The main characteristic of the electron configuration of transition elements is that they have full outer sub-orbitals and the second outermost d sub-orbitals incompletely filled.
An exception to this is copper which loses one 4s orbital electron to the 3d suborbital in order to increase stability.
The ionization energies of transition elements remain fairly low even when the atomic number increases.
Transition metal ions have their electrons removed not from the higher energy orbitals, but from the valence shell orbitals.
Transition metals form one or more stable ions with a completely filled d orbital.
http://chemwiki.ucdavis.edu/Inorganic_Chemistry/Electronic_Configurations/Electron_Configuration_of_Transition_Metals_and_Ions%3A_Mn_vs._Cu
http://chemed.chem.wisc.edu/chempaths/GenChem-Textbook/Ionization-of-Transition-and-Inner-Transition-Elements-904.html
http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch12/trans.php
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