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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?
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.
Because Cl is affected by shielding, O is actually higher in electronegativity. Also, oxygen is considered one of the most electronegative alongside, Nitrogen and Fluorine which is why H Bonding only happens between those three elements.
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