(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the \(3 s\) and \(3 p\) valence electrons in P? (b) Repeat these calculations using Slater's rules. (c) Detailed calculations indicate that the effective nuclear charge is \(5.6+\) for the \(3 s\) electrons and \(4.9+\) for the \(3 p\) electrons. Why are the values for the \(3 s\) and \(3 p\) electrons different? (d) If you remove a single electron from a Patom, which orbital will it come from?

In summary, for Phosphorus (P) with the electron configuration 1s² 2s² 2p⁶ 3s² 3p³, the effective nuclear charge (Z_eff) for both 3s and 3p valence electrons without valence electron screening would be +5. Using Slater's rules, Z_eff is +12.05 for 3s valence electrons and +12.9 for 3p valence electrons. The difference between these values and the detailed calculation result (5.6+ for 3s and 4.9+ for 3p electrons) is due to Slater's rules being an approximation and not accounting for certain electron interactions accurately. The 3s and 3p electrons experience different shielding levels due to their different spatial distributions. When a P atom loses an electron, the electron is removed from the 3s orbital since it has a lower energy and shielding effect than the 3p orbital.