The normal boiling point of 2-propanol, (ch3)2choh, is 83 âºc, while that of acetone, (ch3)2c=o, is 56 âºc. 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 answer is: (D) 2-Propanol experiences stronger hydrogen bonding than acetone.

2- propanol has greater boiling point, because hydrogen bonds between 2-propanol molecules, more energy is required to breake those bonds.

Hydrogen bond is an electrostatic attraction between two polar groups that occurs when a hydrogen atom (H), covalently bound to a highly electronegative atom such as flourine (F), oxygen (O) and nitrogen (N) atoms.

In molecule of 2-propanol there are hydrogen forces between negatively charged oxygen from one molecule of 2-propanol and positively charger hydrogen of another molecule of 2-propanol.

2-propanol is alcohol and acetone is ketone, both are organic compounds.

m=9

step-by-step explanation:

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