The formula for an effective nuclear charge is- if - is screening constant

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Standard XII

Chemistry

Shielding Effect

The formula f...

Question

The formula for an effective nuclear charge is:
(if $σ$ is screening constant)

Z - σ

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Z + σ

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Z σ^{- 1}

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Z σ

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Solution

The correct option is D $Z - σ$
The effective nuclear charge is the net positive charge experienced by valence electrons. It can be approximated by the equation: Z_eff = Z – $σ$ , where Z is the atomic number and $σ$ is the number of shielding electrons or screening constant. Hence the answer is option (A)

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Similar questions

Q. As per Pauling, the radius of an isoelectronic ion in a given crystal is inversely proportional to the effective nuclear charge,

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; where

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Q. To determine the radii of a univalent ion, Pauling gave a method as follows:
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ii.

r_{M}^{+} + r_{X}^{-} = \frac{c}{Z_{e f f} (M^{+})} + \frac{c}{Z_{e f f} (X^{-})}

Z_{e f f}

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Z_{e f f} = Z - σ

; where

σ

is the screening constant. For

Ne, σ = 4.5

∴ r_{M}^{+} = \frac{c}{Z_{eff} (M^{+})}

and

r_{X}^{-} = \frac{c}{Z e f f (X^{-})}

The actual interionic distance in

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Q. To determine the radii of a univalent ion, Pauling gave a method as follows:
i. In an ionic crystal of the type

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, cations and anions are in contact with each other. Therefore, the sum of their ionic radius is equal to the interionic distance.
ii.

r_{M}^{+} + r_{X}^{-} = \frac{c}{Z_{e f f} (M^{+})} + \frac{c}{Z_{e f f} (X^{-})}

Z_{e f f}

is the effective nuclear charge

Z_{e f f} = Z - σ

; where

σ

is the screening constant. For

Ne, σ = 4.5

∴ r_{M}^{+} = \frac{c}{Z_{eff} (M^{+})}

and

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The actual interionic distance in

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should be:

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The

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Q. Assuming

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axis inter nuclear axis. which orbitals overlap to form

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The formula for an effective nuclear charge is: (if σ is screening constant)

The formula for an effective nuclear charge is:
(if $σ$ is screening constant)