Q2) What is the mass of 0.0500 mol of dichlorodifluoromethane,CF₂Cl₂?

A)4.14 × 10^-4 g

B)6.05 g

C)12.1 g

D)24.2 g

Answer: B

Q3) To the nearest whole number,the molar mass of Cu(NO₃)₂ is ________ g/mol.

Answer: 188

Q4) The fundamental SI unit for measuring matter is the ________.

Answer: mole

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Chapter 4: Reactions in Aqueous Solutions

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Sample Questions

Q1) The reaction HNO₃(aq)+ KOH(aq) KNO₃(aq)+

H₂O(l)is best classified as a(n)

A)acid-base neutralization reaction.

B)oxidation-reduction reaction.

C)precipitation reaction.

D)single replacement reaction.

Q2) CH₃CO₂H is an example of a ________ electrolyte.

Q3) What is the molarity of a solution prepared by diluting 25 mL of 2.0 M HCl with enough water to make 250 mL of solution?

Q4) The reaction Na₃PO₄(aq)+ 3 AgNO₃(aq) Ag₃PO₄(s)+ 3 NaNO₃(aq)is best classified as a(n)

A)acid-base neutralization reaction.

B)oxidation-reduction reaction.

C)precipitation reaction.

D)single replacement reaction.

Q5) Metals that do not dissolve in non-oxidizing acids are found at the ________ of the activity series.

Q6) The best oxidizing agents are found at the ________ of the activity series.

Q7) The oxidation number of hydrogen in CaH₂ is ________.

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Chapter 5: Periodicity and the Electronic Structure of Atoms

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Sample Questions

Q1) What are the possible values of l if n = 3?

A)3

B)0,1,or 2

C)-4,-3,-2,-1,0,+1,+2,+3,or +4

D)-5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5

Q2) According to the Balmer-Rydberg equation,which transition results in the emission of a photon in the ultraviolet region of the electromagnetic radiation spectrum?

A)m = 1 n = 2

B)m = 3 n = 4

C)m = 2 n = 1

D)m = 4 n = 3

Q3) For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?

A)2s 3p

B)2p 6d

C)6p 4s

D)7f 5d

Q4) The number of orbitals in the n = 3 shell is ________.

Q5) Using shorthand notation,the electron configuration of Ni is ________.

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Chapter 6: Ionic Compounds: Periodic Trends and Bonding

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Sample Questions

Q1) Atoms of which element,indicated by letter on the periodic table above,would be expected to have the highest first ionization energy,E_i1? A)A B)B C)C D)D

Q2) Which liberates the most energy?

A)Li(g)+ e^- Li^-(g)

B)Na(g)+ e^- Na^-(g)

C)K(g)+ e^- K^-(g)

D)Rb(g)+ e^- Rb^-(g)

Q3) Of the following,which element has the highest first ionization energy? A)Cl

Q4) The ion Q²⁺ contains 36 electrons.The identity of element Q is

Q5) The number of electrons in the ion K⁺ is ________.

Q6) The element in period 3 with the smallest seventh ionization energy is ________.

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Chapter 7: Covalent Bonding and Electron-Dot Structures

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Sample Questions

Q1) The number of Lewis electron dot resonance structures required to describe NO₂^- is ________.

Q2) The Lewis electron-dot structure of H₂CO has ________ nonbonding electron pairs,________ bonding electron pairs,and a carbon-oxygen bond order of ________.

Q3) Which one of the following is expected to exhibit resonance?

A)NH₄⁺

B)HCN

C)CS₂

D)NO₃^-

Q4) How many lone pairs are there in the Lewis structure of O₂?

A)3

B)1

C)0

D)4

Q5) Using only the elements Be,Cl,and/or P,give the formula of a compound having largely ionic bonds.

Q6) The Lewis electron-dot structure of N₂ has ________ nonbonding electrons pairs,________ bonding electron pairs,and a bond order of ________.

Page 9

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Chapter 8: Covalent Compounds: Bonding Theories and

Molecular Structure

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Sample Questions

Q1) What is geometry around the carbon atom labeled C₃?

A)bent

B)tetrahedral

C)trigonal planar

D)trigonal pyramidal

Q2) The dipole moment of BrF is 1.29 D,and its bond length is 178 pm.What is the percent ionic character of the Br-F bond?

A)3.9%

B)8.5%

C)15%

D)33%

Q3) Which of the following compounds exhibits only dispersion and dipole-dipole intermolecular interactions?

A)Na

B)HCl

C)BH₃

D)CH₃NHC₄H₉

Q4) According to molecular orbital theory,is the highest energy orbital that contains an electron antibonding or bonding in O₂^2-?

Page 10

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Chapter 9: Thermochemistry: Chemical Energy

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Sample Questions

Q1) In which case is the work done on the system always positive?

A) E > 0

B) V > 0

C) V = 0

D) V < 0

Q2) 10.0 g of a metal,initially at 25°C,are placed into 10.0 g of water,initially at 100°C.Which metal will have the highest final temperature? Shown after each metal is its specific heat in J/(g°C).

A)sodium (1.23)

B)calcium (0.650)

C)lead (0.160)

D)nickel (0.440)

Q3) At 253 K the sign of G for the physical change shown below is ________. H₂O(s) H₂O(l)

Q4) The reaction represented in the above drawing is likely to be

A)nonspontaneous at all temperatures.

B)nonspontaneous at low temperatures and spontaneous at high temperatures.

C)spontaneous at low temperatures and non spontaneous at high temperatures.

D)spontaneous at all temperatures.

Q5) Is thermal energy a form of kinetic or potential molecular energy?

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Chapter 10: Gases: Their Properties and Behavior

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Sample Questions

Q1) Which of the following gases has the lowest average speed at 25°C?

A)He

B)BF₃

C)H₂

D)NH₃

Q2) A balloon filled with helium gas at 20°C occupies 3.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,raising the pressure to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?

A)0.20 L

B)2.6 L

C)5.3 L

D)77 L

Q3) Which of the following gases has the lowest average speed at 25°C?

A)C₂H₆

B)H₂Se

C)PH₃ 

D)F₂

Q4) If 1.0 gram each of Cl₂,CO₂,N₂,and O₂ are contained in a 5-L flask,the gas with the highest partial pressure is

Page 12

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Chapter 11: Liquids, solids, and Phase Changes

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Sample Questions

Q1) The normal boiling point occurs when the

A)intermolecular forces within the liquid phase are broken.

B)temperature of the pure liquid equals the external temperature.

C)vapor pressure of a pure liquid equals an external pressure of one atmosphere.

D)vapor pressure of the liquid equals the external pressure.

Q2) Ethyl chloride,C₂H₅Cl,is used as a local anesthetic.It works by cooling tissue as it vaporizes.The heat of vaporization is 26.4 kJ/mol.How much heat could be removed by 60.0 g of ethyl chloride?

A)24.6 kJ

B)1584 kJ

C)2.28 kJ

D)1703 kJ

Q3) If cation M has a 2+ charge and anion A has a 2- charge,what is the oxidation state of cation M'?

Q4) The cubic closest-packed arrangement of atoms is the same as which cubic unit cell?

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Chapter 12: Solutions and Their Properties

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Sample Questions

Q1) At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg,respectively.Calculate the total vapor pressure over a solution of benzene and toluene with X_benzene = 0.400.

A)110 mm Hg

B)133 mm Hg

C)109 mm Hg

D)242 mm Hg

Q2) The change in the Gibbs free energy for dissolving solute in a saturated solution is A)negative.

B)zero.

C)positive.

D)positive at low temperatures and negative at high temperatures.

Q3) A saturated solution is defined as

A)a concentrated solution.

B)a solution that is in equilibrium with pure solute.

C)a solution than is in equilibrium with undissolved solute.

D)a solution that is not in equilibrium with both pure solvent and undissolved solute.

Q4) Molarity is defined as ________,whereas molality is defined as ________.

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Page 14

Chapter 13: Chemical Kinetics

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Sample Questions

Q1) The second-order reaction 2 Mn(CO)₅

Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 5.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

A)1.7 × 10^-15 s

B)1.9 × 10^-14 s

C)6.0 × 10^-5 s

D)1.5 × 10² s

Q2) Which part of the Arrhenius equation contains a term which measures the number of molecules that have the correct orientation for reaction?

A)activation energy

B)e^-Ea/RT

C)frequency factor

D)none of these

Q3) Platinum in the catalytic converter of an automobile catalyzes the conversion of CO to CO₂ is an example of a ________ (heterogeneous,homogeneous)catalyst.

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15

Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g) 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

Q2) What is the best balanced chemical equation for the reaction?

A)A₂ + B A₂B

B)A₂ + 2 B A₂B₂

C)A₂ + 2 B 2 AB

D)6 A₂ + 9 B 3 A₂ + 3B + 6 AB

Q3) According to Le Châtelier's principle,if the volume of the vessel containing the equilibrium system shown below is decreased,there will be an increase in the concentration of ________ and a decrease in the concentration of ________. H₂(g) 2 H(g)

Q4) The reaction CaCO₃(s) CaO(s)+ O₂(g)is endothermic 298 K.The effect of adding CaO to the system at equilibrium will ________ (decrease,increase,have no effect on)the total quantity of CaO once equilibrium is reestablished.

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Page 16

Chapter 15: Aqueous Equilibria: Acids and Bases

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Sample Questions

Q1) Of the elements indicated on the periodic table shown above,which forms the weakest oxoacid acid with the formula H₂XO₃ or HXO₃,where X = A,B,C,or D?

A)A

B)B

C)C

D)D

Q2) Arrange the acids in order of increasing value of K_a.

A)K_a(HZ)< K_a(HY)< K_a(HX)

B)K_a(HY)< K_a(HZ)< K_a(HX)

C)K_a(HZ)< K_a(HX)< K_a(HY)

D)K_a(HX)< K_a(HZ)< K_a(HY)

Q3) The Br nsted-Lowry acids in the chemical equation below are ________ and ________.

HNO₂(aq)+ H₂O(l) H₃O⁺(aq)+

NO₂^-(aq)

Q4) Identify the Br nsted-Lowry acid/base conjugate pairs.

A)(1)/(2)and (3)/(4)

B)(1)/(3)and (2)/(4)

C)(1)/(4)and (2)/(3)

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Chapter 16: Applications of Aqueous Equilibria

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Sample Questions

Q1) What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

A)0.85

B)1.85

C)12.15

D)13.15

Q2) Oxalic acid,H₂C₂O₄ has acid dissociation constants K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H₂C₂O₄?

A)1.23

B)2.10

C)2.80

D)4.19

Q3) Addition of 0.0125 mol HCl to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________.The K_a of formic acid is 1.8 × 10^-4.

Q4) What is the pH of the solution formed when 25 mL of 0.173 M NaOH is added to 35 mL of 0.342 M HCl?

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Chapter 17: Thermodynamics: Entropy, free Energy, and Equilibrium

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Sample Questions

Q1) Solid NaHCO₃ is heated to 90°C.At equilibrium the total pressure of the gases produced is 0.545 atm.Calculate G° at 90°C for the reaction 2 NaHCO₃(s) Na₂CO₃(s)+ H₂O(g)+ CO₂(g).

A)-7.85 kJ

B)-3.67 kJ

C)+3.67 kJ

D)+7.85 kJ

Q2) Which of the following processes are spontaneous? I.dissolving more solute in an unsaturated solution

II.dissolving more solute in a saturated solution

III.dissolving more solute in a supersaturated solution

A)none of these

B)I

C)I and II

D)I,II,and III

Q3) The sign (+ or -)of H is ________ and the sign (+ or -)of S is ________ for the evaporation of water.

Q4) A 1.8 mole sample of gas at STP has a ________ entropy than 1.8 mole of gas at 273 K and 835 mm Hg.

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Chapter 18: Electrochemistry

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Sample Questions

Q1) Which statement below is not true?

A)The cell reactants in a fuel cell are continuously supplied from an external source.

B)A fuel cell is a galvanic cell.

C)Modern fuel cells can be easily regenerated using household current.

D)One of the reactants in a fuel cell is a traditional fuel.

Q2) When the equation below is balanced in basic solution using the smallest whole numbers,the coefficient in front of the OH^-(aq)is ________.

CN^-(aq)+ MnO₄^-(aq) CNO^-(aq)+ MnO₂(s)

Q3) Write the overall cell reaction for the galvanic cell given below. Pt(s) H₂(g) H⁺(aq) Cl₂(g) Cl^-(aq) Pt(s)

A)Pt(s)+ H₂(g)+ Cl^-(aq) Pt(s)+ 2 H⁺(aq)+ 2 Cl₂(g)

B)2 H⁺(aq)+ 2 Cl₂(g) 2 HCl(aq)

C)H₂(g)+ Cl₂(g) 2 H⁺(aq)+ 2 Cl^-(aq)

D)No reaction would occur because there is no salt bridge.

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Page 20

Chapter 19: Nuclear Chemistry

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Sample Questions

Q1) What percentage of a radioactive substance remains after 6.00 half-lives have elapsed?

A)0.781%

B)1.56%

C)3.12%

D)6.25%

Q2) When more than 3000 known nuclides are plotted on a neutron/proton grid,they make up a group called

A)the "island of stability."

B)the "band of nuclear stability."

C)the "sea of instability."

D)none of these

Q3) Among the types of radiation, , , ,and X,the one that requires the least amount of protective clothing is ________ radiation.

Q4) Radiation is dangerous to organisms because

A)all radionuclides are poisonous.

B)it causes electrolysis of water in the cells.

C)it causes nuclear reactions in the cells.

D)it ionizes molecules in the cells.

Q5) In a nuclear reaction,the symbol for a beta particle is ________.

Page 21

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Chapter 20: Transition Elements and Coordination Chemistry

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Q1) Which of the Co(III)complexes above are enantiomers of each other?

A)(A)and (B)

B)(C)and (D)

C)(A), (B),and (C)

D)(A), (B), (C),and (D)

Q2) Which of the following statements best explains why transition metals lose electrons from s orbitals before d orbitals?

A)Electrons from s orbitals are lower in energy than d orbitals.

B)The d orbitals experience a greater drop in energy when electrons are removed.

C)Electrons from d orbitals are less shielded from the nucleus than electrons in s orbitals.

D)Electrons in s orbitals are paired.

Q3) Which complex is optically active?

A)[CoCl₄en]^2-

B)trans-[CrCl₂(en)₂]⁺

C)cis-[CrCl₂(en)₂]⁺

D)[PtCl₂(NH₃)₂]

Q4) The element that forms a 2+ ion with the electron configuration [Xe] 4f¹⁴ 5d⁸ is ________.

Page 22

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Chapter 21: Metals and Solid-State Materials

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Q1) The reaction,MnO (s)+ SiO₂ (s) MnSiO₃ (l)can be considered as an acid base reaction.Which of the following statements best explains why?

A)MnO is a proton donor.

B)SiO₂ is a proton acceptor.

C)MnO is an electron donor.

D)SiO₂ is an electron donor.

Q2) According to band theory,the element having all of its bonding molecular orbitals filled and all of its antibonding orbitals empty in the 4s-3d composite band is

Q3) Which of these materials has the highest electrical conductivity?

A)material (1)

B)material (2)

C)material (3)

D)material (4)

Q4) Which is the hardest metal?

A)metal (1)

B)metal (2)

C)metal (3)

D)metal (4)

Page 23

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Chapter 22: The Main-Group Elements

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Sample Questions

Q1) From the above models of hydrides,indicate the one most representative of an interstitial metallic hydride.

A)I

B)II

C)III

D)IV

Q2) The ratio of oxygen atoms to silicon atoms in orthosilicate,single-strand silicates,double-strand silicates,and cyclic silicates is ________,________,________,and ________,respectively.

Q3) What statement is not consistent with the chemistry of tin?

A)It is abstracted from the mineral cassiterite by reduction of the oxide with carbon.

B)It is an important component of alloys such as bronze,pewter,and some solders.

C)It is a relatively abundant ore within the earth's crust.

D)It is used as a protective coating over steel in making tin cans.

Q4) Binary oxides can be classified as acidic,amphoteric,or basic.MgO,Al₂O₃,and SO₃ are classified as ________,________,and ________ oxides,respectively.

Q5) The oxidation number of the oxygen atoms in CaO₂ is ________.

Q6) Fullerene is an ________ of carbon.

Page 24

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Chapter 23: Connections to Organic and Biological Chemistry

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Sample Questions

Q1) Which name is not correct?

A)1,2-dichloropentane

B)2,3-dimethylbutane

C)2-ethylbutane

D)4-propylheptane

Q2) The number of different monochloro substitution products (C₅H₁₁Cl)that can form from the reaction of 2-methylbutane with Cl₂ is ________.

Q3) The C-Br bond in CH₃Br is a ________ (nonpolar,polar)covalent bond with a ________ ( +, -)charge on the carbon atom and a ________ ( +, -)charge on the bromine atom.

Q4) What is the sugar component in RNA called?

A)fructose

B)galactose

C)glucose

D)ribose

Q5) The molecule H₂NCH₂CH₂CH₂OH contains an ________ functional group and an ________ functional group.

Q6) Cytosine is a base that occurs in ________ (DNA,RNA,DNA and RNA).

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