Consider the isoelectronic ions Cl- and K+. (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S, calculate Zeff for these two ions. (c) Repeat this calculation using Slater’s rules to estimate the screening constant, S.

Verified step by step guidance

1. Step 1: Understand the concept of effective nuclear charge (Z_{eff}). It is the net positive charge experienced by an electron in a multi-electron atom. The formula is Z_{eff} = Z - S, where Z is the atomic number and S is the screening constant.
2. Step 2: For part (b), calculate Z_{eff} using the assumption that core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S. Identify the number of core electrons for Cl^- and K^+.
3. Step 3: For Cl^-, the atomic number (Z) is 17. Determine the number of core electrons and calculate S. Then, use Z_{eff} = Z - S to find the effective nuclear charge for Cl^-.
4. Step 4: For K^+, the atomic number (Z) is 19. Determine the number of core electrons and calculate S. Then, use Z_{eff} = Z - S to find the effective nuclear charge for K^+.
5. Step 5: For part (c), apply Slater's rules to estimate the screening constant, S, for both Cl^- and K^+. Slater's rules provide a more detailed method to calculate S by considering different contributions from electrons in various shells. Use these rules to recalculate Z_{eff} for both ions.