Periodic Table Trend

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205154661_Dis2J
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Periodic Table Trend

Postby 205154661_Dis2J » Fri Dec 06, 2019 12:16 pm

What is the trend for electronegativity and ionization energy?

FDeCastro_1B
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Re: Periodic Table Trend

Postby FDeCastro_1B » Fri Dec 06, 2019 12:25 pm

Ionization energy and electronegativity both decrease down a group and increase across a period.

jessicaosuna_3E
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Re: Periodic Table Trend

Postby jessicaosuna_3E » Fri Oct 09, 2020 7:40 pm

Electronegativity increases as you go diagonally up and to the right on the periodic table!

Michelle Nguyen 2C
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Re: Periodic Table Trend

Postby Michelle Nguyen 2C » Fri Oct 09, 2020 8:58 pm

Electronegativity increases going right on the periodic table because the number of protons in the nucleus increases, the electronegativity or attraction will increase. The nucleus brings in the electrons closer together because of the increase in attraction. Electronegativity will then decrease going down the periodic table because of the increased distance between the valence electrons and the nucleus, and the nucleus will not be able to pull those electrons closer.

Amanda Bueno-Kling 2L
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Re: Periodic Table Trend

Postby Amanda Bueno-Kling 2L » Sat Oct 10, 2020 8:05 pm

When we learned about periodic table trends in high school chemistry, my teacher had us draw arrows to represent the trends in our notes. If you're a visual learner, it can be very helpful!
Here's an example of this. I find it useful to refer to.
https://www.google.com/url?sa=i&url=htt ... AdAAAAABAb

Morgan Gee 1F
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Re: Periodic Table Trend

Postby Morgan Gee 1F » Thu Oct 15, 2020 5:01 pm

As you go in the top right direction, the electronegativity and electron affinity of the elements increase up until the noble gases. This means that fluorine has the greatest electronegativity out of all elements! As a result, oxygen and chlorine have slightly less electronegativity than fluorine. The reason for why elements in the top right have greater electronegativity is because they have a greater positive charge in the nucleus compared to other elements in the left of their row. Additionally, smaller elements in a group have valence electrons in lower principal levels, contributing to a greater electronegativity.

Muskaan Abdul-Sattar
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Re: Periodic Table Trend

Postby Muskaan Abdul-Sattar » Mon Oct 26, 2020 11:03 pm

They will both increase across a period and also decrease down a group!

Nina Tartibi 1F
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Re: Periodic Table Trend

Postby Nina Tartibi 1F » Sun Nov 01, 2020 11:31 pm

The trends for ionization energy and electronegativity are the same: they increase in electronegativity/ionization energy as you go across a row and up a column. Flourine is the most electronegative element.

Samudrala_Vaishnavi 3A
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Re: Periodic Table Trend

Postby Samudrala_Vaishnavi 3A » Mon Nov 02, 2020 7:48 am

So the trend for ionization energy basically corresponds to the atomic radius of the element. The bigger the atomic radius, the lower the ionization energy. The atomic radii decrease along a period and increase down a group. SO we can say the ionization energy increases down a period and decreases down a group. In terms of electronegativity or electron affinity, I may be wrong but I think that it has to do with the properties of the elements and where they are placed specifically. Noble gases don't want electrons, so they require energy to add electrons and have a lower electronegativity while elements before them have a high electronegativity since they want electrons to turn into noble gases, and release energy.

Annette Fishman 2A
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Re: Periodic Table Trend

Postby Annette Fishman 2A » Mon Nov 02, 2020 8:36 am

The trends for ionization energy and electronegativity are the same. They increase in electronegativity/ionization energy as you go across a row and up a column. Fluorine is the most electronegative element. This is because for ionization energy, or the energy to remove an electron, the elements with smaller atomic radiuses are held together tighter by a greater nuclear charge. Thus that energy to remove must be higher than an element with one electron in the valence shell - which is dying to get rid of that electron.

Inderpal Singh 3B
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Re: Periodic Table Trend

Postby Inderpal Singh 3B » Tue Nov 03, 2020 5:44 pm

Increase across a period and decrease down a group :)

Allan Nguyen 2E
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Re: Periodic Table Trend

Postby Allan Nguyen 2E » Tue Nov 03, 2020 6:46 pm

They both increase across a period and decrease down a group.

Vanessa Perez
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Re: Periodic Table Trend

Postby Vanessa Perez » Tue Nov 03, 2020 10:43 pm

Michelle Nguyen 2C wrote:Electronegativity increases going right on the periodic table because the number of protons in the nucleus increases, the electronegativity or attraction will increase. The nucleus brings in the electrons closer together because of the increase in attraction. Electronegativity will then decrease going down the periodic table because of the increased distance between the valence electrons and the nucleus, and the nucleus will not be able to pull those electrons closer.

thank you! this was very helpful!

claire ikemiya_2I
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Re: Periodic Table Trend

Postby claire ikemiya_2I » Thu Nov 05, 2020 3:33 am

Increase across a period, decrease down a group

Rose_Malki_3L
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Re: Periodic Table Trend

Postby Rose_Malki_3L » Thu Nov 05, 2020 10:26 am

Increases as you go across the table and decreases as you go down

Kiara Phillips 1L
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Re: Periodic Table Trend

Postby Kiara Phillips 1L » Thu Nov 05, 2020 12:51 pm

Increases across a period and increases as you move up/decreases down a group.

Sophia Wendin 2B
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Re: Periodic Table Trend

Postby Sophia Wendin 2B » Thu Nov 05, 2020 1:52 pm

Michelle Nguyen 2C wrote:Electronegativity increases going right on the periodic table because the number of protons in the nucleus increases, the electronegativity or attraction will increase. The nucleus brings in the electrons closer together because of the increase in attraction. Electronegativity will then decrease going down the periodic table because of the increased distance between the valence electrons and the nucleus, and the nucleus will not be able to pull those electrons closer.

Thank you! This explanation helped me a lot.

Katherine_Douglas_1F
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Re: Periodic Table Trend

Postby Katherine_Douglas_1F » Thu Nov 05, 2020 4:27 pm

The way I think of it is that atomic radius and electronegativity have an inverse relationship. As the atomic radius increases, the electrons stray further away from the nucleus, meaning the protons have less of a pull on them and they are easier to remove. In the same sense, the elements with small atomic radii hold their electrons closely to the nucleus, allowing the protons to have more of a hold and making it more difficult to remove. The radius decreases and the electronegativity increases going diagonally up and to the right. If you remember one, you should be able to figure out the behavior of the other.

Eric Cruz 3L
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Re: Periodic Table Trend

Postby Eric Cruz 3L » Sat Nov 14, 2020 1:15 am

The trend for electronegativity and ionization energy are virtually identical and this makes sense because what they relate with is similar: the behavior of electrons. Ionization energy focuses on how much energy it takes to give up an electron. Electronegativity also relates to electrons, since it focuses on the ability of an atom to attract electrons. If an atom readily attracts electrons, then it must be able to hold on to its electrons. Therefore, atoms that have a high ionization energy (an atom that requires a lot of energy to lose an electron since their electrons are tightly held) also have a high electronegativity. Conversely, those with a low ionization energy have low electronegativity.

Selena Quispe 2G
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Re: Periodic Table Trend

Postby Selena Quispe 2G » Sat Nov 14, 2020 1:35 am

The trend for electronegativity and ionization energy generally decreases down a group and increases across the periodic table from left to right. Ionization energy is the minimum energy needed to remove an electron and as you go down a group the shells increase so the electrons are further from the nucleus causing them to be easily removed (lower ionization energy). Also, as you move across a period the nuclear charge increases so the electrons have a tighter pull to the nucleus causing you to need more energy to remove the electron. Electronegativity is the ability of an atom to attract electrons to itself and as you go down a group as said before the electrons are further from the nucleus causing the attraction to decrease (making the atom have less of an attraction for electrons). As you move across a period the nuclear charge increases causing it to have higher attraction for electrons (be more electronegative). Fluorine is your most electronegative element and Cesium is your least electronegative element.

Hannah Rim 2D
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Re: Periodic Table Trend

Postby Hannah Rim 2D » Sat Nov 14, 2020 12:33 pm

Both electronegativity and ionization energy increase as you go left to right and bottom to up. This is why Fluorine (F) is the most electronegative element

Jasraj Parmar 3H
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Re: Periodic Table Trend

Postby Jasraj Parmar 3H » Sat Nov 14, 2020 12:59 pm

They both follow the same trend which is that if you go diagonally across the periodic table then both will increase.

Ava Nickman
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Re: Periodic Table Trend

Postby Ava Nickman » Sat Nov 14, 2020 1:49 pm

Ionization energy and electronegativity both decrease down a group and increase across a period. As you move to the right the electrostatic attraction increase because the elements have more protons. As you move downwards the electrostatic attraction decreases as the the electrons move farther and farther from the nucleus with the addition of orbitals

305392242
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Re: Periodic Table Trend

Postby 305392242 » Thu Nov 26, 2020 1:38 pm

Ionization energy and electronegativity decrease down a group.
Ionization energy and electronegativity also increase across a period.

What helps me remember this is to remember that fluorine is the smallest and most electronegative atom, if you look at the periodic table you will see that it is at the very top right corner of the periodic table, so as atoms are closer to this element..then they are more electronegative!

Maya Johnson 1c
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Re: Periodic Table Trend

Postby Maya Johnson 1c » Thu Nov 26, 2020 2:56 pm

Ionization energy and electronegativity both follow the same trend- they increase across a period and decrease down a group.

Ariel Guan 1G
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Re: Periodic Table Trend

Postby Ariel Guan 1G » Thu Nov 26, 2020 3:20 pm

Both follow the same trend of increasing across a period and decreasing down a group

Massimo_Capozza_1H
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Re: Periodic Table Trend

Postby Massimo_Capozza_1H » Thu Nov 26, 2020 5:16 pm

Hi if found this image very helpful to study periodic trends

https://www.thoughtco.com/chart-of-periodic-table-trends-608792

John_Tran_1L
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Re: Periodic Table Trend

Postby John_Tran_1L » Thu Nov 26, 2020 8:14 pm

It increases from left to right and from down to up. In other words, electro negativity increases as you approached to the top right corner of the periodic table.

AHUNT_1A
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Re: Periodic Table Trend

Postby AHUNT_1A » Fri Nov 27, 2020 9:31 am

As there is an increases in electronegativity you would move up diagonally and to the right on the periodic table.

Hope this helps!

AHUNT_1A
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Re: Periodic Table Trend

Postby AHUNT_1A » Fri Nov 27, 2020 9:32 am

John_Tran_1L wrote:It increases from left to right and from down to up. In other words, electro negativity increases as you approached to the top right corner of the periodic table.

simple but helpful explanation. Thank you.

BKoh_3H
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Re: Periodic Table Trend

Postby BKoh_3H » Fri Nov 27, 2020 11:17 am

Since Fluorine has the highest electronegativity, I try to remember the trend as the closer you get to Fluorine (top & right) the more electronegative.

Heidi Buri 2I
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Re: Periodic Table Trend

Postby Heidi Buri 2I » Mon Nov 30, 2020 1:14 pm

Hi! On the periodic table, electronegativity increases from left to right and decreases from top to bottom. For ionization energy, it generally decreases from top to bottom and increases from left to right.


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