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ionization energy

Posted: Sat Dec 08, 2018 7:16 pm
by Clarissa Nava 3H
is this energy the energy that required in order to remove an electron from an atom ?

Re: ionization energy

Posted: Sat Dec 08, 2018 10:33 pm
by Chem_Mod
Correct

Re: ionization energy

Posted: Sun Dec 09, 2018 12:35 am
by 904901860
yes, it also decreases across the period and down a group

Re: ionization energy

Posted: Thu Oct 10, 2019 11:36 pm
by 505106414
When would I use this in a calculation, like what would the problem be asking?

Re: ionization energy

Posted: Sun Oct 20, 2019 12:34 am
by Nare Arakelian Dis 3E
The problem could just be asking to compare the ionization energies of two elements and state which is larger. The energy of a photon = ionization energy plus the kinetic energy so the value of the ionization energy could also be used here for a photoelectric effect problem.

Re: ionization energy

Posted: Sun Oct 20, 2019 6:43 pm
by AmyL_3L
Yes; the ionization energy increases from left to right and bottom to top on the periodic table of elements.

Re: ionization energy

Posted: Sun Oct 20, 2019 6:44 pm
by Rishika Yadav 3D
You are right, and just as a tip to help you remember, I like to think of it as the energy required to create an ion, thus ionization energy

Re: ionization energy

Posted: Sun Oct 20, 2019 7:19 pm
by Jennifer Yang 3F
That is correct, and they might ask you to compare the ionization energy of two atoms.

Re: ionization energy

Posted: Sun Oct 20, 2019 8:41 pm
by Tahlia Mullins
A good way to remember what this is would be to relate its trends to the trends in atomic radius since the larger the atomic radius, the greater the ionization energy, so their trends line up since they are in direct relationship with one another.

Re: ionization energy

Posted: Sun Oct 20, 2019 8:45 pm
by Elizabeth Harty 1A
Yes and for the periodic trends you can always determine the trend based on stuff you already know (for instance atomic radius). As atomic radius increases as you go down a group, the nuclear pull on the outer electrons is less and thus the ionization energy is lower. Moreover, as you go across a period, the atomic radius decreases and as you adding electrons to the same energy shell, and therefore the ionization energy increases.

Re: ionization energy

Posted: Sun Oct 20, 2019 11:30 pm
by Abraham De Luna
Ionization energy is indeed the energy required to remove an electron from an atom.

Re: ionization energy

Posted: Sun Oct 20, 2019 11:32 pm
by Sean Tran 2K
The first ionization energy of an electron is the energy required to remove the first electron from a ground state atom. The trend for this is seen on the periodic table as you go to the right and up.