Implications of ionization energy

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Chloe Thorpe 1J
Posts: 77
Joined: Fri Sep 28, 2018 12:16 am

Implications of ionization energy

Postby Chloe Thorpe 1J » Thu Nov 01, 2018 12:21 pm

Can someone explain why we place the atom with the lowest ionization energy in the middle of a Lewis structure?

Kevin ODonnell 2B
Posts: 62
Joined: Fri Sep 28, 2018 12:24 am

Re: Implications of ionization energy

Postby Kevin ODonnell 2B » Thu Nov 01, 2018 12:52 pm

This is typically because the elements with lower ionization energies have more open spaces (have more opportunity) for bonding. For example, Carbon can form 4 bonds and has a lower ionization energy than Fluorine who can only form 1 bond (we get these numbers by looking at how many valence electrons each element has). It would make sense then that we would put Carbon in the middle, since we can branch out from there more effectively.

Manas_Varma_4B
Posts: 30
Joined: Fri Sep 28, 2018 12:29 am

Re: Implications of ionization energy

Postby Manas_Varma_4B » Thu Nov 01, 2018 12:58 pm

The atoms with a lower ionization energy have a greater ability to bond with other atoms since they have more "open spots" to form an octet. Because of this, the atom with more spots to bond goes in the middle and the ones with less go on the outside (for example Hydrogen).


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