A W element that is in the IIA family combines with a Y element in the VIIA family and results in an ionic compound whose only likely formula is: (demonstrate the bond)
a)WY
b)Y²W
c)WY²
d)W²Y
I assume the superscripts should be subscripts (unless you're a student in France).
Next, why are b and c not the same. BaCl2 is an example so either b or c should be correct. USUALLY the metal is written first so c is more correct than b.
Also, I don't understand how the formula demonstrates the bond. I would write the bond
WY2 ==> W^2+ + 2Y^-
To determine the formula of the ionic compound formed by combining the W element from the IIA family and the Y element from the VIIA family, we need to consider the charges of the individual ions.
The IIA family elements typically have a +2 charge, while the VIIA family elements typically have a -1 charge.
Since one W ion (from the IIA family) combines with one Y ion (from the VIIA family), we need to ensure that the overall charges on the ions are balanced in the resulting compound.
To do this, we can use the crisscross method.
The charge on the W ion is +2, and the charge on the Y ion is -1. We can write these charges as superscripts to represent the ions:
W²+ Y¹-
To balance the charges, we crisscross the numerical values of the charges to obtain the subscripts in the formula of the compound.
This means the W ion will have a subscript of 1 (since 2 divided by 2 is 1), and the Y ion will have a subscript of 2 (since 1 divided by 1 is 1).
The resulting formula is WY₂, which corresponds to option c)WY².
Therefore, the only likely formula for the ionic compound formed by the combination of the W and Y elements is WY².