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zorro
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Why is the screening effect of d orbital electrons less than that of s and p electrons?
Abdul Quadeer said:how is angular momentum related to electron density?
The screening effect in atoms refers to the reduction of the effective nuclear charge experienced by an electron due to the shielding effect of other electrons in the same atom. This means that the outer electrons are not held as tightly by the nucleus and are therefore easier to remove. The lower screening effect of d orbital electrons is due to their higher energy and larger size, which results in them being less effective at shielding other electrons from the nucleus compared to the smaller and lower energy s and p electrons.
The lower screening effect of d orbital electrons can have a significant impact on the reactivity of elements. Since these electrons are less shielded from the nucleus, they are more tightly held and less likely to participate in chemical reactions. This is why transition metals, which have partially filled d orbitals, tend to be less reactive compared to elements with filled s and p orbitals.
The screening effect of d orbital electrons can be challenging to predict accurately. This is due to the complex arrangement of electrons in these orbitals, which can interact in different ways with other electrons in the atom. However, various theoretical models and calculations have been developed to estimate the screening effect of d orbital electrons in different elements.
The screening effect of d orbital electrons is a significant factor in determining the properties and trends of elements in the periodic table. As mentioned earlier, elements with partially filled d orbitals (transition metals) tend to have lower reactivity compared to elements with filled s and p orbitals. This is why transition metals are located in the middle of the periodic table, between highly reactive metals on the left and less reactive non-metals on the right.
The screening effect of d orbital electrons also plays a role in determining the atomic radius of elements. Since these electrons are not as effective at shielding other electrons from the nucleus, the outermost electrons experience a higher effective nuclear charge, resulting in a smaller atomic radius. This is why, in general, the atomic radius decreases from left to right across a period in the periodic table, which corresponds to the increase in the number of d orbital electrons.