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The D-And-f-Block Elements
Question
The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
Solution
copper displays two oxidation states (+1 and +2). In the +1 oxidation state, an electron is removed from the s-orbital. However, in the +2 oxidation state, an electron is removed from the d-orbital. Thus, the d-orbital now becomes incomplete (3d9). Hence, it is a transition element. wherein it will have incompletely filled d-orbitals (4d), hence a transition metal.
Some More Questions From The d-And-f-Block Elements Chapter
How would you account for the irregular variation of ionisation enthalpies (first and second) in the first series of the transition elements?
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Which is a stronger reducing agent Cr2+ or Fe2+ and why?
Explain why Cu+ ion is not stable in aqueous solutions?
Actinoid contraction is greater from element to element than lanthanoid contraction. Why?
On what ground can you say that scandium (Z = 21) is a transition element but zinc (Z = 30) is not?
The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
Why the melting points of transition elements are high?
Why Zn, Cd and Hg are not regarded as transition elements?
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Mock Test Series
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