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The d-And-f-Block Elements
Why is copper sulphate pentahydrate coloured?
In copper sulphate pentahydrate (CuSO4.5H2O) copper is divalent (Cu2+). Copper(II) have the configuration
1s2 2s2 2p6 3s2 3p6 3d9
An ion or compound is coloured when it has unpaired electron in its d-orbitals. Cu(II) has one unpaired electron in its d-orbital, hence it is coloured.
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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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