Show how one could synthesize-and resolve methylethylallylamine oxide from allylamine, with the knowledge that amine oxides are somewhat basic substances having \(\mathrm{K}_{\mathrm{B}}\) values at about \(10^{-11}\).

First, we need to determine the chemical structures of both compounds: - Allylamine (\( H_2C=CH-CH_2NH_2 \)) is an organic compound with a double bond between the first and second carbons and an amine group on the third carbon. - Methylethylallylamine oxide (\( CH_3CH_2NHCH_2CH=CH_2 \)) has a methyl group (CH3) and ethyl group (CH2CH3) attached to the nitrogen atom and is an oxide.

The main difference between the two structures is that allylamine (\(H_2C=CH-CH_2NH_2\)) contains only an amine group, while methylethylallylamine oxide (\( CH_3CH_2NHCH_2CH=CH_2\)) has an amine group with a methyl group and an ethyl group attached to the nitrogen atom.

To convert allylamine into methylethylallylamine oxide, we need to perform two reactions: 1. Alkylation: The first reaction is the alkylation of allylamine, in which we add both a methyl group and an ethyl group to the nitrogen atom. Following are the reagents and conditions required for this reaction: - Allylamine - Methyl iodide (CH3I) and sodium ethoxide (NaOEt) as alkylating agents - Anhydrous conditions and an inert solvent, such as THF or DCM - Low temperature to control the extent of alkylation The reaction will be as follows: \( H_2C=CH-CH_2NH_2 + CH_3I + NaOEt \rightarrow CH_3CH_2NHCH_2CH=CH_2 + NaI + H_2O \) 2. Oxidation: The second reaction is the oxidation of the amine to form the amine oxide: - Methylethylallylamine as the substrate - Hydrogen peroxide (H2O2) as an oxidizing agent - A weak base such as sodium bicarbonate (NaHCO3) to maintain the pH of the reaction mixture The reaction will be as follows: \( CH_3CH_2NHCH_2CH=CH_2 + H_2O_2 \rightarrow CH_3CH_2N(CH_2CH=CH_2)O + H_2O \)

Amine oxides are somewhat basic substances, with \(\mathrm{K}_{\mathrm{B}}\) values around \(10^{-11}\). The basicity of amine oxides arises from the lone pair of electrons on the nitrogen atom, which can act as a Lewis base and accept a proton (H+) from an acid, forming a conjugate acid. However, since amine oxides have a partial positive charge on the nitrogen atom due to the oxygen atom's higher electronegativity, their basicity is weaker than that of the corresponding amines.