Answer Happy

35 ALL BUT ONE of the following sentences provide reasonable explanations for the overall trend and the irregularities observed in the first ionization energies (i.e., IE1) of the neutral atoms of the elements shown in the table. Identify the one statement that is INCORRECT. Na Mg ΑΙ Si P S CI Ar IE [kJ/mol] 496 738 577 787 1012 1000 1251 1520 When one electron is removed from a neutral sulfur atom, it adopts a configuration where all 3p orbitals are equally populated with one unpaired electron which helps stabilizing the resulting Stion. That is why the E of sulfur has a slightly lower than expected ionization energy Ob For elements in a same row, the effective nuclear charge is directly proportional to the atomic number. That explains the overall trend we observe when ionization energy increases as we move to the right in the periodic system Oc Removing a paired electron from a 3s subshell consumes more energy than removing an unpaired electron from a 3p subshell. This could explain why the ionization energy of Mg is significantly higher than that of Al od The higher the energy level is the more energy will be required to remove electrons from the atom. The same apply to the orbitals in the same energy level: electrons in higher-energy orbitals will have a higher ionization energy than those in lower-energy orbitals