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The D-And-f-Block Elements
Though copper, silver and gold have completely filled sets of d-orbitals yet they are considered as transition metals. Why?
These metals in their common oxidation states have incompletely filled d-orbitals e.g., Cu2+ has 3d10 and Au3+ has 5d8 configuration.
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
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?
Name the first element of 3rd transition series.
Though copper, silver and gold have completely filled sets of d-orbitals yet they are considered as transition metals. Why?
Why are transition elements so named?
Why are transition elements known as d-block elements?
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Mock Test Series
Mock Test Series