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# AS Chem AlCl3 question watch

1. Hi guys,

I'm a bit confused by a question I've got here, it says:

Solid aluminium chloride has the empirical formula AlCl3. Use the information in part b* to suggest how many aluminium ions surround each chloride ion in the ionic lattice. Explain your answer.

The information from part b reads: The ionic lattice has a structure in which 6 chloride ions surround one aluminium ion, in an octahedral arrangement.

I don't really know how to go about this question. I've drawn out the basic dot and cross diagram for the solid aluminium chloride and I've drawn the 3D octahedral arrangement but I don't know where to go from here.

Thanks in advance for any help,
Blake
2. So you know each Al is bonded to 6 chlorines. However there is only a 1:3 ratio of Al:Cl in the solid.

What does this tell you about how many Als are bonded to each Cl?
3. (Original post by alow)
So you know each Al is bonded to 6 chlorines. However there is only a 1:3 ratio of Al:Cl in the solid.

What does this tell you about how many Als are bonded to each Cl?
A third of an Al is bonded to each Cl?
4. (Original post by Blake Jones)
A third of an Al is bonded to each Cl?
Kind of, you have 3 Cls for every Al, but Al forms six bonds.

How many bonds do you have to each Cl?
5. (Original post by alow)
Kind of, you have 3 Cls for every Al, but Al forms six bonds.

How many bonds do you have to each Cl?
2?
6. (Original post by Blake Jones)
2?
Yeah. Here's a picture:

7. (Original post by alow)
Yeah. Here's a picture:

Oh I see! Thank you so much! It's not letting me rep you at the moment (says I have to rep someone else first) but I definitely will! You're so helpful!
8. (Original post by Blake Jones)
Oh I see! Thank you so much! It's not letting me rep you at the moment (says I have to rep someone else first) but I definitely will! You're so helpful!
No problem

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