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Calculating radius of Rubidium in unit cellHelp.

  1. Oct 31, 2012 #1
    1. The problem statement, all variables and given/known data

    Calculate the Radius of Rubidium ion (which adopts sodium chloride structure.), if the density of Rubidium chloride is 2.76g*cm^(-3) and if we assume that the ions touch each other along the sides of the edge of the unit cell.


    I'm a bit lost here. I assume the density is the density of the whole unit cell. But how can I find a radius without knowing any length at all?
     
  2. jcsd
  3. Oct 31, 2012 #2

    Borek

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    Staff: Mentor

    How many moles of RbCl per one cubic centimeter of the crystal? How many molecules it is? Unit cells?
     
  4. Oct 31, 2012 #3
    In one unit cell there must be 4 moles of sodium and 4 chloride units even thought the cation sodium is much smaller than Cl.
     
  5. Oct 31, 2012 #4

    Borek

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    Staff: Mentor

    Atoms, not moles. And mole is known number of atoms (molecules, ions, whatever).
     
  6. Oct 31, 2012 #5
    Ahh yes, so perhaps if we know the radii ratio? It's not given in the problem, but i could imagine we would have to know how many times one atom is bigger than another?
     
  7. Nov 1, 2012 #6

    Borek

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    Staff: Mentor

    On the second thought, while apparently mole step is necessary to calculate volume of the unit cell, I don't see how to calculate radius. Sum of radii of the cation and the anion is obvious, but separating them is not, unless I am missing something.

    It happens that the radii are almost identical, but it is not said in the question.
     
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