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The d-And-f-Block Elements
Why are the ionization enthalpies of 5d elements greater than those of 3d and 4d elements?
When we move downward in a particular group the atomic number is increased, consequently nuclear charge is also increased. Due to this reason 5d-elements have higher nuclear change than 3d and 4d elements, therefore, the outer electrons are attracted strongly by the nucleus in 5d elements. On the other hand, the shielding effect of 4f electrons is very poor due to lanthanide contraction in 5d elements, which further increases from 5d elements than 3s and 4d electrons, where no 4f electrons and lanthanide contraction is present.
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How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?
The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
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