Final answer:
Element 115 is expected to have a lower ionization energy than bismuth, mainly due to its position below bismuth in the periodic table and the effects of increased electron shielding.
Step-by-step explanation:
Would you expect element 115 to have an ionization energy greater than, equal to, or less than that of bismuth? Given the information about ionization energies across the periodic table, we can predict the following for element 115 compared to bismuth. Bismuth is in group 15 and is known for its relatively low reactivity, often giving up three valence electrons to form Bi³+. This is indicative of its ionization energy.
As you move down a group in the periodic table, ionization energy generally decreases, mainly due to increased electron shielding. Since element 115 would be below bismuth in the periodic table, it would likely have more electron shielding due to additional electron shells. The increased distance and electron shielding between the outer electrons and the nucleus in element 115 would result in a lower ionization energy compared to bismuth, as it would be easier to remove an electron from element 115 than from bismuth.