Question

What are the lewis structures for ethanol, hexane, and ethyl acetate, and what intermolecular forces exist in each?

Answer 1

In ethanol there are three types of intermolecular forces bonding them together.

i) First one, London force. This happens between all molecules, no matter what.

ii) The second force would be Dipole-dipole. Because ethanol is a polar molecule, it has positive and negative ends. This allows itself to bond to other Ethanol molecules.

iii) The third and strongest intermolecular force would be the Hydrogen bond between H and O

In Hexane: It is a nonpolar, organic compound/solvent. So it lacks any kind of polar interaction with its neighbour molecule. hence the molecules are held together by London dispersion forces only .

There are two types of bond present in ethyl acetate.
i) C-C : London forces (or) Dispersion forces
ii) C-O : Dipole-Dipole Attraction.