Amide
can also refer
to a conjugate base of ammonia and an organic amine, represented as anions R2N–. For discussion of these "anionic amides," see the
articles sodium amide and lithium diisopropilamide.
The simplest amides are derivatives of
ammonia wherein one hydrogen atom has been replaced by an acyl group. The ensemble is generally represented
as RC(O)NH2. Closely related and even more numerous are amides
derived from primary amines (R'NH2) with the formula RC(O)NHR'.
Amides are also commonly derived from secondary amides (R'RNH) with the formula
RC(O)NR'R. Amide are usually regarded as derivatives of carboxylic acid in which the hydroxil group has been replaced by
an amine or ammonia.
Properties
Basicity
Compared to amines, amides are very weak bases. While the conjugate acid of an amines has a pKa of about 9.5, the conjugate acid of an amide has a pKa
around -0.5. Therefore amides don't have as clearly noticeable acid-base properties in water. This lack of basicity is explained by the electron-withdrawing nature of the carbonyl group where the lone pair of electrons on the nitrogen is delocalized by resonance.
On the other hand, amides are much stronger bases than carboxylic, esters, aldehyde, and ketones (conjugated acid pKa between -6 and -10). It
is estimated in silico that acetamide is represented by resonance structure A for 62% and by B for 28%. Resonance is largely
prevented in the very strained quinuclidone.
Because of the greater electronegativity of
oxygen, the carbonyl (C=O) is a stronger dipole than the N-C dipole. The
presence of a C=O dipole and, to a lesser extent a N-C dipole, allows amides to
act as H-bond acceptors. In primary and secondary amides, the presence of N-H
dipoles allows amides to function as H-bond donors as well. Thus amides can
participate in hydrogen bonding with water and other protic solvents; the
oxygen atom can accept hydrogen bonds from water and the N-H hydrogen atoms can
donate H-bonds. As a result of interactions such as these, the water solubility
of amides is greater than that of corresponding hydrocarbons.
The proton of a primary or secondary amide
does not dissociate readily under normal conditions; its pKa is usually well above 15.
Conversely, under extremely acidic conditions, the carbonyl oxygen can become protonated with a pKa of roughly –1.
Solubility
The solubilities of amides and esters are
roughly comparable. Typically amides are less soluble than comparable amines
and carboxylic acids since these compounds can both donate and accept hydrogen
bonds. Tertiary amides, with the important exception of N,N-dimethylformamide,
exhibit low solubility in water.
Characterization
The presence of the functional group is
generally easily established, at least in small molecules. They are the most
common non-basic functional group. They can be distinguished from nitro and
cyano groups by their IR specta. Amides exhibit a moderately
intense νCO band near 1650 cm−1. By 1H NMR spectroscopy, CONHR signals
occur at low fields. In X-ray crystallography, the C(O)N center together with
the three immediately adjacent atoms characteristically define a plane.
Applications and occurrence
Amides are pervasive in nature and technology
as structural materials. The amide linkage is easily formed, confers structural
rigidity, and resists hydrolisis. Nylons are polyamides as are
the very resilient materials Aramid, Twaron, and Kevlar. Amide
linkages in a biochemical context are called peptide linkage. Amide linkages
constitute a defining molecular feature of proteins, the secondary structure of which is due in part to the hydrogen bonding abilities of amides. Low
molecular weight amides, such as dimethylformamide (HC(O)N(CH3)2),
are common solvents. Many drugs are amides, including penicilin and LSD.
Amide synthesis
Amides are commonly formed via reactions of a carboxylic acid with an amine. Many methods are known for driving the unfavorable
equilibrium to the right:
RCO2H + R'R"NH RC(O)NR'R" + H2O
For the most part, these
reactions involve "activating" the carboxylic acid and the best known
method, the Schotten-bouman reaction, which involves conversion of the acid to the acid chlorides.
Amides are commonly formed via reactions of a carboxylic acid with an amine. Many methods are Hi Rarra canti, here I'm Via ***** wants t ask about your blog, as i known for driving the unfavorable equilibrium to the right:
BalasHapusRCO2H + R'R"NH \overrightarrow{\leftarrow} RC(O)NR'R" + H2O
tell me why can it happen?
compare the amines, amides are very weak bases. in the other hand, amides are more stronger bases than carboxylic acid, ester, aldehides, and ketone. why could it happen?
BalasHapus