Bonds.

Bonds.
Two orbitals with similar symmetry, lying in adjacent atoms, can lead to a bond. Multiple pairs of orbitals can even be formed between the same pair of atoms; this is a multiple bond. A σ bond is characterized by an overlap zone with the greatest electron density situated on the bond line between the two atoms. This occurs when the orbitals each "point" to the other atom. There is rotational symmetry around a σ-type bond, and the overlap between the orbitals persists upon rotation. If there is more than one bond between two atoms, the orbitals responsible for it overlap on two sides of the bonding axis. When there is a π bond between two atoms, that bond no longer has rotational freedom. π-bonds are usually formed by unhybridized p-orbitals on the two atoms. Thus, if 2 atoms form one double bond, the rest of the orbitals (1 s and 2 p orbitals) will hybridize to sp2. As another example, if an atom forms 2 double bonds, 1 s and 1 p (e.g. px) orbitals remain to form 2 sp orbitals. These point to the left and right, respectively. One of the remaining p orbitals (e.g. pz) forms a double bond "top and bottom" with a second atom, and the other (py) "front and back" with a third atom.
Or simply: "making love"....