Question #cb24f

1 Answer
qin
Apr 23, 2017

The energy level of the ionic compound formed should be considered instead.

Explanation:

Given that Mg is in group 2 and has two valence electrons, it can achieve a noble gas configuration or stable electronic configuration after losing 2 electrons.

Yes, the energy level of #Mg^(2+)# will be higher than that of #Mg^(+)#. However, since Mg will form an ionic compound with an gaseous anion, the energy released from ionic bonding is enough to compensate for this extra ionisation energy calculated.

This means that forming a compound of #MgO# will give out much more energy than forming #Mg(2)O#, leading to greater stability.

Related questions
See all questions in Net Charge
Impact of this question
1667 views around the world
You can reuse this answer
Creative Commons License