Ionization Energy

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Ionization Energy

Postby Vuong_2F » Sun Oct 20, 2019 10:49 pm

Why is the second (and third and fourth, etc) ionization energy usually so much larger than the first one?

Alfred Barrion 2H
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Re: Ionization Energy

Postby Alfred Barrion 2H » Sun Oct 20, 2019 10:53 pm

As you remove more electrons from an atom, the attraction between electrons and the nucleus increase because repulsion decreases. So as you go through successive ionization energies, more energy is required to remove electrons due to the lack of repulsion.

Aadil Rehan 1D
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Re: Ionization Energy

Postby Aadil Rehan 1D » Sun Oct 20, 2019 11:09 pm

Yeah, think of it as the shielding of the electron cloud decreasing, and thus the positive nucleus is able to exert a stronger force.

Kelsey Ash 1D
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Re: Ionization Energy

Postby Kelsey Ash 1D » Mon Oct 21, 2019 12:09 pm

Electrons repel each other so the more electrons you have the greater the repulsion you have from the nuclear. By that logic, if you start to remove electrons the attractive forces between the surrounding electrons and the nucleus increases because there are less forces which repel the electrons. Therefore, as you increase in ionization energies, there is more energy required to remove electrons since there are less repulsive forces working to expel the electron.

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Re: Ionization Energy

Postby selatran1h » Mon Oct 21, 2019 9:13 pm

Once one electron is removed, the effective nuclear charge increases, making the remaining valence electrons pulled closer to the nucleus. This makes it more difficult for the second or third electron to be removed.

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Re: Ionization Energy

Postby PriscillaLi_3G » Wed Oct 23, 2019 11:19 am

As you take away an electron, you have the same positive energy power holding onto less electrons, so each electron gets a stronger pull, which makes it harder to take away a second, third, etc. electron

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Re: Ionization Energy

Postby RoshniVarmaDis1K » Wed Oct 23, 2019 3:24 pm

When you remove electrons, there is less electron-electron repulsion remaining in the cation. This means every remaining electron is held tighter and is harder to remove.

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Re: Ionization Energy

Postby aphung1E » Wed Oct 23, 2019 3:37 pm

Does the ionization energy increase/decrease down a group in the periodic table?

Hannah Romano 4D
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Re: Ionization Energy

Postby Hannah Romano 4D » Wed Oct 23, 2019 4:09 pm

As you get to removing electrons of the inner shells, they are experiencing a greater positive attraction to the nucleus at a closer distance and are therefore more difficult to remove.

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