ionization energy

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Clarissa Nava 3H
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ionization energy

Postby Clarissa Nava 3H » Sat Dec 08, 2018 7:16 pm

is this energy the energy that required in order to remove an electron from an atom ?

Chem_Mod
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Re: ionization energy

Postby Chem_Mod » Sat Dec 08, 2018 10:33 pm

Correct

904901860
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Re: ionization energy

Postby 904901860 » Sun Dec 09, 2018 12:35 am

yes, it also decreases across the period and down a group

505106414
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Re: ionization energy

Postby 505106414 » Thu Oct 10, 2019 11:36 pm

When would I use this in a calculation, like what would the problem be asking?

Nare Arakelian Dis 3E
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Re: ionization energy

Postby Nare Arakelian Dis 3E » Sun Oct 20, 2019 12:34 am

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.

AmyL_3L
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Re: ionization energy

Postby AmyL_3L » Sun Oct 20, 2019 6:43 pm

Yes; the ionization energy increases from left to right and bottom to top on the periodic table of elements.

Rishika Yadav 3D
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Re: ionization energy

Postby Rishika Yadav 3D » Sun Oct 20, 2019 6:44 pm

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

Jennifer Yang 3F
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Re: ionization energy

Postby Jennifer Yang 3F » Sun Oct 20, 2019 7:19 pm

That is correct, and they might ask you to compare the ionization energy of two atoms.

Tahlia Mullins
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Joined: Thu Jul 25, 2019 12:15 am

Re: ionization energy

Postby Tahlia Mullins » Sun Oct 20, 2019 8:41 pm

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.

Elizabeth Harty 3A
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Re: ionization energy

Postby Elizabeth Harty 3A » Sun Oct 20, 2019 8:45 pm

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.

Abraham De Luna
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Joined: Sat Sep 14, 2019 12:16 am

Re: ionization energy

Postby Abraham De Luna » Sun Oct 20, 2019 11:30 pm

Ionization energy is indeed the energy required to remove an electron from an atom.

Sean Tran 3D
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Re: ionization energy

Postby Sean Tran 3D » Sun Oct 20, 2019 11:32 pm

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.


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