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The D-And-f-Block Elements

Question
CBSEENCH12007217
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What may be the possible oxidation states of the transition metals with the following d electronic configurations in the ground state of their atoms: 3d34s2,3d54s2 and 3d64s2. Indicative relative stability of oxidation states in each case.

Solution

(a) Configuration

3d34s2

3d5 4s2

3d6 4s2

(a) Stable oxidation state

+3, +3

+2, +7

+2, +8

The stability of any oxidation state of any element generally depends upon the electronic configuration of that particular ion. If any ion has stable configuration (d5, d10 etc.), the particular oxidation state will be more stable.

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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