Download App

STD 11 - 8.4. Organic chemistry reaction mechanism — NEET STD 11 Science — Question

Gujarat BoardEnglish MediumSTD 11 ScienceNEETSTD 11 - 8.4. Organic chemistry reaction mechanism4 Marks
MCQ
Among the following, total number of meta directing functional groups is__________ (Integer based)

$ -\mathrm{OCH}_3,-\mathrm{NO}_2,-\mathrm{CN},-\mathrm{CH}_3-\mathrm{NHCOCH}_3, $

$ -\mathrm{COR},-\mathrm{OH},-\mathrm{COOH},-\mathrm{Cl}$

  • A
    $3$
  • B
    $2$
  • ✓
    $4$
  • D
    $1$
✓

Answer

Correct option: C.
$4$
c
$-\mathrm{NO}_2,-\mathrm{C} \equiv \mathrm{N},-\mathrm{COR},-\mathrm{COOH}$

are meta directing.

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Explore more

NEET STD 11 Science question papers→Gujarat Board STD 11 Science question papers→Gujarat Board question paper generator→

Similar questions

The vapour pressure of pure water is $92.5\, mm$ at $300\,K$. The vapour pressure of $1$ molal solution of $X$ in water is :-
→
In the given reaction, Find out X, Y and Z respectively :
Image
→
The equivalent conductance of NaCl at concentration C and at infinite dilution are $\lambda_{ c }$ and $\lambda_{\infty}$ relationship. The correct relationship between $\lambda_{ c }$ and $\lambda_{\infty}$ is given as (where, the constant B is positive)
→
The rate for a first order reaction is $0.6932 \times {10^{ - 2}}\,mol\,{l^{ - 1}}\,mi{n^{ - 1}}$ and the initial concentration of the reactants is $1\,M$, ${T_{1/2}}$ is equal to ........ $\min$
→
Electron affinity is the lowest for
→
Product $(A)$ is
→
If in a voltaic cell $5\,gm$ of zinc is consumed, then we get how many ampere hours ?(Given that $E.C.E.$ of $Zn$ is $3.387 \times {10^{ - 7}}\,kg/coulomb$)
→
Two reactions are given below:

$2 \mathrm{Fe}_{(\mathrm{s})}+\frac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_2 \mathrm{O}_{3(\mathrm{~s})}, \Delta \mathrm{H}^{\mathrm{o}}=-822 \mathrm{~kJ} / \mathrm{mol}$

$\mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{(\mathrm{g})}, \Delta \mathrm{H}^{\mathrm{o}}=-110 \mathrm{~kJ} / \mathrm{mol}$

Then enthalpy change for following reaction

$3\mathrm{C}_{(\mathrm{s})}+\mathrm{Fe}_2 \mathrm{O}_{3(\mathrm{~s})} \rightarrow 2 \mathrm{Fe}_{(\mathrm{s})}+3 \mathrm{CO}_{(\mathrm{g})}$

→
The compound used as an explosive is
→
Consider an electrochemical cell: $A ( s )\left| A ^{ n +}( aq , 2 M ) \| B ^{2 n +}( aq , 1 M )\right| B ( s )$. The value of $\Delta H ^{\ominus}$ for the cell reaction is twice that of $\Delta G ^{\ominus}$ at $300 K$. If the emf of the cell is zero,  the $\Delta S ^{\ominus}$ (in $J K ^{-1} mol ^{-1}$ ) of the cell reaction per mole of $B$ formed at $300 K$ is. . . . . . . (Given: $\ell n (2)=0.7, R$ (universal gas constant) $=8.3 J K ^{-1} mol ^{-1} . H , S$ and $G$ are enthalpy, entropy and Gibbs energy, respectively.)
→