Draw the Lewis structure of [tex]CNO^-[/tex] (C-N-O) and find the formal charges on carbon, nitrogen, and oxygen.

The formal charge on C is [X], on N is [Y], and on O is [Z].

(For the formal charge, write + or - sign)

Question

High School

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Answer :

PratikshaS PratikshaS · Answer 1 · 2023-11-13T07:23:21-05:00

Oxygen (O) has 6 valence electrons and is connected to one atom, so it has 2 lone pairs (4 electrons).

N-C O. The formal charges on carbon (C), nitrogen (N), and oxygen (O) are all zero (0).

Start by counting the valence electrons for each atom:

Carbon (C) has 4 valence electrons.

Nitrogen (N) has 5 valence electrons.

Oxygen (O) has 6 valence electrons.

Connect the atoms by single bonds:

Place the nitrogen (N) atom in the center, with carbon (C) and oxygen (O) on either side. Connect each atom with single bonds (|N-C-O|).

Distribute the remaining electrons:

Carbon (C) has 4 valence electrons and is connected to one atom, so it has no lone pairs.

Nitrogen (N) has 5 valence electrons and is connected to two atoms, so it has 3 lone pairs (6 electrons).

Oxygen (O) has 6 valence electrons and is connected to one atom, so it has 2 lone pairs (4 electrons).

N-C O

The figure is given below.

Calculate the formal charges:

Formal charge = (Number of valence electrons) - (Number of lone pair electrons) - (Number of shared electrons/2)

Formal charge on Carbon (C) = 4 - 0 - (8/2) = 0

Formal charge on Nitrogen (N) = 5 - 6 - (8/2) = 0

Formal charge on Oxygen (O) = 6 - 4 - (4/2) = 0

Therefore, the formal charges on carbon (C), nitrogen (N), and oxygen (O) are all zero (0).

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