Answer :
The overall charge of a molecular species can be determined by summing up the formal charges on all its atoms. In the Lewis diagram provided, the overall charge is zero since there are no charges indicated.
To calculate the formal charge on the nitrogen atom, we need to compare the number of valence electrons the atom should have (5 for nitrogen) with the number of electrons assigned to it in the diagram. In this case, nitrogen is bonded to three hydrogen atoms and has one lone pair of electrons. Each bond contributes one electron, so the nitrogen atom has a total of five assigned electrons. Since nitrogen should have five valence electrons, the formal charge on the nitrogen atom is zero.
The formal oxidation number of an atom is the hypothetical charge it would have if all the shared electrons in the bonds were assigned to the more electronegative atom. In this case, the nitrogen atom is less electronegative than hydrogen, so it retains its full valence of five electrons. Therefore, the formal oxidation number of the nitrogen atom is also zero.
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