1. Magnesium has an electronic configuration of 2.8.2 Oxygen has an electronic configuration of 2.6
Explain, in terms of their electronic configuration, how magnesium and oxygen atoms react to
form the ionic compound magnesium oxide, MgO, and include the description of the structure of
solid magnesium oxide *
(6 Points)

Explanation:

Magnesium and oxygen forms ionic bonds between them. In the formation of an ionic bond, a metal will lose an amount of electron to the non - metal. This way two ions are produced  and the electrostatic attraction between the two ions results in the formation of the ionic bond.

  Magnesium : 2 8 2

  Oxygen : 2 6

For magnesium to be stable and be isoelectronic with neon, it must lose two electrons to form an ion:

          Mg →   Mg²⁺ + 2e⁻  

For oxygen to be stable it must gain two electrons:

     O  + 2e⁻  →  O²⁻  

Mg²⁺ + O²⁻ →  MgO

So the attraction between the ions results in the formation of the MgO.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.