Amines: Organic compounds derived from ammonia, characterized by the presence of nitrogen.
Properties: Amines contain polar bonds, enabling primary and secondary amines to form hydrogen bonds with each other and with water, contributing to their solubility.
Types of Amines:
Primary and Secondary Amines: Able to form hydrogen bonds with both water molecules and each other.
Tertiary Amines: Can only form hydrogen bonds with water, not with themselves.
Strength of Bonds: Hydrogen bonds in amines are weaker than those in alcohols due to nitrogen's lower electronegativity compared to oxygen.
Comparative Boiling Points:
Amines have higher boiling points than alkanes but lower than alcohols.
Primary Amines: Can form more hydrogen bonds, resulting in higher boiling points than secondary amines of similar mass.
Tertiary Amines: Do not form hydrogen bonds with each other, leading to lower boiling points compared to primary and secondary amines of the same mass.
Hydrogen Bonding: Amines with polar bonds can create hydrogen bonds with water.
Solubility Considerations: Amines containing one to six carbon atoms, including tertiary amines, are generally soluble in water.
Effect of Carbon Atoms: As the carbon chain in amines increases, the nonpolar characteristics of the hydrocarbon portion diminish hydrogen bonding effects, decreasing solubility.
Diagram: Illustrates interactions between primary, secondary, and tertiary amines with water through hydrogen bonding.
Amines with over Six Carbon Atoms:
Diminished impact of hydrogen bonding.
Increased nonpolar hydrocarbon chain reduces solubility in water.
Question: Identifies various compounds and asks which are soluble in water.
Answer Options: A and B are soluble in water; C (an alkane) is not, and D (an amine with over six carbons) is not soluble in water.
Role as Bases: Amines exhibit behavior as Brønsted–Lowry bases.
Mechanism: The lone pair on nitrogen accepts a proton from water, resulting in an ammonium ion and a hydroxide ion.
Formation of Amine Salts: Occurs when amines with odors (like fish) react with acids.
Chemical Reaction: As amines react as Brønsted–Lowry bases, they form ammonium salts that eliminate unpleasant odors.
Acid and Amine Interaction:
Amine acts as a base; nitrogen's lone pair receives a proton from the acid to form an ammonium salt without the generation of water.
Nomenclature: Named by combining the alkylammonium ion with the anion’s name.
Chemical Equations:
Methylamine + HCl → Methylammonium chloride
Dimethylamine + HCl → Dimethylammonium chloride
Definition: A nitrogen atom is bonded to four carbon groups, classifying it as a quaternary amine.
Charge: The nitrogen carries a positive charge and is not bonded to any hydrogen atoms.
Example: Choline, a quaternary ammonium ion found in glycerophospholipids.
Characteristics:
Ionic nature results in strong attraction between the ammonium ion and anions (often chloride).
Generally solids at room temperature, odorless, and soluble in both water and biological fluids.
Often, amines are converted to ammonium salts for medicinal applications.
Active Ingredients: Examples include:
Ephedrine: A bronchodilator in Sudafed.
Diphenylhydramine: Found in Benadryl for skin irritation relief.
Cocaine Hydrochloride: An ammonium salt that is often smuggled and used illegally.
Free Base Form: Crack cocaine, a solid product absorbed rapidly when smoked, leading to stronger effects than hydrochloride form.
Conversion Process: Cocaine hydrochloride can be reverted back to its free amine or base form, known as crack cocaine, via treatment with a strong base.
Task: Draw the structural formula for the ammonium salt formed from trimethylamine and HCl.
Answer: Structural formula for the compound resulting from the reaction of trimethylamine and HCl.