Ionization Energy

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Jarrett Peyrefitte 2K
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Joined: Sat Aug 24, 2019 12:16 am

Ionization Energy

Postby Jarrett Peyrefitte 2K » Sun Nov 10, 2019 6:42 pm

What is the ionization energy periodic trend? And what is the conceptual reasoning behind it?

BritneyP- 2c
Posts: 101
Joined: Sat Sep 14, 2019 12:15 am

Re: Ionization Energy

Postby BritneyP- 2c » Sun Nov 10, 2019 6:49 pm

ionization energy increases as it goes up and to the right. Up because the radius is much smaller so that the energy of removing an electron is higher and to the right because there are more protons to attract the electrons so the energy to remove an electron is much higher.

Rosa Munoz 2E
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Joined: Wed Sep 18, 2019 12:21 am

Re: Ionization Energy

Postby Rosa Munoz 2E » Sun Nov 10, 2019 6:55 pm

The elements closer to the noble gases have higher ionization energy.

RasikaObla_4I
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Joined: Thu Jul 25, 2019 12:15 am

Re: Ionization Energy

Postby RasikaObla_4I » Sun Nov 10, 2019 7:05 pm

Ionization decreases down a group and increases across a period. The ionization energy decreases down a group because as the number of shells increases, the electrons are shielded from the nucleus, so it takes less energy to remove the last electron. The ionization energy increases across a period because the atomic radius decreases, so the nuclear charge increases and the electrons are pulled closer together to the nucleus so the energy to remove an electron is higher.

Camille 4I
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Joined: Sat Aug 24, 2019 12:18 am

Re: Ionization Energy

Postby Camille 4I » Sun Dec 01, 2019 2:04 pm

What is the reasoning behind Na having a smaller first ionization energy than Mg?

005162902
Posts: 102
Joined: Wed Sep 18, 2019 12:15 am

Re: Ionization Energy

Postby 005162902 » Sun Dec 01, 2019 3:43 pm

Ionization energy increases as you go up the periodic table and to the right of the table. As you travel up the periodic table, the atomic radius of a molecule gets smaller. This places electrons much closer to the nucleus than in a larger molecule making the electrons harder to remove from the smaller molecule. This means they require a higher ionization energy to remove the electrons.


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