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Which orbital electrons are known to shi...

Which orbital electrons are known to shield the nuclear charge improperly? Does this enerate some irregularity in properties of elements?

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`d`-and `f`-orbital electrons are known for poor shielding of nuclear charge, because of their scattered structure. This poor shielding generates some irrengularities in properties like atomic radii and ionisation enthalpy of `d`-block element, `f`-block elements and group-13 elements.
`d`-and `f`-orbital electrons are known for poor shielding of nuclear charge, because of their scattered structure. This poor shielding generates some irrengularities in properties like atomic radii and ionisation enthalpy of `d`-block element, `f`-block elements and group-13 elements.
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Explore conceptually related problems

Which of the following does not exhibit the periodicity in properties of the elements?

Assertion : SO_(2),NO_(3)^(-) and CO_(3)^(2-) are isoelectronic as well as isostructural species. Reason :The d and f-orbital do not shield the nuclear charge very effectively. Therefore there is signified rediduction in the size of the ions, just after d or f orbital have been completely filled.

Assertion : To obtain effefctive p pi-p pi overlap, the size of the de-orbital must be similar to the p- orbital so the chlorine p pi-p pi bonding is strongest in their oxoanions. Reason :On moving period from left to right in the periodic table, the nuclear charge is incresed and more s and p-electrons are added. Since these s- and p- electron shield the nuclear charge incompletely, the size of the atom and that of the d- orbital decreases .This leads to progressively stronger p pi-d pi bonding.

Poor shielding of nuclear charge by d or f-orbital elements is responsible for which of the following facts?

Poor shielding of nuclear charge by d or f -orbital electrons is responsible for which of the following facts?

Nuclear charge actually experienced by an electron is termed as effective nuclear charge The effective nuclear Z^(**) actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is . s gt p gt d gt f (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding 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 ionizatio energy. In 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 Z^(**) actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is . s gt p gt d gt f (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding 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 ionizatio energy. 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 Z^(**) actually depends on type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate is . s gt p gt d gt f (for the same value of n) The phenomenon in which penulitmate shell electrons act as screen or shield in between nucleus adn valence shell electrons and there by reducing nuclear charge is known as sheilding 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 ionizatio energy. Ionization energy is not influenced by :

RESONANCE-PERIODIC TABLE & PERIODICITY-Exercise
  1. Why the third period of Modern periodic table contains 8 elements and ...

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  2. Tell the relation between effective nuclear charge (Z(eff)) atomic num...

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  3. Which orbital electrons are known to shield the nuclear charge imprope...

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  4. Ph^(+)compounds are very good oxidising agents. Explain.

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  5. Arange the following in correct order of stability. (i) Ga' In, TI' ...

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  6. Explain why callions are smaller and anions larger in radii than their...

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  7. The atmoic radii of palladium and platinum are nearly same. Why?

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  8. In the ionic compound KF, the K^(+) and F^(-) ions are found to have p...

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  9. Why second ionization enthalpy is always higher than the first ionisat...

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  10. The first ionization enthalpy of carbon is greater than that of boron,...

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  11. Among the elements B, AI,C and Si, (i) Which elements has the highes...

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  12. Be and Ne have positive values of electron gain enthalpy against the g...

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  13. Nitrogen has positive electron gain enthalpy whereas oxygen has negati...

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  14. Among alkali metals, which element do you expect to be least electrone...

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  15. Explain the following according to Modern periodic table: ltbr. (a) El...

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  16. The period number in the long form of the periodic table is equal to:

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  17. Which one of the following statements related to the modern periodic t...

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  18. The elements in which electrons are progressively filled in 4f-orbital...

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  19. Which of the following statements is not correct regarding hydrogen:

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  20. Atomic number of Ag is 4.7. in the same group, the atomic numbers of e...

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