Below are data on the first four ionization energies for a fictitious element X. First ionization energy = 500 kJ/mol Second ionization energy = 2000 kJ/mol Third ionization energy = 3500 kJ/mol Fourth ionization energy = 25000 kJ/mol From the data,which of the following statements is incorrect? A)The third ionization energy is greater than the second ionization energy because X²⁺ has a bigger charge than X⁺. B)X could belong to Group IIIA. C)X could belong to Group IIIB. D)X could belong to group VA. E)The fourth ionization energy is much greater than the third ionization energy because X³⁺ consists of a noble-gas core or a pseudo-noble-gas core.

Question

Quizplus · Accepted Answer

We can determine the group based on the number of valence electrons and the periodic trends in ionization energy. X has four valence electrons because the fourth ionization energy is much higher than the third, indicating the removal of a core electron. Group VA elements have five valence electrons, so X could belong to this group. The incorrect statement is A, which incorrectly correlates ionization energy with the charge on the ion. The correct correlation is that ionization energy increases with the number of valence electrons and decreases with increasing atomic radius. Neither B nor C can be determined from the data given.

Below Are Data on the First Four Ionization Energies for a Fictitious