![]() The decrease in force of attraction on valence e due to inner shell e is called screening effect or shielding effect. When more than one electron is present, however, the total energy of the atom or the. Valence shell e suffer force of attraction due to nucleus and force of repulsion due to inner shell electrons. Effective Nuclear Charge (Z eff) For an atom or an ion with only a single electron, we can calculate the potential energy of an electron by considering only the electrostatic attraction between the positively charged nucleus and the negatively charged electron. ![]() This is because as Z increases by a small interval, the shell number increases, and so the electrons in the valence shell are much farther from the nucleus and are more shielded by all the electrons in the lower shell numbers. It can be approximated by the equation: Zeff Z - S, where Z is the atomic number and S is the number of shielding electrons. Screening effect ( ) and effective nuclear charge (Z eff)1. This rule calculates Zeff from the actual number of protons in the nucleus and the effect. \( \newcommand\) (from Ne to Na, for example). The effective nuclear charge can be determined by using Slaters rule.
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