Shielding and Screening Effect of Inner Shells
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This document discusses the shielding or screening effect of inner electron shells in atoms. It explains how valence electrons in multi-electron atoms experience a reduced pull from the nucleus due to repulsion from inner shell electrons. The effect impacts ionization energy and is more pronounced in certain subshells.
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The shielding or screening effect of inner shells : The valence electrons in a multi–electron atom are pulled by the nucleus but are repelled by the electrons of the inner shells. The valence electrons, therefore, do not experience the total pull of the nucleus. Instead the total pull of the...
The shielding or screening effect of inner shells : The valence electrons in a multi–electron atom are pulled by the nucleus but are repelled by the electrons of the inner shells. The valence electrons, therefore, do not experience the total pull of the nucleus. Instead the total pull of the nucleus is reduced by the electrons in inner shells. This effect of reducing the force of attraction of nucleus by the inner shells is called screening effect. This effect is exhibited maximum by 2sp (the most stable) shell. Therefore, the ionisation energy of K is much less than Cu, however, both have one electron in their fourth shell.
