Ionization Energy

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Matia Kim 1B
Posts: 60
Joined: Fri Apr 06, 2018 11:03 am

Ionization Energy

Postby Matia Kim 1B » Wed May 02, 2018 2:31 pm

In lecture today he said that lower ionization energy levels are cations. What is considered a low ionization energy? is it by value or position of the periodic table?

Yadira Flores 1G
Posts: 41
Joined: Wed Nov 15, 2017 3:01 am

Re: Ionization Energy

Postby Yadira Flores 1G » Wed May 02, 2018 4:40 pm

Pretty sure we're focusing on the position it has on the periodic table and not specifically by any value.

Patience Olsen 1A
Posts: 28
Joined: Fri Apr 06, 2018 11:04 am

Re: Ionization Energy

Postby Patience Olsen 1A » Thu May 03, 2018 11:08 pm

Yes, lower is just meant to be a relative term and doesn't correspond to a specific value. An element with a lower IE is more likely to become a cation than an element with a higher IE because it doesn't take as much energy to remove an electron from the element with lower IE.

Endri Dis 1J
Posts: 33
Joined: Fri Apr 06, 2018 11:02 am

Re: Ionization Energy

Postby Endri Dis 1J » Fri May 04, 2018 1:46 am

What's the difference between Ionization energies and electron affinities?

Patience Olsen 1A
Posts: 28
Joined: Fri Apr 06, 2018 11:04 am

Re: Ionization Energy

Postby Patience Olsen 1A » Fri May 04, 2018 2:02 am

Ionization energy refers to the energy required to remove an electron from an atom while electron affinity refers to the energy released when an electron is added to an atom. The trends for both correlate.
For example, a halogen element (group 17) is very likely to gain an electron, so it will have a high ionization energy (because it takes a lot of energy to remove an electron) and a high electron affinity (because a lot of energy is released when an electron is added).


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