3 posts • Page 1 of 1
Yesterday in the peer review we ranked C,N,O and F on ionization energies and I remember the ranking was an exception to the usual rule of ionization energies increasing across the period. Can someone explain this?
The reason that nitrogen has a higher ionization energy than oxygen is because oxygen has an orbital with 2 electrons in it, which results in some electron-electron repulsion. Whereas nitrogen has just one electron in each of its 2p orbitals and therefore lacks that same electron-electron repulsion.
Who is online
Users browsing this forum: No registered users and 1 guest