ok the actual element has two dots in it already... and i missed it... kinda didn;t expect it.. but still now its H3C:
wouldn't it have 9 electrons, only needs 8 to complete, unless this is an exception?
H3C: has two electrons in a lone pair, and 3 bonds, each to a hydrogen.
So the formal charge on H3C: is
(Valence Electrons) - (Electrons in Lone Pairs) - (# of bonds)
= 4 - 2 - 3
This is only true for CH3 when the C has a full lone pair to itself. CH3, the collection of four atoms, can exist together in the three ways shown in the picture above. The three C-H bonds would exist in sp2 hybrid orbitals, and the only thing that varies is the number of electrons in the remaining 2p orbital.
CH3+ is a methyl cation...no electrons in the 2p orbital
CH3 is a neutral radical...one unpaired electron in the 2p orbital
CH3- is a methyl anion...two electrons in the 2p orbital
Hope that clears everything up