the minimum energy required to remove an electron is called
ionization energy. Ionization energy is defined as the minimum amount of energy required to completely remove an electron from an isolated gaseous atom or ion. It is often measured in electron volts (eV). Ionization energy is an important concept in chemistry and physics and is applicable to various processes such as the formation of ions, chemical reactions, and the study of atomic and molecular structure.
The ionization energy of an atom depends on several factors, including the atomic number, electron configuration, and the shielding effect of inner electrons. Generally, ionization energy increases as you move across a period in the periodic table from left to right since the number of protons increases, resulting in a stronger attraction between the nucleus and the electrons.
Additionally, ionization energy generally decreases as you move down a group or column in the periodic table. This is because the outermost electrons are further away from the nucleus and are shielded by the inner electrons, reducing the attractive force.
The concept of ionization energy is essential in understanding the behavior of atoms and molecules in chemical reactions and provides insights into the stability and reactivity of different elements.