Question

Given their location on the periodic table, identify the ionic charge for each element and predict the compound formed by the barium and chloride ions.

Answer 1

Barium has a 2+ charge as it is in group 2 in the periodic table and so it has two electrons in its outer shell and chloride has a -1 charge on its chloride ion. So we will need two of the chloride ions as we have a 2+ charge to match the amount of charge on one barium ion- forming barium ion

BaCI2

Answer 2

Explanation:

Atomic number of barium is 56 and its electronic configuration is $[Xe]6s^{2}$.

Since, barium is a group 2 metal so in order to attain stability it will readily lose two electrons. Hence, barium will acquire a +2 charge and forms $Ba^{2+}$ ion.

On the other hand, chlorine is a group 17 element and its electronic distribution is 2, 8, 7. Hence, to attain stability it will gain one electron and forms $Cl^{-}$ ion.

Thus, we can conclude that charge on barium ion is +2 and charge on chlorine ion is -1.