The face-centered gold crystal has an edge length of 407 pm. based on the unit cell, calculate the density of gold.

The molecules of a solid is compactly arranged. It is made up of repeating blocks called unit cells. The density of a unit cell is:

ρ = nA/VNₐ

where

n is the number of atoms per unit cell

A is the atomic weight of solid

V is the volume of unit cell

Na is Avogadro's number (6.022*10²³)

For a face-centered cubic unit cell, there are 4 atoms (n=4). The volume of the unit cell follows the formula of the cube, s³. The atomic weight of gold is 197 g. So, the solution is as follows:

ρ = (4 atoms) (197 g/mol) (1 kg/1000 g) / (407*10⁻¹² m) ³ (6.022*10²³ atoms/mol)

ρ = 19,408.5 kg/m³