- ✓$IIB$
- B$IIA$
- C$IA$
- D$IB$
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$(i)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,OC{H_3}}
\end{array}$
$(ii)\,\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus - C{H_3}} \\
| \\
{\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iii)\begin{array}{*{20}{c}}
{C{H_3} - \mathop C\limits^ \oplus {H_2} - NH} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,|} \\
{\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,C{H_3}}
\end{array}$
$(iv)\,C{H_3} - \mathop C\limits^ \oplus {H_2}$

$(I)$ $CH_3CH_2CH_2Cl$ $(II)$ $\begin{array}{*{20}{c}} {C{H_2} = CH\,CH\,C{H_3}} \\ {\,\,\,\,\,\,\,\,\,\,|} \\ {\,\,\,\,\,\,\,\,\,\,Cl} \end{array}$
$(III)$ $\begin{array}{*{20}{c}} {C{H_3}C{H_2}\,CH\,C{H_3}} \\ {\,\,\,|} \\ {\,\,\,\,Cl} \end{array}$
$(I)$ the highest oxidation state of iron is $+ 6$ in $K_ 2FeO_4$
$(II)$ that the iron shows $+ 2$ oxidation state with six electrons in the $3d$ orbitals
$(III)$ the common oxidation state of iron is $+3$ with five unpaired electrons in $3d$ orbital
