Question

1st: 620 kJ/mol

2nd : 1048 kJ/mol
3rd : 9144 kJ/mol
4th : 18724 kJ/mol
5th : 24141 kJ/mol
6th : 30724 kJ/mol
7th : 38761 kJ/mol
8th : 47867 kJ/mol
9th : 59877 kJ/mol
Use the successive ionization energies for this unknown element to identify the family it
belongs to.

Answer 1

Judging by the large increase in ionization energy after the third electron is removed, it indicates that the unknown element likely belongs to Group 3 of the periodic table.

Step-by-step explanation:

To determine which family the unknown element with the given successive ionization energies belongs to, we must look at the pattern of the ionization energies. A significant jump between successive ionization energies typically indicates the removal of an electron from a new, closer to the nucleus energy level, signifying that the previous energy level has been emptied. This usually happens after the valence electrons have been removed.

In the given data, there's a substantial increase from the third ionization energy (9144 kJ/mol) to the fourth (18724 kJ/mol). This suggests that the first three electrons are much easier to remove and are likely the valence electrons. Thus, the element is likely from Group 3 on the periodic table because it appears to have three valence electrons.

An element from Group 3 would exhibit such a pattern of ionization energies, indicative of having three electrons in its outermost shell.

Answer 2

Since there is a big jump between the 2nd and 3rd electron, it is difficult to lose the 3rd electron so it must have a +2 charge. In others words, it belongs to the alkaline earth metals group.