Question

Identify the element of Period 3 that has the following successive ionization energies, in kJ/mol.

IE1 = 1314 IE2 = 3389 IE3 = 5298 IE4 = 7471 IE5 = 10992 IE6 = 13329 IE7 = 71345 IE8 = 84087

a. Li
b. Ne
c. B
d. O

Answer 1

The Period 3 element with the given ionization energies is Oxygen (O), identified by the significant jump in ionization energy between the sixth and seventh ionizations. The correct answer is option: d. O

Step-by-step explanation:

The question is asking to identify the element from Period 3 of the periodic table that matches the given successive ionization energies.

To solve this, you need to look at the trends of ionization energy across the periodic table and relate the large jump in ionization energy to the removal of an electron from a new, lower energy level.

In this case, IE7 is significantly higher than IE6, indicating that the first six electrons were removed from outer energy levels and the seventh electron is being removed from a more tightly bound inner energy level.

This kind of large jump commonly occurs when the electrons start to be removed from a noble gas configuration.

Since the element in question has six electrons before reaching a noble gas configuration, it would correspond to Oxygen (O), which has the electron configuration of Neon after the removal of six electrons.