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Explain the following observations : (...

Explain the following observations :
(i) Copper atom has completely field d orbitals `(3d^(10))` in its ground state, et it is regarded as a transition element.
(ii) `Cr^(2+)` is a stronger reducing agent than `Fe^(2+)` in awueous solutions.

Text Solution

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Transition element is defined as the one which has incompletely filled .d. orbitals in its ground state or in their most common oxidation state. Cu in its `+2` oxidation astate exhibit `4d^(9)` E.C. That is why it is considered as a transition element.
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Explain the following observations : (i) Copper atom has completely field d orbitals (3d^(10)) in its ground state, it is regarded as a transition element. (ii) Cr^(2+) is a stronger reducing agent than Fe^(2+) in aqueous solutions.

Copper atom has completely filled d orbitals (3d^(10)) in its ground state. How can we say that it is a transition element

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Silver atom has completely filled d orbitals (4d^(10)) in its ground state. How can you say it is a transition element?

(i) Give the general electronic configuration of d-block elements, (ii) Silver atom has completely filled d-orbitals (4d^10) in its ground state. Yet, it is considered as transition element. Why? (iii) Cu^+ ion is not stable in aqueous solution. Explain. (iv) Actinoids contraction is greater from element to element than lanthanoid contraction. Why?

In aqueous solution Cr^(2+) is stronger reducing agent than Fe^(2+) . This is because