What is the relationship between first ionization energies and metallic and non-metallic properties ?
Hello, By definition, The energy needed to remove one or more electrons from a neutral atom to form a positively charged ion is a physical property that influences the chemical behavior of the atom. By definition, the first ionization energy of an element is the energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase. ______________________________________… In a metallic atom, the ionization energy to remove a loosely bound electron is minmum compared to miserly non-metallic atom. Why? Because the electronegativity, the tendency for electron attraction, is high in the non-metals side, it will take huge amount of ionization energy to remove just one electron from a non-metal atom. ______________________________________… Metals, on the other hand, have low eletronegativity due to their properties of losing electrons rather than gaining electrons to achieve the stable octet stage of maximum of 8 valence electrons like the noble gas electron
