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.

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

so since they all have the same shape? i mean maybe because m& m and reeses are both chocolates