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
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!
Dec 21, 2024
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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