Answer:
The second structure is the most stable of all three.
Explanation:
The Formal Charge in the different resonance structures of HCNO is,
[tex]\rm FC=V-N+B[/tex]
Where,
FC- Formal charge
V- Valence Electron
N- Non-bonding Electron
B- Number of bonds
So, Formal charge In the atoms of first resonance structure is
H = 1-0+1=0
C = 4 -4+2 = -2
N = 5 - 0+4 = 1
O = 6 - 2 + 3 = 1
Formal charge In the atoms of Second resonance structure is
H = 1-0+1 = 0
C = 4 - 0 + 4 =0
N = 5 - 0 + 4 = 1
O = 6 - 6+1 = -1
Formal charge In the atoms of Third resonance structure is
H = 1-0 + 1 = 0
C = 4 - 2 +3 = -1
N = 5 - 0 + 4 = 1
O = 6 - 4 +2 = 0
To Figure out the most stable resonance structure we have to keep two things in mind:
1) The stable molecular structure tend to have the least number of charged atom.
2) In a stable molecular structure the negative charge is present in the more electronegative atom.
Here decreasing order of electronegativity is,
N > O > C > H
From the Explanation above, the second structure (B) follows both points
Therefore, The second structure is the most stable of all three.
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