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The order of screening effect of electro...

The order of screening effect of electrons of s, p, d and f orbitals of a given shell of an atom on its outer shell electrons is
* Thinking process:To solve question, keep in mind that shielding effect represent the repulsive force felt by the valence shell from the electrons presents in the inner shells.

A

`s gt p gt d gt f`

B

`f gt d gt p gt s`

C

`p lt d lt s gt f`

D

`f gt p gt s gt d`

Text Solution

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The correct Answer is:
To determine the order of the screening effect of electrons in s, p, d, and f orbitals on outer shell electrons, we need to understand the concept of the screening effect and how it varies with the type of orbital. ### Step-by-Step Solution: 1. **Understand the Screening Effect**: - The screening effect refers to the reduction in the effective nuclear charge experienced by outer shell electrons due to the presence of inner shell electrons. This occurs because inner shell electrons repel outer shell electrons, reducing the attraction between them and the nucleus. 2. **Identify the Orbital Types**: - The orbitals in question are s, p, d, and f. Each of these orbitals is located at different energy levels relative to the nucleus: - **s orbitals** are closest to the nucleus. - **p orbitals** are at a higher energy level than s. - **d orbitals** are even further away. - **f orbitals** are the furthest from the nucleus. 3. **Determine the Order of Screening Effect**: - The closer the electrons are to the nucleus, the more they can shield the outer shell electrons from the nuclear charge. Therefore, the order of the screening effect from most effective to least effective is: - **s > p > d > f** - This means that s electrons provide the greatest shielding effect, while f electrons provide the least. 4. **Conclusion**: - The final order of screening effect of electrons in s, p, d, and f orbitals on outer shell electrons is: - **s > p > d > f**
To determine the order of the screening effect of electrons in s, p, d, and f orbitals on outer shell electrons, we need to understand the concept of the screening effect and how it varies with the type of orbital. ### Step-by-Step Solution: 1. **Understand the Screening Effect**: - The screening effect refers to the reduction in the effective nuclear charge experienced by outer shell electrons due to the presence of inner shell electrons. This occurs because inner shell electrons repel outer shell electrons, reducing the attraction between them and the nucleus. 2. **Identify the Orbital Types**: ...
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The order of screeing effect of electrons of s,p,d and f orbitals of a given shell of an atom on its outer shell electrons is:

The order of screeing effect of electrons of s,p,d and f orbitals of a given shell of an atom on its outer shell electrons is:

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Nuclear charge actually experienced by an electron is termed as effective nuclear charge. The effective nuclear charge Z^(**) actuall ydepends on 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 gt p gt d gt f (for the same value of n) The phenomenon in which penultimate shell electrons act as screen or sheild 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 nucleus. it is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy. Q. Which of the following valence electron experience maximum effective nuclear charge?

Nuclear charge actually experienced by an electron is termed as effective nuclear charge. The effective nuclear charge Z^(**) actuall ydepends on 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 gt p gt d gt f (for the same value of n) The phenomenon in which penultimate shell electrons act as screen or sheild 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 nucleus. it is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy. Q. Which of the following valence electron experience maximum effective nuclear charge?

Nuclear charge actually experienced by an electron is termed as effective nuclear charge. The effective nuclear charge Z^(**) actuall ydepends on 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 gt p gt d gt f (for the same value of n) The phenomenon in which penultimate shell electrons act as screen or sheild 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 nucleus. it is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy. Q. Which of the following is not concerned to effective nuclear charge?

Nuclear charge actually experienced by an electron is termed as effective nuclear charge. The effective nuclear charge Z^(**) actuall ydepends on 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 gt p gt d gt f (for the same value of n) The phenomenon in which penultimate shell electrons act as screen or sheild 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 nucleus. it is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy. Q. Ionzation enegy is not influenced by:

Nuclear charge actually experienced by an electron is termed as effective nuclear charge. The effective nuclear charge Z^(**) actuall ydepends on 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 gt p gt d gt f (for the same value of n) The phenomenon in which penultimate shell electrons act as screen or sheild 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 nucleus. it is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy. Q. Ionzation enegy is not influenced by:

Assertion: Shielding effect increases as we go down the group. Reason: More is the number of electrons in the penultimate shell, more is shielding.