Silver atom has completely filled d orbi...

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

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The configuration of silver is `[Kr]4d^(10)5s^(1)`. It acquires `4d^(10)` configuration by losing `5s^(1)` electron. Moreover, the last electon is filled in the 4d sub-shell. Threfore , the element is regarded as a transition metals.

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(a) Silver atom has completely filled 'd' orbitals (4d^10) in its ground state. How can you say that it is a transition element ? (b) Actinoids exhibit a large number of oxidation states in comparison to corresponding members of Lanthanoid series. Why?

Copper atom has completely filled d orbitals (3d^(10)) in its ground state. How can we say that 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?

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.

Statement-1: silver is a transition element. Statement-2: silver atom has completely filled d-robitals (4d^(10)) in its ground state.

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