The Baeyer Laboratory, Munich, 1893 (This photograph is in the hallway across from 110 SCL) Adolf von Baeyer (1835-1917); Nobel Prize 1905. (center, seated with derby), who was a student of KekulÈ, succeeded Liebig at Munich. In the photograph (second row; third from right) is Henry Lord Wheeler (1867-1914); Yale Faculty 1896-1911. As was the custom in the 19th century, many Americans, such as Wheeler, did advanced study in chemistry in Europe. Karl is the laboratory assistant. (The only person wearing an apron and no tie; upper left.) In 1885, as an addendum to a paper on acetylenic compounds, Baeyer proposed that cyclopentane was the least strained of the cycloalkanes. While he accepted the idea that the carbon atoms in cycloalkanes were tetrahedral, he treated the cycloalkanes as though they were flat. He argued that there is only one cyclohexane carboxylic acid, not two (axial and equatorial) as was predicted by a chair cyclohexane. Equatorial is frequently misspelled. A Projection of Melvin Newman (Son of Yale: 1929, BS; 1932, PhD)

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a. Work through How to Draw Cyclohexanes (PowerPoint)

b. The Conformation Module in the Study Aids will give you a good overview of the subject of conformation.

c. View The Evolution of Formulas and Structure in Organic Chemistry During the 19th Century (PowerPoint).

1. Redraw (line angle formula) and name (IUPAC) the hydrocarbon in this problem. For a dynamic view click here. For a static view click here. How to manipulate Jmol structures. [What if there are two different longest chains? Check here.]

2. Compound A (MW=162.61), a 1,4-disubstituted cyclohexane, has the following composition: C, 51.70%; H, 6.82%; Cl, 21.80%. The difference in conformational energy for the two chair conformations of A is 1.9 kcal/mol. Using the A-value data (Energy Differences Between ..... Cyclohexanes), determine the structure of A. Illustrate and explain. What is the conformational energy difference for the stereoisomer of A, ---namely A'. Explain and illustrate. Show the chair comformations of A and A' with the appropriate equilibrium arrows to illustrate the major and minor conformations. Label each conformation with its energy.

The first order of business is to determine the molecular formula of the compound. Does compound A contain only C, H and N? No! The sum of the percentages adds up to 80.32%. Since oxygen is determined by difference it must constitute 19.68% of the remaining matter. For the calculation:

Atom	At. Wt.	%/At. Wt.	%/At. Wt./0.61	Rounding
C	12.01	4.30	7.05	7
H	1.008	6.97	11.42	11
Cl	35.45	0.61	1	1
O	16	1.23	2.02	2

The formula is C₇H₁₁ClO₂. M.W. calculated: 162.61, which agrees with the given value. [Note: A compound composed of these four elements must, if it has an odd number of halogens,, must have an odd number of hydrogens. Thus, the number 11.42 in the chart must be rounded down and NOT up. Check here.] Compound A is a 1,4-disubstituted cyclohexane. Cyclohexane is C₆H₁₂. Subtracting two hydrogens for the positions of the two substituents leaves a cyclohexane nucleus of C₆H₁₀. Subtracting: C₇H₁₁ClO₂ - C₆H₁₀ = CHClO₂ for the sum of the composition of the two substituents. Although there are several permutations for these groups, There is only one chlorine containing group --- chlorine (0.5 kcal/mol) itself. Therefore, the other group must be CO₂H (1.4 kcal/mol). Since the energy difference between the two chair conformations of A is the sum of the two groups, both groups must be axial (1.9 kcal/mol) in one conformation and diequatorial (0 kcal/mol) in the other conformation. A is trans-4-chlorocyclohexanecarboxylic acid. Stereoisomer A' is the cis isomer whose energy difference between the two chair conformations is 1.4 - 0.5 = 0.9 kcal/mol. See below:

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3. Predict the heat of formation of 2-methyloctane using the data presented here. Explain.

There are several 2-substituted alkanes listed: 2-methylbutane (-36.7 kcal/mol), 2-methylpentane (-41.7 kcal/mol), 2-methylhexane

(-46.6 kcal/mol) and 2-methylheptane (-51.1 kcal/mol). This series adds one -CH₂- group at an average value of -5 kcal/mol/CH₂. Thus, 2-methyloctane's heat of combustion can be estimated as -51.5 -5 = -56.5 kcal/mol.

4. Examine the heats of formation of the four octanes listed in the heats of formation tables.

a)What trend do you notice?

b) Draw a diagram that shows the heat of formation and heat of combustion of the two extreme cases: n-octane and 2,2,3,3-tetramethylbutane. Show calculations.

c) Using the Jmol structures located here, measure the C-H, CH₃-CH₂ and CH₂-CH₂ bond lengths for n-octane. Measure the three different bond lengths for 2,2,3,3-tetramethylbutane. Record all six values. What trend do you see?

d) If bond breaking is critical to combustion, how do the results in 4c account for the heats of formation of these two octanes?

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5. Calculate the heat of combustion of cyclobutane using the data (ΔH_f^o of cyclobutane, CO₂ and H₂O) in the heats of formation tables.  Compare your value with the value in Table 3-5 in your text.

6. Draw Newman projections for the eclipsed and staggered conformations of 2-methylbutane viewed along the C₂-C₃ axis. Calculate the energy of each conformation, both staggered and eclipsed.