The intermolecular force(s) responsible for the fact that ch4 has the lowest boiling point in the set ch4, sih4, geh4, snh4 is/are

London forces.

All of them are covalent compounds – I know you may find strange for metals to make covalent bonds, but you know all rule has its exceptions. Take a look at their electronegativity, and calculate the difference:

EnGe – EnH < 2

EnSn – EnH < 2

So all these differences are below 2. Usually, when the difference is lower than 2, they are covalent. Besides, if they are gasses, there’s no way they can be ionic!

Now that we know they are all covalent, let’s take a look at its geometry. C, Si, Ge, and Sn, are all within group IVA in a traditional periodic table, which means they all have 4 outer electrons. So they need 4 bonds to complete their octete – that’s why they bond with 4 H. Remember H has 1 electron and is stable with 2 electrons, so it also needs 1 bond.

So all of them have 4 bonds, one with each H. And no free electrons. That means they are tetraedric. A tetraedric molecule where all bonds are equal, is always non polar – because of simetry.

So CH4 is the less polarizable, which means it has less London forces, so it’s easier to separate one molecule of CH4 from another molecule of CH4, which means it is easier to make it boil – so the boiling point is lower.

i think   the answer is c hope i'm right