Final answer:
The ranking of amine derivatives based on acidity is determined by their pKa values; lower pKa values indicate higher acidity. Amines with electron-withdrawing groups will be more acidic (lower pKa), while those with electron-donating substituents will be less acidic (higher pKa). Specific rankings require details about the substituent effects on the amine.
Step-by-step explanation:
The question asks to rank the amine derivatives based on their acidity levels, represented by their pKa values. Amine derivatives with the lowest pKa values have the highest acidity. To determine the order of acidity, we can look at the general pKa range for amines and consider any additional groups present that may affect the acidity. Amines typically have a pKa around 40 for their conjugate acid (–NH3+), making them weak acids. However, if an amine has electron-withdrawing groups attached, the acidity may increase as the pKa value decreases. On the other hand, electron-donating groups will generally decrease the acidity, increasing the pKa value.
The ompounds are to be arranged in order of decreasing acid strength and increasing base strength. Acid strength is gauged by the tendency to donate a proton, with a lower pKa indicating stronger acid. Base strength is given by the ability to accept a proton, and stronger bases will have a higher pKa of their conjugate acid.
A specific ranking of amine derivatives is not possible without the actual chemical structures or substituent effects. For basic amino acids such as lysine, the side chain amine group contributes to its basicity and solubility. Acidic amino acids, with an additional carboxyl group in the side chain, will have increased acidity.