Argon has a cubic closest packed structure as a solid. Assuming that argon has a radius of \(190 . \mathrm{pm}\), calculate the density of solid argon.

The density of solid argon can be calculated using the given radius and the cubic closest packed structure formula. The steps are as follows: 1. Calculate the edge length of the unit cell: \(a = 2\sqrt2 (190 \, \text{pm})\). 2. Calculate the volume of the unit cell: \(V = (2\sqrt2 (190 \, \text{pm}))^3\). 3. Determine the number of argon atoms in one unit cell: 4 atoms. 4. Calculate the mass of one unit cell: \(m = \frac{4 \times 39.95 \, \text{g/mol}}{6.022 \times 10^{23} \, \text{atoms/mol}}\). 5. Calculate the density of solid argon: \(\rho = \frac{4 \times 39.95 \, \text{g/mol}}{(6.022 \times 10^{23} \, \text{atoms/mol}) \times (2\sqrt2 (1.90 \times 10^{-8} \, \text{cm}))^3}\). After evaluating the final expression, we obtain the density of solid argon in g/cm³.