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How does the shielding effect affect atomic radius?

Last updated date: 20th Jun 2024
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Hint: This abatement in the force of attraction applied by the nucleus on the valence electrons because of the presence of electrons in the inner shells is called screening effect or shielding effect. Its symbol can be represented by\[\sigma \] .

Complete step by step answer:
The net positive charge experienced by valence electrons is defined as effective nuclear charge. It tends to be approximated by the condition\[:{\text{ }}{Z_{eff}} = {\text{ }}Z{\text{ }}-{\text{ }}S\] , where \[Z\]is the atomic number and \[S\] is the quantity of shielding electrons
Shielding is when electrons in the inner electron shells of an atom can shield the external electrons from the pull of the nucleus.
The nucleus can pull the external electrons in tighter when the attraction is strong and less close when the attraction is debilitated.
In this way, the more shielding that happens, the less attraction there is between the external electrons and nucleus, so the further the electrons in the external shell can spread out. This implies the atomic span will be bigger

Note: 1)The shielding impact portrays the balance between the draw of the protons on valence electrons and the repulsion powers from internal electrons.
2)The extent of the screening effect relies on the quantity of inner electrons higher the quantity of inner electrons more noteworthy will be the estimation of the screening effect
3)The shielding impact clarifies why valence-shell electrons are all the more handily eliminated from the atom. The impact additionally clarifies atomic size. The more shielding, the further the valence shell can spread out and the greater atoms will be.