* Transition metals tend to lose electrons to form positively charged ions (cations). This is due to their relatively low ionization energies and the presence of d-electrons that can be easily removed.
* Chlorine is a highly electronegative element, meaning it strongly attracts electrons. It gains one electron to form a negatively charged ion (anion), Cl⁻.
The strong electrostatic attraction between the positively charged metal cation and the negatively charged chloride anion results in the formation of an ionic bond.
Example:
The reaction of iron (Fe) with chlorine (Cl₂) forms iron(III) chloride (FeCl₃):
2Fe(s) + 3Cl₂(g) → 2FeCl₃(s)
In FeCl₃, iron exists as Fe³⁺ ions and chlorine exists as Cl⁻ ions, held together by ionic bonds.
