Electronegativity

(Polar molecules, Non-polar molecules, etc.)

Rosa Munoz 2E
Posts: 105
Joined: Wed Sep 18, 2019 12:21 am

Electronegativity

Should we memorize some of the common values of electronegativity?

Anish Patel 4B
Posts: 59
Joined: Thu Jul 11, 2019 12:17 am

Re: Electronegativity

You don't need to know the exact values but the general trends (F being the most) and the fact that noble gases have none.

Megan Cao 1I
Posts: 103
Joined: Sat Sep 07, 2019 12:18 am

Re: Electronegativity

I don't think we need to know the exact numerical electronegative values of the elements. however, I think we should know that Fluorine is the most electronegative and that on the periodic table electronegativity increases as you move from left to right and from the bottom up.

Lauren Stack 1C
Posts: 100
Joined: Sat Aug 17, 2019 12:18 am

Re: Electronegativity

I do not believe we need to know exact values for electronegativity. I think that knowing the general periodic trends associated with it are sufficient in that noble gases are not electronegative and electronegativity increases up a column and across a row. Comparing relative electronegativity can be helpful when drawing Lewis structures and comparing atoms in general.

Julie Park 1G
Posts: 100
Joined: Thu Jul 25, 2019 12:15 am

Re: Electronegativity

When it comes to trends across the periodic table, it would be a good idea to know the general reasoning as to why those trends occur. Since
electronegativity measures an atom's tendency to attract and form bonds with electrons, electronegativity increases up and to the right on a periodic table (where F is the most electronegative)...

Left to right: If the valence shell of an atom is less than half full, it requires less energy to lose an electron than to gain one. This means that it's easier to pull in an e- than to donate one as you move to the right side of the table (since the number of ve- increases as you move to the right).

Top to bottom: Atomic number increases down a group, meaning that there is more distance between the valence electrons and nucleus, and thus a greater atomic radius