Arrange s, p and d sub-shells of a shell in the increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electron present in them.

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Solution

The increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electrons present in them is $d < p < s$

Understanding the concept of effective nuclear charge $(Z_{e f f})$

Net positive charge experienced by an outer electron is known as effective nuclear charge $(Z_{e f f})$ , which is closest or equal to the actual nuclear charge.

When we move away from the core electrons to the outer valence electrons, $Z_{e f f}$ decreases significantly.

This is due to the shielding, electrons in an atom can shield each other from the pull of the nucleus. The electrons closest to the nucleus cause a decrease in the amount of nuclear charge exerted on the outer electrons.

Analyzing the order of effective nuclear charge of subshell

This shielding effect, describes the decrease in attraction between an electron and the nucleus in any atom with more than one electron shell. The more the number of electron shells, the greater the shielding effect experienced by the outermost electrons.

s-orbital, being spherical in shape, shields the electrons from the nucleus more effectively than p-orbital and d-orbital and the electrons in it experience the maximum nuclear attraction.

p-orbital being dumb-bell shaped and
d-orbital being double dumb-bell shaped,
d-orbitals have more dispersion of charge than
p-orbital and thus, p-orbital shields nucleus
more effectively than d-orbital.

Hence, the increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electrons present in them is $d < p < s$

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Question 22

Arrange s, p and d subshells of a shell in the increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electron present in them.

Q. Arrange

s, p

and

d

sub-shells of a shell in the increasing order to effective nuclear charge

(Z_{e f f})

experienced by the electron present in them.

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.
Ionization energy is not influenced by :

Q. The maximum number of electrons in s, p and d sub shells are:

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.

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Nature of Matter

Standard XII Chemistry

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Arrange s, p and d sub-shells of a shell in the increasing order of effective nuclear charge (Zeff)experienced by the electron present in them.

Arrange s, p and d sub-shells of a shell in the increasing order of effective nuclear charge $(Z_{e f f})$ experienced by the electron present in them.