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The D-And-f-Block Elements
Question
Silver atom has a completely filled d orbitals (4d10) in its ground state. How can you say that it is a transition element?
Solution
Ag has a completely filled 4d orbital (4d10 5s1) in its ground state. Now, silver 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 (4d9). 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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