The oxygen has a formal charge of 6 - 4 - 2 = 0 (same ordering of terms). The central carbon has a formal charge of 4 (valence electrons) - 0 (lone pairs) - 4 (bonds) = 0. All atoms in the molecule have zero formal charge, the "happiest" situation for any molecule. Each hydrogen atom has one electron as a neutral atom, no lone pairs and shares one bond, for a formal charge of zero. Ribbon: draws ribbon diagram (default representation) Cylinder and plate: solid. It has no lone pairs, and it shares four bonds, so the formal charge is zero. You can also view the full chain structure by enabling the Bonds option. The carbon in CH 4 has four electrons as a neutral atom. Subtract the number of bonds shared by the atom.Subtract the number of non-bonding electrons (usually in lone pairs).Count the number of valence electrons of the neutral atom.The sum of the formal charges, with a couple of extra rules, will help us to decide which of multiple-possible valid Lewis structures is likely to be the correct one. Formal charge is just a way of bookkeeping that helps us to decide which of multiple Lewis structures is the likely true bonding arrangement of a covalent molecule. In those cases we resort to calculating what's called the formal charge of each atom. Sometimes it's difficult to tell which of two possible Lewis structures of a compound represents the actual bonding of the molecule.
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