top of page

State the general trend in first ionization energy as the elements in Period 3 are considered from l


First ionization energy is the amount of energy needed to take first electron from an atom. The trend for ionization energy is that it increases from the bottom to the top and from the left to the right.


Why? The bigger an atom's radius is, the further away outer electrons from the pulling of the nucleus are and the less energy is needed to take them away. Thus, ionization energy trend is opposite of that of radius.


Therefore, as the elements in Period 3 are considered from left to right, the first ionization energy will increase since the radius decreases in this direction.

The ionization energy for the second electron is much greater than first, since it's harder to put a charge on an already charged ion.

For more information please talk to our incredible Chemistry Tutors in Washington DC, NYC, Brooklyn and online and call 646-407-9078. We have tutors students from most of NYC private and public schools, as well as various colleges.

0 comments

Ready For Chemistry Tutoring?

I tutor all levels of chemistry including general and organic chemistry.

Click To Learn More

What subject are you taking?
Regents Chemistry
General Chemistry
Organic Chemistry

Join our email list 

bottom of page