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Chromium metal crystallizes with a body-...

Chromium metal crystallizes with a body-centred cubic lattice. The edge length of the unit cell is found to be 287 pm. Calculate the atomic radius. What would be the density of chromium in g `cm^(-3)` ? (atomic mass of Cr = 52.99)

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To solve the problem, we need to calculate the atomic radius of chromium and its density given that chromium crystallizes in a body-centered cubic (BCC) lattice with an edge length of 287 pm (picometers). The atomic mass of chromium is given as 52.99 g/mol. ### Step 1: Calculate the Atomic Radius In a body-centered cubic (BCC) lattice, the relationship between the edge length (A) and the atomic radius (r) is given by the formula: \[ A = \frac{4r}{\sqrt{3}} ...
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