With the help of `F.C`. Explain which Lewis structure is more stable for the following molecules :
(a) `N_(2)O: (i) :^(Theta)ddotN =overset(2+)O=ddotN:^(Theta) or (ii) :N -=overset(o+)N-ddotunderset(..)O:^(Theta)`
(b). `H_(2)SO_(4): (i) H-O-overset( :ddotO:^(Theta))overset(|)underset(Theta)underset( :underset(..)O: )underset(|)(S^(+2))-O-H or (ii) H-O-underset( underset(..):O)underset(||)overset(ddotO: )overset(||)S-O-H`
`HNO_(3)(i) H-O-underset(Theta)underset( :underset(..)O: )underset(|)overset(o+)N=ddotO: or (ii) H-O-underset(underset(..):O:_(Theta))underset(|)overset(+2)N-underset(..)ddotO:^(Theta)`
(d). `CI_(2)O: (i) underset(..):ddotCI-ddotunderset(..)O-underset(..)ddotCI: or (ii) :underset(..)ddotO-underset(..)ddot(CI)-underset(..)ddotCI:`

Explanation

To determine the stability of the Lewis structures for the given molecules using formal charge (F.C.), we will analyze each molecule step by step.

### (a) N₂O

1. **Structure (i):**
- :^(Theta)N = O^(2+) = N:
- Formal charges:
- Nitrogen (left): 5 (valence) - 0 (non-bonding) - 4/2 (bonding) = 5 - 0 - 2 = +3
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