Screening effect of Br and effective nuclear charge for valency electron

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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. The formula for an effective nuclear charge is:

(if

σ

is screening constant)

Ionic radii vary in
(a) inverse proportion to the effective nuclear charge
(b) Inverse proportion to the square of effective nuclear charge
(c) direct proportion to the screening effect
(d) direct proportion to the square of screening effect

Q. Screening effect of inner shells decreases the effective nuclear charge. The order of screening effect of subshells is s>p>d>f.
State whether the given statement is true or false.

Q. Calculate the effective nuclear charge for 3d-electron of nickel atom.

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