Amines, organic compounds with a nitrogen atom, play a crucial role in chemistry. Their unique structure, featuring a of electrons on nitrogen, gives them special properties. These properties influence their behavior in reactions and their physical characteristics.
Understanding amines is key to grasping many organic reactions. From their to their ability to undergo , amines showcase fascinating chemical behavior. Their solubility and also set them apart from other organic compounds, highlighting their importance in various applications.
Structure and Properties of Amines
Bonding and geometry of alkylamines
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contain nitrogen atom bonded to carbon atoms
Nitrogen is resulting in around nitrogen atom (ammonia, methylamine)
Lone pair on nitrogen occupies one of four sp³ hybrid orbitals
in alkylamines slightly less than ideal 109.5° due to lone pair-bond pair repulsion
Typical bond angles range from 106° to 108° (trimethylamine, triethylamine)
Nitrogen-carbon (N-C) bond lengths in alkylamines approximately 1.47 Å
Slightly shorter than carbon-carbon (C-C) single bond length of 1.54 Å due to higher electronegativity of nitrogen compared to carbon
Pyramidal inversion in amines
process where nitrogen atom in amine passes through plane formed by three substituents attached to it
Lone pair on nitrogen changes orientation during this process
Energy barrier for pyramidal inversion relatively low, typically around 24-26 kJ/mol (6-7 kcal/mol)
Rapid pyramidal inversion in amines at room temperature has consequences for
If amine has three different substituents attached to nitrogen atom, it can potentially be chiral
However, due to fast inversion, rapidly interconvert making it impossible to isolate individual enantiomers at room temperature (methylethylamine, methylisopropylamine)
Pyramidal inversion can be slowed down or prevented by:
Increasing size of substituents on nitrogen atom, which raises energy barrier for inversion ()
Lowering temperature, which reduces kinetic energy available for inversion
Protonating amine, which eliminates lone pair and prevents inversion ()
Physical properties of amines vs organics
Solubility:
Amines more soluble in water compared to hydrocarbons of similar molecular weight due to ability to form with water (ethylamine vs ethane)
Solubility of amines in water decreases as size of alkyl group increases, as nature of alkyl group becomes more dominant (octylamine vs ethylamine)
Amines less soluble in water than alcohols of similar molecular weight because amines have one less hydrogen bond donor site () compared to alcohols () (ethylamine vs ethanol)
Boiling points:
Amines have higher boiling points than hydrocarbons of similar molecular weight due to presence of intermolecular hydrogen bonding between amine molecules (propylamine vs propane)
Boiling points of amines increase with increasing molecular weight and surface area, as strength of intermolecular forces increases (ethylamine vs butylamine)
have higher boiling points than , which in turn have higher boiling points than (ethylamine vs diethylamine vs triethylamine)
Trend due to decreasing number of N-H hydrogen bond donor sites from primary to tertiary amines
Amines have lower boiling points than alcohols of similar molecular weight because N-H···N hydrogen bond is weaker than O-H···O hydrogen bond in alcohols (propylamine vs propanol)
Chemical properties of amines
Basicity: Amines are generally basic due to the lone pair of electrons on the nitrogen atom, which can accept a proton
: The lone pair also makes amines good nucleophiles, allowing them to participate in various reactions
: A reaction where undergo elimination to form alkenes
: A method used to distinguish between primary, secondary, and tertiary amines based on their reactivity with benzenesulfonyl chloride