Covalency
Covalency
This type of bonding involves a sharing of electrons in
pairs, each atom contributing one electron to form a shared pair, each pair of
electrons having their spins antiparallel. This method of completing an octet
(or any of the other possible values) gives rise to the covalent bond.
Hydrogen is usually unicovalent: occasionally it is
unielectrovalent, e.g., in sodium hydride, hydrogen exists as the hydride
anion, formed by accepting an electron from the sodium:
Na. + H. → Na+H:-
Carbon almost invariably forms covalent compounds. The
electron configuration of carbon is (1s)2(2s)2(2p)2. Since the two 2s electrons
are paired, it would appear that carbon is bivalent, only the two single 2p
electrons being involved in compounds formation. As pointed out previously,
carbon is almost always quadrivalent; thus the 2s and 2p electrons must be
involved.
In methane the four hydrogen atoms each contribute one
electron and the carbon atom four electrons towards the formation of fur shared
pairs:
Each hydrogen atom has its duplet (as in helium), and the
carbon atom has an octet.
Each pair of shared electrons is equivalent to the ordinary
‘valency-bond’, and so electronic formulae are readily transformed into the
usual structural formulae, each bond representing a shared pair, e.g.,
From these examples it can be seen that there is a very
important difference between an electronic formula and its equivalent
structural formula. In the former, all valency electrons as shown whether they
are used to form covalent bonds or not; in the latter, only those electrons
which are actually used to form covalent bonds are indicated. This is a
limitation of the usual structural formula. A widely used scheme is to
represent structures with ordinary valency bonds and to indicate lone pairs by
pairs of dots.
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