Total Number of Basic Groups in Lysine Form

To determine the total number of basic groups in the given form of lysine, we analyze the structure provided:

$\overset{\oplus}{\text{H}_3\text{N}}-\text{CH}_2-\text{CH}_2-\text{CH}_2-\text{CH}_2-\underset{\substack{|\text{NH}_2}}{\text{CH}}-\text{C}\text{O}\text{O}^\ominus$

A basic group, according to the Brønsted-Lowry definition, is a chemical species capable of accepting a proton ($\text{H}^+$) due to the presence of an available lone pair of electrons or a negative charge.

Let's evaluate each functional group present in the structure:

1. Unprotonated $\alpha$-amino group ($-\text{NH}_2$):
   The nitrogen atom has a lone pair of electrons that can readily accept a proton to form $-\text{NH}_3^+$. Therefore, it acts as a basic group.

2. Carboxylate anion ($-\text{COO}^\ominus$):
   The carboxylate group possesses a negative charge and can accept a proton to convert into a neutral carboxylic acid group ($-\text{COOH}$). Therefore, it acts as a basic group.

3. Protonated $\epsilon$-amino group ($-\overset{\oplus}{\text{H}_3\text{N}}$):
   This group is already protonated and carries a positive charge without any available lone pair for accepting another proton. Thus, it acts as an acidic group (proton donor), not a basic group.

Thus, the total number of basic groups in the given form of lysine is $2$ ($-\text{NH}_2$ and $-\text{COO}^\ominus$).