Question

What is the relationship between critical temperature and intermolecular forces?

Determine the strongest type of intermolecular force present in the solids of each of the following substances:

a)BaSO₄

b)H₂S

c)Xe

d)C₂H₆

e)Cs

f)Hg

g)P₄

h)H₂O

Predict which substance in each of the following pairs would have the greater IMF

a)CO₂ or OCS

b)PF₃ or PF₅

c)SF₂ or SF₆

d)SO₃ or SO₂

Answer 1

a)

BaSO4 ------------ Electrostatic attractive forces because ionic bond is present

b) H2S -------------- Dipole-Dipole forces because it is polar compound.

c) Xe ------------    Vanderwaals forces

d)C2H6 -------------- Vanderwaals forces

e)Cs ---------------------- Metallic forces

f)Hg ----------------------------- Metallic forces

g)P4 --------------   Vanderwaals forces

g)H2O --------------- Hydrogen bondings

a) OCS has greater IMF because it is a polar molecule, but CO2 is a non-polar

b)PF5 -. PF3 contains one lone pair of electrons.

c)SF6.

d) SO3 has greater IMF because it has no lone pair of electrons.