36. Silver crystallizes in a cubic closest packing (ccp) structure, which corresponds to a face-centered cubic (fcc) unit cell, as shown. The atomic radius of silver is r = 1.44 Å. Calculate the density of silver by completing the following steps. Report all calculated values to 3 significant figures.
(1) There are effectively _ silver atoms in one unit cell.
(2) The edge length of the unit cell, d, is _ Å.
(3) The volume of the unit cell is _ cm³.
(4) The total mass of silver in one unit cell is _ g.
(5) The density of solid silver is _ g/cm³.