Exam 16: Liquids and Solids

You are given a small bar of an unknown metal, X. You find the density of the metal to be 10.5 g/cm³. An X-ray diffraction experiment measures the edge of the unit cell as 409 pm. Assuming that the metal crystallizes in a face-centered cubic lattice, what is X most likely to be?

A certain solid substance that is very hard, has a high melting point, and is nonconducting unless melted is most likely to be

A certain metal fluoride crystallizes in such a way that the fluoride ions occupy simple cubic lattice sites, while the metal atoms occupy the body centers of half the cubes. What is the formula for the metal fluoride?

A salt, MY, crystallizes in a body-centered cubic structure with a Y^- anion at each cube corner and an M⁺ cation at the cube center. Assuming that the Y^- anions touch each other and the M⁺ cation at the center, and that the radius of Y^- is 1.46  10² pm, what is the radius of M⁺?

Cs crystallizes in a body-centered cubic arrangement. Assuming that the dimensions of the unit cell for Cs and for CsCl are equivalent, determine the ratio of the density of Cs to the density of CsCl.

The triple point of iodine is at 90 torr and 115°C. This means that liquid I₂