JEE Main 2026 Jan 22 Shift 1, Chemistry Q2: Important Concepts Of Chemical Bonding

JEE Main2026Jan 22, Shift 1Chemistry

The formal changes on the atoms marked as (1) to (4) in the Lewis representation of $H n O_{3}$ molecule respectively are

Solution

Apply $Formal charge = valence electrons - non-bonding electrons - \frac{bonding electrons}{2}$ to each labelled atom.

Atom 1 (O bonded to H and to N by single bonds, 2 lone pairs): $6 - 4 - 4/2 \cdot 2 = 6 - 4 - 2 = 0$ .

Atom 2 (central N, three bonds: one single to OH, one double to O(3), one single to O(4), no lone pair): $5 - 0 - 8/2 = 5 - 4 = + 1$ .

Atom 3 (O doubly bonded to N, 2 lone pairs): $6 - 4 - 4/2 = 6 - 4 - 2 = 0$ .

Atom 4 (O singly bonded to N, 3 lone pairs): $6 - 6 - 2/2 = 6 - 6 - 1 = - 1$ .

So the charges in order are $0, + 1, 0, - 1$ .

Concept behind this question

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