Basic Chemistry Test Preparation - 3207 Verified Questions

Course Introduction

Basic Chemistry Test Preparation

Basic Chemistry introduces students to the foundational principles of chemistry, including atomic structure, chemical bonding, stoichiometry, states of matter, and chemical reactions. The course emphasizes the development of problem-solving skills and the application of chemical concepts to real-world situations. Students will explore the periodic table, chemical equations, and the properties of acids, bases, and solutions, preparing them for more advanced studies in science and related fields. Laboratory experiments complement theoretical knowledge, fostering critical thinking and scientific inquiry.

Recommended Textbook

Chemistry A Molecular Approach 2nd Canadian Edition by Nivaldo J. Tro

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25 Chapters

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Page 2

Chapter 1: Units of Measurement for Physical and Chemical Change

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Sample Questions

Q1) A recipe requires 1.89 litres of milk for a soup base.How many quarts are needed?

A)1.79 qts

B)2.00 qts

C)1.89 qts

D)2.10 qts

E)2.15 qts

Answer: B

Q2) How many significant figures are there in the answer to the following problem?

(9.992 × 3.200)+ 0.610

A)one

B)two

C)three

D)four

Answer: D

Q3) Describe the difference between an intensive and extensive property using examples.

Answer: An intensive property does not depend on the amount of the substance present,such as colour or density.An extensive property is one that does depend on the amount of the substance,such as mass or volume.

Page 3

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Chapter 2: Atoms and Elements

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Sample Questions

Q1) If 3.6 g of chlorine combines with sodium to make 6.0 g of sodium chloride,what mass of sodium is required?

A)3.6 g

B)2.4 g

C)6.0 g

D)9.6 g

E)1.2 g

Answer: B

Q2) Bromine has two naturally occurring isotopes,Br-79 and Br-81.The atomic mass of Br-79 is 78.9183 u with a percent abundance of 50.69% and the atomic mass of Br-81 is 80.9163 u.Calculate the atomic mass of bromine.

A)80.91 u

B)78.92 u

C)79.90 u

D)80.92 u

E)80.03 u

Answer: C

Q3) Give an example of a halogen.

Answer: F,Br,I,Cl,or At

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Chapter 3: Molecules,compounds,and Nomenclature

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Sample Questions

Q1) What is the mass (in kg)of 6.89 × 10²⁵molecules of CO₂?

The molar mass of CO₂ is 44.01 g mol^-1.

A)3.85 kg

B)5.04 kg

C)2.60 kg

D)3.03 kg

E)6.39 kg

Answer: B

Q2) Which of the following has the greatest mass?

A)3.88 × 10²² molecules of O₂

B)1.00 g of O₂

C)0.0312 mol of O₂

D)All of the above have the same mass.

Answer: A

Q3) The compound Cu(NO₂ )₂,is named

A)copper nitrite(II).

B)copper(I)nitrite.

C)copper(I)nitrite(II).

D)copper(II)nitrite.

Answer: D

Page 5

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Chapter 4: Chemical Reactions and Stoichiometry

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Sample Questions

Q1) Lithium and nitrogen react to produce lithium nitride: 6Li(s)+ \(\mathrm { N } _ { 2 }\) (g)? \(2 \mathrm { Li } _ { 3 }\) N(s)

How many moles of \(\mathrm { N } _ { 2 }\) are needed to react with 0.400 mol of lithium?

A)2.40

B)0.400

C)0.133

D)1.2

E)0.0667

Q2) What precipitate is most likely formed from a solution containing Ba²⁺,Na¹⁺,OH^1-,and CO₃^2-.

A)NaOH

B)BaCO₃

C)Na₂CO₃

D)Ba(OH)₂

Q3) Which pair of compounds is soluble in water?

A)HgBr₂ and Hg₂I₂

B)CuS and Na₂S

C)LiI and Ca(NO₃)₂

D)KNO₃ and CaCO₃

Page 6

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Chapter 5: Gases

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Sample Questions

Q1) Calculate the root mean square velocity of nitrogen molecules at 25 °C.

A)729 m s^-1

B)515 m s^-1

C)149 m s^-1

D)297 m s^-1

Q2) What is the volume of 5.60 g of O₂ at 7.78 bar and 415 K?

A)1.53 L

B)565 L

C)24.5 L

D)25.0 L

E)0.776 L

Q3) Determine the density of \(\mathrm { CO } _ { 2 }\) gas at 278 K and 1.00 bar.

A)1.14 g \(\mathrm { L } ^ { - 1 }\)

B)2.37 g \(\mathrm { L } ^ { - 1 }\)

C)1.90 g \(\mathrm { L } ^ { - 1 }\)

D)3.08 g \(\mathrm { L } ^ { - 1 }\)

E)2.11 g \(\mathrm { L } ^ { - 1 }\)

Q4) Consider a container of gas under a particular P,V,T set of conditions.Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of 2.

Page 7

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Chapter 6: Thermochemistry

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Sample Questions

Q1) Calculate the kinetic energy of a 150 g baseball moving at a speed of 39.m \(s ^ { - 1 }\) (87 mph).

A)5.8 J

B)1.1 × 10²J

C)5.8 × 10³ J

D)1.1 × 10⁵ J

Q2) Which of the following is TRUE if \(\Delta\)_sysU = -95 J?

A)The system is gaining 95 J,while the surroundings are losing 95 J.

B)The system is losing 95 J,while the surroundings are gaining 95 J.

C)Both the system and the surroundings are gaining 95 J.

D)Both the system and the surroundings are losing 95 J.

E)None of the above are true.

Q3) Given w = 0,an endothermic reaction has which of the following properties?

A)+ H and - U

B)- H and + U

C)+ H and + U

D)- H and - U

Q4) Explain the difference between H and U.

Q5) Define chemical energy.

Q6) The standard state of carbon is ________.

Page 8

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Chapter 7: The Quantum-Mechanical Model of the Atom

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Sample Questions

Q1) Calculate the energy of an electron in the orbital n = 6 of a hydrogen atom.

A)3.19 × 10^-20 J

B)4.18 × 10^-20 J

C)-6.06 × 10^-20 J

D)-7.80 × 10^-20 J

E)-8.62 × 10^-20 J

Q2) Identify the colour of a flame test for potassium.

A)violet

B)red

C)white

D)yellow

E)blue

Q3) What are the possible values of n and m_l for an electron in a 3d orbital?

A)n = 1,2,or 3 and m_l = 2

B)n = 1,2,or 3 and m_l = -2,-1,0,+1,or +2

C)n = 4 and m_l = 2

D)n = 3 and m_l = -2,-1,0,+1,+2

Q4) Give the ground-state electron configuration for Cd⁺².

Q5) Why don't we observe the wavelength of everyday macroscopic objects?

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Chapter 8: Periodic Properties of the Elements

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Sample Questions

Q1) How many valence electrons do the noble gases possess?

A)1

B)3

C)7

D)6

E)8

Q2) Which ionization process requires the most energy?

A)S(g) S⁺(g)+ e^-

B)S⁺(g) S²⁺(g)+ e^-

C)Cl(g) Cl⁺(g)+ e^-

D)Cl⁺(g) Cl²⁺(g)+ e^-

Q3) Use the periodic table to predict the most stable oxidation state for the following element: Na

A)+1

B)+2 C)+3 D)-1

E)-2

Q4) Why do successive ionization energies increase?

Q5) Define electron affinity.

Page 10

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Chapter 9: Chemical Bonding I: Lewis Theory

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Sample Questions

Q1) Which of the following resonance structures for OCN^- will contribute most to the correct structure of OCN ?

A)O(2 lone pairs)=C=N(2 lone pairs)

B)O(1 lone pair) C-N(3 lone pairs)

C)O(1 lone pair)=C(2 lone pairs)=N(1 lone pair)

D)O(3 lone pairs)-C N(1 lone pair)

E)They all contribute equally to the correct structure of OCN^-.

Q2) Identify an ionic bond.

A)Electrons are pooled.

B)Electrons are shared.

C)Electrons are transferred.

D)Electrons are gained.

E)Electrons are lost.

Q3) Define formal charge.

Q4) A triple covalent bond contains ________ of electrons.

A)0 pairs

B)1 pair

C)2 pairs

D)3 pairs

E)4 pairs

Page 11

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Chapter 10: Chemical Bonding II: Molecular Shapes, valence

Bond Theory, and Molecular Orbital Theory

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Sample Questions

Q1) Determine the electron geometry (eg)and molecular geometry (mg)of XeF₂.

A)eg = trigonal bipyramidal,mg = bent

B)eg = linear,mg = linear

C)eg = tetrahedral,mg = linear

D)eg = trigonal bipyramidal,mg = linear

E)eg = tetrahedral,mg = bent

Q2) Determine the electron geometry (eg),molecular geometry (mg),and polarity of TeCl₆.

A)eg = octahedral,mg = octahedral,nonpolar

B)eg = trigonal bipyramidal,mg = trigonal bipyramidal,nonpolar

C)eg = octahedral,mg = square planar,polar

D)eg = trigonal bipyramidal,mg = seesaw,polar

E)eg = tetrahedral,mg = trigonal pyramidal,polar

Q3) Use molecular orbital theory to determine whether He₂²⁺ or He₂⁺ is more stable.

Q4) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Q5) According to molecular orbital theory,what is an antibonding orbital?

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Chapter 11: Liquids, solids, and Intermolecular Forces

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Sample Questions

Q1) At atmospheric pressure,dry ice ________.

A)freezes

B)deposits

C)sublimes

D)melts

E)boils

Q2) Give the term for the temperature at which the gas and liquid phases form a supercritical fluid.

A)absolute temperature

B)definite temperature

C)fluid temperature

D)critical temperature

E)solid temperature

Q3) The normal boiling point of water is ________.

A)0 °C

B)32 °C

C)212 °C

D)100 °C

E)273 °C

Q4) Define volatile.

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Chapter 12: Solutions

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Sample Questions

Q1) Calculate the freezing point of a solution of 40.0 g salicylaldehyde,C₇H₆O₂,dissolved in 800.g of benzene,C₆H₆. K_f for benzene is \( 5.10^{\circ} \mathrm{C} \mathrm{m}^{-1} \) and the freezing point is 5.50 °C for benzene.

A)-2.09 °C

B)2.09 °C

C)3.41 °C

D)7.59 °C

Q2) Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈,molar mass = 128.16 g mol^-1)dissolved in 722 mL of benzene (d = 0.877 g mL^-1).Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m^-1.

A)2.2 °C

B)2.5 °C

C)82.3 °C

D)80.4 °C

E)82.6 °C

Q3) Why isn't pentanol (CH₃CH₂CH₂CH₂CH₂OH) very soluble in water?

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Chapter 13: Chemical Kinetics

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Sample Questions

Q1) Calculate the frequency factor,A,for a reaction with a rate constant of 162.3 s^-1 and an activation energy,E_a,of 68 kJ mol^-1 at 298 K.

A)2.1 × 10² s^-1

B)2.5 × 10³ s^-1

C)2.6 × 10¹²¹ s^-1

D)1.3 × 10¹⁴ s^-1

E)3.8 × 10¹¹ s^-1

Q2) Given the following proposed mechanism,predict the rate law for the overall reaction.

\(\quad\)A₂ + 2B 2AB (overall reaction) \(\quad\)\(\underline{\text{Mechanism}}\)

\(\quad\)A₂ 2A \(\quad\)\(\quad\) fast \(\quad\)A + B AB \(\quad\)slow

A)Rate = k[A][B]

B)Rate = k[A₂][B]

C)Rate = k[A₂][B]^1/2

D)Rate = k[A₂]

E)Rate = k[A₂]^1/2[B]

Q3) What function do enzymes serve?

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Chapter 14: Chemical Equilibrium

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Sample Questions

Q1) At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: \(\quad\)\(\quad\)\(\quad\)2ICl(g) I₂(g)+ Cl₂(g)

What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0 L flask?

A)0.23 mol L^-1

B)0.28 mol L^-1

C)0.225 mol L^-1

D)0.56 mol L^-1

Q2) For the reaction: N₂(g)+ 2O₂(g) 2NO₂(g),K_c = 8.3 × 10^-10 M^-1at 25

°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

A)3.3 × 10^-¹¹ mol L^-1

B)1.7 × 10^-10 mol L^-1

C)6.0 × 10⁹ mol L^-1

D)3.0 × 10¹⁰ mol L^-1

Q3) Explain dynamic equilibrium.Use the generic reaction A(g) B(g)to explain.

Q4) Why is a thermodynamic equilibrium constant unitless?

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Chapter 15: Acids and Bases

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Sample Questions

Q1) Which one of the following salts,when dissolved in water,produces the solution with the lowest pH?

A)NaCl

B)KCl

C)MgCl₂

D)AlCl₃

Q2) Which of the following acids will have the strongest conjugate base?

A)HCl

B)HClO₄

C)HNO₃

D)HCN

E)HI

Q3) Determine the pOH of a 0.188 mol L^-1 NH₃ solution at 25 °C.The K_bof NH₃ is 1.76 × 10^-5.

A)5.480

B)2.740

C)8.520

D)11.260

E)12.656

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Chapter 16: Aqueous Ionic Equilibrium

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Sample Questions

Q1) Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

A)9.22 × 10^-9 mol L^-1

B)4.26 × 10^-17 mol L^-1

C)8.51 × 10^-17 mol L^-1

D)2.77 × 10^-6 mol L^-1

E)4.40 × 10^-6 mol L^-1

Q2) A solution contains 0.021 mol L^-1 Cl^- and 0.017 mol L^-1 I^-.A solution containing copper(I)ions is added to selectively precipitate one of the ions.At what concentration of copper(I)ion will a precipitate begin to form? What is the identity of the precipitate? K_sp(CuCl)= 1.0 × 10^-6,K_sp(CuI)= 5.1 × 10^-12.

A)3.0 × 10^-10mol L^-1,CuI

B)3.0 × 10^-10 mol L^-1,CuCl

C)4.8 × 10^-5 mol L^-1,CuCl

D)4.8 × 10^-5 mol L^-1,CuI

E)3.0 × 10^-5 mol L^-1,both CuCl and CuI are in the precipitate

Q3) Explain the common ion effect with respect to molar solubility.

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Page 18

Chapter 17: Gibbs Energy and Thermodynamics

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Sample Questions

Q1) Use the following thermodynamic values to calculate ?_r \(G ^ { 0 }\) .

\(\Delta_{r}\)\( H^{\circ} \) = +95 kJ \(\mathrm { mol } ^ { - 1 }\) \(\Delta_{r}\)\(S

^ { 0 }\) = -157 J \(\mathrm { mol } ^ { - 1 }\) ,T = 298 K

A)-48 kJ \(\mathrm { mol } ^ { - 1 }\)

B)-68 kJ \(\mathrm { mol } ^ { - 1 }\)

C)+39 kJ \(\mathrm { mol } ^ { - 1 }\)

D)-157 kJ \(\mathrm { mol } ^ { - 1 }\)

E)+142 kJ \(\mathrm { mol } ^ { - 1 }\)

Q2) Use the following thermodynamic values to calculate ?_r \( G^{0} \) .

\(\Delta_{r}\)\( H^{\circ} \) = -95 kJ \(\mathrm { mol } ^ { - 1 }\) ,\(\Delta_{r}\)\(S

^ { 0 }\) = -157 J \(\mathrm { mol } ^ { - 1 }\) ,T = 298 K

A)-48 kJ \(\mathrm { mol } ^ { - 1 }\)

B)-68 kJ \(\mathrm { mol } ^ { - 1 }\)

C)+ 39 kJ \(\mathrm { mol } ^ { - 1 }\)

D)-157 kJ \(\mathrm { mol } ^ { - 1 }\)

E)+142 kJ \(\mathrm { mol } ^ { - 1 }\)

Q3) Define the third law of thermodynamics.

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Page 19

Chapter 18: Electrochemistry

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Sample Questions

Q1) Identify the battery type that has a high overcharge tolerance.

A)NiCad battery

B)lithium-ion battery

C)nickel-metal hydride battery

D)lead-acid storage battery

E)zinc-manganese battery

Q2) What is the shorthand notation that represents the following galvanic cell reaction? \(\quad\)\(\quad\)Pb(s)+

Cu(NO₃)₂(aq) Pb(NO₃)₂(aq)+ Cu(s)

A)Pb(s)| Pb²⁺(aq)|| Cu²⁺(aq)| Cu(s) B)Cu(s)| Cu²⁺(aq)|| Pb²⁺(aq)| Pb(s)

C)Pb(s)| NO₃^-(aq)|| NO₃^-(aq)| Cu(s) D)Cu(s)| Cu(NO₃)₂(aq)|| Pb(NO₃)₂(aq)| Pb(s)

Q3) Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

Q4) Why are iron nails coated with zinc?

Q5) Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

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Chapter 19: Radioactivity and Nuclear Chemistry

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Sample Questions

Q1) Carbon-11 is used in medical imaging.The half-life of this radioisotope is 20.4 min.What percentage of a sample remains after 50.0 min?

A)40.8%

B)2.45%

C)81.7%

D)0.183%

E)18.3%

Q2) Calculate the mass defect in Mo-96 if the mass of a Mo-96 nucleus is 95.962 amu.The mass of a proton is 1.00728 amu and the mass of a neutron is 1.008665 amu.

A)0.197 amu

B)0.795 amu

C)0.212 amu

D)0.812 amu

E)0.188 amu

Q3) Define chain reaction in terms of the fission of uranium nucleus.

Q4) Why is an alpha emitter much more harmful if it is ingested than when applied to the skin?

Q5) Define radioactivity.

Q6) Describe what is meant by the "valley of stability."

Page 21

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Chapter 20: Organic Chemistry I: Structures

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Sample Questions

Q1) Which of the following is TRUE regarding constitutional isomers?

A)Constitutional isomers have the same molecular formula but different structures,physical,and chemical properties.

B)Constitutional isomers have the same molecular formula and physical properties but different structures and chemical properties.

C)Constitutional isomers have the same molecular formula,physical,and chemical properties but different structures.

D)Constitutional isomers have the same chemical structure and molecular formula but different physical and chemical properties.

E)Constitutional isomers have the same chemical structure but different formulas,physical,and chemical properties.

Q2) Which of the following compounds is ethanol?

A)C₂H₆

B)C₂H₅OH

C)CH₃CO₂H

D)CH₃CO₂CH₃

E)CH₃-O-CH₃

Q3) What is meant by the term,"structural isomer"?

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Chapter 21: Organic Chemistry II: Reactions

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Q1) Draw a clear mechanism for S_N1 substitution reactions.Make sure to indicate each step of the mechanism (if there is more than one)as well as to use arrows to show the electron flow.

Q2) Draw a clear mechanism for E1 elimination reactions.Make sure to indicate each step of the mechanism (if there is more than one)as well as to use arrows to show the electron flow.

Q3) Identify the organic product for the following reaction. \(\mathrm { CH } _ { 3 } \mathrm { CH } _ { 2 } \mathrm { COOH } + \mathrm { CH } _ { 3 } \mathrm { CH } _ { 2 } \mathrm { CH } _ { 2 } \mathrm { NH } _ { 2 } \stackrel { \text { with } \mathrm { SOCl } _ { 2 } } { \longrightarrow }\)

A)CH₃CH₂NHCH₂CH₂CH<sub>3</sub >

B)CH₃CH₂CON(CH₂CH₂CH<sub>3</s ub>)₂

C)CH₃CH₂CH₂CONHCH₂CH<sub>3</s ub>

D)CH₃CH₂CONHCH₂CH₂CH<sub>3</s ub>

E)CH₃CH₂N(CH₂CH₂CH₃ )₂

Q4) Why doesn't benzene typically undergo addition reactions like the alkenes do?

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Chapter 22: Biochemistry

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Sample Questions

Q1) Identify the polysaccharide.

A)glucose

B)cholesterol

C)fructose

D)cellulose

E)sucrose

Q2) Which of the following hold two strands of DNA in an a-helix?

A)ester linkages

B)disulfide linkages

C)peptide bonds

D)hydrogen bonds

E)glycosidic linkages

Q3) Which one of the following amino acids contains a hydrophobic side chain?

A)valine

B)histidine

C)glutamine

D)glutamic acid

Q4) What is a codon?

Q5) How do cis- and trans-fats differ?

Q6) Why are lipids well-suited as structural components of cell membranes?

Page 24

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Chapter 23: Chemistry of the Nonmetals

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Sample Questions

Q1) Draw the Lewis structure for IF₄ and determine the geometry of the ion.

Q2) Determine the oxidation state of carbon in the carbonate ion CO₃^2-.

A)+2

B)+4

C)+3 D)+6 E)+8

Q3) Determine the formula for an aluminosilicate where one-quarter of the silicons are replaced by an aluminum atom.The charge is balanced by sodium ions.

A)Na₂(AlO₂)₂(SiO₂)

B)Na₂(AlO₂)₂(SiO₂)₃

C)Na(AlO₂)₂(SiO₂)

D)Na₂(AlO₂)₂(SiO₂)₂

E)Na(AlO₂)(SiO₂)₃

Q4) Why are phosphate compounds added to detergents?

Q5) Describe the major production method for obtaining oxygen.

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Chapter 24: Metals and Metallurgy

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Q1) Why does a "two-phase" structure occur in a substitutional alloy?

Q2) Identify the substances that are homogeneous,naturally occurring,crystalline inorganic solids.

A)slag

B)minerals

C)ores

D)gangue

E)alloy

Q3) An interstitial alloy contains nitrogen in half of the octahedral holes of a closest-packed metal,M.What is the formula of this alloy?

A)MN

B)MN₂

C)M₄N

D)M₂N

E)MN₄

Q4) Describe the difference between a substitutional alloy and an interstitial alloy.

Q5) Why is zinc used to coat steel objects?

Q6) What is the difference between ferromagnetism and paramagnetism?

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Chapter 25: Transition Metals and Coordination Compounds

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Sample Questions

Q1) Identify the isomers that have ligands that coordinate to a metal in different orientations.

A)linkage isomers

B)cis-trans isomers

C)coordination isomers

D)optical isomers

E)stereoisomers

Q2) Name the following: Fe[AlF₆]

A)ironaluminumhexafluoride

B)iron(II)hexafluoroaluminum

C)iron (III)hexafluoroaluminate

D)iron(I)aluminumhexafluoride

E)aluminumhexafluoroferrate

Q3) How many unpaired electrons would you expect for the complex ion [Fe(CN)₆]^4-?

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