Intermoleculer Forces (again)

What types of intermolecular force is (are) common to a) Xe and methanol (CH3OH), b) CH3OH and acetonitrile (CH3CN), c) NH3 and HF?

XE-CH3OH

London-molecule isn't non polar so can't be - wrong
Dipole-Dipole-moleclue is polar so dipole-dipole
Hydrogen-no N, O, F or C on the left so can't be
Ionic- Can't be because this isnt between a metal and nonmetal


CH3OH-CH3CN

London-the EN is very close i want to say this is a london
Dipole-Dipole-EN come close , the math would say its a close polar molecule so i'd say Dipole-Dipole
Hydrogen-I see H bonded to O and C but not sure if i'm making a mistake here to label this a hydrogen bond
Ionic- Can't be because this isn't between a metal and nonmetal



NH3-HF

London-isn't polar so can't be
Dipole-Dipole-is polar so does have this but hydrogen since of very high polarity
Hydrogen- H is bonded to an N and F so i'd assume this is a hydrogen bond
Ionic- Can't be because this isn't between a metal and nonmetal



not exactly sure if the question was asking which do they all have in common jointly, if it was I would say Dipole-Dipole from what i wrote above. Please correct any flaws with my reasoning!

the next question is

Which member of the following pairs has the stronger intermolecular dispersion forces

a) Br2 or O2


b) CH3CH2SH or CH3CH2CH2CH2SH


c) CH3CH2CH2CL or (CH3)2 CHCL


I'm a bit confused on the wording of the question. Is it asking Molecule A vs Molecule B which has the stronger forces for each letter?

Van der Waals forces are induced dipole-dipole interactions and exist between ALL particles.

So that means all of the examples would contain london dispersion forces?

XE-CH3OH

London-molecule isn't non polar so can't be - wrong (I'm confused on why this is wrong)
Dipole-Dipole-moleclue is polar so dipole-dipole
Hydrogen-no N, O, F or C on the left so can't be
Ionic- Can't be because this isnt between a metal and nonmetal

the next question is

Which member of the following pairs has the stronger intermolecular dispersion forces

a) Br2 159.8gmol or O2 32gmol

therefore Br2 has stronger intermolecular dispersion forces



b) CH3CH2SH 62.15gmol or CH3CH2CH2CH2SH 90.21gmol

therefore CH3CH2CH2CH2SH has stronger intermolecular dispersion forces



c) CH3CH2CH2CL 78.55 or (CH3)2 CHCL 78.55

both have the same weight but i think CH3CH2CH2CL is stronger because it has less branches in the structure?

What types of intermolecular force is (are) common to a) Xe and methanol (CH3OH), b) CH3OH and acetonitrile (CH3CN), c) NH3 and HF?

XE-CH3OH

London-seems like it can be this as well?
Dipole-Dipole-moleclue is polar so dipole-dipole
Hydrogen-no N, O, F or C on the left so can't be
Ionic- Can't be because this isnt between a metal and nonmetal


CH3OH-CH3CN

London-the EN is very close i want to say this is a london
Dipole-Dipole-EN come close , the math would say its a close polar molecule so i'd say Dipole-Dipole
Hydrogen-I see H bonded to O and C but not sure if i'm making a mistake here to label this a hydrogen bond
Ionic- Can't be because this isn't between a metal and nonmetal



NH3-HF

London-isn't polar so can't be
Dipole-Dipole-is polar so does have this but hydrogen since of very high polarity
Hydrogen- H is bonded to an N and F so i'd assume this is a hydrogen bond
Ionic- Can't be because this isn't between a metal and nonmetal



not exactly sure if the question was asking which do they all have in common jointly, if it was I would say Dipole-Dipole from what i wrote above. Please correct any flaws with my reasoning!