Why doesn't chlorine form hydrogen bonds even though it is more electronegative than nitrogen?
Chlorine has a higher electronegativity, but as it has a large atomic radius the electron density is spread out over a large area. This means that the electron density is too low to form proper hydrogen bonds, and will only be attracted via dipole-dipole attraction.
CL
Related Chemistry A Level answers
All answers ▸State what is meant by the term 'first ionisation energy' and explain why the first ionisation energy of barium is lower than that of calcium
State the meaning of the term first ionisation energy
In organic chemistry, how can functional groups be easily identified and how can I memorise organic mechanisms?
The following equilibrium is set up in a glass syringe. 2(NO2) (brown gas) ‹-› N2O4 (colourless gas) ∆H = -58 kJmol-1. Using le Chatelier's principle, predict and explain how heating up the mixture would affect it's appearance.