Question

explain why 3d orbitals have poor shielding effect

Answer 1

Explanation:

Screening effect order

s>p>d>f

Answer 2

Answer:

Due to the presence of s and p electrons the effective nuclear charge is reduced as a result of inter-electronic repulsion.

Explanation:

Poor shielding effect - This is known as shielding effect or screening effect. Poor shielding therefore means poor screening of nuclear charge. In other words, the nuclear charge is not effectively screened by electrons in question. - s orbitals have the largest screening effect for a given n value since s electrons are closer to the nucleus.

So as they (D and F electrons) are loosely attracted to the nucleus which means that they cannot shield the nucleus which means they have poor shielding (screening) effect.