Question

which model correctly shows a stable ionic compound of magnesium chloride?
oa
ob
oc
od

Explanation:

Step1: Determine ion - charges

Magnesium (Mg) forms a $Mg^{2 + }$ ion by losing 2 electrons, and chlorine (Cl) forms a $Cl^{-}$ ion by gaining 1 electron.

Step2: Balance charges

To form a neutral ionic compound, for every $Mg^{2+}$ ion, we need 2 $Cl^{-}$ ions to balance the + 2 charge of magnesium. So the formula of magnesium chloride is $MgCl_{2}$.

Answer:

B.