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While dealing with multielectron atoms o...

While dealing with multielectron atoms or ions, we must use the concept of effective nuclear charged, `Z_(eff)` which is calculated by the formula

A

`Z_(eff) = Z + sigma`

B

`Z_(eff) = Z//sigma`

C

`Z_(eff) = Z - sigma`

D

`Z_(eff) = Zsigma^(2)`

Text Solution

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The correct Answer is:
C
`Z_(eff)` is taken to be equal to the actual nuclear charge `(Z)` minus the screening or shielding) constant, `sigma`, of the inner screening electrons. The attraction of the outermost electrons by the nucleus is partly counterbalanced by the repulsion of teh outermost electrons by the electrons in the inner shell.
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J.C. Slater proposed an empirical constant that represents the cumulative extent to which the other electrons of an atom shield (or screen) any particular electron from the nuclear charge. Thus, slater's screening contant sigma is as : Z^(**)=Z-sigma Here, Z is the atomic number of the atom, and hence is equal to the actual number of protons in the atom. the parameter Z^(**) is the effective nuclear charge, which according to is smaller than Z, since the electron in question is screened (shielded) from Z by an amount sigma . Conversely, an electron that is well shielded from the nuclear charge Z experiences a small effective nuclear charge Z^(**) . The value of sigma for any one electron in a given electron configuration (i.e., in the presence of the other electrons of the atom in question) is calculated using a set of empirical rules developed by slater. according to these rules, the value of sigma for the electron in question is the cumulative total provided by the various other electrons of the atom. Q. Which of the following statement is correct?

According to I.C slater effective nuclear charge, Z^(**) , due to screening, is not exactly equal to the actual nuclear charge Z of the nucleus of the atom. Z^(**) depends on the type of orbitals in which the electron is housed, and on the ability of other electrons in more penetrating orbitals to screen the electron in question from the nucleus. The relative extent to which the various orbitals penetrate the electron clouds of other orbitals is s gt p gt f . The effective nuclear charge Z^(**) due to screening is given by Z^(**)=Z-sigma , where Z is the atomic atomic number and sigma is the slater screening constant values 0 lt sigma lt Z Screening effect of one electron in the outermost orbitals, is not considered in calculate of sigma . In which of the following cases the concept of Z^(**) is applicable?

J.C. Slater proposed an empirical constant that represents the cumulative extent to which the other electrons of an atom shield (or screen) any particular electron from the nuclear charge. Thus, slater's screening contant sigma is as : Z^(**)=Z-sigma Here, Z is the atomic number of the atom, and hence is equal to the actual number of protons in the atom. the parameter Z^(**) is the effective nuclear charge, which according to is smaller than Z, since the electron in question is screened (shielded) from Z by an amount sigma . Conversely, an electron that is well shielded from the nuclear charge Z experiences a small effective nuclear charge Z^(**) . The value of sigma for any one electron in a given electron configuration (i.e., in the presence of the other electrons of the atom in question) is calculated using a set of empirical rules developed by slater. according to these rules, the value of sigma for the electron in question is the cumulative total provided by the various other electrons of the atom. Q. The effective nuclear charge at the periphery of chromium atom [Z=24]:

J.C. Slater proposed an empirical constant that represents the cumulative extent to which the other electrons of an atom shield (or screen) any particular electron from the nuclear charge. Thus, slater's screening contant sigma is as : Z^(**)=Z-sigma Here, Z is the atomic number of the atom, and hence is equal to the actual number of protons in the atom. the parameter Z^(**) is the effective nuclear charge, which according to is smaller than Z, since the electron in question is screened (shielded) from Z by an amount sigma . Conversely, an electron that is well shielded from the nuclear charge Z experiences a small effective nuclear charge Z^(**) . The value of sigma for any one electron in a given electron configuration (i.e., in the presence of the other electrons of the atom in question) is calculated using a set of empirical rules developed by slater. according to these rules, the value of sigma for the electron in question is the cumulative total provided by the various other electrons of the atom. Q. According to Slater's rule, order of effective nuclear charge (Z^(**)) for last electron in case of Li, Na and K.

R SHARMA-CLASSIFICATION OF ELEMENTS AND PERIODICITY IN ELEMENTS-Follow-up Test
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  3. While dealing with multielectron atoms or ions, we must use the concep...

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  6. The first ionzation enthalpies generally increase form to right across...

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  7. The largest ionization enthalpies in any period occur for the

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  9. Ionization enthalpies tend to decrease going down any column of main g...

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  10. Ionizarion is not limited to the removal of a single electron from an ...

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  11. Which of the following elements has a large jump between its fourth an...

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  13. The first four ionization enthalpies of an element are 578 kJ mol^(-1)...

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  14. Electron gain enthalpy of an element is a measure of its atom's abilit...

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  15. Which of the following is a measure of the firmness or strength with w...

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  16. Electron gain enthalpy is greater than zero for

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  17. Which of the following elements have the most negative electron gain e...

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  18. The general horizontal trend is that electron gain enthalpies become m...

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  19. Electron gain enthalpies of free anions are always

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