Periodic Table Trend

[205154661_Dis2J]

What is the trend for electronegativity and ionization energy?

[FDeCastro_1B]

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

[jessicaosuna_1F]

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

[Michelle Nguyen 3F]

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]

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 3B]

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]

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

[Nina Tartibi 1F]

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]

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]

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 2L]

Increase across a period and decrease down a group :)

[Allan Nguyen 2G]

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

[Vanessa Perez]

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]

Increase across a period, decrease down a group

[Rose_Malki_3G]

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

[Kiara Phillips 3L]

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

[Sophia Wendin 3L]

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]

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 2G]

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 2I]

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]

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]

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

[Ava Nickman]

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

[Anastasia Yulo 1C]

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 2a]

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

[Ariel Guan 1H]

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

[Massimo_Capozza_1G]

Hi if found this image very helpful to study periodic trends

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

[John_Tran_3J]

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]

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]

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_2E]

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]

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.

[Edwin Liang 1I]

Electronegativity increases from the lower left side of the table to the top right and the ionization energy increases as you go from the bottom left to top right.

[Jaclyn Schwartz 1I]

For ionization energy trend, it increases left to right because more energy is needed to remove the electrons from their valence shells. Like in group 1 and 2, they have low ionization energy because they give their electrons, often becoming cation. And in group 7, they have high ionization energy because they only need one more electron to form an octet.

Electronegativity is the attraction of another electron. It follows the same trend of ionization energy(increases left to right) for similar reasons. An atom wants to complete its octet so groups 1 and 2 have low ionization energies because they don't want more electrons, they are more willing to give them away to complete their octet. While group 7 has a higher ionization because it wants to complete its octet.

I hope this helps!

[DPatel_2L]

Both increase across a period and decrease down a group.

[Brianna Chen 3F]

Electronegativity and ionization energy both have trends that increase as you move towards the right corner of the periodic table (towards Fluorine).

[Caelin Brenninkmeijer 1G]

Ionization energy decreases down a group and increases across a period. Because electronegativity is calculated using ionization energy, electronegativity follows the same periodic trend.

[Brandon Carris]

Ionization energy increases as you go the right because the attraction of the electrons to the nucleus increases because the nucleus is more massive.

[Samantha Quevedo 2L]

Electronegativity and ionization energy both increase from left to right and decrease as you move top to bottom on the periodic table.

[Mahima Manoj 1F]

Like the other respondents said ionization energy decrease down a group and increases across a period.

[michaelcrisera]

Electronegativity and ionization energy both have the same periodic trend. They increase going across (left to right) a period and decrease going down a group.