we are saying it will have high viscocity /boiling point etc ( which has higher force ) means they are all in liquid state but dipole-d interaction may occur in solid also so overall if we need to consider the forces(attractive) then will not we consider all the 3 states our is it just that we are considering liquid state.
@markbondking007 Typical questions are for liquid state, but you can consider other states if you want. Additional factors may come in with other states.
If you mean the first example with CH4 and CCl4, then neither molecule has a dipole or H-bond. Also note, all molecules have London forces. Whenever you don't find a dipole or H-bond, then you can always write London.
I'd say dipole. H-bonding can be a complex issue but most will simply summarize it as this: an H on one molecule that is directly bonded to an electronegative element (N, O, or F) forms an H-bond when it interacts with an electronegative element of another molecule (N, O, or F). Intramolecular H-bonds are also possible if both possibilities are present on a single, large molecule. For CHF3, there is no H atom that is directly bonded to the F atom (the electronegative element).
@EnderlePhD Can you please explain why NH3 has intERmolecular H-bond when the H bond to N does not interact with (N,O,F) from another molecule. Thanks
@EnderlePhD How is that CH4 CCl4 are both london dispersion forces?? Shouldn't CCl4 be a hydrogen bond? Hydrogen bonds occur in molecules where H is connected to to a highly electronegative atom such as O, F, N and Cl, so why isn't CCl4 written as a hydrogen bond?
@EnderlePhD I don't quite have enough space to explain here, but I'll try a simple explanation. First, Cl is not always included in the list of atoms that qualify for the H-bond. However, that point is not relevant in this case. If CCl4 is only interacting with itself, then there are no H atoms in solution to cause an H-bond. Not only is an H needed, but that H should be bonded to an electronegative atom.
we are saying it will have high viscocity /boiling point etc ( which has higher force ) means they are all in liquid state but dipole-d interaction may occur in solid also so overall if we need to consider the forces(attractive) then will not we consider all the 3 states our is it just that we are considering liquid state.
markbondking007 4 months ago
@markbondking007 Typical questions are for liquid state, but you can consider other states if you want. Additional factors may come in with other states.
EnderlePhD 3 months ago
my force can make you gay
kilstas16 11 months ago
Thank you, this is very helpful!
seaviee1 1 year ago
@seaviee1 bonded*
Ali22M21 1 year ago
i dont understand why they are both london forces??
reck1ess77 2 years ago
If you mean the first example with CH4 and CCl4, then neither molecule has a dipole or H-bond. Also note, all molecules have London forces. Whenever you don't find a dipole or H-bond, then you can always write London.
EnderlePhD 2 years ago
Oh thanks! i do get it now.
Also, i have a question about CHF3
what would the main intermolecular force in it be. I think its hydrogen bonds but not sure if it also be dipole-dipole
reck1ess77 2 years ago
I'd say dipole. H-bonding can be a complex issue but most will simply summarize it as this: an H on one molecule that is directly bonded to an electronegative element (N, O, or F) forms an H-bond when it interacts with an electronegative element of another molecule (N, O, or F). Intramolecular H-bonds are also possible if both possibilities are present on a single, large molecule. For CHF3, there is no H atom that is directly bonded to the F atom (the electronegative element).
EnderlePhD 2 years ago
thanks again for the explanation :)
reck1ess77 2 years ago
@EnderlePhD Can you please explain why NH3 has intERmolecular H-bond when the H bond to N does not interact with (N,O,F) from another molecule. Thanks
Ali22M21 1 year ago
@EnderlePhD How is that CH4 CCl4 are both london dispersion forces?? Shouldn't CCl4 be a hydrogen bond? Hydrogen bonds occur in molecules where H is connected to to a highly electronegative atom such as O, F, N and Cl, so why isn't CCl4 written as a hydrogen bond?
donshan123 8 months ago
@EnderlePhD I don't quite have enough space to explain here, but I'll try a simple explanation. First, Cl is not always included in the list of atoms that qualify for the H-bond. However, that point is not relevant in this case. If CCl4 is only interacting with itself, then there are no H atoms in solution to cause an H-bond. Not only is an H needed, but that H should be bonded to an electronegative atom.
EnderlePhD 8 months ago