Copper crystallises with face centred cubic unit cell . If the radius of copper atom is 127.8 pm , calculate the density of copper metal.
(Atomic mass of Cu = 63.55 u and Avogadro's number `N_(A) = 6.02 xx 10^(23) mol^(-1)`)

Explanation

To calculate the density of copper metal, which crystallizes in a face-centered cubic (FCC) unit cell, we can follow these steps:

### Step 1: Identify the given data
- Radius of copper atom (r) = 127.8 pm = \(127.8 \times 10^{-12}\) m
- Atomic mass of copper (M) = 63.55 u
- Avogadro's number (\(N_A\)) = \(6.022 \times 10^{23} \, \text{mol}^{-1}\)

### Step 2: Calculate the edge length (a) of the unit cell
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