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1 Note that in chair cyclohexane, there are two different types of C-H bonds, and thus two chemically different types of hydrogens. 2  The C-H bonds which point vertically upward or downward are called axial. 3  There are 6 of these, 3 upward and 3 downward bonds, and they alternate up/down/up, etc., around the ring. The ground state conformation of cyclohexane is a fully staggered conformation which is shaped somewhat like a chair. 2  In this conformation there is no torsional strain at all, and as we shall see later, no strain of any kind.
The cyclopropane molecule is a ring of three carbon atoms, each bonded to the other two through s bonds and each bonded to two hydrogens, also through s bonds. Since each C has four sigma bonds, we can say the C atom hybridization is sp3.But the CCC bond angle, 60Â°, is much less than the perfect sp3 tetrahedral bond angle of about 109Â°. One says that cyclopropane is highly strained because the CCC bond angles are so small.he atomic geometry around C number 4 is roughly trigonal planar; all four atoms shown here lie in the same plane. The lone pairs on O occupy two of the three sp2 hybrids, while the third is used to make the s bond of the double bond to C. The other bond in the double bond is a p bond between p orbitals of O and C.