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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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s-orbital, being spherical in shape, shields the electrons from the nucleus more effectively than p-orbital which in turn shields more effectively than d-orbital. Hence, the increasing order of effective nuclear charge `(Z_("eff"))` experienced by the electrons present in them is: `d lt p lt s`
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Calculate the effective nuclear charge experienced by the 4s -electron in potassium atom (Z = 19) .

Down the group in the Periodic Table, the effective nuclear charge experienced by valence electrons ___ ___.

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

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

    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:

    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 Z^(**) for a 1st electron in Fe atom is:

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