Question

considering periodic trends, valence electrons in which of the following atoms experience the greatest effective nuclear charge (zeff)?

Answer 1

The effective nuclear charge is the difference between the atomic number an element and the shielding constant. Hence, the atom which experiences the greatest nuclear charge is Sulphur, S.

Calculating the greatest effective nuclear charge, :

• $Z_{eff} = Z - S$

• Z = Atomic number ; S = shielding constant

For Magnesium, Mg:

Z = 12

S = 10

$Z_{eff} = 12 - 10 = 2$

For Aluminium, Al:

Z = 13

S = 10

$Z_{eff} = 12 - 10 = 3$

For Sulphur, , S:

Z = 16

S = 10

$Z_{eff} = 16 - 10 = 6$

Therefore, the atom whuch experience the greatest $Z_{eff}$ is Sulphur.

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