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 and explain the evidence for the delocalisation of electrons in benzene (6 marks)
Why is the Mg2+ ion smaller in radius than the Na+ ion?
State and explain the general trend in the first ionisation energies of the Period 2 elements Lithium to Fluorine.
Explain how the electron pair repulsion theory can be used to deduce the shape of, and the bond angle in, PF3