chapter 3 mcmurry
TRANSCRIPT
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Chapter 3: Alkanes and their Stereochemistry
Coverage:
1. Survey of Functional Groups
2. Alkane Isomers3. Alkyl Groups
4. Nomenclature of Alkanes
5. Properties of Alkanes
6. Conformations of Ethane, Propane, Butane
7. Special Topic: Refining of Petroleum
Goals:
1. Be able to recognize and identify the functional group(s) in a molecule.
2. Be able to predict the hybridization of an atom in a functional group.
3. Know the definition of constitutional and stereoisomers and be able to apply definitions
to alkanes.
4. Know the structures of alkyl groups up to 4 carbons.5. Know the IUPAC system of nomenclature for naming alkanes.
6. Know trends in boiling points and melting points of alkanes, both branched and straight
chain.
7. Know the meaning of gauche, anti, eclipsed, staggered in conformations.
8. Be able to draw Newman projections of ethane, propane, butane and others.
9. Know the sources of hydrocarbons, particularly petroleum refining.
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Classification of Organic Molecules
Functional Groups
1. Hydrocarbons - molecules that possess only hydrogen and carbon
a1. Alkanesnoncyclic hydrocarbons with only C-C single bonds.
Formula CnH2n+2 where n is an integer.
a2. Cycloalkanescyclic hydrocarbons with only C-C single bonds.
Formula CnH2n where n is an integer.
Example: Butane CH3CH2CH2CH3 C4H10
Example: Cyclobutane C4H8
b1. Alkenesnoncyclic hydrocarbons with C=C double bonds.
Formula CnH2n where n is an integer.
Example: 2-Butene CH3CH=CHCH3 C4H8
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c. Alkynesnoncyclic hydrocarbons with C=C triple bonds.
Formula CnH2n-2 where n is an integer.
Example: Butyne CH3C=CCH3 C4H6
b2. Cycloalkenescyclic hydrocarbons with C=C double bonds.
Formula CnH2n-2 where n is an integer.
Example: Cyclobutene C4H6
d. Aromatic Hydrocarbonsbenzene and its derivatives
C
CC
C
CC H
H
H
H
H
H
or C6H6
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2. Compounds containing Oxygen
a. Alcohols R-OH
Functional Group OH hydroxyl group
CH3OH methyl alcohol HOCH2CH2OH ethylene glycol (antifreeze)
b. Ethers R-O-R
CH3CH2-O-CH2CH3 Diethylether
c. Aldehydes and Ketones
R-C-H
O
R-C-R'
O
Functional Group C=O carbonyl group
O
O
O
H
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d. Carboxylic Acids
Functional Group -CO2H -COOH -COH Carboxyl Group
R-C-OH
O
O
CH3-C-OH
O
OH2
H3O+ CH
3CO-
O
+ +
Acetic Acid
e. Derivatives of Carboxylic Acids
R-C-OR'
O
R-C-Cl
O
R-C-NH2
O
Ester Acid Chloride Amide
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3. Nitrogen-Containing Molecules
a. Amines R-NH2
Functional Group -NH2 amino group
CH3NH
2
NH
N
Amines are Lewis and Bronsted basesbecause of the nonbonded pair of electrons
NH2
ClH NH3+ Cl+..
b. Amides (see above)
c. NitrilesR C N
Functional Group Cyano GroupC N
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Use of Wedges and Dashed Lines
CH
H
H
HSolid Wedge indicates coming toward you
Dashed Line indicates going awayNarrow Line indicates in the plane of paper
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Single versus Double Bonds
C C
H
H
HH
H
H
Ethane
The carbon-carbon single bond in ethane freely rotates at room temperature.
CC
HH
HH
Ethylene
The carbon-carbon double bond in ethylenedoes not freely rotate at room temperature.
Why not?
CC
HH
HH
C C
H H
H
H H
H
Answer: The Pi bond would have to be broken. It will not break at room temperature
Pi bond broken
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Isomersdifferent compounds with the same formula
a. Constitutional (Structural) Isomersisomers that differ in their bonding sequence
CH3CHCH
2CH
3\
CH3
CH3CH
2CH
2CH
2CH
3vs
C5H12 C5H12
C=C
Cl
H H
Br
C=CH
H Cl
Br
C2H2BrCl C2H2BrCl
b. Stereoisomersisomers that differ in their spatial orientation
C=CCl
H H
Br
C=CCl
H Br
H
C2H2BrCl C2H2BrCl
Cis isomer Trans isomer
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Alkyl Groups
Ris the general symbol for an alkyl group.
For example R-OH represents an alcohol where R is an alkyl group.R-Cl is an alkyl chloride.
Alkyl Groupsknow the following
-CH3
methyl
-CH2CH
3ethyl
-CH2CH
2CH
3propyl
-CH2CH
2CH
2CH
3butyl
-CH2CHCH3
CH3
-CHCH2CH
3
CH3
-C
CH3
CH3
CH3
isobutyl
sec-butyl
tert-butyl
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Carbon Substitution
a. Primary carbon (1o
) - carbon attached to one other carbon.
R-CH3 1o
b. Secondary carbon (2o) - carbon attached to two other carbons.
R-CH2-R
2o
c. Tertiary carbon (3o)carbon attached to three other carbons
3o
R-CH-R
R
d. Quaternary (4o)carbon attached to four other carbons.
C
R
R
R
R4o
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Alkane Nomenclature
1. Find the parent hydrocarbon
a. Find the longest continuous chain of carbon atoms and name it accordingly.
Number Carbons Name
1 methane
2 ethane
3 propane
4 butane
5 pentane
6 hexane
7 heptane
8 octane
9 nonane
10 decane
Named as a hexane
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b. If two different chains of equal length are present, choose the one with the
larger number of branch points.
Named as hexane with 2 substituents not hexane with 1 substituent
2. Number the atoms in the main chain
a. Begin at the end nearer the first branch point.
1
2
3
4
5
6
b. If there are branch points at equal distances away, begin at the end nearer the second
branch point.
7
6
5
4
3
2
1
8
9
Named as a nonane with branch points
at carbons 3, 4, 7.
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3. Identify and number the substituents.
7
6
5
4
3
2
1
8
9
3-ethyl
4-methyl
7-methyl
4. Write the name as a single word.
a. Use prefixes such asmono, di, tri, tetra, etc. to indicate multiple substituents.
b. List substituents alphabetically, ignoring prefixes.c. Use dashes to separate substitutents, use commas to separate numbers.
The above example would have the name
3-ethyl-4,7-dimethylnonane
Name this alkane: Answer: 5-sec-butyldecane
1
2
3
4
5
6
7
8
9
10
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Physical Properties of Alkanes
1. Combustion - Alkanes are inflammable, i.e. they burn.
CH4 O2 CO2 OH2+ +2 2
2. Boiling and melting points
a. Both bp and mp increase with increasing carbon number for straight-chainalkanes with formula CnH2n+2
Carbon Number Physical State
C1- C4 gases
C5C16 liquids
C17C30 oils and greases
C30C50 paraffin waxes>C50 plastics (polyethylene)
b. Branching tends to raise the melting point and lower the boiling point.
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b. Branching tends to lower the boiling point and raise the melting point
BP 60oC 58oC 50oC
MP -154oC -135oC -98oC
Explanation:
MP Branching reduces the flexibility of the molecule which reduces the entropy term
S in the equation Tmp = H/S. Since S is in the denominator, Tmp increases.
BP Branching reduces surface area (more compact structure), and therefore London
dispersion forces which control boiling point for these molecules.
3. Solubilityalkanes are nonpolar molecules and therefore insoluble in water, which
is polar. Alkanes are hydrophobic.
4. Densitiesalkanes are less dense than water, with densities near 0.7 g/mL. Therefore
they float on water, e.g. Exxon Valdez oil spill.
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1. Conformation of Ethane
CH3CH
3
C C
H
H
H
H
H
H
Rotate 60o
HH
HH
H
H HH
H
H
H
H
Staggered Conformation Eclipsed Conformation
Lower Energy Higher Energy
More Stable Less Stable
The staggered conformation is more stable by 3.0 kcal/mol
Sawhorse
Newman
projection
C1
C2
H
H
HH
H
H
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Eclipsed Staggered Eclipsed Staggered Eclipsed Staggered Eclipsed
0.0 kcal/mol
3.0 kcal/mol
Dihedral Anglethe angle defined by the C-H bond on the front carbon
and the C-H bond on the back carbon in a Newman projection.
HH
H
H
H
H
600
HH
H
H
H
H
00
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Why is the staggered conformation more stable than the eclipsed conformation?
In the eclipsed conformation, the C-H bonds are closer, resulting in arepulsion
of the electron clouds.
This effect is referred to torsional strain. Torsional strain exists anytime C-H
bonds are eclipsed.
HH
H
H
H
H
1.0 kcal/mol
1.0 kcal/mol
1.0 kcal/mol
Total Energy: 3.0 kcal/mol
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2. Conformations of Propane
Rotate 60
0
C2
C1
H
H
HH
H
CH3
C1
C2
H
H
H
H
H
CH3
HH
HH
CH3
HRotate 600
More stable Less stable
0.0 kcal/mol 3.3 kcal/mol
1.3 kcal/mol
1.0 kcal/mol1.0 kcal/mole The additional 0.3 kcal/mol energy is due
to steric strain.
Steric strainelectronic repulsion that
occurs when two atoms or groups are
forced together.
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3. Conformations of Butane
C3C2
H
H
CH3 H
H
CH3
C2
C3
CH3
H
H
HH
CH3
Anti Conformation
Staggered
180o dihedral
Gauche Conformation
Staggered
60o dihedral
HH
CH3
H
CH3
H CH3H
H
H
H
CH3
CH3
H
HH
CH3
H HH
CH3
H
H
CH3
HCH3
HH
CH3
H HCH3
H
H
H
CH3
Anti
60o
60o
Eclipsed
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There are two staggered conformations of
different energy.
There are two eclipsed conformations ofdifferent energy.
Remember, staggered conformations are
more stable than eclipsed conformatiions
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Petroleum Refining
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1. The first step in petroleum refining is fractional distillation.
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2. Upstream processing of the distillates.
a. Catalytic hydrocrackingproduces small alkanes from large alkanes by
adding hydrogen.
H2, heat
Si-Al catalyst
b. Catalytic crackingproduces small alkenes and alkanes by cracking in the absence
of hydrogen.
heat
Si-Al catalyst
c. Catalytic Reformingthe alkanes and cycloalkanes are upgraded to higher octane number
by conversion into aromatic compounds.
-3H2-H2
catalyst, heat catalyst, heat
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Octane Number
Straight-chain hydrocarbons have low octane and make poor fuels.
Octane Number = 0
Branched Alkanes burn more slowly and reduce the knocking in the engine.
heptane
2,2,4-trimethylpentane
Octane Number = 100