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The term shielding is used to describe the differences in electrostatic interactions between the nucleus and electrons. This is because the outer electrons are separated from the nucleus by both distance and the inner electrons. So in summary the inner electrons are being pulled with more strength opposed to the outer electrons by the nucleus. As for specifically s and p orbitals I would assume that it has to do with how Lavelle says how the p orbital has more energy than the s orbital, so they are probably a little farther out compared to the s orbital. I forgot to mention the electrons themselves interact with each other so the more electrons the further they are repulsed from each other.
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