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The D-And-f-Block Elements

Question
CBSEENCH12010198
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Explain the following giving an appropriate reason in each case.
Structures of Xenon fluorides cannot be explained by Valence Bond approach.

Solution

According to the valence bond approach, covalent bonds are formed by the overlapping of the half-filled atomic orbital. But xenon has a fully filled electronic configuration. Hence the structure of xenon fluorides cannot be explained by VBT.

For example: In case of XeF2

Hybridization is:
Total, valence electron =8 for Xe

Monovalent atom F=2

So, total hybrid orbitals =1/2 [valence electron + monovalent atom + cation + anion] as no cation and anion so term is zero

 So hybrid orbital are ½[8+2+0+0] = 5
So hybridization = sp3d

According to sp3d hybridization, the structure should be Trigonal bipyramidal, but the actual structure is linear. So, VBT fails to answer this however VSPER theory explains the liner shape.

 

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

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?

Write the general electronic configuration of d-block elements.

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