Glycine exists as `(H_(3)N^(+)CH_(2)COO^(-))` while anthranilic acid `(P-NH_(2)-C_(6)H_(4)-COOH)` does not exist as dipolar ion.

Explanation

To understand why glycine exists as a dipolar ion while anthranilic acid does not, we can break down the reasoning into several steps:

### Step 1: Understanding Glycine Structure
Glycine is the simplest amino acid with the formula \( H_2NCH_2COOH \). In its dipolar ion form, it can be represented as \( H_3N^+CH_2COO^- \).

### Step 2: Basic and Acidic Groups in Glycine
In glycine, the amino group (\( NH_2 \)) can accept a proton (H+) due to its basic nature, while the carboxylic acid group (\( COOH \)) can donate a proton, making it acidic. When glycine is in solution, it can exist in a form where the amino group is protonated (NH3+) and the carboxylic group is deprotonated (COO-), resulting in the dipolar ion.

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