Calcium crystallizes in a body-centered cubic structure at 467°C. (b) How many nearest neighbors does each Ca atom possess? (c) Estimate the length of the unit cell edge, a, from the atomic radius of calcium (1.97 Å). (d) Estimate the density of Ca metal at this temperature.

A body-centered cubic structure is a type of crystal lattice where atoms are located at each corner of a cube and a single atom is positioned at the center of the cube. In this arrangement, each atom has eight nearest neighbors, which are the corner atoms. Understanding this structure is crucial for determining the coordination number and the geometric properties of the material.

The unit cell is the smallest repeating unit in a crystal lattice that reflects the symmetry and structure of the entire crystal. For a BCC structure, the relationship between the atomic radius and the unit cell edge length can be derived from geometry, specifically using the formula a = 4r/√3, where 'a' is the edge length and 'r' is the atomic radius. This relationship allows for the calculation of the unit cell dimensions based on atomic size.

Density is defined as mass per unit volume and can be calculated using the formula ρ = m/V, where 'm' is the mass of the substance and 'V' is the volume. In the context of a crystal structure, the mass can be determined from the molar mass and the number of atoms in the unit cell, while the volume is derived from the cube of the unit cell edge length. This concept is essential for estimating the density of materials based on their crystalline structure.