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Configuration energies (CE) of the d-block elements (Groups 3−11) are electronegativities evaluated
from the formula CE = (pεs + qεd)/(p + q). εs and εd are the multiplet-averaged one-electron energies of the
s- and d-orbitals of atoms which are in the lowest energy of the configurations s
n
d
m
and s
n
-1d
m
+1, and whose
highest known oxidation state is (p + q). The orbital energies are obtained from spectroscopic data. Configuration
energies generally increase across a row, with the highest values occurring at nickel, silver, and gold; all are
lower than the CE of silicon, the least electronegative nonmetal (except for gold which has a CE equal to that
of silicon). Down the groups configuration energies invariably decrease from the first row to the second row;
for Groups 7−12, the third-row element has a CE higher than that of the second-row element, due to increasing
relativistic stabilization of the 6s orbitals.
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