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A

Anonymous

Jan 07, 2025

Determine the formal charge on each atom in each of the following molecules or ions.?

Determine the formal charge on each atom in the following molecules or ions:

(a) SCO (sulfur carbon monoxide)
(b) NO3⁻ (nitrate ion) - N with a +1 charge, one O attached by a double bond, and two O atoms
(c) CS2 (carbon disulfide)
(d) HCO2H (formic acid) - H, C, O, O, H

Please provide the formal charges for each atom in these structures.

4 Answers

A
Anonymous

Feb 06, 2025

KEY: = is a double bond, – is a single bond

(a) SCO has 16 valence electrons. S=C=O

S and O have two unshared electrons.

According to what the other girl said,

S, C, and O all have a formal charge of ZERO.

(b) 24 valence electrons

2 N-O bonds, 1 N=O bond

N: formal charge of 1

O single bond: formal bond of -1

O=double bond: formal charge of 0

(c) 16 valence electrons

S=C=S

Carbon: formal charge of 0

Sulfur: formal charge of 0 (it has four unshared electrons)

(d) C-O, C-H, C=O-H (combine these, sry)

Carbon: 0 formal charge

Both Hydrogen: 0 formal charge

Single-bond oxygen: -1 formal charge

Double-bond oxygen: +1 formal charge

Hope this helps!

Draw the Lewis structures for each, and the formal charge on each atom will be:

FC = # of valence electrons on atom – # of lone pair electrons on the atom – half of the atom’s shared electrons.

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