Which of these molecule have correct charges on Carbon

Ok so if from a carbon in a benzene molecule i remove a H then is that C supposed to have a positive or a negative charge ?
Like in this one
http://i.imgur.com/AA5bk.png
Is (1) correct or the second one (2) ?
According to my formal charge intuition (2) should be correct ,

Then how In my book its shows a molecule like this
http://i.imgur.com/1xafg.png

How is this correct ?

First of all, you need to realize that there are no actual charges on the atoms in a benzene molecule. Formal charge is a "mathematical construct" not an actual charge. In benzene, each carbon atom has a formal charge of zero. Don't confuse formal charge an oxidation number. H is assigned an oxidation number of +1, which gives each carbon atom an oxidation number of -1. Again, oxidation numbers are not actual charges.

As for your diagram, the structure on left doesn't exist, since the "top" carbon is shown with five bonds. Benzene is C6H6. There is only one hydrogen atom per carbon atom.

If you took an H along with the bonding pair of electrons away from from C6H6, then the carbon in question would have a formal charge of +1. This comes from the formula for formal charge:
FC = VE - NBE - 1/2BE .... VE = valence electrons, NBE = nonbonding electrons, BE = bonding electrons
FC = 4 - 0 - 1/2(6) = +1

If you simply removed H, but left the bonding pair of electrons, there would be a lone pair on the carbon, and the formal charge on carbon would be -1.
FC = 4 - 1 - 1/2(6) = -1

Put simply both (1) and (2) are nonsense. As is your starting molecule, which has too much hydrogen.


And your book shows the stabilisation of a carbocation in a non-aromatic system, it has little relevance in this case.

if any hydrogen is removed from any carbon of benzene molecule, that carbon will adopt positive charge and the whole specie is called hexacarbodienyl cation.