Basic nature of amines is due to the presence of lone pair of electrons on nitrogen atom which is available for the bond formation with Lewis acid. Due to the +I-effect, \(2^{\circ}\) amine is more basic than \(1^{\circ}\) amine and \(\mathrm{NH}_{3}\). In case of aromatic amines, the lone pair on nitrogen atom are involved in resonance, therefore not available for bond formation, so aromatic amines are less basic.Hence, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) is the strongest base among the given options.
CHXII13:AMINES
324064
Increasing \(\mathrm{pK}_{\mathrm{b}}\) values of \(\mathrm{o}-, \mathrm{m}\) - and \(\mathrm{p-}\) toluidines is
1 p \( < \) m \( < \) o
2 o \( < \) m \( < \) p
3 p \( < \) o \( < \) m
4 m \( < \) o \( < \) p
Explanation:
The basicity of o-, m-and p-toluidines decreases in the order \(\mathrm{p}>\mathrm{m}>\mathrm{o}\). In other words, their \(\mathrm{pK}_{\mathrm{b}}\) values will increase in the reverse order, i.e., \(\mathrm{p} < \mathrm{m} < \) o.
CHXII13:AMINES
324065
The correct statement regarding the basicity of arylamines is:
1 Arylamines are generally more basic than alkyl amines, because the nitrogen atom in arylamines is sp-hybridized.
2 Arylamine are generally less basic than alkyl amine because the nitrogen lone-pair electrons are delocalised by interaction with the aromatic ring \(\pi\)-electron system.
3 Arylamines are generally more basic than alkyl amines because the nitrogen lone-pair electrons are not delocalised by interaction with the aromatic ring \(\pi\)-electron system.
4 Arylamines are generally more basic than alkyl amines because of aryl group.
Explanation:
delocalised lone pair of nirogen atom of arylamine with benzene ring in aryl amine. \({\rm{R}}\mathop {\rm{N}}\limits^{..} {{\rm{H}}_{\rm{2}}} \to \) lone pair of electrons of nitrogen atom are not delocalized in alkyl amine.
NEET - 2016
CHXII13:AMINES
324066
Aniline dissolves in \(\mathrm{HCl}\) due to the formation of
Basic nature of amines is due to the presence of lone pair of electrons on nitrogen atom which is available for the bond formation with Lewis acid. Due to the +I-effect, \(2^{\circ}\) amine is more basic than \(1^{\circ}\) amine and \(\mathrm{NH}_{3}\). In case of aromatic amines, the lone pair on nitrogen atom are involved in resonance, therefore not available for bond formation, so aromatic amines are less basic.Hence, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) is the strongest base among the given options.
CHXII13:AMINES
324064
Increasing \(\mathrm{pK}_{\mathrm{b}}\) values of \(\mathrm{o}-, \mathrm{m}\) - and \(\mathrm{p-}\) toluidines is
1 p \( < \) m \( < \) o
2 o \( < \) m \( < \) p
3 p \( < \) o \( < \) m
4 m \( < \) o \( < \) p
Explanation:
The basicity of o-, m-and p-toluidines decreases in the order \(\mathrm{p}>\mathrm{m}>\mathrm{o}\). In other words, their \(\mathrm{pK}_{\mathrm{b}}\) values will increase in the reverse order, i.e., \(\mathrm{p} < \mathrm{m} < \) o.
CHXII13:AMINES
324065
The correct statement regarding the basicity of arylamines is:
1 Arylamines are generally more basic than alkyl amines, because the nitrogen atom in arylamines is sp-hybridized.
2 Arylamine are generally less basic than alkyl amine because the nitrogen lone-pair electrons are delocalised by interaction with the aromatic ring \(\pi\)-electron system.
3 Arylamines are generally more basic than alkyl amines because the nitrogen lone-pair electrons are not delocalised by interaction with the aromatic ring \(\pi\)-electron system.
4 Arylamines are generally more basic than alkyl amines because of aryl group.
Explanation:
delocalised lone pair of nirogen atom of arylamine with benzene ring in aryl amine. \({\rm{R}}\mathop {\rm{N}}\limits^{..} {{\rm{H}}_{\rm{2}}} \to \) lone pair of electrons of nitrogen atom are not delocalized in alkyl amine.
NEET - 2016
CHXII13:AMINES
324066
Aniline dissolves in \(\mathrm{HCl}\) due to the formation of
Basic nature of amines is due to the presence of lone pair of electrons on nitrogen atom which is available for the bond formation with Lewis acid. Due to the +I-effect, \(2^{\circ}\) amine is more basic than \(1^{\circ}\) amine and \(\mathrm{NH}_{3}\). In case of aromatic amines, the lone pair on nitrogen atom are involved in resonance, therefore not available for bond formation, so aromatic amines are less basic.Hence, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) is the strongest base among the given options.
CHXII13:AMINES
324064
Increasing \(\mathrm{pK}_{\mathrm{b}}\) values of \(\mathrm{o}-, \mathrm{m}\) - and \(\mathrm{p-}\) toluidines is
1 p \( < \) m \( < \) o
2 o \( < \) m \( < \) p
3 p \( < \) o \( < \) m
4 m \( < \) o \( < \) p
Explanation:
The basicity of o-, m-and p-toluidines decreases in the order \(\mathrm{p}>\mathrm{m}>\mathrm{o}\). In other words, their \(\mathrm{pK}_{\mathrm{b}}\) values will increase in the reverse order, i.e., \(\mathrm{p} < \mathrm{m} < \) o.
CHXII13:AMINES
324065
The correct statement regarding the basicity of arylamines is:
1 Arylamines are generally more basic than alkyl amines, because the nitrogen atom in arylamines is sp-hybridized.
2 Arylamine are generally less basic than alkyl amine because the nitrogen lone-pair electrons are delocalised by interaction with the aromatic ring \(\pi\)-electron system.
3 Arylamines are generally more basic than alkyl amines because the nitrogen lone-pair electrons are not delocalised by interaction with the aromatic ring \(\pi\)-electron system.
4 Arylamines are generally more basic than alkyl amines because of aryl group.
Explanation:
delocalised lone pair of nirogen atom of arylamine with benzene ring in aryl amine. \({\rm{R}}\mathop {\rm{N}}\limits^{..} {{\rm{H}}_{\rm{2}}} \to \) lone pair of electrons of nitrogen atom are not delocalized in alkyl amine.
NEET - 2016
CHXII13:AMINES
324066
Aniline dissolves in \(\mathrm{HCl}\) due to the formation of
Basic nature of amines is due to the presence of lone pair of electrons on nitrogen atom which is available for the bond formation with Lewis acid. Due to the +I-effect, \(2^{\circ}\) amine is more basic than \(1^{\circ}\) amine and \(\mathrm{NH}_{3}\). In case of aromatic amines, the lone pair on nitrogen atom are involved in resonance, therefore not available for bond formation, so aromatic amines are less basic.Hence, \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{NH}\) is the strongest base among the given options.
CHXII13:AMINES
324064
Increasing \(\mathrm{pK}_{\mathrm{b}}\) values of \(\mathrm{o}-, \mathrm{m}\) - and \(\mathrm{p-}\) toluidines is
1 p \( < \) m \( < \) o
2 o \( < \) m \( < \) p
3 p \( < \) o \( < \) m
4 m \( < \) o \( < \) p
Explanation:
The basicity of o-, m-and p-toluidines decreases in the order \(\mathrm{p}>\mathrm{m}>\mathrm{o}\). In other words, their \(\mathrm{pK}_{\mathrm{b}}\) values will increase in the reverse order, i.e., \(\mathrm{p} < \mathrm{m} < \) o.
CHXII13:AMINES
324065
The correct statement regarding the basicity of arylamines is:
1 Arylamines are generally more basic than alkyl amines, because the nitrogen atom in arylamines is sp-hybridized.
2 Arylamine are generally less basic than alkyl amine because the nitrogen lone-pair electrons are delocalised by interaction with the aromatic ring \(\pi\)-electron system.
3 Arylamines are generally more basic than alkyl amines because the nitrogen lone-pair electrons are not delocalised by interaction with the aromatic ring \(\pi\)-electron system.
4 Arylamines are generally more basic than alkyl amines because of aryl group.
Explanation:
delocalised lone pair of nirogen atom of arylamine with benzene ring in aryl amine. \({\rm{R}}\mathop {\rm{N}}\limits^{..} {{\rm{H}}_{\rm{2}}} \to \) lone pair of electrons of nitrogen atom are not delocalized in alkyl amine.
NEET - 2016
CHXII13:AMINES
324066
Aniline dissolves in \(\mathrm{HCl}\) due to the formation of
