wisc.pb.unizin.org/chem103and104/chapter/core-valence-electrons-shielding-zeff-m7q8/
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electrons in the same valence shell do not block the nuclear attraction experienced by each other as efficiently
Zeff = Z – S, where S is the number of core electrons that are shielding the valence electrons.
Shielding is determined by the probability of another electron being between the electron of interest and the nucleus, as well as by the electron–electron repulsions the electron of interest encounters.
the electron farther away experiences an effective nuclear charge (Zeff).
The electrons occupying the outermost shell orbital(s) are called valence electrons
those occupying the inner shell orbitals are called core electrons
the nuclear charge an electron actually experiences because of shielding from other electrons closer to the nucleus
the Zeff is always less than the actual nuclear charge, Z.
Thus, each time we move from one element to the next across a period, Z increases by one, but the shielding increases only slightly. Thus, Zeff for valence electrons increases as we move from left to right across a period.
Zeff = Z – S, where S is the number of core electrons that are shielding the valence electrons.
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