Which is the strongest type of intermolecular force between solute and solvent in br2(l) in ccl4(l)?

Br₂ is a completely non-polar molecule as it has two bromine atoms of equal electronegativities, which results in no dipole moment. CCl₄ is also a completely non-polar molecule. Although, there is a dipole moment for every C-Cl bond in the molecule. But since the structure of CCl₄ is tetrahedral, this results in every dipole cancelling out which provides an overall molecule with no dipole moment.

Since both molecules are non-polar with no net dipole moments, and there are no hydrogens capable of hydrogen-bonding, the only intermolecular forces between the two species are van der waals forces, more specifically London dispersion forces.

The London dispersion forces are instantaneous dipole moments created when the two molecules interact which causes a very weak attraction.

the catch is that the top numbers are atomic masses the bottom numbers are the numbers of protons and electrons in an uncharged atom. they are the number of that atoms as you would find them on the periodic table. further, the numbers on the left are used to determine the missing numbers on the right

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer