Carbon has two properties that enable it to form such an extensive range of compounds: catenation (the ability to form chains of atoms) and multiple
bonding (that is the ability to form double and triple bonds). Extensive use of multiple bonding is found in compounds of carbon, nitrogen, and
oxygen. Carbon shows the greatest propensity for catenation of all elements. [Note: Sulfur shows the second most] For catenation, three conditions
are necessary:
A bonding capacity (valence) greater then or equal to 2.
An ability of the element to bond with itself; the self-bond must be about as strong as its bonds with other elements.
A kenetic inertness of the catenated compound toward other molecules and ions.
We can see why catenation is frequently found in carbon compounds but only rarely in silicon compounds by comparing bond energy data for those two
elements. Notice that the energies of the carbon-carbon and carbon-oxygen bonds are very similar. However, the silicon-oxygen bond is much stronger
than that between two silicon atoms. Thus, in the presence of oxygen, silicon will form -Si-O-Si-O- chains rather then -Si-Si- linkages. We will see
later that the silicon-oxygen chains dominate the chemistry of silicon. There is much less of an energy "incentive" to break carbon-carbon
bonds in favor of the formation of carbon-oxygen bonds.
It is sobering to realize that two "quirks" of the chemical world make life possible: the hydrogen bond and the catenation of carbon.
Without these two phenomena, life of any form (that we can imagine) could not exist.
C-C BE = 346 KJ/Mol
C-O BE = 358 KJ/Mol
Si-Si BE = 222 KJ/Mol
Si-O BE = 452 KJ/Mol
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