A metal element is more likely to form an ion by losing electrons. This is because metals tend to have fewer electrons in their outermost energy level, known as the valence shell. By losing these valence electrons, the metal can achieve a stable octet configuration, which is energetically favorable. Additionally, metals have low ionization energies, which means that it takes relatively little energy to remove an electron from a metal atom. As a result, metals tend to be good reducers and are more likely to form cations than anions.
A metal element is more likely to form an ion by losing electrons rather than gaining them. This is because metals typically have few valence electrons, which are the electrons involved in chemical bonding. By losing these electrons, metals can achieve a stable electron configuration similar to that of a noble gas, which makes them more stable. This process is referred to as "oxidation" and results in the formation of positively charged ions, known as cations.
