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why d subshell has poor screening effect

The size of d shell is very much larger than that of s and p. Thus, electrons in d shell are more scattered and are unable to shield the electrons in the valence shell from the attractive force of the nucleus.

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Since, shielding effect is defined as  a reduction in the effective nuclear charge on the electron cloud, due  to a difference in the attraction forces of the electrons on the  nucleus. If the electron is in s shell, it means it is nearest to nucleus and if in f shell, it means it is farthest from nucleus. Since, atomic shielding spends on electron density in a shell and electron density is very less for d and f shells, hence it has poor shielding effect
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