Cobalt crystallizes in a HCP unit cell. Its atomic radius is 0.1253 nm. Its density is 8,900 kg/m^3. Using this information, estimate Avogadro's number.

A hypothetical metal with an atomic radius of 0.171 nm has an orthorhombic unit cell for which the a, b, and c lattice parameters are 0.479, and 0.725, and 0.978 nm, respectively. It has an atomic weight of 126.91 g/mol and a theoretical density of 4.92 g/cm3. Determine the APF of the metal. Use NA = 6.022 x 1023

Metallic strontium crystallizes in a face-centered cubic lattice. The volume of the unit cell is 2.25 × 10⁸ pm³. What is the density of strontium metal in g/cm³?

6. A compound consists of A-atoms and B-atoms, and its solid crystal forms a cubic unit cell structure, as shown below. A-atoms occupy corners and faces of the cube. B-atoms are inside the cube and are not shared by adjacent cubic unit cells. Based on the information here, we can conclude that (a) A-atoms form an FCC structure; the empirical formula of the compound is A,B2. (b) A-atoms form an FCC structure; the empirical formula of the compound is AB. (c) A-atoms form a BCC structure; the empirical formula of the compound is A¬B2. (d) A-atoms form a BCC structure; the empirical formula of the compound is AB. (e) None of the above. A-atoms (corners and faces) B-atoms (inside, not shared) a m n T OF THE FL EMENTS