231482
The only o p-directing group which is deactivating in nature is
1 $-\mathrm{NH}_{2}$
2 $-\mathrm{OH}$
3 $-\mathrm{X}$ (halogens)
4 $-\mathrm{R}$ (alkyl groups)
Explanation:
The $-\mathrm{NH}_{2}$, :ỌH and $-\mathrm{R}$ (alkyl group) is activate the $o$ and $p$ position. Because it have $+M,+M$ and $+\mathrm{I}$ effect respectively. But the $-\mathrm{X}$ have $-\mathrm{I}$ and $+\mathrm{M}$ effect hence $-\mathrm{I}$ effect deactivate the $-\mathrm{O}$ and $-\mathrm{p}$ position. Hence, (c) option is correct.
JIPMER-2010
GENERAL ORGANIC CHEMISTRY
231498
The correct order of increasing basic nature for the bases $\mathrm{NH}_{3}, \mathrm{CH}_{3} \mathrm{NH}_{2}$ and $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}$ in aqueous solutions
Steric Hindrance to H-bonding occur if the alkyl group is bigger than $\mathrm{CH}_{3}$. Hence, $+\mathrm{I}$ effect predominant over H-bonding. Alkyl group is greatly influenced by inductive effect, solvation effect $\&$ steric hindrance which decide strength of akyl amine in aqeous state.
Karnataka CET-2017
GENERAL ORGANIC CHEMISTRY
231510
Chloroacetic acid is a stronger acid than acetic acid. This can be explained using :
1 $-\mathrm{M}$ effect
2 - I effect
3 + M effect
4 + I effect
Explanation:
$-\mathrm{Cl}$ is an electron withdrawing (ie, $-\mathrm{I}$ showing) group. It withdraws electrons when attached to the carboxylic acid and decreases the electron density on the oxygen atom. This will facilitate the release of $\mathrm{H}^{+}$by making $\mathrm{O}-\mathrm{H}$ bond more polar and thus $-\mathrm{Cl}$ increases the acidity of acetic acid when attached at, a position because of $-\mathrm{I}$ effect.
Karnataka CET
GENERAL ORGANIC CHEMISTRY
231515
The carbon-carbon bond length in benzene is
1 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$
2 same as in $\mathrm{C}_{2} \mathrm{H}_{4}$
3 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
4 in between $\mathrm{C}_{2} \mathrm{H}_{4}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
Explanation:
The carbon-carbon bond length in benzene $(1.39 \AA)$ is between that of $\mathrm{C}-\mathrm{C}(1.54 \AA)$ and $\mathrm{C}=\mathrm{C}$ $(1.34 \AA)$ ie, in between that of $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$.
231482
The only o p-directing group which is deactivating in nature is
1 $-\mathrm{NH}_{2}$
2 $-\mathrm{OH}$
3 $-\mathrm{X}$ (halogens)
4 $-\mathrm{R}$ (alkyl groups)
Explanation:
The $-\mathrm{NH}_{2}$, :ỌH and $-\mathrm{R}$ (alkyl group) is activate the $o$ and $p$ position. Because it have $+M,+M$ and $+\mathrm{I}$ effect respectively. But the $-\mathrm{X}$ have $-\mathrm{I}$ and $+\mathrm{M}$ effect hence $-\mathrm{I}$ effect deactivate the $-\mathrm{O}$ and $-\mathrm{p}$ position. Hence, (c) option is correct.
JIPMER-2010
GENERAL ORGANIC CHEMISTRY
231498
The correct order of increasing basic nature for the bases $\mathrm{NH}_{3}, \mathrm{CH}_{3} \mathrm{NH}_{2}$ and $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}$ in aqueous solutions
Steric Hindrance to H-bonding occur if the alkyl group is bigger than $\mathrm{CH}_{3}$. Hence, $+\mathrm{I}$ effect predominant over H-bonding. Alkyl group is greatly influenced by inductive effect, solvation effect $\&$ steric hindrance which decide strength of akyl amine in aqeous state.
Karnataka CET-2017
GENERAL ORGANIC CHEMISTRY
231510
Chloroacetic acid is a stronger acid than acetic acid. This can be explained using :
1 $-\mathrm{M}$ effect
2 - I effect
3 + M effect
4 + I effect
Explanation:
$-\mathrm{Cl}$ is an electron withdrawing (ie, $-\mathrm{I}$ showing) group. It withdraws electrons when attached to the carboxylic acid and decreases the electron density on the oxygen atom. This will facilitate the release of $\mathrm{H}^{+}$by making $\mathrm{O}-\mathrm{H}$ bond more polar and thus $-\mathrm{Cl}$ increases the acidity of acetic acid when attached at, a position because of $-\mathrm{I}$ effect.
Karnataka CET
GENERAL ORGANIC CHEMISTRY
231515
The carbon-carbon bond length in benzene is
1 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$
2 same as in $\mathrm{C}_{2} \mathrm{H}_{4}$
3 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
4 in between $\mathrm{C}_{2} \mathrm{H}_{4}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
Explanation:
The carbon-carbon bond length in benzene $(1.39 \AA)$ is between that of $\mathrm{C}-\mathrm{C}(1.54 \AA)$ and $\mathrm{C}=\mathrm{C}$ $(1.34 \AA)$ ie, in between that of $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$.
231482
The only o p-directing group which is deactivating in nature is
1 $-\mathrm{NH}_{2}$
2 $-\mathrm{OH}$
3 $-\mathrm{X}$ (halogens)
4 $-\mathrm{R}$ (alkyl groups)
Explanation:
The $-\mathrm{NH}_{2}$, :ỌH and $-\mathrm{R}$ (alkyl group) is activate the $o$ and $p$ position. Because it have $+M,+M$ and $+\mathrm{I}$ effect respectively. But the $-\mathrm{X}$ have $-\mathrm{I}$ and $+\mathrm{M}$ effect hence $-\mathrm{I}$ effect deactivate the $-\mathrm{O}$ and $-\mathrm{p}$ position. Hence, (c) option is correct.
JIPMER-2010
GENERAL ORGANIC CHEMISTRY
231498
The correct order of increasing basic nature for the bases $\mathrm{NH}_{3}, \mathrm{CH}_{3} \mathrm{NH}_{2}$ and $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}$ in aqueous solutions
Steric Hindrance to H-bonding occur if the alkyl group is bigger than $\mathrm{CH}_{3}$. Hence, $+\mathrm{I}$ effect predominant over H-bonding. Alkyl group is greatly influenced by inductive effect, solvation effect $\&$ steric hindrance which decide strength of akyl amine in aqeous state.
Karnataka CET-2017
GENERAL ORGANIC CHEMISTRY
231510
Chloroacetic acid is a stronger acid than acetic acid. This can be explained using :
1 $-\mathrm{M}$ effect
2 - I effect
3 + M effect
4 + I effect
Explanation:
$-\mathrm{Cl}$ is an electron withdrawing (ie, $-\mathrm{I}$ showing) group. It withdraws electrons when attached to the carboxylic acid and decreases the electron density on the oxygen atom. This will facilitate the release of $\mathrm{H}^{+}$by making $\mathrm{O}-\mathrm{H}$ bond more polar and thus $-\mathrm{Cl}$ increases the acidity of acetic acid when attached at, a position because of $-\mathrm{I}$ effect.
Karnataka CET
GENERAL ORGANIC CHEMISTRY
231515
The carbon-carbon bond length in benzene is
1 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$
2 same as in $\mathrm{C}_{2} \mathrm{H}_{4}$
3 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
4 in between $\mathrm{C}_{2} \mathrm{H}_{4}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
Explanation:
The carbon-carbon bond length in benzene $(1.39 \AA)$ is between that of $\mathrm{C}-\mathrm{C}(1.54 \AA)$ and $\mathrm{C}=\mathrm{C}$ $(1.34 \AA)$ ie, in between that of $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$.
231482
The only o p-directing group which is deactivating in nature is
1 $-\mathrm{NH}_{2}$
2 $-\mathrm{OH}$
3 $-\mathrm{X}$ (halogens)
4 $-\mathrm{R}$ (alkyl groups)
Explanation:
The $-\mathrm{NH}_{2}$, :ỌH and $-\mathrm{R}$ (alkyl group) is activate the $o$ and $p$ position. Because it have $+M,+M$ and $+\mathrm{I}$ effect respectively. But the $-\mathrm{X}$ have $-\mathrm{I}$ and $+\mathrm{M}$ effect hence $-\mathrm{I}$ effect deactivate the $-\mathrm{O}$ and $-\mathrm{p}$ position. Hence, (c) option is correct.
JIPMER-2010
GENERAL ORGANIC CHEMISTRY
231498
The correct order of increasing basic nature for the bases $\mathrm{NH}_{3}, \mathrm{CH}_{3} \mathrm{NH}_{2}$ and $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}$ in aqueous solutions
Steric Hindrance to H-bonding occur if the alkyl group is bigger than $\mathrm{CH}_{3}$. Hence, $+\mathrm{I}$ effect predominant over H-bonding. Alkyl group is greatly influenced by inductive effect, solvation effect $\&$ steric hindrance which decide strength of akyl amine in aqeous state.
Karnataka CET-2017
GENERAL ORGANIC CHEMISTRY
231510
Chloroacetic acid is a stronger acid than acetic acid. This can be explained using :
1 $-\mathrm{M}$ effect
2 - I effect
3 + M effect
4 + I effect
Explanation:
$-\mathrm{Cl}$ is an electron withdrawing (ie, $-\mathrm{I}$ showing) group. It withdraws electrons when attached to the carboxylic acid and decreases the electron density on the oxygen atom. This will facilitate the release of $\mathrm{H}^{+}$by making $\mathrm{O}-\mathrm{H}$ bond more polar and thus $-\mathrm{Cl}$ increases the acidity of acetic acid when attached at, a position because of $-\mathrm{I}$ effect.
Karnataka CET
GENERAL ORGANIC CHEMISTRY
231515
The carbon-carbon bond length in benzene is
1 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$
2 same as in $\mathrm{C}_{2} \mathrm{H}_{4}$
3 in between $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
4 in between $\mathrm{C}_{2} \mathrm{H}_{4}$ and $\mathrm{C}_{2} \mathrm{H}_{2}$
Explanation:
The carbon-carbon bond length in benzene $(1.39 \AA)$ is between that of $\mathrm{C}-\mathrm{C}(1.54 \AA)$ and $\mathrm{C}=\mathrm{C}$ $(1.34 \AA)$ ie, in between that of $\mathrm{C}_{2} \mathrm{H}_{6}$ and $\mathrm{C}_{2} \mathrm{H}_{4}$.
