Fundamentals Of General Organic And Biological Chemistry 7th Edition By John E. McMurry Test Bank

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Fundamentals Of General Organic And Biological Chemistry 7th Edition By John E. McMurry Test Bank

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Fundamentals Of General Organic And Biological Chemistry 7th Edition By John E. McMurry Test Bank

Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry)

Chapter 5 Classification and Balancing of Chemical Reactions

1) In a chemical reaction

A) there are equal numbers of atoms on each side of the reaction arrow.
B) there are equal numbers of molecules on each side of the reaction arrow.
C) there are always the same number of products as there are reactants.
D) the number of atoms present in a reaction can vary when the conditions change during the reaction.
E) none of the above

Answer: A

Diff: 3

Section: 5.1

2) Consider the balanced equation shown and identify the statement that is not true.

Na2SO4 (aq) + BaCl2 (aq) 2 NaCl (aq) + BaSO4 (s)

A) The coefficient of sodium sulfate is one.
B) Barium sulfate is produced in solid form.
C) Barium chloride is dissolved in water.
D) The products are barium sulfate and sodium chloride.
E) 2 NaCl (aq) could also be correctly written as Na2Cl2(aq).

Answer: E

Diff: 1

Section: 5.1

3) In a precipitation reaction the insoluble product can be identified by the symbol ________.

A) (aq)
B) (l)
C) (g)
D) (s)
E) none of the above

Answer: D

Diff: 1

Section: 5.1

4) Consider the reaction shown and identify the statement that is not true.

CaCO3 (s) CaO (s) + CO2 (g)

A) This reaction is balanced as written.
B) The reactant must be heated for this reaction to occur.
C) The products are a solid and a gas.
D) Water must be present for this reaction to occur.
E) There are no solutions used in this reaction.

Answer: D

Diff: 1

Section: 5.1

5) The scientific principle which is the basis for balancing chemical equations is

A) the Law of Conservation of Energy.
B) the Law of Conservation of Mass.
C) the Law of Conservation of Mass and Energy.
D) the Law of Definite Proportions.
E) Avogadros Law.

Answer: B

Diff: 2

Section: 5.1

6) Which statement regarding balanced chemical equations is not true?

A) The number of each kind of atoms must be the same on each side.
B) Coefficients are used in front of formulas to balance the equation.
C) Subscripts may be changed to make an equation simpler to balance.
D) When no coefficient is written in front of a formula, the number one is assumed.
E) Reactants are written to the left of the arrow.

Answer: C

Diff: 2

Section: 5.2

7) Which is the correct equation for the reaction of magnesium with hydrochloric acid to produce hydrogen and magnesium chloride?

A) Mg + 2 HCl H2 + MgCl2
B) Mg + HCl H + MgCl
C) 2 Mg + 6 HCl 3 H2 + 2 MgCl2
D) Mg + 2 HCl 2 H + MgCl2
E) Mg + 3 HCl 3 H + MgCl2

Answer: A

Diff: 2

Section: 5.2

8) Which of the following equations is not balanced?

A) 2 Na + 2 H2O 2 NaOH + H2
B) C3H8 + 5 O2 3 CO2 + 4 H2O
C) 2 H2 + O2 2 H2O
D) SO2 + O2 SO3
E) 2 Al + 6 HCl 2 AlCl3 + 3 H2

Answer: D

Diff: 2

Section: 5.2

9) Which of the following equations is not balanced?

A) C7H16 + O2 7 CO2 + 8 H2O
B) K2CrO4 + Pb(NO3)2 2 KNO3 + PbCrO4
C) 4 Fe3O4 + O2 6 Fe2O3
D) 3 AgNO3 + (NH4)3PO4 Ag3PO4 + 3 NH4NO3
E) 2 Al2O3 4 Al + 3 O2

Answer: A

Diff: 2

Section: 5.2

10) When the reaction shown is correctly balanced, the coefficients are:

KClO3 KCl + O2

A) 1, 1, 1
B) 2, 2, 2
C) 2, 2, 3
D) 2, 2, 1
E) 4, 4, 6

Answer: C

Diff: 2

Section: 5.2

11) When the reaction shown is correctly balanced, the coefficients are:

C6H14 (l) + O2 (g) CO2 (g) + H2O (g)

A) 1, 6, 6, 7
B) 2, 19, 12, 14
C) 1, 3.5, 6, 7
D) 1, 9.5, 6, 7
E) 2, 16.5, 12, 7

Answer: B

Diff: 2

Section: 5.2

12) When the following reaction is balanced the coefficient in front of carbon dioxide is:

____ C5H12 + ____ O2 ____ CO2 + ____ H2O

A) 5
B) 6
C) 12
D) 10

Answer: A

Diff: 1

Section: 5.2

13) When the following reaction is balanced the coefficient in front of oxygen is:

____ C8H18 + ____ O2 ____ CO2 + ____ H2O

A) 25
B) 12
C) 18
D) 9

Answer: A

Diff: 3

Section: 5.2

14) In the correctly balanced reaction the coefficient for the H2O is:

____ Al(OH)3 + ____ H2SO4 ____ Al2 (SO4)3 + ____ H2O

A) 1
B) 2
C) 3
D) 6
E) 8

Answer: D

Diff: 2

Section: 5.2

15) When the reaction shown is correctly balanced, the coefficients are:

____ HBr + ____ Ca(OH)2 ____ CaBr2 + ____ H2O

A) 2, 1, 1, 1
B) 1, 1, 1, 2
C) 2, 1, 1, 2
D) 2, 2, 1, 1
E) 2, 1, 2, 2

Answer: C

Diff: 2

Section: 5.2

16) When the reaction shown is correctly balanced, the coefficients are:

Li + Br2 LiBr

A) 1, 1, 1
B) 1, 2, 2
C) 1, 2, 1
D) 2, 2, 1
E) 2, 1, 2

Answer: E

Diff: 2

Section: 5.2

17) When the reaction shown is correctly balanced, the coefficients are:

HNO3 + KOH KNO3 + H2O

A) 0, 0, 0, 0
B) 1, 1, 1, 1
C) 2, 2, 2, 2
D) 3, 1, 1, 3
E) 2, 1, 2, 1

Answer: B

Diff: 2

Section: 5.2

18) When the reaction shown is balanced, there are ________ atoms of oxygen and ________ atoms of hydrogen on each side.

(NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + NH4C2H3O2 (aq)

A) 6; 11
B) 16; 18
C) 8; 14
D) 4; 7
E) 16; 28

Answer: C

Diff: 3

Section: 5.2

19) The balanced equation for the reaction occurring when calcium nitrate solution is mixed with sodium phosphate solution is

A) 3 Ca(NO3)2(aq) + 2 Na3PO4 (aq) Ca3(PO4)2 (aq) + 6 NaNO3 (aq).
B) 2 Ca(NO3)2(aq) + 3 Na3PO4 (aq) 2 Ca3(PO4)2 (s) + 6 NaNO3 (aq).
C) 3 CaNO3(aq) + Na3PO4 (aq) Ca3PO4 (aq) + 3 NaNO3 (s).
D) 3 Ca(NO3)2(aq) + 2 Na3PO4 (aq) Ca3(PO4)2 (s) + 6 NaNO3 (aq).
E) Ca(NO3)2(aq) + 2 NaPO4 (aq) Ca(PO4)2 (s) + 2 NaNO3 (aq).

Answer: D

Diff: 3

Section: 5.3

20) The balanced equation for the reaction occurring when iron(III) oxide, a solid, is reduced with pure carbon to produce carbon dioxide and molten iron is

A) 2 Fe3O + C (s) 6 Fe (l) + CO2 (g).
B) 2 FeO3 + 3 C (s) 2 Fe (l) + 3 CO2 (g).
C) 4 Fe2O3 + 6 C (s) 8 Fe (l) + 6 CO2 (g).
D) 2 FeO + C (s) 2 Fe (l) + CO2 (g).
E) 2 Fe2O3 + 3 C (s) 4 Fe (l) + 3 CO2 (g).

Answer: E

Diff: 3

Section: 5.3

21) The balanced equation for the reaction between aqueous ammonium sulfate and aqueous barium acetate is

A) (NH4)2SO4(aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + NH4C2H3O2 (aq).
B) (NH4)2SO4(aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + 2 NH4C2H3O2 (aq).
C) NH4SO4(aq) + BaC2H3O2 (aq) BaSO4 (s) + NH4C2H3O2 (aq).
D) (NH4)2SO4(aq) + Ba(C2H3O2)2 (aq) BaSO4 (aq) + 2 NH4C2H3O2 (s).
E) (NH4)2SO3(aq) + Ba(C2H3O2)2 (aq) BaSO3 (aq) + NH4C2H3O2 (aq).

Answer: B

Diff: 3

Section: 5.3

22) The reaction 2 AgNO3 (aq) + K2SO4 (aq) 2 KNO3 (aq) + Ag2SO4 (s) is an example of a(an) ________ reaction.

A) acid-base
B) oxidation-reduction
C) precipitation
D) combustion
E) none of the above

Answer: C

Diff: 1

Section: 5.3

23) Which reaction is an example of a precipitation reaction?

A) H2CO3(aq) H2O (l) + CO2 (g)
B) H2SO4(aq) + Ca(OH)2 (aq) CaSO4 (aq) + 2 H2O (l)
C) 6 HCl (aq) + 2 Al (s) 2 AlCl3 (aq) + 3 H2 (g)
D) FeCl3(aq) + 3 KOH (aq) Fe(OH)3 (s) + 3 KCl (aq)
E) 2 Hg (l) + O2 (g) 2 HgO (s)

Answer: D

Diff: 1

Section: 5.3

24) Which reaction is an example of both a precipitation and a neutralization?

A) H3PO4(aq) + 3 KOH (aq) K3PO4 (aq) + 3 H2O (l)
B) FeCl3(aq) + 3 KOH (aq) Fe(OH)3 (s) + 3 KCl (aq)
C) (NH4)2CO3(s) 2 NH3 (g) + CO2 (g) + H2O (l)
D) H2SO4(aq) + Ba(OH)2 (aq) BaSO4 (s) + 2 H2O (l)
E) 2 C (s) + O2(g) 2 CO (g)

Answer: D

Diff: 2

Section: 5.3

25) The following reaction can be classified as what type(s) of reaction(s)?

2 Al(OH)3 (aq) + 3 H2SO4 (aq) Al2(SO4)3 (s) + 6 H2O (l)

A) precipitation
B) acid-base neutralization
C) redox reaction
D) both A and B

Answer: D

Diff: 2

Section: 5.3

26) The formation of which one of the compounds below will act as the driving force for an acid-base reaction?

A) H2O
B) MgCl2
C) NaNO3
D) KOH

Answer: A

Diff: 2

Section: 5.3

27) The combination of ions most likely to produce a precipitate is

A) Li+and PO43-.
B) Pb2+and NO3-.
C) NH4+and SO42-.
D) Fe3+and OH-.
E) Mg2+and C2H3O2-.

Answer: D

Diff: 2

Section: 5.4

28) The combination of ions least likely to produce a precipitate is

A) Ba2+and SO42-.
B) Pb+and Cl-.
C) Ca2+and PO43-.
D) Fe3+and OH-.
E) Mg2+and C2H3O2-.

Answer: E

Diff: 2

Section: 5.4

29) Which of the following is not soluble in water?

A) potassium sulfide
B) iron(II) bromide
C) iron(III) hydroxide
D) iron(III)nitrate
E) ammonium sulfate

Answer: C

Diff: 2

Section: 5.4

30) When a solution of iron(III) nitrate is mixed with a solution of sodium hydroxide, a rust colored precipitate forms. This precipitate is probably

A) iron (III) nitrate.
B) sodium hydroxide.
C) sodium nitrate.
D) iron (III) hydroxide.
E) none of the above

Answer: D

Diff: 3

Section: 5.4

31) Which reaction is an example of an acid-base reaction?

A) H2CO3(aq) H2O(l) + CO2 (g)
B) H2SO4(aq) + Ca(OH)2(aq) CaSO4 (aq) + 2 H2O(l)
C) 6 HCl(aq) + 2 Al(s) 2 AlCl3(aq) + 3 H2 (g)
D) FeCl3(aq) + 3 KOH(aq) Fe(OH)3 (s) + 3 KCl(aq)
E) 2 Hg(l) + O2(g) 2 HgO(s)

Answer: B

Diff: 2

Section: 5.5

32) Which one of the following substances is produced during an acid/base (or neutralization) reaction?

A) H2
B) H2O
C) CO2
D) NaOH
E) NaCl

Answer: B

Diff: 2

Section: 5.5

33) Fe(s) + CuCl2 (aq) Cu(s) + FeCl2 (aq)In the redox reaction shown, ________ is oxidized and becomes ________.

A) Fe; Fe+
B) Fe; Fe2+
C) Cu; Cu2+
D) Cu2+; Cu
E) none of the above

Answer: B

Diff: 2

Section: 5.6

34) All of the statements regarding redox reactions are true except

A) a reducing agent causes another substance to be reduced.
B) halogens usually behave as oxidizing agents because they readily gain electrons.
C) metal ions are produced when pure metals are oxidized.
D) when a substance is oxidized its charge (or oxidation number) decreases.
E) alkali metals often behave as reducing agents because they readily lose electrons.

Answer: D

Diff: 2

Section: 5.6

35) Which reaction is not an example of a redox reaction?

A) 2 Hg (l) + O2 (g) 2 HgO (s)
B) 2 (NH4)3PO4(aq) + 3 Ba(NO3)2 (aq) Ba3(PO4)2 (s) + 6 NH4NO3 (aq)
C) CH4(g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
D) 6 HCl (aq) + 2 Al (s) 2 AlCl3 (aq) + 3 H2 (g)
E) 2 Al2O3(s) 4 Al (s) + 3 O2 (g)

Answer: B

Diff: 2

Section: 5.6

36) All of the reactions shown are oxidation-reduction reactions except

A) N2(g) + O2(g) 2 NO(g).
B) 2 Fe2O3(s) 4 Fe(s) + 3 O2(g).
C) Zn(s) + 2 HCl(aq) ZnCl2 (aq) + H2 (g).
D) 2 NaI(aq) + Cl2(g) 2 NaCl(aq) + I2.
E) K2SO4(aq) + BaCl2(aq) BaSO4 (s) + 2 KCl(aq).

Answer: E

Diff: 3

Section: 5.6

37) The element chlorine is very reactive as a(an) ________ agent because it readily ________ electrons to form the chloride ion.

A) oxidizing; loses
B) oxidizing; gains
C) reducing; loses
D) reducing; gains
E) none of the above

Answer: B

Diff: 3

Section: 5.6

38) When a substance loses electrons it is ________; the substance itself is acting as a(an) ________ agent.

A) oxidized; oxidizing
B) oxidized; reducing
C) reduced; oxidizing
D) reduced; reducing
E) dissolved; neutralizing

Answer: B

Diff: 3

Section: 5.6

39) In the reaction shown, ________ is the oxidizing agent because it ________.

Ni (s) + CuCl2 (aq) Cu (s) + NiCl2 (aq)

A) Ni; causes reduction
B) Ni; gets reduced
C) CuCl2; causes reduction
D) CuCl2; gets reduced
E) NiCl2; gets reduced

Answer: D

Diff: 3

Section: 5.6

40) Reduction is the process of

A) gaining hydrogen.
B) losing oxygen.
C) gaining electrons.
D) forming an anion from a neutral atom.
E) all of the above

Answer: E

Diff: 3

Section: 5.6

41) In the following reaction which species is being oxidized and which is being reduced?

2 Cr (s) + 3 Cl2 (g) 2 CrCl3 (s)

A) oxidized: Cr; reduced: CrCl3
B) oxidized:CrCl3; reduced: Cr
C) oxidized: Cr; reduced: Cl2
D) oxidized: Cl2; reduced: Cr

Answer: C

Diff: 3

Section: 5.5

42) The oxidation number of iron in the compound FeBr3 is ________.

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

Answer: E

Diff: 1

Section: 5.7

43) The oxidation number of sulfur in calcium sulfate, CaSO4, is ________.

A) +6
B) +4
C) +2
D) 0
E) -2

Answer: A

Diff: 1

Section: 5.7

44) The oxidation number of chlorine in the compound FeCl3 is ________.

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

Answer: C

Diff: 1

Section: 5.7

45) As a pure element the oxidation number of zinc is ________, but in compounds such as ZnCO3 its oxidation number is ________.

A) 0; 0
B) 0; +1
C) +1; 0
D) 0; +2
E) none of the above

Answer: D

Diff: 2

Section: 5.7

46) 2 AgNO3 (aq) + K2SO4(aq) 2 KNO3 (aq) + Ag2SO4s)

The net ionic reaction for the balanced equation shown above is

A) Ag++ AgNO3.
B) 2 K++ K2SO4.
C) K++ KNO3.
D) 2 Ag++ Ag2SO4.
E) H++ OH- H2

Answer: D

Diff: 3

Section: 5.8

47) The net ionic equation for the reaction between zinc and hydrochloric acid solution is

A) Zn (s) + 2 H+ (aq) Zn2+ (aq) + H2 (g).
B) Zn (s) + 2 HCl (aq) ZnCl2 (aq) + H2 (g).
C) Zn2+(aq) + H2 (g) ZnS (s) + 2 H+ (aq).
D) ZnCl2(aq) + H2 (g) ZnS (s) + 2 HCl (aq).
E) none of these

Answer: A

Diff: 3

Section: 5.8

48) 2 AgNO3 (aq) + K2SO4 (aq) 2 KNO3 (aq) + Ag2SO4 (s)

The spectator ions in the reaction shown are

A) silver ion and nitrate ion.
B) potassium ion and sulfate ion.
C) potassium ion and nitrate ion.
D) silver ion and sulfate ion.
E) hydrogen ion and hydroxide ion.

Answer: C

Diff: 3

Section: 5.8

49) What are the spectator ions in the reaction between KOH and HNO3?

A) K+and H+
B) H+and OH-
C) K+and NO3-
D) H+and NO3-

Answer: C

Diff: 3

Section: 5.8

50) Which of the following is always a spectator ion in a chemical reaction?

A) Na+
B) Cl-
C) S2-
D) Mg2+
E) All of these ions.

Answer: A

Diff: 3

Section: 5.8

Match the following.

A) redox
B) acid-base
C) precipitation

51) M (s) + 2 LX (aq)

2 L (s) + MX2 (aq)

Diff: 1

Section: 5.3

52) LX (aq) + MY (aq)

LY (s) + MX (aq)

Diff: 1

Section: 5.3

53) HR (aq) + XOH (aq)

XR (aq) + H2O (l)

Diff: 2

Section: 5.3

Answers: 51) A 52) C 53) B

Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry)

Chapter 15 Amines

1) What is the IUPAC name of the compound shown?

A) isopropylamine
B) propylamine
C) 2-propylamine
D) 1-methylethylamine
E) N-methylethylamine

Answer: E

Diff: 1

Section: 15.1

2) Which molecule is N,N-dimethylpropylamine?

A) CH3CH2CH2CH2CH2 H2

Answer: C

Diff: 1

Section: 15.1

3) Which molecule shown is trimethylamine?

A) CH3CH2CH2CH2CH2 H2

Answer: D

Diff: 1

Section: 15.1

4) Which molecule shown is N,N-dimethylethylamine?

A) CH3CH2CH2CH2CH2 H2

Answer: E

Diff: 1

Section: 15.1

5) What is the correct IUPAC name of the compound shown?

A) N-methyl aniline
B) 2-methyl aniline
C) 1-methyl aniline
D) 1-methyl-2-aniline
E) 1-methyl-1-aniline

Answer: B

Diff: 2

Section: 15.1

6) What is the correct IUPAC name for the following compound?

A) ethyl phenyl amine
B) N-ethyl aniline
C) ethyl aniline
D) 2-ethyl aniline

Answer: B

Diff: 2

Section: 15.1

7) When the nitrogen atom in an organic compound has four covalent bonds, it is called a

A) primary amine.
B) secondary amine.
C) tertiary amine.
D) quaternary ammonium ion.
E) tetraammine.

Answer: D

Diff: 1

Section: 15.1

8) All of the following compounds are amines except

A) amphetamine.
B) histamine.
C) aniline.
D) aspirin.
E) caffeine.

Answer: D

Diff: 2

Section: 15.1

9) Which compound is a secondary amine?

A) trimethylamine
B) diethylamine
C) isopropylamine
D) N,N-dimethylethylamine
E) N-ethyl-N-methylpropylamine

Answer: B

Diff: 2

Section: 15.1

10) Which compound is a primary amine?

A) trimethylamine
B) diethylamine
C) isopropylamine
D) N,N-dimethylethylamine
E) N-ethyl-N-methylpropylamine

Answer: C

Diff: 2

Section: 15.1

11) Which of the following molecules is an example of a primary amine?

Answer: A

Diff: 2

Section: 15.1

12) Which of the following molecules is an example of a secondary amine?

Answer: B

Diff: 2

Section: 15.1

13) Which molecule is a tertiary amine?

Answer: A

Diff: 2

Section: 15.1

14) Amines are classified by

A) the number of alkyl groups attached to the nitrogen.
B) the number of hydrogens attached to the nitrogen.
C) the number of carbons attached to the carbon bonded to the nitrogen.
D) the number of carbons present in the molecule.
E) none of the above

Answer: A

Diff: 3

Section: 15.1

15) Amines are most similar in chemical structure and behavior to

A) the hydronium ion.
B) ammonia.
C) sodium hydroxide.
D) a primary alcohol.
E) water.

Answer: B

Diff: 1

Section: 15.2

16) Amines can be considered organic derivatives of the inorganic compound

A) ammonia.
B) carbon dioxide.
C) sodium hydroxide.
D) water.
E) none of these

Answer: A

Diff: 1

Section: 15.2

17) Which organic functional group is important for its basic properties?

A) amine
B) aromatic
C) carbonyl
D) hydroxyl
E) phenol

Answer: A

Diff: 1

Section: 15.2

18) All of the following are properties of amines except

A) they frequently have offensive odors.
B) those that can form hydrogen bonds have higher boiling points than expected for their molecular weight.
C) those with low molecular weights are soluble in water.
D) they react with acids to form amides.
E) they act as bases in many reactions.

Answer: D

Diff: 2

Section: 15.2

19) Which amine has the lowest boiling point?

Answer: C

Diff: 2

Section: 15.2

20) Which class of amines can form intermolecular hydrogen bonds?

A) 1
B) 2
C) 3
D) A and B
E) all of the above

Answer: D

Diff: 3

Section: 15.2

21) When comparing amine compounds of different classes but similar molar masses, which type will most likely be the highest boiling point?

A) primary amines
B) secondary amines
C) tertiary amines
D) quaternary ammonium salts

Answer: A

Diff: 1

Section: 15.1

22) Which amine has the highest boiling point?

Answer: A

Diff: 2

Section: 15.2

23) Arrange the following compounds in order of increasing boiling point. List and describe the criteria that must be considered in answering this question.

Compounds

CH3CH2CH2CH2OH 2. CH3CH2CH2NHCH3

CH3CH2CH2CH2CH3 4. CH3CH2N(CH3)CH3

CH3CH2CH(OH)CH3

Answer: 3 < 4 < 2 < 5 < 1;

Criteria considered include:

molar mass, but in this case all were similar
polarity and possibility for hydrogen bonding: #3 is nonpolar; #4 is polar but cannot form hydrogen bonds; #2 is polar, but its hydrogen bonds will be weaker than those in an alcohol; #5 is a secondary alcohol, so will form fewer hydrogen bonds than its primary isomer.

Diff: 3

Section: 15.2

24) The boiling point of ethylamine is higher than that of propane but lower than that of 1-propanol. This means that

A) a molecule of ethylamine cannot form a hydrogen bond with another molecule of itself
B) hydrogen bonds between two amino groups are weaker than those between two alcohol groups
C) the intermolecular forces between two amine molecules are only dipole-dipole
D) the intermolecular forces between two amine molecules are ionic in nature
E) the intermolecular forces between two amine molecules are only London dispersion forces.

Answer: B

Diff: 3

Section: 15.2

25) Which molecule listed is heterocyclic?

A) aniline
B) phenol
C) pyridine
D) benzoic acid
E) naphthalene

Answer: C

Diff: 1

Section: 15.3

26) Which molecule is a heterocyclic compound?

E) none of these

Answer: E

Diff: 2

Section: 15.3

27) Which of the following is a heterocyclic amine?

Answer: B

Diff: 1

Section: 15.3

28) The reaction that occurs between an amine and an acid is best illustrated by

A) (CH3)2NH + HCl (CH3)2NH + Cl-.
B) (CH3)2NH + HCl (CH3)2NH Cl- + H3O+.
C) (CH3)2NH + HCl (CH3)2NH2 + Cl-.
D) (CH3)2NH + HCl (CH3)2NH2+ + OH-.
E) (CH3)2NH + H2O (CH3)2N + H3O+.

Answer: C

Diff: 2

Section: 15.4

29) Which formula best represents the form an amine takes in acidic solution?

A) RNH2
B) RNH-
C) RNH2-
D) RNH2+
E) RNH3+

Answer: E

Diff: 2

Section: 15.4

30) When an amine behaves as a base it ________ a hydrogen ion to form a(an) ________ ion.

A) loses; hydronium
B) loses; ammonium
C) loses; hydroxide
D) gains; ammonium
E) gains; hydronium

Answer: D

Diff: 3

Section: 15.4

31) The reaction of an amine with water is best represented by

A) R-NH2 + 2 H2O R-N2- + 2 H3O+.
B) R-NH2 + H2O R-NH- + H3O+.
C) R-NH2 + H2O R-NH3+ + OH-.
D) R-NH2 + 2 H2O R-NH4+2 + 2 OH-.
E) R-NH2 + H2O R-N2- + M+ + H3O+.

Answer: C

Diff: 3

Section: 15.4

32) What is the most important chemical property of amines?

A) They are weak bases.
B) They are strong bases.
C) They are weak acids.
D) They are strong acids.
E) They are oxidizing acids.

Answer: A

Diff: 3

Section: 15.4

33) Which type of amine will react with mineral acids to form soluble ammonium salts?

A) 1
B) 2
C) 3
D) A and B
E) A, B and C

Answer: E

Diff: 3

Section: 15.5

34) An amine that is insoluble in water can be made to dissolve by adding it to an aqueous solution of

A) HCl.
B) NaOH.
C) a different amine.
D) an amide.
E) none of the above; it cant be made water soluble.

Answer: A

Diff: 2

Section: 15.5

35) Which of these types of compounds forms salts with acids?

A) ketones
B) amines
C) alcohols
D) carboxylic esters
E) ethers

Answer: B

Diff: 1

Section: 15.5

36) Which compound is an example of an amine salt?

A) histamine
B) methylammonium chloride
C) thioacetamide
D) sulfanilamide
E) pyridoxine

Answer: B

Diff: 2

Section: 15.5

37) Some amine drugs are administered in the form of salts in order to

A) make them form into pills more easily
B) make them taste bitter
C) make them more basic
D) make them more soluble in body fluids

Answer: D

Diff: 1

Section: 15.4

38) If methylamine reacts with hydrochloric acid, the major product will be

A) ammonium chloride.
B) dimethylammonium chloride.
C) methylammonium chloride.
D) trimethylammonium chloride.
E) methylammonium hydroxide.

Answer: C

Diff: 2

Section: 15.5

39) Lemon juice can be used to remove the odor of fish on a persons hands after cleaning fish. The chemical explanation for this is that the

A) pleasant odor of the lemon juice covers the fishy odor.
B) acid in the lemon juice reacts with the odor-causing amines to form an odorless salt.
C) acid in the lemon juice increases the volatility of the odor-causing amines.
D) lemon juice dilutes the odor-causing amines.
E) lemon juice removes the bitter flavor often associated with nitrogen compounds.

Answer: B

Diff: 3

Section: 15.5

40) The following is an example of a

A) tertiary amine.
B) quanternary amine.
C) tertiary ammonium salt.
D) quaternary ammonium salt.
E) secondary ammonium salt.

Answer: D

Diff: 2

Section: 15.5

41) Which compound is an example of an amine salt?

Answer: C

Diff: 3

Section: 15.5

42) The reaction of the pyridinium ion with water is best represented as ________.

A) C5H5NH+ + H2O C5H5N + H3O+
B) C5H5NH+ + H2O C5H5NH22+ + OH-
C) C5H5N + H2O C5H4N + H3O+
D) C5H5N + H2O C5H6NH+
E) none of these

Answer: A

Diff: 3

Section: 15.5

43) All of the following are characteristics of alkaloids except

A) bitter tasting.
B) physiologically active.
C) basic.
D) toxic to humans in high doses.
E) pleasant smelling.

Answer: E

Diff: 1

Section: 15.6

44) An alkaloid used in treating malaria is

A) quinine.
B) histamine.
C) atropine.
D) nicotine.

Answer: A

Diff: 1

Section: 15.5

45) All of the following are nitrogen-containing compounds found in living organisms except

A) nucleotides.
B) proteins.
C) neurotransmitters.
D) carbohydrates.
E) alkaloids.

Answer: D

Diff: 2

Section: 15.6

46) An alkaloid is best described as any

A) basic compound obtained from a plant.
B) amide obtained from a plant.
C) basic compound obtained from either an animal or a plant.
D) diamine obtained from an animal.
E) both A and B.

Answer: A

Diff: 1

Section: 15.6

Fundamentals of General, Organic, and Biological Chemistry, 7e (McMurry)

Chapter 29 Body Fluids

1) Most of the water in the human body is found

A) in blood plasma.
B) inside cells.
C) as interstitial fluids.
D) in miscellaneous fluids, such as cerebrospinal fluid and lymph.
E) none of the above

Answer: B

Diff: 1

Section: 29.1

2) The major cation and anion inside cells are ________ and ________, respectively.

A) potassium; chloride
B) potassium; hydrogen phosphate
C) sodium; bicarbonate
D) sodium; chloride
E) sodium; hydrogen phosphate

Answer: B

Diff: 1

Section: 29.1

3) The major cation and anion in extracellular fluids are ________ and ________, respectively.

A) potassium; chloride
B) potassium; hydrogen phosphate
C) sodium; bicarbonate
D) sodium; chloride
E) sodium; hydrogen phosphate

Answer: D

Diff: 1

Section: 29.1

4) Which ion is not a major constituent of body fluids?

A) Na+
B) Fe2+
C) K+
D) C1-
E) HPO42-

Answer: B

Diff: 1

Section: 29.1

5) The minor, but important, fluid that lubricates joints is

A) plasma.
B) lymph.
C) cerebrospinal fluid.
D) urine.
E) synovial fluid.

Answer: E

Diff: 1

Section: 29.1

6) Each of the following characteristics of molecules allows them to dissolve in water except

A) being a gas.
B) being a charged particle.
C) being a large complex molecule with ionic or polar groups on the surface.
D) being hydrophobic on the surface.
E) being a small polar covalent molecule.

Answer: D

Diff: 2

Section: 29.1

7) The osmolarities of blood plasma, intracellular fluid, and interstitial fluid are ________ because ________.

A) the same; their compositions are identical
B) the same; they contain the same total number but different kinds of dissolved particles
C) different; they contain the same kinds and proportions of dissolved particles but different total numbers of particles
D) different; osmosis cannot occur fast enough to balance the differences
E) different; each fluid contains different numbers of each kind of solute particles

Answer: B

Diff: 2

Section: 29.1

8) Different concentrations of potassium ion between intracellular and interstitial fluid are maintained by

A) osmosis.
B) simple diffusion.
C) facilitated diffusion.
D) active transport.
E) none of the above

Answer: D

Diff: 2

Section: 29.1

9) The body fluids that are found outside of cells are known as ________.

A) extracellular fluids
B) intracellular fluids
C) plasma
D) serum
E) cytosol

Answer: A

Diff: 3

Section: 29.1

10) The process of maintaining proper nutrient balance and temperature is called ________.

A) homeostasis
B) osteoporosis
C) metabolism
D) heterolysis
E) oligomerization

Answer: A

Diff: 3

Section: 29.1

11) Which bodily fluid has the highest concentration of potassium ion?

A) intracellular fluid
B) extracellular fluid
C) blood plasma
D) blood serum
E) none of the above

Answer: A

Diff: 3

Section: 29.1

12) The composition of blood plasma and interstitial fluid are almost identical, except that interstitial fluid contains ________ than blood plasma.

A) more water
B) less water
C) more proteins
D) fewer proteins
E) more phosphate

Answer: D

Diff: 2

Section: 29.1

13) The human body contains approximately 64% __________ fluid.

A) extracellular
B) intracellular
C) blood plasma
D) none of the above

Answer: B

Diff: 2

Section: 29.1

14) Which of the following fluids contains the most proteins?

A) plasma
B) interstitial
C) intracellular
D) extracellular
E) They are equally distributed among all fluids.

Answer: C

Diff: 2

Section: 29.1

15) The balance between water and electrolytes in the body is maintained by the

A) bladder.
B) kidneys.
C) liver.
D) lungs.
E) skin.

Answer: B

Diff: 1

Section: 29.2

16) The hormone that regulates the level of water in the urine (also known as the antidiuretic hormone) is

A) aldosterone.
B) vasopressin.
C) insulin.
D) progesterone.
E) glucogon.

Answer: B

Diff: 2

Section: 29.2

17) How would urinary output be affected if the antidiuretic hormone was overexcreted?

A) increased output
B) decreased output
C) greatly decrease output
D) no affect on output

Answer: C

Diff: 2

Section: 29.2

18) How would urinary output be affected if the antidiuretic hormone was underexcreted?

A) increased output
B) decreased output
C) greatly increase output
D) no affect on output

Answer: C

Diff: 2

Section: 29.2

19) Other than water, the major component of plasma is

A) blood cells.
B) electrolytes.
C) nutrients.
D) proteins.
E) waste.

Answer: D

Diff: 1

Section: 29.3

20) Whole blood is composed of each of the following components except

A) plasma.
B) lymph.
C) erythrocytes.
D) platelets.
E) white blood cells

Answer: B

Diff: 2

Section: 29.3

21) All of the following are functions of blood except

A) defense from foreign organisms.
B) transport of waste products.
C) regulation of body temperature.
D) production of energy for anabolic processes.
E) regulation of acid-base balance in the body.

Answer: D

Diff: 2

Section: 29.3

22) Two components of blood that carry out the transport function are ________ and ________.

A) immunoglobulins; platelets
B) albumins; fibrinogen
C) albumins; red blood cells
D) white blood cells; albumins
E) platelets; red blood cells

Answer: C

Diff: 2

Section: 29.3

23) Two components of blood that carry out the protection function are ________ and ________.

A) immunoglobulins; platelets
B) albumins; fibrinogen
C) albumins; red blood cells
D) white blood cells; albumins
E) platelets; red blood cells

Answer: A

Diff: 2

Section: 29.3

24) All of the following are small molecules commonly found dissolved in blood except

A) oxygen.
B) nitrogen.
C) carbon dioxide.
D) glucose.
E) amino acids.

Answer: B

Diff: 2

Section: 29.3

25) The major function of platelets in the blood is

A) to help stop bleeding.
B) to transport CO2to the lungs.
C) to transport O2to the tissues.
D) maintain body pH.
E) to prevent infection.

Answer: A

Diff: 2

Section: 29.3

26) Distinguish between inflammatory and immune responses to antigens.

Answer: The inflammatory response to an invader is a generalized response that leads to production of chemicals that cause redness, swelling, warmth and pain. The first three effects are the result of increased blood flow to the area. In addition, the increased blood flow brings additional white cells which destroy the invader by hydrolyzing its proteins. The pain in this response is the result of the production of prostaglandins.

Immune responses can be cell-mediated or antibody-mediated. In both cases the response depends on recognition of an invader by its antigens. In a cell-mediated response, a T cell recognizes the invader and causes production of killer T cells, which kill the invader. As a secondary effect, memory T cells are produced so that the invader can be recognized again in the future. In the antibody-mediated response, B cells identify antigens and bond to them, and then fight them with the assistance of helper T cells. B cells are able to recognize antigens in body fluids, and they are responsible for production of antibodies. Antibodies bond with the antigen and block its action.

Diff: 2

Section: 29.4

27) The non-specific localized response to an antigen is the

A) inflammatory response.
B) cell- and antibody-mediated response.
C) cell-mediated response only.
D) antibody-mediated response only.
E) none of the above

Answer: A

Diff: 1

Section: 29.4

28) Chemically, antibodies can be classified as

A) amino acids.
B) anions.
C) cations.
D) immunoglobulins.
E) nonpolar covalent molecules.

Answer: D

Diff: 1

Section: 29.4

29) The body fluid responsible for the proper functioning of the immune system is

A) plasma.
B) lymph.
C) cerebrospinal fluid.
D) urine.
E) synovial fluid.

Answer: A

Diff: 1

Section: 29.4

30) The amino acid that is the precursor to the substance associated with the inflammatory response is

A) antihistamine.
B) histamine.
C) histidine.
D) proline.
E) phenylalanine.

Answer: C

Diff: 2

Section: 29.4

31) An antigen at the site of inflammation will probably be attacked and destroyed by

A) erythrocytes.
B) lymphocytes.
C) phagocytes.
D) helper T cells.
E) memory T cells.

Answer: C

Diff: 2

Section: 29.4

32) The function of memory T cells is to

A) destroy killer T cells after they have performed their function.
B) produce helper T cells when an antigen appears.
C) destroy killer and helper T cells after they have performed their functions.
D) produce killer T cells when a previously encountered antigen appears again.
E) produce phagocytes to assist in the functions of T cells.

Answer: D

Diff: 2

Section: 29.4

33) B cells are associated with the

A) inflammatory response.
B) cell-mediated immune response.
C) antibody-mediated immune response.
D) clotting of blood.
E) production of histamine.

Answer: C

Diff: 2

Section: 29.4

34) Comment on the tertiary structure of the defensive proteins immunoglobulins and fibrin. Explain how the structure of each protein contributes to its function.

Answer: Immunoglobulins, as the name implies, are globular proteins. Since their function is recognition of a particular antigen, it makes sense that they would be globular so that they have a particular site, analogous to the active site on an enzyme, that is chemically similar to the antigen it must recognize.

Fibrin, as its name implies, is a fibrous protein. Since its function is to form blood clots, it makes sense that it would form a network that can block the flow of liquid. One could visualize fibrin as similar to a gauze pad that is placed on a wound to stop the flow of blood.

Diff: 3

Section: 29.4

35) All of the chemicals listed are associated with blood clotting except

A) vitamin K.
B) calcium ion.
C) collagen.
D) fibrinogen.
E) hemoglobin.

Answer: E

Diff: 2

Section: 29.5

36) The first two steps in the process of hemostasis are ________ and ________.

A) release of thrombin; formation of fibrin clot
B) constriction of blood vessels; formation of a plug of platelets
C) release of thrombin; constriction of blood vessels
D) formation of fibrin clot; formation of a plug of platelets
E) release of zymogens; inflammation

Answer: B

Diff: 2

Section: 29.5

37) Blood clotting is a specific example of the bloods general function of

A) defense.
B) transport.
C) regulation.
D) energy production.
E) none of the above

Answer: A

Diff: 2

Section: 29.5

38) Which is the correct order for the steps in the process of blood clotting?

release of thrombin
activation of zymogens

III. formation of fibrin clot

constriction of blood vessels
interaction of blood with collagen or tissue factor
A) I, II, III, IV, V
B) V, IV, III, II, I
C) V, IV, II, III, I
D) IV, V, II, I, III
E) III, I, V, IV, II

Answer: D

Diff: 3

Section: 29.5

39) Fibrinogen can be classified as a(an) ________ because it circulates in the bloodstream in an inactive form until it is converted to its active form when needed.

A) amino acid
B) coenzyme
C) enzyme
D) lipid
E) zymogen

Answer: E

Diff: 3

Section: 29.5

40) The inorganic component of hemoglobin that is critical to its function is ________.

A) Fe2+
B) Fe3+
C) Na+
D) K+
E) H2O

Answer: A

Diff: 1

Section: 29.6

41) Hemoglobin contains how many heme groups for each molecule?

A) 1
B) 2
C) 3
D) 4
E) 5

Answer: D

Diff: 1

Section: 29.6

42) The major function of red blood cells is

A) glycolysis.
B) glycogenesis.
C) transport of waste products to the kidneys.
D) transport of oxygen and carbon dioxide.
E) transport of glucose.

Answer: D

Diff: 2

Section: 29.6

43) What pH value is associated with the onset of respiratory alkalosis?

A) 7.8
B) 7.4
C) 7.2
D) 7.0
E) 6.8

Answer: A

Diff: 3

Section: 29.6

44) The protein in red blood cells that is most important to their major function is

A) fibrin.
B) fibrinogen.
C) hemoglobin.
D) heme.
E) immunoglobulin.

Answer: C

Diff: 2

Section: 29.6

45) Carbon dioxide is transported to the lungs in all of the following forms except ________.

A) H2CO3.
B) HCO3-
C) CO2(aq)
D) bonded to Hb
E) none of the above

Answer: A

Diff: 2

Section: 29.6

46) An increase in blood pH due to increased loss of CO2 through hyperventilation is called

A) respiratory acidosis.
B) respiratory alkalosis.
C) metabolic acidosis.
D) metabolic alkalosis.
E) diabetic ketosis.

Answer: B

Diff: 2

Section: 29.6

47) Hemoglobin is capable of carrying ________ oxygen molecules.

A) 4
B) 1
C) 2
D) 3
E) 5

Answer: A

Diff: 3

Section: 29.6

48) Which of the following buffer systems is associated with the respiratory system?

A) phosphate
B) bicarbonate
C) protein
D) amino acids

Answer: B

Diff: 1

Section: 29.6

49) Carbon dioxide transport is an important aspect of maintaining proper pH in blood because

A) carbon dioxide is basic when dissolved in water.
B) a high pH causes more carbon dioxide to dissolve in blood.
C) the multiple equilibria between CO2and bicarbonate ion involve hydrogen ions.
D) carbon dioxide can affect the acidity of hemoglobin molecules.
E) none of the above

Answer: C

Diff: 3

Section: 29.6

50) Most of the carbon dioxide carried in the blood from the tissues to the lungs is in what form?

A) carbonic acid, H2CO3
B) CO2dissolved in the blood
C) CO2bound to the N-terminal end of hemoglobin chains
D) CO2 bound to the C-terminal end of the hemoglobin chains
E) as the bicarbonate ion dissolved in the blood

Answer: C

Diff: 3

Section: 29.6

51) In which part of the kidney is most of the water reabsorbed from the urine?

A) glomerulus
B) Henles loop
C) kidney tubule
D) Bowmans capsule
E) nephrons

Answer: C

Diff: 2

Section: 29.7

52) All of the following are functions of the kidneys except

A) filtration.
B) reabsorption.
C) detoxification.
D) secretion.
E) control of concentrations of electrolytes.

Answer: C

Diff: 2

Section: 29.7

53) The functional units in the kidney are the numerous

A) hemoglobin molecules.
B) tubules.
C) glomeruli.
D) nephrons.
E) neurons.

Answer: D

Diff: 2

Section: 29.7

54) All of the following can be found in a normal urine sample except

A) potassium ions.
B) sodium ions.
C) urea.
D) red blood cells.
E) creatinine.

Answer: D

Diff: 1

Section: 29.8

55) Which of the following is considered to be a normal constituent of urine?

A) protein
B) ketone bodies
C) amino acids
D) hemoglobin

Answer: C

Diff: 2

Section: 29.9

56) The hormone that helps to regulate the level of sodium ions in the blood is

A) aldosterone.
B) vasopressin.
C) insulin.
D) progesterone.

Answer: A

Diff: 1

Section: 29.9

57) Excess hydrogen ion is eliminated from the body in the urine without lowering the pH excessively by reaction of H+ with ________ or ________.

A) CO2; H2O
B) NH4+; H3PO4
C) NH3; HPO42-
D) urea; water
E) NH3; CO2

Answer: C

Diff: 3

Section: 29.8

Match the following.

A) any substance that is foreign to the body and therefore causes an immune response
B) a protein molecule that identifies foreign substances and mediates certain immune responses
C) an abnormal condition in which the acidity of the blood is higher than normal and the pH is lower
D) fluid inside cells
E) fluid outside of cells, such as blood plasma or interstitial fluid
F) an abnormal condition in which the acidity of the blood is lower than normal and the pH is higher

58) extracellular fluid

Diff: 2

Section: 29.1

59) intracellular fluid

Diff: 2

Section: 29.1

60) antigen

Diff: 2

Section: 29.4

61) antibody

Diff: 2

Section: 29.4