The first molecule of butane shown is antibonding, meaning that the carbon groups are 180 degrees apart. This is the most stable conformation of butane because there is no strain on the molecule. The second molecule of butane shown is eclipsed, the eclipsed molecule has torsional strain between the carbon hydrogen bonds making it less stable than the anti or gauche form. The gauche form is the second most stable configuration of butane where the two methyl groups are staggered 60° apart from each other. The gauche conformation exhibits steric strain repulsion between the two methyl groups that are sticking out. The last molecule is the syn conformation of butane and it is the least stable conformation. The syn conformation consists of steric and torsional strain between its carbon carbon bonds and carbon …show more content…
In the cyclohexane molecule all of the hydrogens are staggered and because the atoms are closer than 2.40 Angstroms apart, steric strain exists between the carbon hydrogen bonds. Overall, cyclohexane is a very stable molecule, which is shown by its low energy and low steric strain. Cyclopropane is a very unstable molecule because it has steric and torsional strain and a high energy.

The chair conformation of cyclohexane is the most stable form of cyclohexane. This is because it has the lowest energy due to having minimal steric strain caused by the distance of the hydrogen atoms. The boat conformation of cyclohexane is less stable than the chair form of cyclohexane because it has a higher energy due to the eclipsed hydrogen bonds. The hydrogen bonds are generating steric strain due to hydrogens being in the same plane.

The axial axial 1,2-dimethylcyclohexane is the least most stable configuration, followed by This is because axial bonds are less stable than equatorial bonds due to less strain on the molecule. This conclusion can be applied to all molecules in cyclohexane