Which is more stable the cis or the trans alkene?

Note: This problem is a typical example of those instances in science where there is probably no single “correct” explanation for an observed phenomenon.

Key TERMS

Make certain that you can define, and use in context, the key terms below.

• catalytic hydrogenation
• heat of hydrogenation, (ΔH°hydrog)
• hyperconjugation

Study Notes

The two alkenes, cis 𝖢𝖧𝟥𝖢𝖧=𝖢𝖧𝖢𝖧𝟥CH3CH=CHCH3 and (𝖢𝖧𝟥)𝟤𝖢=𝖢𝖧𝟤(CH3)2C=CH2 have similar heats of hydrogenation (−120 kJ/mol and −119 kJ/mol, respectively), and are therefore of similar stability. However, they are both less stable than trans 𝖢𝖧𝟥𝖢𝖧=𝖢𝖧𝖢𝖧𝟥CH3CH=CHCH3 (−116 kJ/mol).

You may wonder why an sp2 –sp3 bond is stronger than an sp3-sp3 bond. Bond strength depends on the efficiency with which orbitals can overlap. In general, s orbitals overlap more efficiently than do p orbitals; therefore, the s–s bond in the hydrogen molecule is stronger than the p–p bond in fluorine. In hybrid orbitals, the greater the s character of the orbital, the more efficiently it can overlap: an sp2 orbital, which has a 33% s character, can overlap more effectively than an sp3 orbital, with only 25% s character.

Alkene hydrogenation is the syn-addition of hydrogen to an alkene, saturating the bond.  The alkene reacts with hydrogen gas in the presence of a metal catalyst which allows the reaction to occur quickly. The energy released in this process, called the heat of hydrogenation,  indicates the relative stability of the double bond in the molecule (see Catalytic Hydrogenation).

Introduction

The reaction begins with H2 gas and an alkene (a carbon-carbon double bond). The pi bond in the alkene acts as a nucleophile; the two electrons in it form a sigma bond with one of the hydrogen atoms in H2. With the pi bond broken, the other carbon (the one that did not newly receive a hydrogen) is left with a positive formal charge. This is the carbocation intermediate. The remaining (unreacted) hydrogen is now a hydride anion, as it was left with two electrons previously in the H-H sigma bond. Next, the electrons of the negatively charged hydride ion form a bond with the positively charged carbon. This reaction is exothermic. It will occur, but it is very slow without a catalyst.

The Catalyst

A catalyst increases the reaction rate by lowering the activation energy of the reaction. Although the catalyst is not consumed in the reaction, it is required to accelerate the reaction sufficiently to be observed in a reasonable amount of time. Catalysts commonly used in alkene hydrogenation are: platinum, palladium, and nickel. The metal catalyst acts as a surface on which the reaction takes place. This increases the rate by putting the reactants in close proximity to each other, facilitating interactions between them. With this catalyst present, the sigma bond of H2 breaks, and the two hydrogen atoms instead bind to the metal (see #2 in the figure below).  The [latex] \pi [/latex] bond of the alkene weakens as it also interacts with the metal (see #3 below).

Since both the reactants are bound to the metal catalyst, the hydrogen atoms can easily add, one at a time, to the previously double-bonded carbons (see #4 and #5 below). The position of both of the reactants bound to the catalyst makes it so the hydrogen atoms are only exposed to one side of the alkene. This explains why the hydrogen atoms add to same side of the molecule, called syn-addition.

Figure 1:  Hydrogenation takes place in the presence of a metal catalyst.

Note: The catalyst remains intact and unchanged throughout the reaction.

Heats of Hydrogenation

The stability of alkene can be determined by measuring the amount of energy associated with the hydrogenation of the molecule.  Since the double bond is breaking in this reaction, the energy released in hydrogenation is proportional to the energy in the double bond of the molecule. This is a useful tool because heats of hydrogenation can be measured very accurately. The [latex] \Delta H^o [/latex] is usually around -30 kcal/mol for alkenes. Stability is simply a measure of energy.  Lower energy molecules are more stable than higher energy molecules. More substituted alkenes are more stable than less substituted ones due to hyperconjugation. They have a lower heat of hydrogenation.  The following illustrates stability of alkenes with various substituents:

In disubstituted alkenes, trans isomers are more stable than cis isomers due to steric hindrance.  Also, internal alkenes are more stable than terminal ones.  See the following isomers of butene:

Figure 7.6.3: Trans-2-butene is the most stable because it has the lowest heat of hydrogenation.

Note: In cycloalkenes smaller than cyclooctene, the cis isomers are more stable than the trans as a result of ring strain.

Which alkene is more stable cis alkene or trans alkene?

The compounds with less steric hindrance are more stable. Whereas cis alkenes have less high steric hinderance. Thus, trans alkenes are more stable than cis alkenes.

Which has more stability cis or trans?

Cis Isomers Can Be More Stable than Trans.

Why cis alkene is less stable than trans alkene?

Between cis and trans isomers of an alkene, the cis isomer tends to be less stable due to the molecular crowding created nonbonding interaction between two alky groups on the same side of the double bond.