BASIC PRINCIPLES OF ORGANIC CHEMISTRY

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Carbon form covalent bond

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Carbon is a non metal with atomic number 6.

electronic configuration of carbon in ground state:

1s2 2s2 2p2.

To get the octet in its outer shell it has to gain 4 more electrons to form C4- ion. the electronegativity of carbon is only 2.5 and its nucleus has only 6 protons. therefore its difficult for a nucleus with 6 protons to hold 10 electrons.

Hence carbon cannot form C4- ions so easily.

If carbon looses 4 electrons from its outer shell, it has to form C 4 + ion. This requires huge amount of energy which is not available normally.

Therefore C4+ formation also is a remote possibility.

Carbon has to satisfy tetravalency, by sharing electrons with other atoms. So it has to form 4 covalent bonds either with its own atoms or atoms of other elements.

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Electrons in an atom can be identified in the shells. The maximum number of electrons in a shell depends on the formula 2n2, where n is the number of the shell. Each shell has orbitals, known as s, p, d and f. The first shell has one orbital, s, while the second shell has two orbitals, s and p.

To get the number of unpaired electrons, we must see the electron configuration. Oxygen's atomic number is 8, so it has eight protons and electrons. These eight electrons are distributed in the shells. The electron configuration is 1s2 2s2 2p4. The maximum number of electrons in the second shell is 2n2 = 2 * 22 = 8. In this case, total electrons in the second shell = 2 (in s orbital) + 4 (in p orbital) = 6. So, the number of unpaired electrons = 8 - 6 = 2.

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