Vanadium (V) crystallises in a bcc structure and has an atomic radius of 131 pm. Determine the density if the edge length of the bcc unit cell is 4r/v3 and the atomic mass is 50.94 g/mol. (NA = 6.022×1023 mol-1) A. 3.06 g/cm³ B. 6.11 g/cm³ C. 2.77 g/cm³ D. 12.2 g/cm3 F. 8.46 a/cm³

Barium oxide (BaO] crystallizes in a structure in which the O² io are in a face-centered cubic lattice and the Ba²+ ions are in octahedral holes. What is the number of Ba²+ ions in the unit ce 2 V = a³ = (4.47x10-8cm)³ = 8.93x10-23 cm³ 4.72x10¯ 5.28 g cm formul 3 8 = 4.01 formula units

11. An element with atomic mass 106.9amu crystallizes in a face–centered cubic unit cell.  Its density is 11.0 g/cm3 at 27°C.  Calculate the atomic radius of an atom of the element in centimeters.