dannythewhale_
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Why is the melting point of XeF4 higher than that of PF3 even though PF3 is polar but XeF4 isn't?
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Pigster
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(Original post by dannythewhale_)
Why is the melting point of XeF4 higher than that of PF3 even though PF3 is polar but XeF4 isn't?
Shed loads more e-.

Why is iodine a solid and water a liquid.? Hang on, I thought hydrogen bonds are stronger than London forces?!?
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dannythewhale_
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(Original post by Pigster)
Shed loads more e-.

Why is iodine a solid and water a liquid.? Hang on, I thought hydrogen bonds are stronger than London forces?!?
You make a very good point thank you, our teachers made us think its always hydrogen > dipole-dipole > London
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Prof Harambe
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(Original post by dannythewhale_)
Why is the melting point of XeF4 higher than that of PF3 even though PF3 is polar but XeF4 isn't?
I said that PF3 is polar, but I justified the van der waal/london forces being bigger in XeF4 as PF3 is only slightly polarised, F is still very electronegative. This small polarity shouldn't outweigh the fact that Xe is much heavier than P and has an extra bonding pair. Also XeF4 is square planar, planarity means that the molecules can fit together neater than in the trigonal pyramidal, as each of the bonds in the PF3 is in its own plane (you could compare this to why alloys have a lower melting point, because the arrangement of ions is not regular). Bonds that are packed closer experience stronger van der waals therefore have a higher boiling point. That's my guess on the matter. This question came up for me, so thats what I said roughly.
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ribenafan55
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https://www.physicsandmathstutor.com...istry-a-level/ there's a model answer to this question in the physical MA document in this link idk how accurate it is but I'm assuming it's reliable
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