The normal boiling point of 2-propanol, (CH3)2CHOH, is 83 ºC, while that of acet

Question

The normal boiling point of 2-propanol, (CH3)2CHOH, is 83 ºC, while that of acetone, (CH3)2C=O, is 56 ºC. What is the principal reason for the greater boiling point of 2- propanol?

(A) The O–H bond in 2-propanol is stronger than the C–H bonds in acetone.

(B) 2-Propanol experiences greater London dispersion forces than acetone.

(C) 2-Propanol experiences stronger dipole-dipole interactions than acetone.

(D) 2-Propanol experiences stronger hydrogen bonding than acetone.

The correct answer is D, but where is the hydrogen bonding in acetone? I answered A because i thought that the only hydrogen bonding present was in the propanol?

Thanks!

Explanation / Answer

The reason behind this is hydrogen bonding because it is weaker force but in the presence of hydrogen bonding many physical properties changes highly and no H bonding will be present in the acetone but the option D is highly suitable

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.