Carbamic acid, ion(1-) (H2NCOO?) is the conjugate base of carbamic acid. Here is its lewis structure and steps to draw it.

Step 1: Calculate total valence electrons

N: 5; C: 4; O: 6 × 2 = 12; H: 1 × 2 = 2;

Carries a net negative charge of 1; add 1 extra electron.

Total valence electrons: 5 + 4 + 12 + 2 + 1 = 26 e?

Step 2: Skeleton arrangement and central atom

Carbon serves as the central skeletal atom, bonding to the NH? group and two oxygen atoms; resonance exists (the C=O double bond alternates between the two oxygen atoms).

Step 3: Construct all σ bonds

List of σ bonds: 2 N-H, 1 N-C, 1 C-O, 1 C-O; total of 5 σ bonds.

Bonding electrons: 5 × 2 = 10 e?

Remaining electrons: 26 - 10 = 16 e?

Step 4: Introduce a double bond to form the resonance structure with lower formal charges

Optimal structure: 1 C=O double bond, 1 C-O single bond.

Total bonding electrons: 10 (σ) + 2 (π) = 12 e?

Remaining electrons: 26 - 12 = 14 e?

Step 5: Assign lone pairs to all peripheral atoms

N in NH?: 3 σ bonds (2 N-H, 1 N-C); requires 1 lone pair (2 e?) to satisfy the octet rule;

Double-bonded O: 4 bonding electrons; assign 2 lone pairs (4 e?);

Single-bonded O (negative charge): 2 bonding electrons; assign 3 lone pairs (6 e?);

Total lone pair electrons: 2 + 4 + 6 = 12 e?

Remaining electrons: 14 - 12 = 2 e?; no electrons remaining.

Total electron check: 12 (bonding) + 14 (lone pair) = 26 e?; matches the total valence electron count.