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LIVE LAB 12 • ATOMIC STRUCTURE
Visualise effective nuclear charge as nuclear attraction minus shielding, apply Slater's rules across Period 2 and Group 1, and compare s, p, d and f penetration.
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COMPLETE CONCEPT GUIDE
An electron in a many-electron atom experiences nuclear attraction together with interactions involving other electrons. Effective nuclear charge is a simplified way to describe the net attraction for a chosen electron.
Z is the atomic number and S is an estimated shielding constant. Slater’s rules assign contributions from different electron groups to estimate S. Zeff is specific to the electron being considered, rather than one universal value for every electron in an atom.
For the 3s electron of sodium, Slater’s rules assign 8 × 0.85 from the second shell and 2 × 1.00 from the first. This gives S = 8.8 and an estimated Zeff = 11 − 8.8 = 2.2. The result is a model estimate, not an exact measured charge.
For a given principal shell, s orbitals generally penetrate closer to the nucleus than p, d and f orbitals. Across a period, increasing nuclear charge is only partly offset by shielding, helping explain the general decrease in atomic size.
Z-EFFECTIVE FAQ
No. Ionic charge is the net charge after gaining or losing electrons. Effective nuclear charge describes an estimated nuclear attraction experienced by a particular electron after shielding.
No. They provide a useful approximate shielding calculation. Detailed atomic behaviour requires a more complete treatment of electron distributions and interactions.
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