What causes shielding effect?

1 Answer
Dec 5, 2016

A greater number of electron between the nucleus and the electron in question.

Explanation:

To understand the shielding effect, consider #Z#eff or the effective nuclear charge.

The value of #Z#effective will stay constant as you go across a period and increase as you travel down. Why do you think this is?
To understand this, try think of the atomic orbital theory.

Remember that #Z#eff = Z - S

where Z is the atomic number and S is the amount of electron between the nucleus and the valence electron.

Example: Why is Cesium a larger element that Potassium?

Cs = #1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^1#

K = #1s^2 2s^2 2p^6 3s^1 3p^6 4s^1#

As you can see there are more orbitals separating the valence electrons from the nucleus of the atom, so the nucleus will have less control of the #6s^1# electron than it will of the #4s^1# electron. This is the shielding affect.