Consider these six-coordinate ionic radii for divalent, first-row transition-metal ions: r(Ti+) = 0.86 , r(V+) = 0.79
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Consider these six-coordinate ionic radii for divalent, first-row transition-metal ions:
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r(Ti+) = 0.86 , r(V+) = 0.79 , r(Cr+) = 0.80 , r(Mn+) = 0.83 , r(Fe+) = 0.78 , r(Co+) = 0.745 , (Ni+) = 0.69 . For a fixed oxidation state, the ionic radius normally decreases on moving left to right across the periodic table due to the increasing effective nuclear charge. Why then does the radius increase on moving from V2+ to Cr+ to Mn+?
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Related Book For
Solid State Materials Chemistry
ISBN: 9780521873253
1st Edition
Authors: Patrick M. Woodward, Pavel Karen, John S. O. Evans, Thomas Vogt
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