Basic Chemistry Test Preparation - 3207 Verified Questions

Basic Chemistry Test Preparation https://quizplus.com/study-set/3470 25 Chapters 3207 Verified Questions

Basic Chemistry Test Preparation Course Introduction 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

Available Study Resources on Quizplus 25 Chapters 3207 Verified Questions 3207 Flashcards Source URL: https://quizplus.com/study-set/3470

Page 2

Chapter 1: Units of Measurement for Physical and Chemical Change Available Study Resources on Quizplus for this Chatper 173 Verified Questions 173 Flashcards Source URL: https://quizplus.com/quiz/68935

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 2: Atoms and Elements Available Study Resources on Quizplus for this Chatper 161 Verified Questions 161 Flashcards Source URL: https://quizplus.com/quiz/68936

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 To view all questions and flashcards with answers, click on the resource link above.

Page 4

Chapter 3: Molecules,compounds,and Nomenclature Available Study Resources on Quizplus for this Chatper 172 Verified Questions 172 Flashcards Source URL: https://quizplus.com/quiz/68937

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 4: Chemical Reactions and Stoichiometry Available Study Resources on Quizplus for this Chatper 247 Verified Questions 247 Flashcards Source URL: https://quizplus.com/quiz/68938

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 5: Gases Available Study Resources on Quizplus for this Chatper 146 Verified Questions 146 Flashcards Source URL: https://quizplus.com/quiz/68939

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 6: Thermochemistry Available Study Resources on Quizplus for this Chatper 145 Verified Questions 145 Flashcards Source URL: https://quizplus.com/quiz/68940

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)+ΔH and -ΔU B)-ΔH and +ΔU C)+ΔH and +ΔU D)-ΔH and -ΔU Q4) Explain the difference between ΔH and ΔU. Q5) Define chemical energy.

Page 8 Q6) The standard state of carbon is ________.

To view all questions and flashcards with answers, click on the resource link above.

Chapter 7: The Quantum-Mechanical Model of the Atom Available Study Resources on Quizplus for this Chatper 164 Verified Questions 164 Flashcards Source URL: https://quizplus.com/quiz/68941

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?

9 click on the resource link above.

To view all questions and flashcards with Page answers,

Chapter 8: Periodic Properties of the Elements Available Study Resources on Quizplus for this Chatper 129 Verified Questions 129 Flashcards Source URL: https://quizplus.com/quiz/68942

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

To view all questions and flashcards with answers, click on the resource link above.

Chapter 9: Chemical Bonding I: Lewis Theory Available Study Resources on Quizplus for this Chatper 136 Verified Questions 136 Flashcards Source URL: https://quizplus.com/quiz/68943

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 10: Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory Available Study Resources on Quizplus for this Chatper 158 Verified Questions 158 Flashcards Source URL: https://quizplus.com/quiz/68944

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.

Page 12 Q5) According to molecular orbital theory,what is an antibonding orbital?

To view all questions and flashcards with answers, click on the resource link above.

Chapter 11: Liquids, solids, and Intermolecular Forces Available Study Resources on Quizplus for this Chatper 127 Verified Questions 127 Flashcards Source URL: https://quizplus.com/quiz/68945

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.

Page 13 To view all questions and flashcards with answers, click on the resource link above.

Chapter 12: Solutions Available Study Resources on Quizplus for this Chatper 153 Verified Questions 153 Flashcards Source URL: https://quizplus.com/quiz/68946

Sample Questions Q1)

Calculate

the

freezing

point

of

a

solution

salicylaldehyde,C₇H₆O₂,dissolved

of

40.0

g

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?

To view all questions and flashcards with answers, click on the resource link above.

Page 14

Chapter 13: Chemical Kinetics Available Study Resources on Quizplus for this Chatper 156 Verified Questions 156 Flashcards Source URL: https://quizplus.com/quiz/68947

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?

To view all questions and flashcards with answers, click on the resource link above.

Page 15

Chapter 14: Chemical Equilibrium Available Study Resources on Quizplus for this Chatper 124 Verified Questions 124 Flashcards Source URL: https://quizplus.com/quiz/68948

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?

To view all questions and flashcards with answers, click on the resource link above.

Page 16

Chapter 15: Acids and Bases Available Study Resources on Quizplus for this Chatper 141 Verified Questions 141 Flashcards Source URL: https://quizplus.com/quiz/68949

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 To view all questions and flashcards with answers, click on the resource link above.

Page 17

Chapter 16: Aqueous Ionic Equilibrium Available Study Resources on Quizplus for this Chatper 159 Verified Questions 159 Flashcards Source URL: https://quizplus.com/quiz/68950

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.

To view all questions and flashcards with answers, click on the resource link above.

Page 18

Chapter 17: Gibbs Energy and Thermodynamics Available Study Resources on Quizplus for this Chatper 119 Verified Questions 119 Flashcards Source URL: https://quizplus.com/quiz/68951

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.

To view all questions and flashcards with answers, click on the resource link above.

Page 19

Chapter 18: Electrochemistry Available Study Resources on Quizplus for this Chatper 107 Verified Questions 107 Flashcards Source URL: https://quizplus.com/quiz/68952

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.

To view all questions and flashcards with answers, click on the resource link above.

Page 20

Chapter 19: Radioactivity and Nuclear Chemistry Available Study Resources on Quizplus for this Chatper 108 Verified Questions 108 Flashcards Source URL: https://quizplus.com/quiz/68953

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 To view all questions and flashcards with answers, click on the resource link above.

Chapter 20: Organic Chemistry I: Structures Available Study Resources on Quizplus for this Chatper 103 Verified Questions 103 Flashcards Source URL: https://quizplus.com/quiz/68954

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"?

To view all questions and flashcards with answers, click on the resource link above.

Page 22

Chapter 21: Organic Chemistry II: Reactions Available Study Resources on Quizplus for this Chatper 93 Verified Questions 93 Flashcards Source URL: https://quizplus.com/quiz/68955

Sample Questions 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?

Page 23 To view all questions and flashcards with answers, click on the resource link above.

Chapter 22: Biochemistry Available Study Resources on Quizplus for this Chatper 49 Verified Questions 49 Flashcards Source URL: https://quizplus.com/quiz/68956

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?

Page 24 Q6) Why are lipids well-suited as structural components of cell membranes?

To view all questions and flashcards with answers, click on the resource link above.

Chapter 23: Chemistry of the Nonmetals Available Study Resources on Quizplus for this Chatper 45 Verified Questions 45 Flashcards Source URL: https://quizplus.com/quiz/68957

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.

To view all questions and flashcards with answers, click on the resource link above.

Page 25

Chapter 24: Metals and Metallurgy Available Study Resources on Quizplus for this Chatper 42 Verified Questions 42 Flashcards Source URL: https://quizplus.com/quiz/68958

Sample Questions 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?

To view all questions and flashcards withPage answers, 26 click on the resource link above.

Chapter 25: Transition Metals and Coordination Compounds Available Study Resources on Quizplus for this Chatper 50 Verified Questions 50 Flashcards Source URL: https://quizplus.com/quiz/68959

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

[Fe(CN)₆]^4-?

A)5 B)2 C)6 D)4 E)0

Page 27

To view all questions and flashcards with answers, click on the resource link above.

ion