+
2 Tutorials that teach Periodic Trends: Ionization Energy
Take your pick:
Periodic Trends: Ionization Energy
Next Generation: HS.PS1.1 HS.PS1.1

Periodic Trends: Ionization Energy

Author: Marilyn Nowicki
Description:
This lesson will explain how the ionization energy changes over representative elements across rows and up and down columns on the periodic table.
(more)
See More
Try a College Course Free

Sophia’s self-paced online courses are a great way to save time and money as you earn credits eligible for transfer to over 2,000 colleges and universities.*

Begin Free Trial
No credit card required

25 Sophia partners guarantee credit transfer.

221 Institutions have accepted or given pre-approval for credit transfer.

* The American Council on Education's College Credit Recommendation Service (ACE Credit®) has evaluated and recommended college credit for 20 of Sophia’s online courses. More than 2,000 colleges and universities consider ACE CREDIT recommendations in determining the applicability to their course and degree programs.

Tutorial

In general, as you move across a period from left to right on the periodic table, it is increasingly difficult to remove an electron from an atom. The ionization energy (energy required to do this) increases.

 

Remember that metals tend to lose electrons to form ions, while nonmetals tend to gain electrons to form ions, so electrons are easier to remove from metals than they are from nonmetals.

 

Ionization energy increases as you go from the bottom to the top of a group (or family) of elements. The smallest atomic radii are located at the top of a group, and the electrons are closer to the nucleus. The positive nucleus exerts more force on those electrons so it is harder to remove them.