Editing Amine (section)

==Basicity==
Like ammonia, amines are [[base (chemistry)|bases]].<ref>{{cite book|chapter=Basicity and complex formation|title= Patai's Chemistry of Functional Groups|pages= 161–204|editor=S. Patai|year=1968|author=J. W. Smith|doi=10.1002/9780470771082.ch4|isbn= 9780470771082}}</ref> Compared to alkali metal hydroxides, amines are weaker.

{| class="wikitable" style="float:center; margin:0 1em;"
|-
!Alkylamine<ref>{{Cite journal | last1 = Hall | first1 = H. K. | title = Correlation of the Base Strengths of Amines | doi = 10.1021/ja01577a030 | journal = Journal of the American Chemical Society | volume = 79 | issue = 20 | pages = 5441–5444 | year = 1957 | bibcode = 1957JAChS..79.5441H }}</ref> or aniline<ref>{{Cite journal | last1 = Kaljurand | first1 = I. | last2 = Kütt | first2 = A. | last3 = Sooväli | first3 = L. | last4 = Rodima | first4 = T. | last5 = Mäemets | first5 = V. | last6 = Leito | first6 = I. | last7 = Koppel | first7 = I. A. | doi = 10.1021/jo048252w | title = Extension of the Self-Consistent Spectrophotometric Basicity Scale in Acetonitrile to a Full Span of 28 pKa Units: Unification of Different Basicity Scales | journal = The Journal of Organic Chemistry | volume = 70 | issue = 3 | pages = 1019–1028 | year = 2005 | pmid =  15675863}}</ref>
! pK<sub>a</sub> of <br />protonated amine
! ''K''<sub>b</sub>{{Clarify|date=April 2022}}
|-
| [[Methylamine]] (MeNH<sub>2</sub>)
| 10.62
| {{val|4.17e-4}}
|-
| [[Dimethylamine]] (Me<sub>2</sub>NH)
| 10.64
| {{val|4.37e-4}}
|-
| [[Trimethylamine]] (Me<sub>3</sub>N)
| {{pad|0.3em}}9.76
| {{val|5.75e-5}}
|-
| [[Ethylamine]] (EtNH<sub>2</sub>)
| 10.63
| {{val|4.27e-4}}
|-
| [[Aniline]] (PhNH<sub>2</sub>)
| {{pad|0.3em}}4.62
| {{val|4.17e-10}}
|-
| [[p-Anisidine|4-Methoxyaniline]] (4-MeOC<sub>6</sub>H<sub>4</sub>NH<sub>2</sub>)
| {{pad|0.3em}}5.36
| {{val|2.29e-9}}
|-
| [[Dimethylaniline|''N'',''N''-Dimethylaniline]] (PhNMe<sub>2</sub>)
| {{pad|0.3em}}5.07
| {{val|1.17e-9}}
|-
| [[3-Nitroaniline]] (3-NO<sub>2</sub>-C<sub>6</sub>H<sub>4</sub>NH<sub>2</sub>)
| {{pad|0.3em}}2.46
| {{val|2.88e-12}}
|-
| [[4-Nitroaniline]] (4-NO<sub>2</sub>-C<sub>6</sub>H<sub>4</sub>NH<sub>2</sub>)
| {{pad|0.3em}}1.00
| {{val|1.00e-13}}
|-
| 4-Trifluoromethylaniline (CF<sub>3</sub>C<sub>6</sub>H<sub>4</sub>NH<sub>2</sub>)
| {{pad|0.3em}}2.75
| {{val|5.62e-12}}
|}

The basicity of amines depends on:
# The electronic properties of the substituents (alkyl groups enhance the basicity, aryl groups diminish it).
# The degree of solvation of the protonated amine, which includes [[steric hindrance]] by the groups on nitrogen.

===Electronic effects===
Owing to inductive effects, the basicity of an amine might be expected to increase with the number of alkyl groups on the amine.  Correlations are complicated owing to the effects of solvation which are opposite the trends for inductive effects. Solvation effects also dominate the basicity of aromatic amines (anilines). For anilines, the lone pair of electrons on nitrogen delocalizes into the ring, resulting in decreased basicity.  Substituents on the aromatic ring, and their positions relative to the amino group, also affect basicity as seen in the table.

===Solvation effects===
Solvation significantly affects the basicity of amines.  N-H groups strongly interact with water, especially in ammonium ions. Consequently, the basicity of ammonia is enhanced by 10<sup>11</sup> by solvation. The intrinsic basicity of amines, i.e. the situation where solvation is unimportant, has been evaluated in the gas phase.  In the gas phase, amines exhibit the basicities predicted from the electron-releasing effects of the organic substituents.  Thus tertiary amines are more basic than secondary amines, which are more basic than primary amines, and finally ammonia is least basic.  The order of pK<sub>b</sub>'s (basicities in water) does not follow this order.  Similarly aniline is more basic than ammonia in the gas phase, but ten thousand times less so in aqueous solution.<ref>{{March6th}}</ref>

In aprotic polar solvents such as [[Dimethyl sulfoxide|DMSO]], [[Dimethylformamide|DMF]], and [[acetonitrile]] the energy of solvation is not as high as in protic polar solvents like water and methanol.  For this reason, the basicity of amines in these aprotic solvents is almost solely governed by the electronic effects.