How many people do you think are squeezed on this street?
Our minds can handle two electrons interacting with one another in a sphere of space. But then we start putting in double bonds and triple bonds. The way we draw these bonds on paper suggests we are squeezing more electrons into the same space, and that doesn’t work. Electrons don’t like to be pushed together (especially since they all have negative charges that repel one another). So we need a more complex picture that works for all these electrons.
Sigma and Pi Bonds
The hybridization model helps explain molecules with double or triple bonds (see Figure below). Ethene (C2H4) contains a double covalent bond between the two carbon atoms and single bonds between the carbon atoms and the hydrogen atoms. The entire molecule is planar.
As can be seen in Figure above, the electron domain geometry around each carbon independently is trigonal planar. This corresponds to sp2 hybridization. Previously, we saw carbon undergo sp3 hybridization in a CH4 molecule, so the electron promotion is the same for ethene, but the hybridization occurs only between the single s orbital and two of the three p orbitals. Thus generates a set of three sp2 hybrids along with an unhybridized 2pz orbital. Each contains one electron and so is capable of forming a covalent bond.
The three sp2 hybrid orbitals lie in one plane, while the unhybridized 2pz orbital is oriented perpendicular to that plane. The bonding in C2H4 is explained as follows. One of the three sp2 hybrids forms a bond by overlapping with the identical hybrid orbital on the other carbon atom. The remaining two hybrid orbitals form bonds by overlapping with the 1s orbital of a hydrogen atom. Finally, the 2pz orbitals on each carbon atom form another bond by overlapping with one another sideways.
It is necessary to distinguish between the two types of covalent bonds in a C2H4 molecule. A sigma bond (
In a conventional Lewis electron-dot structure, a double bond is shown as a double dash between the atoms as in C=C. It is important to realize, however, that the two bonds are different: one is a sigma bond, while the other is a pi bond.
Ethyne (C2H2) is a linear molecule with a triple bond between the two carbon atoms (see Figure below). The hybridization is therefore sp.
The promotion of an electron in the carbon atom occurs in the same way. However, the hybridization now involves only the 2s orbital and the 2px orbital, leaving the 2py and the 2pz orbitals unhybridized.
The sp hybrid orbitals form a sigma bond between each other as well as sigma bonds to the hydrogen atoms. Both the py and the pz orbitals on each carbon atom form pi bonds between each other. As with ethene, these side-to-side overlaps are above and below the plane of the molecule. The orientation of the two pi bonds is that they are perpendicular to one another (see Figure below). One pi bond is above and below the line of the molecule as shown, while the other is in front of and behind the page.
In general, single bonds between atoms are always sigma bonds. Double bonds are comprised of one sigma and one pi bond. Triple bonds are comprised of one sigma bond and two pi bonds.
- Sigma bonds form between two atoms.
- Pi bonds form from p orbital overlap.
- What is the hybridization around each carbon in ethene?
- What are the two bonds in C=C?
- What is the shape of the ethene molecule?
- How are the ethyne pi bonds oriented in relation to each other?