Which type of intermolecular forces exist between 

$(a)H_{2}S$ molecules 
$(b)C{l}_2$ molecules
$(c)CC{l}_4$ molecules ?

$(a)H_{2}S$ molecule :

Sulphur atoms have 6 Valence electrons  and hydrogen atoms have 2 valence electrons So, the Lewis structure of $H_{2}S$ looks like this.

We see that the central sulphur atoms have 4 entities around it. Two hydrogen atoms, and two lone non-bonding electron pairs. According to VSEPR theory, this means that the shape of the molecule is bent and because of the asymmetrical shape, the molecule is polar .

The intermolecular force which polar molecules take part in are dipole-dipole forces.

(b) $C{l}_2$ and $CC{l}_4$molecules :

Chlorine atoms have 7 valence electrons. So, the Lewis structure of $C{l}_2$ looks like this: 

Here, there is no central atom, and both atoms are of the same element. This means that the molecular shape is linear, and because of the symmetrical shape, the molecule is nonpolar.

Nonpolar molecules cannot take part in dipole-dipole interaction due to the lack of permanent dipoles, and there are no other characteristics that give this molecule the ability to have stronger intermolecular forces. This means that $C{l}_2$molecules can only take part in London Dispersion Forces.

We can see here that the central carbon atom has four atoms around it, and no non-bonding lone pairs. According to VSEPR theory, this means that the molecule is tetrahedral in shape, and therefore symmetrical. This means that the molecule is overall nonpolar.

Because both $C{l}_2$ and $CC{l}_4$ are nonpolar and have no other special identifying characteristics, the only intermolecular forces between the two molecules are London Dispersion Forces.