Rhodium has a density of 12.41 g/cm3 and crystallizes with

Chapter 11, Problem 101E

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QUESTION:

Rhodium has a density of \(12.41\ \mathrm{g/cm}^3\) and crystallizes with the face-centered cubic unit cell. Calculate the radius of a rhodium atom.

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QUESTION:

Rhodium has a density of \(12.41\ \mathrm{g/cm}^3\) and crystallizes with the face-centered cubic unit cell. Calculate the radius of a rhodium atom.

ANSWER:

Step 1 of 5

The FCC unit cell is the simplest repeating unit in a cubic-closed packed structure. FCC unit cell contains four atoms per unit cell and its coordination number is twelve. Calculate the radius of FCC lattice using the formula.

\(l=2 \sqrt{2} r\)

Here, l is edge length and r is radius.

 

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