A) \[C{{H}_{3}}CH_{2}^{+}\]
B) \[CH_{3}^{+}\]
C) \[{{C}_{6}}{{H}_{5}}CH_{2}^{+}\]
D) \[C{{H}_{3}}C{{H}_{2}}CH_{2}^{+}\]
Correct Answer: C
Solution :
Key Idea: \[\because \]Cations are electron deficient species. \[\therefore \]Electron donating group increase their stability In\[{{C}_{6}}{{H}_{5}}C{{\overset{+}{\mathop{H}}\,}_{2}},\]the phenyl\[({{C}_{6}}{{H}_{5}})\] group behaves as electron rich group and donates electrons and stabilizes the cation \[({{C}_{6}}{{H}_{5}}\]group can behave as electron rich or electron deficient group depending upon nature of group with which it is attached)
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