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