Rhodium has a face-centered cubic structure and has a density of 12.4 g/cm³.What is its atomic radius? A)134 pm B)268 pm C)380 pm D)1070 pm

Question

Quizplus · Accepted Answer

The atomic radius can be calculated using the formula for density and the face-centered cubic structure. The formula for the density of a face-centered cubic structure is: Density = (Z * M) / (a^3 * N_A), where Z is the number of atoms per unit cell (4 for FCC), M is the molar mass, a is the edge length of the unit cell, and N_A is Avogadro's number. The edge length a is related to the atomic radius r by a = 2√2 * r for FCC. Solving these equations with the given density and known values for rhodium gives an atomic radius of approximately 134 pm.

Rhodium Has a Face-Centered Cubic Structure and Has a Density