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Hi, I'm trying to understand how oxygen and nitrogen, when in a molecule with 4 bonds...

Hi, I'm trying to understand how oxygen and nitrogen, when in a molecule with 4 bonds to them, for example, NH4+ and H3O+ bear a POSITIVE charge when they gain that additional proton? I think I understand that nitrogen's FC would be calculated 5-0-4= +1, but now, I'm having the same problem with nitrogen because wouldn't the formal charge be calculated 6-3-3=0?? Do I have the formula wrong? What is GOING ON!!?

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Answer #1

Formal charge is calculated as Formal charge = No. of valence es-no. of lone pairs of electrons - (no. of bonded electrons/2)

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