Hydrogen bonding: Difference between revisions
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Hydrogen bonding is an intermolecular bond between a hydrogen attached to | Hydrogen bonding is an intermolecular bond between a hydrogen attached to an electronegative atom (Fluorine, Oxygen or Nitrogen) and an electronegative atom on a separate molecule/ different location of the same molecule<ref>Britannica, ND, [cited: 04/12/17] Available from: https://www.britannica.com/science/hydrogen-bonding</ref>. It occurs between bases in DNA and between polar water molecules. As a single bond it is weak, but when there are many hydrogen bonds together the collective strength is large. | ||
=== Evidence for hydrogen bonding === | |||
If the boiling points of the compounds of group 4 were plotted with hydrogen, it is found that the boiling points increase as you go down the group, this happens due to the increasing size of the molecules so more electrons and increasing numbers of van der Waals<ref>https://www.chemguide.co.uk/atoms/bonding/hbond.html</ref>. <br> | |||
=== References === | |||
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Latest revision as of 11:19, 6 December 2017
Hydrogen bonding is an intermolecular bond between a hydrogen attached to an electronegative atom (Fluorine, Oxygen or Nitrogen) and an electronegative atom on a separate molecule/ different location of the same molecule[1]. It occurs between bases in DNA and between polar water molecules. As a single bond it is weak, but when there are many hydrogen bonds together the collective strength is large.
Evidence for hydrogen bonding
If the boiling points of the compounds of group 4 were plotted with hydrogen, it is found that the boiling points increase as you go down the group, this happens due to the increasing size of the molecules so more electrons and increasing numbers of van der Waals[2].
References
- ↑ Britannica, ND, [cited: 04/12/17] Available from: https://www.britannica.com/science/hydrogen-bonding
- ↑ https://www.chemguide.co.uk/atoms/bonding/hbond.html