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Postby eduardomorales5 » Sat Nov 16, 2019 6:49 pm

What exactly causes an atom to have more electronegativity than other atoms?

Anish Patel 4B
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Re: Electronegativity

Postby Anish Patel 4B » Sat Nov 16, 2019 6:55 pm

Elements that have a high need to complete their valence shell through adding electrons have higher electronegativity values (since that is its ability to attract an electron to itself). Fluorine has the highest since it needs one more electron to complete its valence shell and experiences less electron shielding from the protons in the nucleus as its the smallest element in its group.

Rohit Ghosh 4F
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Re: Electronegativity

Postby Rohit Ghosh 4F » Thu Dec 05, 2019 3:48 pm

Electronegativity is the value of how badly an atom attracts electrons. As such, any atom which wants more electrons to fill its valence shell will be more electronegative. You can use periodic trends to determine electronegativity.

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Re: Electronegativity

Postby jessicasilverstein1F » Sat Oct 31, 2020 11:34 am

Electronegativity is the elements ability to attract electrons. Different electrons have different electronegativity values and FONClBrISCH is a good way to remember which ones are the most electronegative.

Chudi Onyedika 3A
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Re: Electronegativity

Postby Chudi Onyedika 3A » Sat Oct 31, 2020 1:43 pm

The closer an atom is to having a complete valence shell (a shell containing either 2 or 8 electrons), the more it will want electrons. This is electronegativity.

Sophia Kalanski 1A
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Re: Electronegativity

Postby Sophia Kalanski 1A » Sat Oct 31, 2020 3:29 pm

typically electronegative atoms make covalent bonds and are non metal. It is more electronegative when it wants more electrons. For example, in H2O, Oxygen is very electronegative and that is why it bonds with 2 hydrogen atoms.

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Re: Electronegativity

Postby reyvalui_3g » Sun Nov 01, 2020 6:15 pm

It is also important to note that in a period on the periodic table, elements with more protons will have a stronger electronegativity since there is a stronger effective nuclear charge.

David Liu 1E
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Re: Electronegativity

Postby David Liu 1E » Sun Nov 01, 2020 9:15 pm

electronegativity is how much an electron is drawn to an atom, and we can see the trends on a periodic table (as we probably won't have to know specific electronegativity numbers for this class)

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Re: Electronegativity

Postby 305572629 » Sun Nov 01, 2020 9:18 pm

As valence electrons in a shell get higher and closer to 8, they want that last electron very strongly, making the electronegativity of that element strong. For example, Chlorine has a very high electronegativity because it has 7 valence electrons.

Ethan Goode 2H
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Re: Electronegativity

Postby Ethan Goode 2H » Sun Nov 01, 2020 9:23 pm

Electronegativity is rating how strong the protons are pulling in the negative electrons. As there are more electrons in a valence shell of an element, it gets more electronegative, as there is more pull. Furthermore, with the same number of valence electrons, ones with more shells have less electronegativity since those valence electrons are farther from the nucleus and protons.

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Re: Electronegativity

Postby Gustavo_Chavez_1K » Sun Nov 01, 2020 11:12 pm

The closer an element is to completing their valence shell then the more electronegative they are. This is because they have a stronger tendency of attracting a bonding pair of electrons since they essentially really want to complete their shell.

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