Silver (atomic mass = 108) has an atomic radius of 144 pm and density 10.6 g/cm³. To which type of c — Solid State Chemistry Question

💡 Solution & Explanation

Let's assume an FCC lattice: Z = 4. The relationship between cell edge (a) and atomic radius (r) is a = 2 √2 r = 2 × 1.414 × 144 pm = 407.2 pm = 4.072 × 10^-8 cm. Volume V = a³ = 6.75 × 10^-23 cm³. Density ρ = (Z × M) / (Na × a³) = (4 × 108) / (6.022 × 10^23 × 6.75 × 10^-23) ≈ 10.6 g/cm³. This matches the given density. Thus, silver crystallizes in an FCC lattice.