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Metallic character refers to the properties of metals, such as their ability to lose electrons and form positive ions, their high electrical and thermal conductivity, malleability, and ductility. In the periodic table, metallic character generally increases as we move from top to bottom within a group and decreases as we move from left to right across a period.

First ionization energy is the energy required to remove the outermost (or least tightly bound) electron from a neutral atom in its gaseous phase. It is usually expressed in terms of kilojoules per mole (kJ/mol). In general, first ionization energy increases as we move from left to right across a period and decreases as we move from top to bottom within a group in the periodic table.

Metallic character and first ionization energy are inversely related. As metallic character increases, first ionization energy tends to decrease. This is due to the fact that, as we move down a group, the electrons are further away from the nucleus, making it easier for them to be removed. Similarly, as we move from left to right across a period, the electrons are more tightly bound to the nucleus due to the increasing effective nuclear charge, making it harder to remove them. Consequently, the first ionization energy tends to be higher for elements with lower metallic character and vice versa. In summary, elements with higher metallic character tend to have lower first ionization energies and elements with lower metallic character tend to have higher first ionization energies.