Electron Affinity vs. Ionization Energy

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905085650
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Joined: Fri Sep 28, 2018 12:19 am

Electron Affinity vs. Ionization Energy

Postby 905085650 » Sun Nov 04, 2018 2:18 pm

Can someone explain to me the difference between electron affinity and ionization energy? Also, could you explain the trends of both of them on the periodic table? Thank you!!

Timothy_Yueh_4L
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Joined: Fri Sep 28, 2018 12:28 am

Re: Electron Affinity vs. Ionization Energy

Postby Timothy_Yueh_4L » Sun Nov 04, 2018 2:52 pm

Ionization energy is the energy required to eject an electron from an element, which increases across a period because the distance and force between proton and electron become greater. Electron affinity is the energy given off when a neutral atom in the gas phase gains an extra electron to form a negatively charged ion, therefore as you move across a period, atoms with more protons with smaller radius wants to attract electrons.

Jacqueline Duong 1H
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Joined: Fri Sep 28, 2018 12:28 am

Re: Electron Affinity vs. Ionization Energy

Postby Jacqueline Duong 1H » Sun Nov 04, 2018 4:00 pm

Ionization energy increases across a period and decreases down a group, while electron affinity is also the same where it increase across a period and decreases down a group.

Mhun-Jeong Isaac Lee 1B
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Joined: Fri Sep 28, 2018 12:17 am

Re: Electron Affinity vs. Ionization Energy

Postby Mhun-Jeong Isaac Lee 1B » Sun Nov 04, 2018 5:28 pm

Just a reminder too that there are some exceptions in these trends like C, N, O, F. Make sure to look out for those.

Saachi_Kotia_4E
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Joined: Fri Sep 28, 2018 12:23 am

Re: Electron Affinity vs. Ionization Energy

Postby Saachi_Kotia_4E » Mon Nov 05, 2018 10:16 pm

electron affinity is the energy it takes for an atom to gain an electron. ionization energy is the energy needed for an atom to lose an electron. the trend for both is the same, it increases across a group and decreases down a period.

Sophie Roberts 1E
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Joined: Fri Sep 28, 2018 12:17 am

Re: Electron Affinity vs. Ionization Energy

Postby Sophie Roberts 1E » Fri Nov 09, 2018 7:37 am

Electron affinity is the energy given off when electrons are added to the atom. So basically, the electron affinity of an atom can determine if the atom wants electrons or not. On the other hand, ionization energy is the energy needed to remove an electron from an atom. They both increase across the periodic table and decrease down a group.

Ashita Tanwar 3H
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Re: Electron Affinity vs. Ionization Energy

Postby Ashita Tanwar 3H » Sat Nov 10, 2018 10:12 pm

For the most part, electron affinity and ionization energy show the same trend across the periodic table. Fluorine has one of the greatest electron affinities and ionization energies, and these values decrease as you get closer to group 1/period 7. That being said, it's important to remember that electron affinity isn't as periodic as ionization energy - there are many, many exceptions for electron affinity. Some examples are group 2 having a lower electron affinity than group 3, and Manganese having a surprisingly low electron affinity as well.

Niveda_B_3I
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Joined: Fri Sep 28, 2018 12:24 am

Re: Electron Affinity vs. Ionization Energy

Postby Niveda_B_3I » Sun Nov 11, 2018 7:00 pm

Electron affinity is the amount of energy released when an atom is given an electron, and ionization energy is the energy not takes to remove an electron.

Lisa Werner 2F
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Joined: Fri Sep 28, 2018 12:17 am

Re: Electron Affinity vs. Ionization Energy

Postby Lisa Werner 2F » Sun Nov 11, 2018 7:08 pm

Also note that C,N,O and F all have exceptions to the trends!
in order from least to greatest in electronic affinity: N,C,O,F
in order from least to greatest in ionization energy: C,O,N,F


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