### Face-centered cubic problem list

Problem #1: Palladium crystallizes in a face-centered cubic unit cell. Its density is 12.023 g/cm3. Calculate the atomic radius of palladium.

Problem #2: Nickel crystallizes in a face-centered cubic lattice. If the density of the metal is 8.908 g/cm3, what is the unit cell edge length in pm?

Problem #3: Nickel has a face-centered cubic structure with an edge length of 352.4 picometers. What is the density?

Problem #4: Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, calculate the density of solid calcium.

Problem #5: Krypton crystallizes with a face-centered cubic unit cell of edge 559 pm. (a) What is the density of solid krypton? (b) What is the atomic radius of krypton? (c) What is the volume of one krypton atom?

Problem #6: You are given a small bar of an unknown metal. You find the density of the metal to be 11.5 g/cm3. An X-ray diffraction experiment measures the edge of the face-centered cubic unit cell as 4.06 x 10-10 m. Find the gram-atomic weight of this metal and tentatively identify it.

Problem #7: A metal crystallizes in a face-centered cubic lattice. The radius of the atom is 0.197 nm. The density of the element is 1.54 g/cm3. What is this metal?

Problem #8: The density of an unknown metal is 2.64 g/cm3 and its atomic radius is 0.215 nm. It has a face-centered cubic lattice. Determine its atomic weight.

Problem #9: Metallic silver crystallizes in a face-centered cubic lattice with L as the length of one edge of the unit cube. What is the center-to-center distance between nearest silver atoms?

Problem #10: Iridium has a face centered cubic unit cell with an edge length of 383.3 pm. The density of iridium is 22.61 g/cm3. Use these data to calculate a value for Avogadro's Number.

Problem #11: Platinum has a density of 21.45 g/cm3 and a unit cell side length 'd' of 3.93 Ångstroms. What is the atomic radius of platinum? (1 Å = 10-8 cm.)

Problem #12: The unit cell of platinum has a length of 392.0 pm along each side. Use this length (and the fact that Pt has a face-centered unit cell) to calculate the density of platinum metal in kg/m3 (Hint: you will need the atomic mass of platinum and Avogadro's number).

Problem #13: A metal crystallizes in a face-centered cubic structure and has a density of 11.9 g cm-3. If the radius of the metal atom is 138 pm, what is the most probable identity of the metal.

Problem #14: Nickel oxide (NiO) crystallizes in the NaCl type of crystal structure. The length of the unit cell of NiO is 4.20 Å. Calculate the density of NiO.

Problem #15: NiO adopts the face-centered-cubic arrangement. Given that the density of NiO is 6.67 g/cm3, calculate the length of the edge of its unit cell (in pm).