At first glance, we expect the zeff of a valence electron of sodium (z = 11) to be 1 but in reality, it is closer to 2. 667 because of the theoretical nuclear charge for sodium and the justification for its discrepancy from the real nuclear charge are the subjects of this problem. In the end, the answers are 1+ because there is a slight chance that the 3s1 electron will be nearer the nucleus.
Effective nuclear charges
In chemistry, the effective nuclear charge is defined as the net positive charge valence electrons experience. In addition, one can approximate it with the equation: Zeff = Z – S, Where Z is the atomic number or number of electrons and S is the core electrons. In such a way, since sodium has 11 electrons and 10 core electrons due to its electron configuration (1s²2s²2p⁶3s¹), one concludes its effective nuclear charge is:
Zeff = 11 - 10 = +1 . On the other hand, given that the actual effective nuclear charge is approximately 2.667, one can infer that the 3s1 electron is likely to experience a stronger attraction than what was predicted by the theoretical model because of its slight tendency to be closer to the nucleus.
Learn more about effective nuclear charges at: brainly.com/question/6965287
#SPJ4
