Question

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905174774
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Question

Postby 905174774 » Thu Nov 14, 2019 7:10 pm

Is ionization or electronegativity the same thing, or what makes them different? I believe they have the same trend on the period table.

Kavya Immadi 3D
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Re: Question

Postby Kavya Immadi 3D » Thu Nov 14, 2019 7:13 pm

Ionization energy is the energy needed to remove electrons from atoms. Electronegativity is how much an atom attracts electrons.

Eunice Nguyen 3K
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Re: Question

Postby Eunice Nguyen 3K » Fri Nov 15, 2019 1:59 am

Electronegativity is an atom's ability to attract and bind with electrons, while ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase.
They have the same trend because if the ionization energy of an atom is high, the atom is more reluctant in giving up an electron. This means that the atom will also be more electronegative, because it would rather attract an electron than give one up.

Megan Jung 3A
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Re: Question

Postby Megan Jung 3A » Fri Nov 15, 2019 9:28 am

Ionization energy is the energy required to remove an electron from an atom's outermost valence shell. Electronegativity refers to the atom's ability to attract electrons.

jisulee3C
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Re: Question

Postby jisulee3C » Fri Nov 15, 2019 12:36 pm

Ionization energy increases across the periodic table as does electronegativity which is a result electrons being more tightly held due to the nuclear pull increasing.

Sjeffrey_1H
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Re: Question

Postby Sjeffrey_1H » Fri Nov 15, 2019 3:03 pm

Also keep in mind that although the trend is the same for both, ionization dips at oxygen (meaning oxygen is an exception to the trend) while electronegativity trend continues through oxygen.

505106414
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Re: Question

Postby 505106414 » Fri Nov 15, 2019 11:59 pm

Can someone explain the exception for oxygen and nitrogen? It was on the midterm and I got it wrong.

Melvin Reputana 1L
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Re: Question

Postby Melvin Reputana 1L » Sat Nov 16, 2019 12:05 am

The first ionization energy of oxygen is lower than the first ionization energy of nitrogen because the repulsive force of electrons in oxygen are stronger than the effective nuclear charge of oxygen. As a result, the first ionization of oxygen is lower as it it is easier to remove the electrons on oxygen compared to nitrogen whose effective nuclear charge is stronger.

Amanda Lin 1C
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Re: Question

Postby Amanda Lin 1C » Sat Nov 16, 2019 12:07 am

505106414 wrote:Can someone explain the exception for oxygen and nitrogen? It was on the midterm and I got it wrong.

Nitrogen has 3 e- in its p orbital. Oxygen has 4 e- in its p orbital, which results in an electron pair. The electron-electron repulsion from this pair causes a lower ionization energy.

Jasmine 3L
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Re: Question

Postby Jasmine 3L » Sun Nov 17, 2019 2:06 pm

505106414 wrote:Can someone explain the exception for oxygen and nitrogen? It was on the midterm and I got it wrong.

I got this question wrong too :(

Deana Moghaddas 3E
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Re: Question

Postby Deana Moghaddas 3E » Sun Nov 17, 2019 2:12 pm

think of ionization energy as the energy needed to make an ion (to remove an electron)
think of electronegativity as an atom's attraction to gain electrons

Siya Shah 1J
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Re: Question

Postby Siya Shah 1J » Sun Nov 17, 2019 2:46 pm

505106414 wrote:Can someone explain the exception for oxygen and nitrogen? It was on the midterm and I got it wrong.

According to the trend, oxygen should have a higher ionization energy than nitrogen. However, nitrogen has its p-subshell half-filled and is relatively stable and low energy. Oxygen has one more electron, paired up with the opposite spin, in its p-subshell than nitrogen, which causes electron repulsion, making oxygen less stable than nitrogen. Therefore, oxygen has a lower ionization energy than nitrogen -- it's easier to remove an electron from oxygen than it is to do the same from nitrogen.

CalvinTNguyen3D
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Joined: Thu Jul 25, 2019 12:16 am

Re: Question

Postby CalvinTNguyen3D » Sun Nov 17, 2019 5:57 pm

They're somewhat related, but they're not the same!
Ionization energy is the amount of energy required to remove an electron from the atom, while electronegativity is how much an atom attracts electrons towards it!

605208780
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Re: Question

Postby 605208780 » Tue Dec 03, 2019 12:50 pm

Electronegativity is how much an atom attracts electrons. Ionization energy is needed to remove electrons from atoms.

Kishan Shah 1G
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Joined: Thu Jul 11, 2019 12:15 am

Re: Question

Postby Kishan Shah 1G » Tue Dec 03, 2019 12:52 pm

They have the same trend but they mean different things. Electronegativity refers to the amount of pull that an atom can have on an outside electron because it wants the electron. Ionization energy means the amount of energy it takes to remove one electron from an atom.

Jessica Tran_3K
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Re: Question

Postby Jessica Tran_3K » Tue Dec 03, 2019 1:18 pm

Ionization energy is the amount of energy required to remove an electron from an atom, while electronegativity is the amount of energy required to add an electron!

BritneyP- lC
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Re: Question

Postby BritneyP- lC » Tue Dec 03, 2019 1:47 pm

Ionization energy is the energy it takes to remove and electron, while electronegativity is the attraction of the electron to the atom.

RichBollini3C
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Joined: Wed Sep 18, 2019 12:18 am

Re: Question

Postby RichBollini3C » Sat Dec 07, 2019 5:33 pm

Kavya Immadi 3D wrote:Ionization energy is the energy needed to remove electrons from atoms. Electronegativity is how much an atom attracts electrons.

very helpful


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