Element X forms a chloride, XCln which melts at 3[tex]\circ[/tex]C. When 0.500 g of the chloride reacts with an excess of acidified silver nitrate, 1.19g of AgCl are formed.
Another 0.500g sample of the chloride is heated strongly and chlorine gas is given off. When the residue is treated with an excess of acidified silver nitrate, only 0.714g of AgCl is precipitated.
(1) Predict the type of bonding in XCln.
(2) Suggest with reasons, to which group of the Periodic Table element X belongs.
(3) Calculate the value of n and attempt to identify X.
The Attempt at a Solution
(1) It is covalent because of the low melting point.
(2) I would say group 5 or 6 because the chlorides exhibits several valencies. (but i don't know which one to choose) and the question asks for reasonS<---
(3) I am completely lost and confused. I calculated the number of mol of AgCl formed in both cases knowing that the difference between these values should give me something important. but i don't know what.
and i think X is phosphorous because PCl5 decomposes into PCl3 on heating. but the question does not ask for this kind of reasoning.