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Answer:
Ionization Energy is defined as the energy required to remove the most loosely bonded atom from an atom in its gas phase. Ionization energy in metals decreases from top to bottom and from right to left and on the periodic table.
Metals have lower ionization energies that help metal atoms to lose electrons to nonmetal atoms easily. The metallic character of a metal increases as ionization energy decreases, it means reactivity of metals increases with decreases in ionization energy.
Hence, the reactivity of metals increases with low ionization energies..
The metals tend to have high reactivity due to low ionization energy.
The ionization energy can be defined as the energy required to remove the atom from metal in its gaseous state. The metals on the left side of the periodic table have loosely bonded electrons, requiring less ionization energy for the removal of an electron. Thus on moving from left to right in a periodic table, the ionization energy increases.
On moving from top to bottom in a periodic table, due to steric hindrance, the electrons are loosely bonded and require less energy for the removal of electrons. Thus on moving down the group, the ionization energy decreases.
The low ionization energy shows that there is easy removal of electrons tends to increase its reactivity.
Thus, low ionization energy results in the high reactivity of metals.
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