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!
Chemistry OCR AS question - 2015 paper Watch
- Thread Starter
- 18-01-2016 19:46
- Official TSR Representative
- 20-01-2016 21:20
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