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    Hi,

    Would someone be able to explain why you end up with positive charges on the resonance structures of nitrobenzene? I thought that if the carbon went from being part of a double bond to being part of a single bond, then it would have a negative charge.

    Many thanks
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    (Original post by VioletPhillippo)
    Hi,

    Would someone be able to explain why you end up with positive charges on the resonance structures of nitrobenzene? I thought that if the carbon went from being part of a double bond to being part of a single bond, then it would have a negative charge.

    Many thanks
    The formal charge is the number of protons - the number of electrons around the atom.

    The number of electrons = the non-bonding electrons + (bonding pairs)/2

    If both of the electrons from a bond go somewhere else the (previously neutral) atom loses a one half share of a bonding pair = 1 electron and so develops a positive charge.

    Look at your example in the attachment and count up the electrons and protons at each atom (not forgetting inner shell electrons)
 
 
 
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