Why are the trend for electronegativity and ionization energy similar?

Jul 20, 2017

Well look at the definitions for each property......

Explanation:

$\text{Electronegativity}$ is conceived to be the ability of atom involved in a chemical bond to polarize electron-density towards itself. There are various scales, of which the $\text{Pauling Scale}$ was the earliest and still very widely used.

Pauling drew upon (i) ionization energies, and (ii) electron affinities, measurable atomic properties to construct his scale, i.e.

$\left(i\right)$ ${\text{Atom(g)"+Deltararr"Atom(g)}}^{+} + {e}^{-}$

$\left(i i\right)$ ${\text{Atom(g)"+e^(-)rarr"Atom(g)}}^{-} + \Delta$

For each property, the magnitude reflects the nuclear charge. Atoms with high ionization energies, i.e. atoms of elements that appear to the right of the Periodic Table as we face it, should also possess high electron affinities, and form negative ions facilely. This is indeed the case for oxygen and fluorine.