In this tutorial, we will learn the relative stability of ethane
conformations as a result of single bond rotation. The structure of
ethane, C2H6, is shown below. The bond between
the two carbon atoms is a single bond which is formed by two sp3
hybrid orbitals overlapping head to head. This symmetric cylindrical
electron distribuation allows for "free" rotation around
the C-C bond. Shown to the right of this structure are "live"
ethane molecules animated to rotate around that bond, with the right
one viewed from the left the molecule.
As the C-C bond rotates, an infinite number of conformations (or
conformers) is created. The two which are of most interest to us
are shown below:
It's now your turn to rotate the two conformers and
examine their spatial properties. After that, answer the following
two questions:
1) which is of lower energy and thus more stable?
2) What are the names we give to the two conformers? (hint: how
are the hydrogens arranged on the front carbon relative to the back
carbon?)