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Arrange s,p and d subshells of a shell i...

Arrange s,p and d subshells of a shell in the increasing order of effective nuclear charge `(Z_(eff))` experienced by the electron present in them.

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Greater the closeness of an electron shell to the nucleus, more is the effective nuclear charge `(Z_("eff")` experienced by it. The increasing order of `Z_("eff")` is `d lt p lt s`.
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Arrange S,P and d sub-shells of a shell in the decreasing order of effective nuclear charge (Zeff) experienced by the electron present in them

The increasing order of effective nuclear charge in Na, AI, Mg and Si atoms

Which of the following is generally true regarding effective nuclear charge (Z_(eff)) :

Calculate the effective nuclear charge experienced by the 4s -electron in potassium atom (Z = 19) .

Effective nuclear charge (Z_(eff)) for a nucleus of an atom is defined as

" The effective nuclear charge of Nitrogen for 2p electron (last electron) is "

The reducing effect of the nuclear charge by the inner electrons for on outer electron is termed aas shielding (or screening). As a result of shielding, the outer electrons in an atom always experience less nnuclear charge than the actual nuclear charge Z. The effective nuclear charge (Z^(**)) as experienced by an electron is then obtained by subtracting the total shielding contributions from alll the other electrons (i.e., except the one under consideration) from the actual nuclear charge. Z^(**)=Z-sigma Where sigma =sum of the shielding contributions. The rules for estimating contributions to sigma are as follows (Slater's rule) Contribution to shielding by each electron is : |{:("Electron","All Higher","Same","Group","Group"le),("Grpoup","Group","Group",n-1,n-2),(1s," "0,0.30,-,-),((ns,sp)," "0,0.35,0.85,1.00),((nd)or(nf)," "0,0.35,1.00,1.00):}| According to Slater's treatment, the energy of an electron in nth shell of an atom having atomic number Z is given by the empirical equation E=-13.6((Z^(**))/(n))^(2)eV Z^(**) = effective nuclear charge The correct order of radii is:

The reducing effect of the nuclear charge by the inner electrons for on outer electron is termed aas shielding (or screening). As a result of shielding, the outer electrons in an atom always experience less nnuclear charge than the actual nuclear charge Z. The effective nuclear charge (Z^(**)) as experienced by an electron is then obtained by subtracting the total shielding contributions from alll the other electrons (i.e., except the one under consideration) from the actual nuclear charge. Z^(**)=Z-sigma Where sigma =sum of the shielding contributions. The rules for estimating contributions to sigma are as follows (Slater's rule) Contribution to shielding by each electron is : |{:("Electron","All Higher","Same","Group","Group"le),("Grpoup","Group","Group",n-1,n-2),(1s," "0,0.30,-,-),((ns,sp)," "0,0.35,0.85,1.00),((nd)or(nf)," "0,0.35,1.00,1.00):}| According to Slater's treatment, the energy of an electron in nth shell of an atom having atomic number Z is given by the empirical equation E=-13.6((Z^(**))/(n))^(2)eV Z^(**) = effective nuclear charge The size of isoelectronic species -F^(-),Na^(+) and Mg^(2+) is effected by:

Knowledge Check

  • Arrange S,P and d sub-shells of a shell in the decreasing order of effective nuclear charge (Zeff) experienced by the electron present in them

    A
    `S lt P lt d`
    B
    `S gt P gt d`
    C
    `S gt d gt P`
    D
    `P gt S gt d`

  • The increasing order of effective nuclear charge in Na, AI, Mg and Si atoms

    A
    `Na lt Mg lt SI lt AI`
    B
    `Na lt Mg lt AI lt Si`
    C
    `Mg lt Na lt AI lt Si`
    D
    `Na = Mg = Al = Si`

  • Which of the following is generally true regarding effective nuclear charge (Z_(eff)) :

    A
    It increases on moving left to right in a period.
    B
    It remains almost constant on moving top to bottom in a group.
    C
    For isoelectronic species, as `Z` increases, `Z_(eff)` decreases.
    D
    Both `(A)` and `(B)`
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