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What is the shielding effect and what is the screening effect?
The shielding effect is another name for the screening effect. Because of the existence of electrons in the inner shell, the nucleus’s force of attraction on the valence electrons is reduced. This is referred to as the screening effect.
The outer electrons are attracted to the nucleus but repelled by the inner electrons. The repulsion between the inner and outer electrons grows as the attraction between the nucleus decreases.
The reduction in the effective nuclear charge on the electron cloud is also known as the shielding effect.” It’s a form of electric field screening that’s unique. Because of the screening, the electrical connection between the electron and the nucleus becomes weaker as the electron shells in space become wider.
The ionisation enthalpy required increases as the nuclear force of attraction increases. As a result, the screening effect is inversely proportional to the enthalpy of ionisation.
The screening effect in shells is generally: s > p > d > f The outer electrons are subjected to two different forces. The first is the nucleus’ attraction, while the second is the repulsion of the inner electrons.
As a result, as the number of electrons between the nucleus and the outer electrons increases, the nucleus’s attraction force diminishes. This is owing to the higher force of repulsion exerted by the numerous electrons in the inner shell, which outweighs the nucleus’s attractive force.
The attraction between an electron and the nucleus in any atom containing more than one electron is known as the shielding effect, also known as atomic shielding or electron shielding.
A difference in the attraction forces on the electrons in the atom causes the shielding effect, which is defined as a reduction in the effective nuclear charge on the electron cloud. It’s a type of electric-field screening that’s unique. This effect is also significant in many material science studies.
