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The D-And-f-Block Elements

Question
CBSEENCH12007099
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What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of their atoms: 3d3, 3d5, 3d8 and 3d4? 

Solution

The stable oxidation state of transition element with the d electron configuration in ground state of atoms are as follows:

S. No. d-electron

configuration

Symbol of element

Stable oxidation states

1.

2.

3.

4.

3d3

3d4

3d5

3d8

Vanadium[V](4s23d3)

Chromium Cr(4s23d4)

Manganes Mn(4s23d5)

Nickel Ni(4s23d8)

+2, +3, +5

+2, +3, +6

+2,+7

+2,+4

It should be noted that lower stable oxidation state generally leads to ionic bond and higher oxidation state corresponds to covalent bond.

 

Some More Questions From The d-And-f-Block Elements Chapter

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?

Write the general electronic configuration of d-block elements.

Why do some exceptions to the general electronic configuration of d-block elements exists?

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