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    Which of the following statements referring to the structures of sodium chloride and caesium chloride is correct?

    A. There are eight chloride ions surrounding each sodium ion.
    B. There are eight chloride ions surrounding each caesium ion.
    C. The chloride ions are arranged tetrahedrally round the sodium ions.
    D. The chloride ions are arranged tetrahedrally round the caesium ions.

    Can someone please explain how you would figure this out? Is it irrelevant to the new CfE AH course, or is it problem solving?

    Thanks for the help!!
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    (Original post by TheSmartGirl)
    Which of the following statements referring to the structures of sodium chloride and caesium chloride is correct?

    A. There are eight chloride ions surrounding each sodium ion.
    B. There are eight chloride ions surrounding each caesium ion.
    C. The chloride ions are arranged tetrahedrally round the sodium ions.
    D. The chloride ions are arranged tetrahedrally round the caesium ions.

    Can someone please explain how you would figure this out? Is it irrelevant to the new CfE AH course, or is it problem solving?

    Thanks for the help!!
    Answer is B

    You need to either know the crystal lattice structure for both compounds or be able to work them out to answer this question. Basically it's because the caesium ion is a lot bigger than the sodium, therefore you can fit more chloride ions (8 rather than the 6 you can fit round sodium) around each ceasium in the lattice. It's definitely not in the curriculum this year but it might just be a particularly evil problem solving question
 
 
 
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