What is the screening effect

What is the screening effect? 

The screening effect occurs when the nucleus’s attractive attraction becomes weaker than the inner electrons’ repulsive force. 

Importance of screening effect:

Because electrons revolve around the nucleus, atoms are stable. The number of protons in the nucleus of heavier elements is relatively high. As a result, the force of attraction between the nucleus and the spinning electrons would be extremely strong.

The electrons would spiral down into the nucleus in a spiral pattern. As a result, the screening effect is required.

Factors affecting screening effect:

• The penetrating capability of electrons in various orbitals. The outer electrons are shielded from the nuclear charge to a greater extent as the orbitals’ penetrating power increases. The following is the order of increasing penetration power: s > p > d > f
• The distance between the nucleus and the electrons. As a result, the inner electrons will have a stronger screening effect, while the outer electrons will have a less screening effect.
• The magnitude of the screening effect is proportional to the number of inner electrons. The higher the number of inner electrons, the stronger the screening effect.
• The screening effect, in which outer electrons do not encounter the full positive charge of the nucleus because the negative charges of the inner electrons partially cancel out the positive charge.
• The screening energy required to expel an electron from an atom decreases when the outer electron shell is shielded from the nucleus by additional electrons. The lower the ionization energy, the greater the screening effect. Screening, often known as the screening effect, is essentially a barrier effect.
• This is because the energy reduces from top to bottom inside a group due to the screening effect. ionization, As a result, we may claim that cesium has the lowest ionisation energy while fluorine has the highest ionization energy.