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Stability of Fully Filled and Half Filled Orbitals

does the shie...

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does the shield that is developed by the inner electrons except the valence electrons cover the nucleus in a 3 dimensional plane?

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The valence "s” electrons act as inner core electrons due to poor shielding of "d” and "f”. This is known as the inert pair effect.

Q. The nuclear charge actually experienced by an electron is termed as the effective nuclear charge. The effective nuclear charge Z* actually depends on the type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate the electron clouds of other orbitals is

s > p > d > f

(for the same value of

n

)
The phenomenon in which penultimate shell electrons act as screen or shield in between nucleus and valence shell electrons and thereby reducing nuclear charge is known as shielding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with the nucleus. It is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy.
Which of the following valence electron experience maximum effective nuclear charge?

Q. Due to inter electronic repulsion, an electron experiences less nuclear charge. It is, therefore, said that inner electronic shells electrons shield the nucleus. The actual nuclear charge experienced by an electron is called effective nuclear charge. If the electrons in K-shell shields the nucleus to the extent of 0.5 (say) each. What will be the wave number of the spectral line arising out of n=4 to n = 2 transition in He atom?

Q. In an atom, electrons are arranged around the nucleus in various shells. What do ‘valence electrons’ refer to?

4 p

4 d

4 f

orbitals of increasing degree to which the electrons present in them are shielded by inner electrons?

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Stability of Fully Filled and Half Filled Orbitals

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