# Problem: Use the Lewis model to predict the formula for the compound that forms between magnesium and nitrogen.

###### FREE Expert Solution

Elements have common charges based on what group they belong to in the periodic table. Elements gain and lose electrons so that they have the same number of electrons as the noble gases.

Metals → lose electrons and gain positive (+) charge to become more like their closest noble gas
Nonmetals → gain electrons and have negative (-) charge to become more like their closest noble gas.

Group 1A       metals                         Lose 1 e-         +1 charge
Group 2A       metals                         Lose 2 e-         +2 charge
Group 3A       metals                         Lose 3 e-         +3 charge
Group 4A       nonmetals                   typically do not gain or lose e- until Tin (Sn) and Lead (Pb)
Group 5A       nonmetals                   Gain 3 e-          -3 charge
Group 6A       nonmetals                   Gain 2 e-          -2 charge
Group 7A       nonmetals                   Gain 1 e-          -1 charge
Group 8A       Noble Gases              Complete Electrons

Now let’s figure out the chemical formula of the ionic compound:

magnesium → group 2A → +2 charge → Mg2+
• nitrogen→ group 5A → –3 charge → N3

###### Problem Details

Use the Lewis model to predict the formula for the compound that forms between magnesium and nitrogen.