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EN Periodic Table<br />
As stated before the electronegativity of an element is a function of its Atomic Structure. Because<br />
the nucleus of a smaller atom is closer to the shared pair of electrons in a bond than that of a<br />
larger atom, the nucleus of the smaller atom attracts the bonding electrons more strongly than<br />
that of the larger atom.<br />
So EN is inversely related to the size of an atom. That is as the size of an atom increases, the EN<br />
decreases. As the size of an atom decreases, the EN increases.<br />
So, in general, since the size of an atom will go up as we proceed down a column (Group) of<br />
elements in the Periodic Table, the EN will go down as we go down a Periodic Table Group (Column).<br />
Also, as we proceed to go up in atomic number across a Row (Period) in the Periodic Table, the size<br />
of atoms generally decreases due to larger numbers of electrons in the outer shell being attracted<br />
to the nucleus. Thus the atomic size will generally decrease and the EN will increase as we go left<br />
to right across a Periodic Table Row (Period).<br />
We have illustrated this for you in the picture below.<br />
One important use of electronegativity is in determining an atom's oxidation number (O.N.) The<br />
oxidation number is sometimes called the valence number of an atom. In Ionic Compounds we<br />
have defined the valence number as the number of electrons that an atom of an element must<br />
give up or accept to achieve an electron-full outer shell.<br />
For covalent compounds, which share electrons, we need a slightly different definition of the<br />
oxidation number. We use the electronegativity and some other atomic structure information to<br />
calculate the oxidation number as follows:<br />
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