The first four ionization energies in kJ/mol of a certain second-row element are 801, 2427, 3660, and 25,025. What is the likely identity of the element?

asked by @mariahl15 • 11 months ago • Chemistry • 5 pts
Add comment
1 answer

Hey there Mariah! So Ionization energy is the energy required to remove an electron from an element. Those energies should not be more than twice the previous energy, roughly. So 2427 is a little more than twice of 801 but its still ok, so is 3660. But you can see an enormous difference in energy between 3660 and 25,025. Its more than 6 times more! Something important must be going on when this element loses the 4th electron.

Most likely explanation for such a big difference is that once this element lost 3 electrons, it gained noble gas status. Once its a noble gas, it will fight very hard not to lose any more electrons. If you look at Boron and remove 3 electrons from it, it becomes Helium (a noble gas). It would take a huge amount of energy to remove an electron from a noble gas. So your element is Boron.

Let us know if you need any further explanation!

answered by @dashab2 • 11 months ago