Question

Element X is in Group 2 and element Y is in Group 17. A compound formed between these two elements is most likely to have the formula:
a.X2Y7
b.XY2
c.X7Y2
d.X2Y

Answer 1

The answer is:  XY₂ .
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For example:
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   MgCl₂  
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Answer 2

Answer: The correct option is B.

Explanation: We are given that Element X is present in Group 2, so its valence electronic configuration will be: $[\text{Noble gas}]ns^2$ . It will loose 2 electrons in order to attain stable electronic configuration.

Element Y is present in Group 17, so its valence electronic configuration is: $[\text{Noble gas}]ns^2np^5$ .It will gain 1 electron to attain stable electronic configuration.

Hence, we can say that 2 atoms of Y-element will be required to combine with 1 atom of X-element.

Therefore, the formula becomes $XY_2$.