the 1s electrons shield the other 2p electron to 0.85 "charges". Determine the electron configuration of nitrogen, then write it in the appropriate form. This permits us to quantify both the amount of shielding experienced by an electron and the resulting effective nuclear charge. One set of estimates for the effective nuclear charge (\(Z_{eff}\)) was presented in Figure 2.5.1. Educ., 1993, 70 (11), p 956, Kimberley A. Waldron, Erin M. Fehringer, Amy E. Streeb, Jennifer E. Trosky and Joshua J. Pearson, "Screening Percentages Based on Slater Effective Nuclear Charge as a Versatile Tool for Teaching Periodic Trends", J. Chem. Step 2: Identify the electron of interest, and ignore all electrons in higher groups (to the right in the list from Step 1).These do not shield electrons in lower groups; Step 3: Slater's Rules is now broken into two cases: What is the shielding constant experienced by a 3d electron in the bromine atom? What is the effective nuclear charge experienced by a valence p- electron in boron? The shielding numbers in Table \(\PageIndex{1}\) were derived semi-empirically (i.e., derived from experiments) as opposed to theoretical calculations. For example, Clementi and Raimondi published "Atomic Screening Constants from SCF Functions." Legal. Slater's rules are fairly simple and produce fairly accurate predictions of things like the electron configurations and ionization energies. 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