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The d-And-f-Block Elements
Explain the following facts:
Transition metals form coloured complexes.
Transition metal form coloured complexes, due to the presence of incomplete d-subshell. The electrons can be excited from one energy level to another with in the d-subshell. The energy required to cause such d-d promotions or transition falls within the visible range for all transition elements. When white light falls on an ion or compound, some of its wave lengths are absorbed due to d-d transition and others are reflected. Therefore, colour of the transition metal ion is that of the reflected light.
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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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