MCQ
Among the following compounds, which will react with acetone to give a product containing $ > C = N - $
- A${C_6}{H_5}N{H_2}$
- B${(C{H_3})_3}N$
- C${C_6}{H_5}NHN{H_2}$
- ✓$(A)$ or $(C)$ both
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${ }^{-} \mathrm{OH}, \mathrm{R} \overline{\mathrm{O}}, \mathrm{CH}_3 \mathrm{CO} \overline{\mathrm{O}}, \mathrm{C} \overline{1}$
$[X]$ $\xrightarrow{{KMn{O_4}/\mathop O\limits^\Theta H/\Delta }}$ $\begin{array}{*{20}{c}}
{\begin{array}{*{20}{c}}
{\begin{array}{*{20}{c}}
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_3}} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{HOOC - {{(C{H_2})}_3} - CH - COOH}
\end{array}}
\end{array}}
\end{array}$
$[X]$ will be:
$A$. All group $16$ elements form oxides of general formula $\mathrm{EO}_2$ and $\mathrm{EO}_3$ where $\mathrm{E}=\mathrm{S}, \mathrm{Se}, \mathrm{Te}$ and Po. Both the types of oxides are acidic in nature.
$B$. $\mathrm{TeO}_2$ is an oxidising agent while $\mathrm{SO}_2$ is reducing in nature.
$C$. The reducing property decreases from $\mathrm{H}_2 \mathrm{~S}$ to $\mathrm{H}_2 \mathrm{Te}$ down the group.
$D$. The ozone molecule contains five lone pairs of electrons.
Choose the correct answer from the options given below: