On the left side of the periodic table we have atoms with what are termed a positive charge. On the right side of the periodic table we see negative charges. All, in reality, are balanced. Each proton has an associated electron to balance it.
Positive atoms on the left side of the periodic table have an extra electron above the previous filled complement of electrons. This electron peels off easily leading to negatively charged ion. These two configurations can be seen as sharp. When the electrons balance the protons the negative charge can be seen as sharp. Where the electron resided the charge is sharp and very negative. When the electron peels off the result will be a dull positive charge. The imbalance caused by more protons than electrons will be felt through the Maxwell-Gauss electric equation.
Negative atoms on the right side of the periodic table have too few electrons to make up a full complement of electrons for a shell. The extra positive charge that presents itself around the atom will tend to draw electrons from farther away. This positive charge can be seen as sharp. When the atom is successful in drawing in another electron the valence shell will be complete. This atom now has a dull negative charge which is spread around the outside of the electron and not quite balanced by the protons' charge in the nucleus of the atom.
Sharp charge vs dull charge can be important in understanding why chemical reactions happen.
No comments:
Post a Comment