Problem Set 3
Chapter 4
Due: Monday, September, 30, 2002
The prevailing theory of organic
structure in the early 19th century was Dualism or the
Electrochemical Theory, principally championed by
Berzelius.
Since inorganic sodium chloride could be considered as
Na+Cl-, then an alkyl halide such as
RCl could be thought of as R+Cl-. The
R group or "radical" of its day, was thought to be
immutable, the carbons and hydrogens behaving as though they
were an element. Liebig and Dumas, influential chemists of
the day, published a joint paper (1837), On
the Present State of Organic
Chemistry., extolling the concept
and claiming all that was left to do was to identify these
immutable radicals (benzoyl, ethyl, acetyl, etc.) A Parisian
reception was to change all of this. The guests were
discomforted by fumes from the candles. Dumas was called in
as a consultant. He found that the waxes (fatty esters) had
exchanged chlorine for hydrogen, the culprit being the
by-product hydrogen chloride. Jean-Baptiste-André Dumas
(1800-1884) The concept of exchanging electropositive
hydrogen for electronegative chlorine was anathema to
dualism, although Liebig
and Wöhler
had done precisely this in 1832 on their work on the benzoyl
radical (C7H5O). Dumas's student,
Laurent, not one to shirk from controversy, was bold enough
to call the process substitution rather than exchange. Thus
was Substitution Theory born. Moreover, Dumas (1838) was
able to substitute three of the four hydrogens of acetic
acid for chlorine to form trichloroacetic acid, having
similar properties to acetic acid. The recognition of these
similar properties led to early Type Theory. In 1842,
Melsen, a student of Dumas, reversed Dumas's experiment by
reducing trichloroacetic acid to acetic acid by the action
of zinc metal. The promulgation of Substitution Theory gave
the wry
wit of Wöhler, a.k.a., S. C.
H. Windler, an opportunity to shine. As Radical Theory of
the early 19th century waned, at the turn of the 20th
century free radicals, to distinguish them from the older
radicals, were detected and investigated. The very process
of substituting chlorine for hydrogen is a free radical
reaction.
1. Study the Alkane Module in Organic
Reactions Go Online (ORGO).
2. Consider 2,3-dimethylbutane.
a) What is the difference in energy between the two lowest energy conformations viewing along the C2-C3 axis? [Draw Newman projections of both and show calculations.]b) How many monochlorination products of this hexane are possible? How much of each? Show work.
3) Why is monochlorination of cyclohexane a more
effective preparative reaction than monochlorination of its
constitutional isomer, methylcyclopentane?
4) Determine the heat of reaction for each of the
propagation steps and for the overall reaction in the bromination of
cyclohexane. Show work. Draw a reaction coordinate diagram for the
reaction (Cf., Fig.4-4, pg. 149)
5) The heat of combustion of cyclopropane is
-499.8 kcal/mol [pg.109]. The combustion of H2 at
25 oC liberates -68.3 kcal/mol while the combustion of
graphite liberates -94.05 kcal/mol. From these data cyclopropane can
be shown to be less stable (+12 to13 kcal/mol) than the elements from
which it is formed. a) Explain and show work. [The
thermochemistry
module will be of assistance to you.]. display the data
graphically. See here.
6) Given information in Table 3-4, pg. 109, estimate the heat of
combustion of n-decane if the heat of combustion of n-octane = 1302.7
kcal/mol.
7) Examine
the difference in the heat of formation of a series of
n-alkanes.
a) What is the average difference in the heat of formation of a series of n-alkanes? Show work.b) Using the value in 7a, calculate the value from Table 3-4 that you used in problem #6 with the aid of the hypothetical reaction CH2 + 3/2 O2 ---> CO2 + H2O).
c) Using the heats of formation of cyclopentane and cyclohexane (click here) and the answer from parts a) and b) above, make an argument for the relative stability of these two cycloalkanes. Show work.
8) The free radical bromination of cyclohexene produces only one of the structures below.
a) Explain with the aid of bond dissociation energies (BDEs).
b) What complication might arise when this reaction is applied to trans-3-hexene (4)? Resonance plays a role here.Explain and illustrate
.