A) \[C{{H}_{3}}C{{H}_{2}}C{{H}_{2}}Cl\]
B) \[C{{H}_{3}}C{{H}_{2}}C{{H}_{2}}OH\]
C) \[C{{H}_{3}}\underset{\begin{smallmatrix} | \\ OH \end{smallmatrix}}{\mathop{C}}\,HC{{H}_{3}}\]
D) \[\underset{\begin{smallmatrix} | \\ OH \end{smallmatrix}}{\mathop{C}}\,{{H}_{2}}-C{{H}_{2}}-C{{H}_{2}}-\underset{\begin{smallmatrix} | \\ OH \end{smallmatrix}}{\mathop{C}}\,{{H}_{2}}\]
Correct Answer: D
Solution :
Key Idea: (i) Boiling point increases with increase in molecular mass in a homologus series. (ii) Alcohols have higher boiling point than corresponding alkyl halides due to the fact that alcohols have stronger forces of attraction because of hydrogen bonding between them as compared to weaker van der Waals forces between alkyl halide molecules. (iii) More the number of OH groups, more will be the boiling point as the molecule will form more number of hydrogen bonds. \[\therefore \] \[\underset{\begin{smallmatrix} | \\ OH \end{smallmatrix}}{\mathop{C}}\,{{H}_{2}}-C{{H}_{2}}-C{{H}_{2}}-\underset{\begin{smallmatrix} | \\ OH \end{smallmatrix}}{\mathop{C}}\,{{H}_{2}}\] will have highest boiling point.
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