The formation of magnesium bromide (MgBr2) through the reaction of magnesium (Mg) with bromine (Br2) involves the transfer of electrons, leading to the formation of an ionic compound.
During the reaction, magnesium, which is a metal, undergoes oxidation, losing two electrons to attain a stable electron configuration. The oxidation state of magnesium changes from 0 to +2. The electron configuration of magnesium is [Ne] 3s^2, and upon losing two electrons, it becomes [Ne] 3s^0.
Bromine, on the other hand, is a halogen and has a tendency to gain one electron to achieve a stable electron configuration. It has an oxidation state of 0 before the reaction. Bromine's electron configuration is [Ar] 3d^10 4s^2 4p^5, and by gaining one electron, it becomes [Ar] 3d^10 4s^2 4p^6, which is the stable configuration of a noble gas (like argon).
During the reaction between magnesium and bromine, magnesium atoms lose two electrons to form Mg2+ ions, while bromine molecules gain two electrons to form Br− ions. The transfer of electrons allows the formation of an ionic bond between the magnesium cations and bromide anions. Two bromide ions combine with one magnesium ion to form the ionic compound magnesium bromide (MgBr2).
The balanced chemical equation for the reaction is:
Mg + Br2 → MgBr2
Overall, the reaction involves the oxidation of magnesium and the reduction of bromine, resulting in the formation of magnesium bromide through the transfer of electrons.