Use the periodic table to predict the most stable oxidation state for the following element: F...

Use the periodic table to predict the most stable oxidation state for the following element: F

+1

+2

+3

-1

-2

Expert Solution

From the position of F in the periodic table, it can be observed that it possesses the highest electronegativity in the period. Moreover, being the first halogen, it also has the highest electronegativity in the group, making it the most electronegative atom in the periodic table. This, combined with the electronic configuration of 1s² 2s² 2p⁵ of F, makes it possess very low electron-low gain enthalpy as accepting one more electron helps it attain the noble gas configuration of Ne as 1s² 2s² 2p⁶. However, if it were to accept one more electron, owing to high effective nuclear charge in the nucleus, the dianion will be destabilized by high interelectronic repulsions arising from closely residing extra electrons. Taking a deeper look into the electron-affinity and electronegativity of F, it can be said that it is almost impossible to extract even a single electron from the atom, which also correlates with its high first ionization energy. Therefore, it can be concluded that the most stable oxidation state that F can possess is -1.

queen_honey_blossom answered 2 years ago

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