Question

Liquid ethyl acetate contains mainly the following intermolecular forces:

• A. London dispersion, dipole-dipole and hydrogen bonding
• B. Hydrogen bonding and London dispersion
• C. Dipole-dipole and hydrogen bonding
• D. London dispersion and dipole-dipole

Answer 1

The correct option is D

London dispersion and dipole-dipole

The explanation for the correct answer:

D. London dispersion and dipole-dipole

• London's dispersion forces develop due to a transient dipole formed due to changes in electron density.
• Another atom or molecule forms a dipole as a result of these instantaneous dipoles.
• As a result of the electrostatic interactions between two or more dipoles, dipole-dipole forces are the strongest intermolecular forces.
• London dispersion and dipole-dipole interaction are the main intermolecular forces in liquid ethyl acetate.
• Dipole-dipole interaction will exist since ethyl acetate is a polar chemical.
• Structure of ethyl acetate-
• 

The explanation for the incorrect answer:

Hydrogen bonding:

• A hydrogen atom is bound to a highly electronegative atom and another highly electronegative atom that is close by interacting with one another to form hydrogen bonds, which are unique kinds of attractive intermolecular interactions.
• This process is known as hydrogen bonding.
• Only in compounds with hydrogen atoms bound to a highly electronegative atom do hydrogen bonds, a particularly specific class of intermolecular attractive interactions, appear.
• In contrast to typical dipole-dipole and dispersion forces, hydrogen bonds are generally powerful.
• In contrast to actual covalent or ionic bonds, they are rather weak.
• And in the case of ethyl acetate, Hydrogen Bonding is not possible because the oxygen element is bonded with carbon, i.e. they are showing that they are bonded with the polar covalent bond.

Final answer: Hence, the correct answer is option D, London dispersion, and dipole-dipole.