Among elements 1–18, which element or elements have the smallest effective nuclear charge if we use the equation zeff=z−s to calculate zeff? check all that apply.

Element H have the smallest effective nuclear charge

The effective nuclear charge is the nuclear charge which is influenced by the shielding effect of electrons

The effective nuclear charge (Zeff) can be formulated as:

with

Z = nuclear charge = atomic number

S = shield constant

Shielding constants are constants that are generated from the core attraction of electrons in the inner shell

Rules for calculating shield constants-S (Slater's Rules)

/ 1s / 2s, 2p / 3s, 3p / 3d / 4s, 4p / 4d / 4f / 5s, 5p / 5d / 5f /

* Electrons in the same shell shielding effects (same ns and np orbitals): 0.35

* Electrons in the deeper shell (n-1, in the lower shell one energy level), shielding effects = 0.85

* Electrons in the shell deeper (left of n-1, in the shell two energy levels and lower) shielding effects = 1.00

Elements with atomic numbers 1-18 lie in periods 1 through period 3

If we want to calculate the smallest effective nuclear charge, then we determine the electron configuration of each element

Logically, with the smallest atomic number, the H atom will have the smallest Z eff

Configuration of H element

H: 1s¹

Z = 1

S = 0

Z eff = Z - S = 1-0 = 1

So the valueof Z eff = Z

The effective nuclear charge

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X is the effective nuclear charge, and it increases across a period.

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The effective nuclear charge of an atom is primarily affected by

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explanation:

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