I recently did a 2015 AS paper for chemistry and I'm a bit confused on one of the questions:
The table shows the boiling points of ammonia, fluorine and bromine.
Ammonia, NH3 = -33 (degrees)
Fluorine, F2 = -188 (degrees)
Bromine, Br2 = 59 (degrees)
Why is it that bromine has the highest boiling point when it only has London forces acting between each molecule whereas ammonia has hydrogen bonding - which is the strongest type of intermolecular attraction? I get why bromine is higher than fluorine - more electrons therefore the London forces are stronger.
If anyone understands why, please help!
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Chemistry OCR AS question - 2015 paper watch
- Thread Starter
- 18-01-2016 19:46
- Official Rep
- 20-01-2016 21:20
Sorry you've not had any responses about this. Are you sure you’ve posted in the right place? Posting in the specific Study Help forum should help get responses.
I'm going to quote in Tank Girl now so she can move your thread to the right place if it's needed.
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