How is the formation of the salt #MgCl_2# rationalized on the basis of the Periodic Table?
Magnesium is in Group II of the Periodic Table. Chlorine is in Group VII.
If the metal is in Group II, then it has
On the other hand, atomic chlorine has 7 valence electrons (as does fluorine and bromine). Chlorine can be (fairly easily) reduced to the chloride ion, with 8 formal valence electrons. Why should it accept electrons? For a start it is a non-metal to the right of the Periodic Table, and its nuclear charge attracts electrons. The ease of reduction with respect to chlorine, and the relative ease of oxidation of the magnesium atom to