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Ionic Character

Posted: Wed Nov 28, 2018 4:06 pm
by Tessa Lawler 1A
In the textbook, there's a question that says "In which of the following compounds do the bonds have greater ionic character? a)P4O10 b)PCl3". The answer is A. I know that ionic character is determined by the difference in the atoms' electronegativity, but since P seems an equal distance from Cl and O on the periodic table, how do you determine which is more electronegative than P?

Re: Ionic Character

Posted: Wed Nov 28, 2018 4:20 pm
by MichelleRamirez_2F
Electronegativity decreases down a group since Cl is lower than O, I want to.say that O is more electronegative than Cl.

Re: Ionic Character

Posted: Tue Dec 04, 2018 6:15 pm
by Sophia Ding 1B
Yeah there is no "definite" trend to electronegativity like there is for trends of atomic radius (and others we learned), but in my head I like to remember that F is the most electronegative element, and then next one would be O. So I guess going down a group results in a lower electronegativity generally, thus Cl has less electronegativity than O thus having less ionic character as PCl3.

Re: Ionic Character

Posted: Fri Dec 07, 2018 8:23 pm
by Mark 1D
I believe oxygen is more electronegative as it is higher than chlorine on the periodic table

Re: Ionic Character

Posted: Fri Dec 07, 2018 9:54 pm
by 305117729
Generally, the greater the difference between two atoms forming the ion, the greater ionic character this ion will show

Re: Ionic Character

Posted: Fri Dec 07, 2018 11:09 pm
by Joaquin Andrade
Oxygen is actually more electronegative since Cl is a period down and thus is affected by shielding. This can be verified in the actual electronegativity values for O and Cl.