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.

a is the answer

explanation:

which statement about trans-fatty acids is false?

a. the conversion of cis-fatty acids to trans-fatty acids is inhibited by the presence of antioxidants.

hope this

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.