Chemistry Organic II Laboratory
Dehydration of Methylcyclohexanols:1
Zaitzevs Rule and the Evelyn Effect2
Experiment 1
Week 1
Background Reading
th
Zubrick, J. W. The Organic Chem Lab Survival Manual, 8 edition, Wiley & Sons, Inc., New York, 2011.
Distillation: Chapt. 20; Pg 164-189.
GC Chromatography: Chapt. 32; Pg 250-259.
[This lab investigates a real mystery, which has been recently documented in the Journal of Chemical Education.]
Scenario:
For many years the dehydration of 2-methylcyclohexanol to a mixture of alkenes has been carried out in
college organic chemistry labs to demonstrate the application of Zaitzevs rule and the occurrence of the E1
reaction mechanism in alcohol dehydration reactions. In 1994 David Todd, then a chemistry p rofessor at Pomona
College, was distilling the product alkenes out of the reaction mixture when he was interrupted by an urgent
summons to lunch with the chemistry department secretary, Evelyn Jacoby. Upon returning from lunch he
decided, out of curiosity, to replace the distillation receiver with a new one and collect a second fraction. He then
worked up both fractions and analyzed them both by gas chromatography. Much to his surprise, the second
fraction contained a markedly lower percentage of the exp ected product, 1-methylcyclohexene, than the first.
Because his decision to replace the receiver with a new one was the direct result of the secretarys request,
Professor Todd named this unexpected result the Evelyn effect.
Although several mechanistic hypotheses have been proposed to explain the Evelyn effect, it is by no means
certain that any of them are correct. Your project groups assignment is to verify the existence of the Evelyn
effect for the dehydration of 2-methylcyclohexanol and to see if a similar effect exists for 4-methylcyclohexanol.
You may then want to speculate about some possible causes of the Evelyn effect.
Scientific Methodology:
As always, you should state the problem as a question, formulate a working hypothesis, follow the cou rse of
action described in the procedure, gather and evaluate evidence, test your hypothesis, arrive at a conclusion, and
report your findings.
Zaitzevs Rule and the Evelyn Effect
More than a century ago at the University of Kazan, Vladimir Vasilevich Mar kovnikov and Alexander Zaitzev
were investigating a chemical reaction both backward and forward. Markovnikov was adding hydrogen iodide to
alkenes to prepare alkyl iodides, and Zaitzev was removing hydrogen iodide from alkyl iodides to prepare
alkenes. Markovnikov discovered that hydrogen iodide adds to propene to form mainly 2 -iodopropane. From this
and other results, Markovnikov formulated his well-known rule, which can be expressed as follows for a hydrogencontaining species represented by HZ:
Markovnikovs rule:
W hen HZ adds to the carbon-carbon double bond of an
unsymmetrical alkene, hydrogen adds preferentially to the carbon atom that already has
more hydrogens.
In the meantime, Zaitzev learned that dehydrohalogenation of 2 -iodobutane by alcoholic potassium hydroxide
yields mainly 2-butene. He proposed an analogous rule for elimination reactions.
Zaitzevs rule: W hen HZ is removed from a species to form an alkene, hydrogen is lost
preferentially from the carbon atom that has fewer hydrogens.
Markovnikovs and Zaitzevs rules together can be paraphrased by the well -known maxim The rich get richer and
the poor get poorer.
These examples show that organic reactants often react selectively, favoring some products and not others
Zaitzevs reaction might have yielded as much 1-butene as 2-butene, but it did not. When a reaction could
produce two or more different structural isomers but in fact yields mainly one of them, the reaction is said to be
regioselective. Zaitzevs rule works because, in most cases, it predicts the formation of the most stable alkene.
1
rd
Lehman, J. W. Operational Organic Chemistry: A Problem-Solving Approach to the Laboratory Course, 3 Ed.,
Prentice-Hall, Inc., Upper Saddle River, New Jersey, 1999, 150-155.
2
Todd, D. J Chem. Educ. 1994, 71, 440.
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2-Butene was the major product of Zaitzevs reaction not because hydrogen -poor carbon atoms have some innate
tendency to lose the hydrogens they have, but because 2-butene is more stable than 1-butene.
Although generalizations like Zaitzevs rule can help us predict the products of many organic reactions,
organic chemistry remains an empirical science we cannot be certain that a rule that is valid for one system
under a given set of conditions will apply equally well under different circumstances. Chemists must study each
system experimentally to see if it behaves in the expected manner, and if it doesnt, try to find out why. For
example, neomenthyl chloride (Figure 1) undergoes dehydrohalogen ation to yield a product mixture that consists
of mostly alkene A, the one predicted by Zaitzevs rule. But menthyl chloride, which differs only in the geometry
of the C-Cl bond, yields 100% of alkene B, and none of the Zaitzev product. It also reacts mu ch more slowly than
neomenthyl chloride.
NaOEt
Cl
+
EtOH
A
78%
Neomenthyl
Chloride
B
22%
NaOEt
EtOH
Cl
B
100%
Menthyl
Chloride
Figure 1. Dehydrohalogenation of Menthyl and Neomenthyl Chloride
This result can be explained by assuming that the reaction occurs by an E2 (elimination, bimolecular) mechanism ,
requiring that the H and Cl atoms being eliminated lie in the same plane and on opposite sides of the C -C bond
separating them; this is called anti-periplanar geometry.
Cl
Cl
H
EtOH
EtO
The C-H and C-Cl bonds are in
the same plane (anti-periplanar)
Figure 2. Anti-Periplanar Geometry for the E2 Elimination of HCl
Neomenthyl chloride, in its most stable ring conformation (Figure 3), has the desired anti -periplanar geometry for
formation of either A or B. Since A is the more stable alkene, it is the major product.
Cl
H
Cl
H
CH 3
CH 3
H
A
H
B
Figure 3. E2 Elimination of Neomenthyl Chloride to Form Alkene A and B
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In its more stable conformation (with all large groups equatorial), menthyl chloride does not have the geometry
necessary to form either product. In its less stable conformation, the anti-periplanar geometry needed to form
product A cannot be attained because the isopropyl group rather than a hydrogen atom is anti to the leaving
group (chlorine). This less stable conformation is suitable for the formation of product B, so it is the only product
H
H
CH 3
Cl
H
H
H
CH 3
B
Cl
Less stable conformer
Leaving group axial
correct geometry for rxn
more stable conformer
leaving group equatorial
wrong geometry for rxn
Figure 4. Reactive Geometry of Menthyl Chloride is its Less Stable Conformer
isolated. Because only a very small percentage of the menthyl chloride molecules are in the less stable
conformation at any time, the reaction is much slower than the reaction of neomenthyl chloride. Th is example
shows that whenever a substrate yields the less stable alkene as a major product of an elimination reaction, there
may be some stereochemical constraints inhibiting the formation of the Zaitzev product.
The acid catalyzed dehydration of alcohols, which usually follows Zaitzevs rule, is generally believed to occur
by an E1 (elimination, unimolecular) mechanism involving protonation of the hydroxyl group, loss of water to form
a carbocation intermediate, and loss of a proton to generate the produ ct alkene. Note that there are no
H OH
H OH 2
H+
CC
-H 2O
CC
H
-H +
CC
Figure 5. E1 Stepwise Mechanism
stereochemical constraints in an E1 reaction because the leaving group leaves before the proton is lost which
forms the -bond. Thus, in an E1 dehydration of an alcohol, H and OH do not need to be anti -periplanar or in any
other particular orientation in order for elimination to occur.
Unlike E2 reactions, E1 reactions may involve rearrangements in which the initial carboc ation rearranges to a
+
more stable carbocation before it loses H . A carbocation rearrangement may involve a hydride shift during which
a hydrogen next to a positively charged carbon moves to that carbon, taking its bonding electron pair along with it.
Such rearrangements lead to alkenes whose double bond connects carbon atoms that were not originally bonded
to the hydroxyl group. Postulating such a rearrangement can explain the formation of 2 -methyl-2-butene in the
dehydration of 2-methyl-1-butanol, for example.
H
H
OH
1) +H +
2) -H 2O
CH 2
1o carbocation
hydride
shift
CH 3
-H +
3o carbocation
2-methyl-2-butene
Figure 6. Hydride-Shift in the Formation of 2-Methyl-2-butene
This brings us to the Evelyn effect. When Professor Todd carried out the dehydration of 2 -methylcyclohexanol he
obtained the following mixture of alkenes. The reaction is p erformed by distilling the alkenes as they are formed,
and the distillate typically contains 75-80% of product A, the product predicted by Zaitzevs rule. When the
distillate is collected in separate fractions and the fractions are analyzed separately, th e first 10 percent of the
distillate contains about 93% A while the final distillate contains as little as 55% A.
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CH 3
CH 3
CH 3
OH
CH 2
H3PO4
+
+
-H 2O
A
B
C
Figure 7. Alkene Products From Dehydration of 2-Methylcyclohexanol
There is a clue to the origin of the Evelyn effect in the cata log of the Aldrich Chemical Company, where the 2methylcyclohexanol used by Professor Todd is described as a mixture of cis and trans isomers. In fact, it is
nearly an equimolar mixture of the two isomers. Previous researchers had reported that the cis-isomer reacted
much faster than trans-isomer, the so Todd reasoned that the initial product mixture formed mainly by dehydration
of the cis-isomer while the product in the final distillate fraction was formed mainly by dehydration of the transisomer.
CH 3
CH 3
OH
H3PO4
-H 2O
cis-2-methylcyclohexanol
CH 3
A>90%
CH 3
CH 3
OH
H3PO4
+
-H 2O
B
A<55%
trans-2-methylcyclohexanol
Figure 8. Different Reactivities of cis- and trans-2-Methylcyclohexanol
Since the trans-isomer yields an unexpectedly large percentage of the less stable alkene, it appears that this
reaction, like the E2 dehydrohalogenation of menthyl chloride , has some stereochemical constraints. The
occurrence of E2 elimination from a protonated alcohol could explain a reduction in the amount of the expected
product A, since elimination via an anti-periplanar geometry can yield only product B and not A. It could also
explain the lower reactivity of the trans-alcohol, which can achieve the anti-periplanar geometry only in its less
stable diaxial conformation.
However it does not explain the existence of a small amount of
methylenecyclohexane (product C) in the product mixture. Product C might be obtained via an E1 mechanism
involving a carbocation rearrangement, but not by an ordinary E2 mechanism.
CH 3
CH 3
OH
CH 3
CH 2
+
H
-H 2O
C
Figure 9. Carbocation Rearrangement Via Hydride-Shift to Form Product C
Does the reaction proceed by both E1 and E2 mechanisms? That possibility, raised by Todd, has been
questioned by two other researchers, John J. Cawley and Patrick E. Lindner. Cawley and Lindner proposed an
E2-like mechanism involving bridged ions (J. Chem. Educ. 1997, 74, 102.), but it remains to be seen whether
their mechanism will gain general acceptance. A mechanism is, after all, a scientific hypothesis about processes
that we cant observe directly and is therefore subject to revision.
The Evelyn effect illustrates how science often works. For decades the results of alcohol dehydration
reactions are adequately explained by the E1 hypothesis; no other explanation seems necessary. Then a chance
observation shows the inadequacy of the accepted hypothesis. A different hypothesis that both E1 and E2
mechanisms are involved- is proposed and contested, followed by another hypothesis, and so on. The road to
scientific discovery is a rocky one and there may be detours along the way, but every failed hypothesis yields new
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information, new ideas, and often new applications. Science is not simply a body of established facts and
theories; the facts and theories of science are always subject to further inquiry that may disprove or modify them.
Science is a dynamic process by which knowledge is acquired, ideas are debated, theories are proposed, and
new ways of doing things are discovered.
Understanding the Experiment
In this experiment, you and your coworkers will carry out the dehydration of 2 -methylcyclohexanol and 4methylcyclohexanol by heating the alcohols in the presence of phosphoric acid. Both alcohols will be mixtures of
cis and trans isomers, so either or both may exhibit the Evelyn effect.
Dehydration of a secondary alcohol proceeds readily with about half a mole of phospho ric acid for every mole
of the alcohol. By protonating an alcohol, the acid catalyst converts the poor leaving group ( -OH) to a much better
+
+
leaving group (-OH2 ). Elimination of H and H2O from the protonated alcohol yields an alkene, with the
unprotonated alcohol serving as the reaction solvent.
According to LeChteliers principle, removing a product from the chemical system at equilibrium shifts the
equilibrium in the direction favoring the formation of products. You will carry out the dehydration rea ction in a
distillation apparatus so that the products (water and the alkene) will continuously distill out of the reaction mixture
as they are formed. Their removal will shift the equilibrium towards formation of the alkene and thus increase the
overall yield. If the reaction mixture is heated to a temperature above the boiling points of the product alkenes but
below that of the reacting alcohol, most of the unreacted alcohol will remain in the reaction flask while the water
and alkenes distill into a receiving flask. Interposing a vertical column between the boiling flask and the still head
will further reduce the amounts of unwanted alcohol, acid, and by-products in the distillate.
You will follow the progress of the reaction by measuring the volume of alkene in the distillate, collecting two
fractions of approximately equal volume. When the reaction is over, the residue in the reaction flask may begin to
foam and emit white vapors. You should remove the heat source at this point because overheating t he residue
will form a black tar and generate toxic fumes.
After washing and drying the organic layer of each fraction, you will analyze the fractions by gas
chromatography. If you started with 2-methylcyclohexanol, your gas chromatograms may show peaks f or both 1and 3-methylcyclohexene (the methylenecyclohexene peak may also be resolved since we are using a capillary
column). If you started with 4-methylcyclohexanol, you may obtain only 4-methylcyclohexene or a mixture of
products including 3-methylcyclohexene and 1-methylcyclohexene. From the relative areas of your peaks, you
can estimate the percentage composition of the product mixture in each fraction.
Procedure:
Reaction and Separation
Measure 75 mmol of 2-methylcyclohexanol or 4-methylcyclohexanol (cis-trans mixtures) into a 25 mL round
bottomed flask. Mix in 3 mL of 85% phosphoric acid and drop in a few boiling chips. Clamp the flask to the lattice
work (monkey bars) and properly position a heating mantle. Remember to plug the heating mantle i nto the
temperature controller before plugging into the outlet. Assemble the glassware for a simple distillation, greasing
the ground glass joints as needed. Use a 10 mL graduated cylinder as the receiver.
Start heating and boil the reactants gently so that vapors ascend slowly up the column and begin to condense
into the receiver. When the vapors reach the still head and the temperature has stabilized, record the still -head
temperature. Observe it at intervals throughout the reaction and keep tabs on i t. Control the rate of heating so
o
that the distillation rate is one drop per second or less and the temperature stays below 120 C (the thermometers
o
o
go to 110-115 C and the bp of the product(s) is ~110 C so estimate). Have ready two clean, labeled test tubes.
Monitor the volume of alkene (which layer would that be?) layer in the distillate. When the alkene volume is about
4 mL, quickly pour the distillate into the first test tube and replace the graduated cylinder. After the alkene volume
reaches ~3mL, observe the still-head temperature continually. Lower the heat source and turn it off when you
observe a marked temperature change at the still-head or foaming and dense white fumes in the reaction flask.
Pour the distillate into the second test tube. For each separate fraction, wash the distillate by shaking it with two 5
mL portions of saturated aqueous sodium bicarbonate and carefully removing the aqueous layer with a Pasteur
pipet. Dry each alkene mixture separately with a small amount of magnesium sulfate. Decant the liquid into a
small tared vial. Weigh each alkene mixture and calculate the total mass of alkenes.
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Analysis:
Analyze both fractions by gas chromatography and NMR. Make GC samples of the appropriate concentration
in methanol (1 drop of product in the vial then fill with methanol). From the GC run, measure the area and
retention time of each peak on your gas chromatogram. Identify the peaks. The alkene peaks should appear on
the gas chromatogram in order of the alkene boiling points. Determine the percent composition of each fraction.
Calculate the percent yield of alkenes based on their combined mass. Repeat the analysis using the NMR data.
You will need to identify the peaks due to the vinyl hydrogens as the first step. Finally, try to explain your results
as clearly and completely as you can. This should all be in your lab notebook.
Questions:
1. W hich kind of mechanism can better account for the product mixture obtained from the dehydration of cis and
trans-4-methylcyclohexanol: E1, E2, or a combination of the two?
2. W rite a detailed mechanism which explains the formation of all observed products from the above reaction.
3. In the section Understanding the Experiment, 1-methylcyclohexene and 3-methylcyclohexene were
mentioned as possible products of the dehydration of 2-methylcyclohexanol. Why was 2-methylcyclohexene
not mentioned as a possible product?
+
4. In an E2 reaction a base removes H as the leaving group leaves the substrate. Draw structures of at least
three possible bases (they may be weak bases) present in the reaction mixture for the reaction of 2 methylcyclohexanol.
5. Predict the major alkene product that would result from dehydrating each of the following alcohols, with no
carbocation rearrangements.
OH
OH
HO
TO BE TURNED IN FOR GRADING:
Please organize your data/results and then provide your interpretation with respect to the overall question of what
mechanism is operating during this process. This should require 2-3 paragraphs. Explain how you have
interpreted the data, why this is a valid way to interpret the data, and how your results allow you to determine the
reaction mechanism which operates during this reaction.
Be able to answer the above questions but they do not need to be turned in for a grade. They will likely appear on
an exam in the future.
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