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Problem

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12 Nov 2021

Given information

A statement regarding the shielding of an electron is given which is as follows.

An electron in an orbital that penetrates closer to the nucleus always experiences more shielding than an electron in an orbital that doesn't penetrate as far.

Whether this statement is true or false must be explained.

Step-by-step explanation

Step 1.

The decreasing order of penetrating power of different orbitals is

> >>

The decreasing order of shielding effect of different orbitals is 

 > > . 

As per Slater's rules effective nuclear charge where are atomic number and screening constant respectively.

An electron in the valence shell contributes screening constant of Electrons in the next inner orbitals contribute screening constant of   

Any electrons beyond this contribute screening constant of  

 

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