Electroegativity

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Kassandra Molina 2B
Posts: 43
Joined: Wed Nov 16, 2016 3:03 am

Electroegativity

Postby Kassandra Molina 2B » Mon Nov 13, 2017 9:52 pm

How can you tell whether one compound is more electronegative than another one without using the electronegativity trend?

Peri Bingham 1G
Posts: 50
Joined: Fri Sep 29, 2017 7:03 am

Re: Electroegativity

Postby Peri Bingham 1G » Mon Nov 13, 2017 10:44 pm

If you happened to know the exact electronegativity values of the two elements that you are comparing, then you would not need to use the trend. However, if you do not know the values, then the trend is very helpful.

Mikaila 3E
Posts: 21
Joined: Fri Sep 29, 2017 7:07 am

Re: Electroegativity

Postby Mikaila 3E » Sat Nov 18, 2017 8:17 am

While this doesn't concern the entire periodic table, remembering that most of the noble gases have no electronegativity because they have a full valence shell of electrons, thus are not likely to add or don't want another electron to accept. Otherwise, knowing the trend is really helpful.

Scott Chin_1E
Posts: 55
Joined: Sat Jul 22, 2017 3:00 am

Re: Electroegativity

Postby Scott Chin_1E » Sat Nov 18, 2017 11:27 am

It would be helpful to know that Halogens and elements like Oxygen and Sulfur tend to have high electronegativity values than that of metals. This is because metals tend to lose electrons to form cations while nonmetals tend to want to gain one, two, or three more electrons to complete their octet because it takes less energy to gain 1, 2 or 3 more electrons rather than losing 5, 6, or 7 electrons.

Lorie Seuylemezian-2K
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Joined: Fri Sep 29, 2017 7:04 am

Re: Electroegativity

Postby Lorie Seuylemezian-2K » Mon Nov 20, 2017 10:21 am

In my opinion knowing the trend is the easiest way to remember the electronegativity of different elements. An easy trick for that is just learning the atomic radius trend and knowing that everything else is the opposite! The only exception there is for the last group of elements because their valence shells are full they don't want more electrons.

juliaschreib1A
Posts: 29
Joined: Fri Sep 29, 2017 7:06 am

Re: Electroegativity

Postby juliaschreib1A » Sun Jun 03, 2018 11:54 pm

You cannot know unless given actual information about the element or using the periodic trend.

905096106
Posts: 30
Joined: Fri Oct 05, 2018 12:17 am

Re: Electroegativity

Postby 905096106 » Fri Oct 26, 2018 8:54 pm

Actual, numeric values for electronegativity are the only way to determine the electronegativity of elements aside from using the periodic trend

Yukta Italia 3I
Posts: 31
Joined: Fri Sep 28, 2018 12:24 am

Re: Electroegativity

Postby Yukta Italia 3I » Thu Nov 01, 2018 1:00 pm

Do you think there will be any circumstances where we have to identify electronegativity trends between elements that are really close together because that seems a little ambiguous?

Ashvi_Luthra_4H
Posts: 33
Joined: Wed Jun 13, 2018 3:00 am

Re: Electroegativity

Postby Ashvi_Luthra_4H » Sun Nov 04, 2018 1:06 pm

You can look at how many valence shells there are. The more shells, the less electronegative.

angelagd3l
Posts: 32
Joined: Fri Sep 28, 2018 12:26 am

Re: Electroegativity

Postby angelagd3l » Sun Nov 04, 2018 1:10 pm

its easier to know the trend, and if you tried to figure it out differently it would probably be less accurate


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