Effective nuclear charge ( $Z_{e f f}$ ) for a nucleus of an atom is defined as:

Shielding of the outermost shell electrons from the nucleus by the innermost shell electrons

No worries! We‘ve got your back. Try BYJU‘S free classes today!

The net positive charge experienced by electron from the nucleus

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

The attractive force experienced by the nucleus from electron

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Screening of positive charge on nucleus by innermost shell electrons.

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B The net positive charge experienced by electron from the nucleus
The effective nuclear charge $Z_{e f f}$ is the net positive charge experienced by an electron from the nucleus in a polyelectronic atom.

The term "effective" is used because the shielding effect of negatively charged electrons prevents higher orbital electrons from experiencing the full nuclear charge of the nucleus due to the repelling effect of inner-layer electrons.

Hence, the correct option is $B$

Suggest Corrections

Similar questions

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. 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. 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.

The force experienced by an electron towards the nucleus is and away from the nucleus is .

On moving across a period, the atomic size decreases and nuclear charge increases and therefore the force of attraction exerted by the nucleus on the electron in the outermost shell increases.
The first ionization potentials (in eV) of As and Se atoms, respectively, are:

Join BYJU'S Learning Program

Effective nuclear charge (Zeff) for a nucleus of an atom is defined as:

Effective nuclear charge ( $Z_{e f f}$ ) for a nucleus of an atom is defined as: