Question

Explain the covalent bond formation of carbon with other atoms??

Answer 1

Number of formed covalent bonds by any atom depends upon the number of valence electrons present in the outermost shell of that atom. And for knowing the valence electrons we have to know about the electronic configuration of that atom.

Complete answer:
As we know that the carbon atom (${\text{C}}$) is situated in the ‘IV A’ group of p – block in the periodic table and its atomic number is 6.
-Atomic number (${\text{Z}}$) of any atom is always equal to the number of electrons present in the orbitals outside the nucleus or number of protons present inside the nucleus.
-From the above point it is clear that in carbon atom six electrons are present and its electronic configuration is written as ${\text{1}}{{\text{s}}^{\text{2}}}{\text{,2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{2}}}$and from the configuration we will ensure that in outermost shell of carbon atom four valence electron are present.
-Also we know that covalent bonds are formed by the sharing of electrons.
-So, in the outermost shell of a carbon atom four valence electrons are present and this valence electrons takes part in the formation of covalent bonds with the other atoms by the sharing process.
Hence, from the above discussion it is clear that carbon atoms (${\text{C}}$) can form four covalent bonds with other atoms.

Note:
Here some of you may think that, why carbon atoms are only formed covalent bonds not ionic bonds, so the reason is that ionic bond is formed between two oppositely charged ions. But here the carbon atom is not that much electronegative or electropositive to bear an exact charge on itself.