Contributed by:
The highlights are:
1. The Special Nature of Carbon and the Characteristics of Organic Molecules
2. The Structures and Classes of Hydrocarbons
3. Some Important Classes of Organic Reactions
4. Properties and Reactivities of Common Functional Groups
5. Synthetic Macromolecules
6. Biological Macromolecules
1.
Chapter 15
Organic Compounds and the
Atomic Properties of Carbon
2.
Organic Compounds and the Atomic Properties of Carbon
15.1 The Special Nature of Carbon and the Characteristics of
Organic Molecules
15.2 The Structures and Classes of Hydrocarbons
15.3 Some Important Classes of Organic Reactions
15.4 Properties and Reactivities of Common Functional Groups
15.5 The Monomer-Polymer Theme I: Synthetic Macromolecules
15.6 The Monomer-Polymer Theme II: Biological Macromolecules
3.
Bonding Properties of Carbon
• Carbon forms covalent bonds in all its elemental forms
and compounds.
– The ground state electron configuration of C is [He]2s22p2; the
formation of carbon ions is therefore energetically unfavorable.
– C has an electronegativity of 2.5, which is midway between that
of most metals and nonmetals. C prefers to share electrons.
• Carbon exhibits catenation, the ability to bond to itself
and form stable chain, ring, and branched compounds.
– The small size of the C atom allows it to form short, strong
bonds.
– The tetrahedral shape of the C atom allows catenation.
4.
Figure 15.1 The position of carbon in the periodic table.
5.
Comparison of Carbon and Silicon
• As atomic size increases down the group, bonds
between identical atoms become longer and weaker.
– A C–C bond is much stronger than a Si–Si bond.
• The bond energies of a C–C bond, a C–O bond, and a
C–Cl bond are very similar.
– C compounds can undergo a variety of reactions and remain
stable, while Si compounds cannot.
• Si has low energy d orbitals available for reaction,
allowing Si compounds to be more reactive than C
compounds.
6.
Diversity and Reactivity of Organic Molecules
• Many organic compounds contain heteroatoms, atoms
other than C and H.
– The most common of these are O, N, and the halogens.
• Most reactions involve the interaction of electron rich
area in one molecule with an electron poor site in
another.
– C–C bonds and C–H bonds tend to be unreactive.
– Bonds between C and a heteroatom are usually polar, creating
an imbalance in electron density and providing a site for
reactions to occur.
7.
Figure 15.2 Heteroatoms and different bonding arrangements
lead to great chemical diversity.
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8.
Carbon Skeletons
Each C atom can form a maximum of 4 bonds.
Groups joined by a single bond can rotate, so there are
often several different arrangements of a given carbon
skeleton that are equivalent:
9.
Figure 15.3 Some five-carbon skeletons.
10.
Drawing Carbon Skeletons
Each C atom can form a maximum of four bonds.
These may be four single bonds, OR one double and two single bonds,
OR one triple and one single bond.
The arrangement of C atoms determines the skeleton, so a
straight chain and a bent chain represent the same
skeleton.
Groups joined by a single bond can rotate freely, so a
branch pointing down is the same as one point up.
11.
Figure 15.4 Adding the H-atom skin to the C-atom skeleton.
H H
C C H C C C
H H
A C atom single-bonded to one A C atom single-bonded to two
other atom gets three H atoms. other atoms gets two H atoms.
H
C
C C C
C C C
C
C
A C atom single-bonded to three
other atoms gets one H atom. A C atom single-bonded to four other atoms
is already fully bonded (no H atoms).
12.
Figure 15.4 continued
H
H
C C H
C C C
A double-bonded C atom is
treated as if it were bonded to
two other atoms. C C H
A double- and single-bonded C
atom or a triple-bonded C atom is
treated as if it were bonded to three
other atoms.
13.
Sample Problem 15.1 Drawing Hydrocarbons
PROBLEM: Draw structures that have different atom arrangements
for hydrocarbons with
(a) Six C atoms, no multiple bonds, and no rings
(b) Four C atoms, one double bond, and no rings
(c) Four C atoms, no multiple bonds, and one ring
PLAN: In each case, we draw the longest carbon chain first and
then work down to smaller chains with branches at
different points along them. Then we add H atoms to give
each C a total of four bonds.
14.
Sample Problem 15.1
(a) Six carbons, no rings
H H H H H H H H H H H
H C C C C C C H H C C C C C H 5-C chain
H H H H H H H H H H
6-C chain H C H
H
H H H
H C H H C H H C H
H H H H H H H H H H
H C C C C C H H C C C C H H C C C C H
H H H H H H H H H H H
5-C chain H C H H C H
H H
4-C chains
15.
Sample Problem 15.1
(b) Four C atoms, one double bond, and no rings
H H H H H H H H
H C C C C H H C C C C H
H H H H
4-C chains
H H
3-C chain H C C C H
H
H C H
H
16.
Sample Problem 15.1
(c) Compounds with four C atoms and one ring
H H H H
C H
H C C H
H C C C H
H C C H
H H H
H H
17.
Alkanes
Hydrocarbons contain only C and H.
Alkanes are hydrocarbons that contain only single bonds
and are referred to as saturated hydrocarbons.
The general formula for an alkane is CnH2n+2, where n is
any positive integer.
Alkanes comprise a homologous series, a group of
compounds in which each member differs from the next by
a –CH2– group.
18.
Naming Organic Compounds
The name of any organic compound is comprised of three
portions:
PREFIX + ROOT + SUFFIX
The root name of the compound is determined from the
number of C atoms in the longest continuous chain.
The suffix indicates the type of organic compound, and is
placed after the root.
The suffix for an alkane is –ane.
The prefix identifies any groups attached to the main
chain.
19.
Table 15.1 Numerical Roots for Carbon Chains and Branches
Roots Number of C
Atoms
meth- 1
eth- 2
prop- 3
but- 4
pent- 5
hex- 6
hept- 7
oct- 8
non- 9
dec- 10
20.
Table 15.2 Rules for Naming an Organic Compound
21.
Figure 15.5 Ways of depicting the alkane 3-ethyl-
H
2-methylhexane.
H C H CH3
H H H H H
CH3 CH CH CH2 CH2 CH3
H C C C C C C H
CH2
H H H H H
CH3
H C H
Condensed formula
H C H
H
Expanded formula
Carbon-skeleton formula Ball-and-stick model Space-filling model
22.
Figure 15.6 Depicting cycloalkanes.
H H
H H
H C C H
C H
H
H C C H
C C
H H H H
Cyclobutane
23.
Figure 15.6 Depicting cycloalkanes.
H H H H
H H C H
H C
C C C C
H H
H
C C H C C H
H C
H H H
H H
H H
Cyclopentane Cyclohexane
24.
Constitutional Isomers
Constitutional or structural isomers have the same
molecular formula but a different arrangement of the
bonded atoms.
A straight-chain alkane may have many branched
structural isomers.
Structural isomers are different compounds and have
different properties.
If the isomers contain the same functional groups, their properties
will still be similar.
25.
Table 15.3 The Constitutional Isomers of C4H10 and C5H12
26.
Figure 15.7 Formulas, molar masses (in g/mol), structures, and
boiling points (at 1 atm pressure) of the first 10
unbranched alkanes.
Alkanes are nonpolar and their physical properties are
determined by the dispersion forces between their molecules.
27.
Chiral Molecules
Stereoisomers are molecules with the same arrangement
of atoms but different orientations of groups in space.
Optical isomers are mirror images of each other that
cannot be superimposed.
A molecule must be asymmetric in order to exist as a pair
of optical isomers. An asymmetric molecule is termed
chiral.
Typically, a carbon atom is a chiral center if it is bonded to four different
groups.
28.
Figure 15.8 An analogy for optical isomers.
If two compounds are mirror images of each other that cannot
be superimposed, they are called optical isomers.
29.
Figure 15.9 Two chiral molecules.
optical isomers of 3- optical isomers of alanine
methylhexane
30.
Optical Activity
A chiral compound is optically active; i.e., it rotates the
plane of polarized light.
A compound that rotates the plane of light clockwise is
called dextrorotatory, while a compound that rotates the
plane of light counterclockwise is called levorotatory.
Optical isomers have identical physical properties, except
that they rotate the plane of polarized light in opposite
directions.
In their chemical properties, optical isomers differ only in
a chiral (asymmetric) environment.
31.
Figure 15.10 The rotation of plane-polarized light by an optically
active substance.
32.
Figure 15.11 The binding site of an enzyme.
An enzyme provides a chiral environment and therefore distinguishes
one optical isomer from another. The shape of one optical isomer fits the
binding site, but the mirror image shape of the other isomer does not.
33.
Naproxen
Many drugs are chiral molecules. One optical isomer has a
certain biological activity while the other has a different type
of activity or none at all.
34.
Alkenes
A hydrocarbon that contains at least one C=C bond is
called an alkene.
Alkenes are unsaturated and have the general formula
CnH2n.
To name an alkene, the root name is determined by the
number of C atoms in the longest chain that also
contains the double bond.
The C chain is numbered from the end closest to the double bond.
The suffix for alkenes is –ene.
35.
Geometric Isomers
The double bond of an alkene restricts rotation, so that
the relative positions of the atoms attached to the double
bond are fixed.
Alkenes may exist as geometric or cis-trans isomers,
which differ in the orientation of the groups attached to
the double bond.
Geometric isomers have different physical properties.
36.
Table 15.4 The Geometric Isomers of 2-Butene
37.
Figure 15.12 The initial chemical event in vision and the change in
the shape of retinal.
38.
Alkynes
An alkyne is a hydrocarbon that contains at least one
CΞC triple bond.
Alkynes have the general formula CnH2n-2 and they are
also considred unsaturated carbons.
Alkynes are named in the same way as alkenes, using
the suffix –yne.
39.
Sample Problem 15.2 Naming Alkanes, Alkenes, and Alkynes
PROBLEM: Give the systematic name for each of the following,
indicate the chiral center in part (d), and draw two
geometric isomers for part (e).
(a) CH3 (b) CH3 (c)
CH3 C CH2 CH3 CH3 CH2 CH CH CH3
CH3 CH2
(d) CH3
CH3 (e) CH3
CH3 CH2 CH CH CH2 CH3 CH2 CH C CH CH3
CH3
PLAN: For (a) to (c), we find the longest continuous chain (root) and
add the suffix –ane because there are only single bonds. Then
we name the branches, numbering the C chain from the end
closest to the first branch. For (d) and (e) the longest chain
must include the double bond.
40.
Sample Problem 15.2
SOLUTION:
(a) methyl
CH3 methyl (b) CH3
methyl
CH3 C CH2 CH3 butane CH3 CH2 CH CH CH3
1 2 3 4 6 5 4 3
CH3 methyl 2 CH2
1 CH3
2,3-dimethylbutane
hexane
3,4-dimethylhexane
methyl
(c) 3
4 2
5 1
ethyl
1-ethyl-2-methylcyclopentane
41.
Sample Problem 15.2
(d) methyl
CH3
CH3 CH2 CH CH CH2 1-pentene 3-methyl-1-pentene
5 4 3 2 1
chiral center
methyl methyl
(e) H CH3 CH3 CH2 CH3
C C 6 5 C C
CH3 CH2 4 3 CH CH3 H CH CH3 3-hexene
2 4 3
6 5 1 2
CH3 1
CH3
methyl methyl
cis-2,3-dimethyl-3-hexene trans-2,3-dimethyl-3-hexene
42.
Figure 15.13 Representations of benzene.
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or
Resonance forms
Resonance hybrid shows the
having alternating single
delocalized electrons as either
and double bonds.
an unbroken or a dashed circle.
Benzene is an aromatic hydrocarbon.
43.
methylbenzene 1,2-dimethylbenzene 1,3-dimethylbenzene
(toluene) (o-xylene) (m-xylene)
bp = 110.6°C bp = 144.4°C bp = 139.1°C
O2N NO2
NO2
1,4-dimethylbenzene 2,4,6-trinitromethylbenzene
(p-xylene) (trinitrotoluene, TNT)
bp = 138.3°C
44.
Tools of the Laboratory Nuclear Magnetic Resonance (NMR)
Spectroscopy
Figure B15.1 The basis of proton spin resonance.
45.
Tools of the Laboratory Nuclear Magnetic Resonance (NMR)
Spectroscopy
Figure B15.2 The 1H-NMR spectrum of acetone.
46.
Tools of the Laboratory Nuclear Magnetic Resonance (NMR)
Spectroscopy
Figure B15.3 The 1H-NMR spectrum of dimethoxymethane.
47.
Tools of the Laboratory Nuclear Magnetic Resonance (NMR)
Spectroscopy
Figure B15.4 An MRI scan showing a brain tumor.
48.
Types of Organic Reactions
An addition reaction occurs when an unsaturated reactant
becomes a saturated product:
X Y
R CH CH R + X Y R CH CH R
The C=C, CΞC, and C=O bonds commonly undergo
addition reactions.
In each case, it is the π bond that breaks, leaving the σ bond intact.
49.
CH2 CH2 + H Cl H CH2 CH2 Cl
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Reactants (bonds broken) Products (bonds formed)
1 C=C = 614 kJ 1 C–C = -347 kJ
4 C–H = 1652 kJ 5 C–H = -2065 kJ
1 H–Cl = 427 kJ 1 C–Cl = -339 kJ
Total = 2693 kJ Total = -2751kJ
H°rxn = H°bonds broken + H°bonds formed = 2693 kJ + (-2751 kJ) = -58 kJ
50.
Figure 15.14 A color test for C=C bonds.
Br2 (in pipet) reacts with a compound This compound has no C=C
that has a C=C bond, and the orange- bond, so the Br2 does not react.
brown color of Br2 disappears.
Br
C C + Br2 C C
Br
51.
Types of Organic Reactions
An elimination reaction occurs when a saturated reactant
becomes an unsaturated product.
This reaction is the reverse of addition.
X Y
R CH CH R R CH CH R + X Y
The groups typically eliminated are H and a halogen atom
or H and an –OH group.
52.
The driving force for an elimination reaction is the
formation of a small, stable molecule such as HCl (g) or
H2O.
OH H
H2SO4
R CH CH R R CH CH R + H OH
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53.
Types of Organic Reactions
A substitution reaction occurs when an atom or group
from an added reagent substitutes for one attached to a
carbon in the organic reagent.
R C X + Y R C Y + X
The C atom at which substitution may be saturated or
unsaturated, and X and Y can be many different atoms.
54.
The main flavor ingredient in banana oil is formed through a
substitution reaction:
O CH3 O CH3
CH3 C Cl + HO CH2 CH2 CH CH3 CH3 C O CH2 CH2 CH CH3
+ H Cl
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55.
Sample Problem 15.3 Recognizing the Type of Organic
Reaction
PROBLEM: State whether each reaction is an addition, elimination,
or substitution:
(a) CH3 CH2 CH2 Br CH3 CH CH2 + HBr
(b) + H2
O O
(c) CH3 C Br + CH3CH2OH CH3 C OCH2CH3 + HBr
PLAN: We determine the type of reaction by looking for any
change in the number of atoms bonded to C.
• An addition reaction results in more atoms bonded to C.
• An elimination reaction results in fewer atoms bonded to C.
•If there are the same number of atoms bonded to C, the
reaction is a substitution.
56.
Sample Problem 15.3
SOLUTION:
(a) CH3 CH2 CH2 Br CH3 CH CH2 + HBr
This is an elimination reaction; two bonds in the reactant, C–H and
C –Br, are absent in the product.
(b) + H2
This is an addition reaction; two more C–H bonds have formed in the
product.
O O
(c) CH3 C Br + CH3CH2OH CH3 C OCH2CH3 + HBr
This is a substitution reaction; the reactant C–Br bond has been
replaced by a C–O bond in the product.
57.
Functional Groups
Organic compounds are classified according to their
functional groups, a group of atoms bonded in a
particular way.
The functional groups in a compound determine both its
physical properties and its chemical reactivity.
Functional groups affect the polarity of a compound, and therefore
determine the intermolecular forces it exhibits.
Functional groups define the regions of high and low electron density in
a compound, thus determining its reactivity.
58.
Table 15.5 Important Functional Groups in Organic Compounds
59.
Table 15.5 Important Functional Groups in Organic Compounds
60.
Alcohols
The alcohol functional group consists of a carbon bonded
to an –OH group.
C O H
Alcohols are named by replacing the –e at the end of the
parent hydrocarbon name with the suffix –ol.
Alcohols have high melting and boiling points since they
can form hydrogen bonds between their molecules.
61.
Reactions of Alcohols
Alcohols undergo elimination and substitution reactions.
OH
H+
+ H2O dehydration (elimination)
cyclohexanol cyclohexene
OH O
K2Cr2O7
CH3 CH2 CH CH3 CH3 CH2 C CH3
H2SO4
oxidation OH O
(elimination)
2-butanol 2-butanone
62.
Figure 15.15 Some molecules with the alcohol functional group.
63.
Haloalkanes
Haloalkanes or alkyl halides contain a halogen atom
bonded to carbon.
C X
Haloalkanes are named by identifying the halogen with a
prefix on the hydrocarbon name. The C bearing the
halogen must be numbered.
64.
Reactions of Haloalkanes
Haloalkanes undergo substitution and elimination reactions.
CH3 CH2 CH2 CH2 Br + OH- CH3 CH2 CH2 CH2 OH + Br-
1-bromobutane 1-butanol
CH3 CH3
- +
CH3 C CH3 + CH3 CH2 O K CH3 C CH2 + KCl + CH3 CH2 OH
Cl potassium ethoxide 2-methylpropene ethanol
65.
Figure 15.16 A tetrachlorobiphenyl, one of 209 polychlorinated
biphenyls (PCBs).
66.
Amines
The amine functional group contains a N atom.
C N
The systematic name for an amine is formed by dropping
the final –e of the alkane and adding the suffix –amine.
Common names that use the name of the alkyl group
followed by the suffix –amine are also widely used.
CH3CH2NH2 CH3CH2 NH CH2CH3
ethanamine OR diethylamine
ethylamine
67.
Figure 15.17 General structures of amines.
Amines are classified according to the number of R groups directly
attached to the N atom.
68.
Figure 15.18 Some biomolecules with the amine functional group.
Lysine (1° amine) Adenine (1° amine)
amino acid found component of
in proteins nucleic acids
(adrenaline; 2° amine) Cocaine (3° amine)
neurotransmitter in brain stimulant;
brain; hormone released widely abused drug
during stress
69.
Properties and Reactions of Amines
Primary and secondary amines can form H bonds;
therefore they have higher melting and boiling points than
hydrocarbons or alkyl halides of similar mass.
Tertiary amines cannot form H bonds between their
molecules because they lack a polar N–H bond.
Amines of low molar mass are fishy smelling, water
soluble, and weakly basic.
Amines undergo a variety of reactions, including
substitution reactions.
70.
Sample Problem 15.4 Predicting the Reactions of Alcohols,
Alkyl Halides, and Amines
PROBLEM: Determine the reaction type and predict the product(s)
for each reaction:
(a) CH3 CH2 CH2 I + NaOH
(b) CH3 CH2 CH2 Br + 2 CH3 CH2 CH2 NH2
Cr2O72-
(c) CH3 CH CH3
H2SO4
OH
PLAN: We first determine the functional group(s) of the reactant(s)
and then examine any inorganic reagent(s) to decide on the
reaction type. Keep in mind that, in general, these functional
groups undergo substitution or elimination.
71.
Sample Problem 15.4
SOLUTION:
(a) In this reaction the OH of the NaOH reaction substitutes for the I
in the organic reagent:
CH3 CH2 CH2 OH + NaI
(b) This is a substitution reaction:
CH3 CH2 CH2 NH + CH3 CH2 CH2 NH2Br
CH2CH3
(c) This is an elimination reaction since acidic Cr2O72- is a strong
oxidizing agent:
CH3 C CH3
O
72.
Alkenes
Alkenes contain the C=C double bond:
C C
Alkenes typically undergo addition reactions.
The electron-rich double bond is readily attracted to the partially
positive H atoms of H3O+ ions and hydrohalic acids.
CH3 CH3
CH3 C CH2 + H3O+ CH3 C CH3 + H+
OH
OH
2-methylpropene 2-methyl-2-propanol
73.
Aromatic Hydrocarbons
Benzene is an aromatic hydrocarbon and is a resonance
hybrid. Its bond electrons are delocalized.
Aromatic compounds are unusually stable and although
they contain double bonds they undergo substitution rather
than addition reactions.
Br
FeBr3
+ Br2 + HBr
benzene bromobenzene
74.
Figure 15.19 The stability of benzene.
Benzene releases less energy
during hydrogenation than expected,
because it is already much more
stable than a similar imaginary
alkene.
75.
Aldehydes and Ketones
Aldehydes and ketones both contain the carbonyl
group, C=O.
O O
R and R′ indicate
H C R R C R' hydrocarbon
aldehyde ketone groups.
Aldehydes are named by replacing the final –e of the
alkane name with the suffix –al.
Ketones have the suffix –one and the position of the
carbonyl must always be indicated.
76.
Figure 15.20 Some common aldehydes and ketones.
Methanal (formaldehyde) Used
to make resins in plywood, Benzaldehyde
dishware, countertops; Artificial almond
biological preservative flavoring
Ethanal (acetaldehyde) 2-Propanone (acetone) 2-Butanone
Narcotic product of ethanol Solvent for fat, rubber, plastic, (methyl ethyl ketone)
metabolism; used to make varnish, lacquer; chemical Important solvent
perfumes, flavors, plastics, feedstock
other chemicals
77.
Figure 15.21 The polar carbonyl group.
The C=O bond is electron rich and is also highly polar. It
readily undergoes addition reactions, and the electron-poor C
atom attracts electron-rich groups.
78.
Reactions of Aldehydes and Ketones
Reduction to alcohols is an example of an addition reaction:
reduction
O OH
cyclobutanone cyclobutanol
Organometallic compounds, which have a metal atom
covalently bonded to C, add to the electron-poor carbonyl C:
-
O OH
- +
R C H + R' Li R CH R' + LiOH
+
79.
Sample Problem 15.5 Predicting the Steps in a Reaction
Sequence
PROBLEM: Fill in the blanks in the following reaction sequence:
Br
- Cr2O72- CH3-Li
OH H2O
CH3 CH2 CH CH3
H2SO4
PLAN: For each step we examine the functional group of the
reactant and the reagent above the yield arrow to decide on
the most likely product.
SOLUTION: The first step involves an alkyl halide reacting with OH-,
so this is probably a substitution reaction, which yields
an alcohol. In the next step the alcohol is oxidized to a
ketone and finally the organometallic reagent adds to the
ketone to give an alcohol with one more C in its skeleton:
80.
Sample Problem 15.5
Br OH Cr2O72-
O
-
OH
CH3 CH2 CH CH3 CH3 CH2 CH CH3 CH3 CH2 C CH3
H2SO4
substitution oxidation
CH3-Li
(elimination)
addition
H2O
OH
CH3 CH2 C CH3
CH3
81.
Carboxylic Acids
Carboxylic acids contain the functional group –COOH, or
O
C OH
Carboxylic acids are named by replacing the –e of the
alkane with the suffix –oic acid.
Carboxylic acids are weak acids in water, and react with
strong bases:
O O
CH3 C OH (l) + NaOH (aq) CH3 C O- (aq) + Na+ (aq) + H2O (l)
methanoic acid methanoate anion
82.
Figure 15.22 Some molecules with the carboxylic acid functional
group.
Methanoic acid (formic acid) Butanoic acid (butyric acid)
An irritating component of ant and Odor of rancid butter; suspected
bee stings component of monkey sex
attractant
Benzoic acid
Calorimetric standard; used in
preserving food, dyeing fabric, Octadecanoic acid (stearic acid)
curing tobacco Found in animal fats; used in making
candles and soaps
83.
Esters
The ester group is formed by the reaction of an alcohol and a
carboxylic acid.
O O
CH3 C OH + H O CH3 CH3 C O CH3 + HOH
ethanoic acid methanol methyl ethanoate
Esterification is a dehydration-condensation reaction.
Ester groups occur commonly in lipids, which are formed by
the esterification of fatty acids.
84.
Figure 15.23 Some lipid molecules with the ester functional
group.
Cetyl palmitate
The most common
lipid in whale
blubber
Tristearin Typical dietary fat
used as an energy store in
animals
Lecithin Phospholipid found in all cell
membranes
85.
Saponification
Ester hydrolysis can be carried out using either aqueous
acid or aqueous base. When base is used the process is
called saponification.
This is the process used to make soaps from lipids.
O O
R C O CH2 R C O- Na+ HO CH2
O 3NaOH O
R' C O CH R' C O- Na+ HO CH
O O
R" C O CH2 R" C O- Na+ HO CH2
a triglyceride 3 soaps glycerol
(salts of fatty acids)
86.
Amides
An amide contains the functional group:
O
C N
Amides, like esters, can be hydrolyzed to give a
carboxylic acid and an amine.
The peptide bond, which links amino acids in a protein,
is an amide group.
87.
Figure 15.24 Some molecules with the amide functional group.
Acetaminophen
Active ingredient in nonaspirin
pain relievers; used to make dyes
and photographic chemicals
N,N-Dimethylmethanamide
Lysergic acid diethylamide (LSD-25)
(dimethylformamide)
A potent hallucinogen
Major organic solvent; used in
production of synthetic fibers
88.
Sample Problem 15.6 Predicting the Reactions of the Carboxylic
Acid Family
PROBLEM: Predict the product(s) of the following reactions:
O OH
H+
(a) CH3 CH2 CH2 C OH + CH3 CH CH3
CH3 O
NaOH
(b) CH3 CH CH2 CH2 C NH CH2CH3
H2O
PLAN: We identify the functional groups in the reactant(s) and see
how they change. In (a), a carboxylic acid reacts with an
alcohol, so the reaction must be a substitution to form an
ester. In (b), an amide reacts with aqueous base, so
hydrolysis occurs.
89.
Sample Problem 15.6
SOLUTION:
O OH O CH3
H+
(a) CH3 CH2 CH2 C OH + CH3 CH CH3 CH3 CH2 CH2 C O CH CH3
+ H2O
CH3 O CH3 O
NaOH
(b) CH3 CH CH2 CH2 C NH CH2CH3 CH3 CH CH2 CH2 C O- Na+
H2O
+
NH2 CH2CH3
90.
Figure 15.25 The formation of carboxylic, phosphoric, and sulfuric
acid anhydrides.
P and S form acids, anhydrides and esters that
are analogous to organic compounds.
91.
Figure 15.26 A phosphate ester and a sulfonamide.
Sulfanilamide
Glucose-6-phosphate
92.
Functional Groups with Triple Bonds
Alkynes contain the electron rich –CΞC– group, which
readily undergoes addition reactions:
H2 H2
CH3 C CH CH3 CH CH2 CH3 CH2 CH3
propyne propene propane
Nitriles contain the group –CΞN and are made by a
substution reaction of an alkyl halide with CN- (cyanide):
CH3 CH2 Cl + NaCN CH3 CH2 C N + NaCl
93.
Sample Problem 15.7 Recognizing Functional Groups
PROBLEM: Circle and name the functional groups in the following molecules:
O
(a) (b) OH (c) O
C OH O
CH CH2 NH CH3
O C CH3
Cl
PLAN: Use Table 15.5 to identify the various functional groups.
SOLUTION:
carboxylic acid alcohol
O
(a) ester (b) OH
(c) O
ketone
C OH O
CH CH2 NH CH3
O C CH3
2° amine Cl
aromatic ring alkene
haloalkane
aromatic ring
94.
Polymers
Addition polymers, also called chain-growth polymers
form when monomers undergo an addition reaction with
each other.
The monomers of most addition polymers contain an alkene group.
Condensation polymers are formed when monomers link
by a dehydration-condensation type reaction.
The monomers of condensation polymers have two functional groups,
and each monomer can link to two others.
95.
Figure 15.27 Steps in the free-radical polymerization of ethylene.
96.
Table 15.6 Some Major Addition Polymers
97.
Table 15.6 Some Major Addition Polymers
98.
Figure 15.28 The formation of nylon-66.
O O
HO C (CH2)4 C OH + nH2N (CH2)6 NH2
O O
HO C (CH2)4 C NH (CH2)6 NH H
n
Nylon-66 is a condensation polymer,
made by reacting a diacid with a
diamine. The polyamide forms
between the two liquid phases.
99.
Figure 15.29 The structure of glucose in aqueous solution and the
formation of a disaccharide.
100.
Figure 15.30 The common amino acids.
101.
Figure 15.30 The common amino acids.
102.
Figure 15.31 The structural hierarchy of proteins.
103.
Figure 15.32 The shapes of fibrous proteins.
collagen silk
fibroin
104.
Figure 15.33 Nucleic acid precursors and their linkage.
105.
Figure 15.34 The double helix of DNA and a section
showing base pairs.
106.
Figure 15.35 Key stages in protein synthesis.
107.
Figure 15.36 Key stages in DNA replication.
108.
Chemical Connections
Figure B15.5 Nucleoside triphosphate monomers.
109.
Chemical Connections
Figure B15.6 Steps in the Sanger method of DNA sequencing.
A. B.
C. D.
110.
Chemical Connections
Figure B15.7 STR analysis of DNA in the blood of seven suspects
and that in blood found at a crime scene.
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