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Atomic Radius

Posted: Sat Oct 27, 2018 1:07 pm
by Jessica Helfond 2F
Could someone explain why removing the second ionization energy of an element is always higher than the first?

Re: Atomic Radius

Posted: Sat Oct 27, 2018 1:09 pm
by chris_tsai_4H
Since one electron has already been removed, the remaining electrons are now experiencing a greater attraction to the nucleus. The subsequent electrons being removed will have a higher ionization energy since they are less easy to remove.

Re: Atomic Radius

Posted: Sat Oct 27, 2018 1:36 pm
by 904936893
When an electron is removed, the atom becomes a cation, or a positively charged ion. This positive charge in the atom makes the electrons more attracted to it, and therefore harder to remove.

Re: Atomic Radius

Posted: Sat Oct 27, 2018 1:48 pm
by rikolivares
There is less electrons to share the nucleus's positive charge once one of the electrons is removed, so the remaining ones have to take on more attraction to the nucleus .

Re: Atomic Radius

Posted: Sun Oct 28, 2018 2:40 pm
by Quinn_Simpson_3D
When an electron is removed, the remaining electrons feel a greater attraction to the nucleus as there is more protons than electrons. This is makes it harder to take other electrons away.

Re: Atomic Radius

Posted: Sun Oct 28, 2018 9:20 pm
by Sang Hyoun Hong 3G
There are fewer electrons that experience a greater force of attraction from the positive nucleus. Thus it is harder to take electrons away!

Re: Atomic Radius

Posted: Sun Oct 28, 2018 9:28 pm
by Ahmed Mahmood 4D
When an electron is removed, the proton:electron ratio heightens. Because of this, the surrounding electrons become more attracted to the protons in the nucleus, requiring more energy to remove said electrons and thus a higher ionization energy.

Re: Atomic Radius

Posted: Sun Oct 28, 2018 10:33 pm
by ThomascnguyenDis1J
Removing an electron gives the atom a greater positive charge, converting it into a cation. This causes the remaining electrons to have a greater attraction to the nucleus.