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CHIM 2045-Other Toolbox #3: Student Name: Solids- Cubic Unit Cell Type Problems Sect. Date: the three tvpes of cubic unit cells, giving in addition for each case: a. The net number of atoms contained within a unit cell: b. The total number of different atoms that contribute to the volume of this type of unit cell 6 Cubic Type: Net # Atom/Unit Cell # of Diff. Atorns/Unit Cell U.C.L Packing EfficiencyPacking Efficiency Cubic Type: Net #Atom/Unit Cell-A-_ # of Diff. Atoms/Unit Cell_ Cubic TypeL Net #Atom/Unit Cell # of Diff. Atoms/Unit Cell U.C.L. 0 Packing Efficiency The most stable solid form of phosphorus arranges itself in a simple cubic type unit cell crystalline lattice. If all the P atoms, each of radius 1.100 x 103 cm are assumed to b 2. e rigid spheres in contact with each other, what is the density of the nonmetal phosphorus (g/cm? (atoms on the corners touch) 3. In metallic silver, slver atoms (Ag) are packed in a face-centered cubic arrangement. If a unit eell's edge length is 4.078 x 108 cm, calculate the density of metallic silver (g/em3). (atoms on a face diagonal touch) 4. Sodium (Na) metal atoms crystallize in a body-centered cubic arrangement. If the sodium's unit cell length (em) is 4,24 x 103 cm, what is metallic sodium's density (g/em3)? (atoms on the front to back diagonal of the cube touch)
BINDER LE CHM 2045 Other Toolbox H3: Student Name: Solids Cubic Unit Cell Type Problems Date: 丶 1. b. The tam neu ber of atoms contained within sunitsell. givingin addition for each ease: n. The net number ofatoms contained within a unit cell: b. The total unber of different 8 atoms that contribute to the volume of this type of unit cell: PIECES V-9u Cubic Type: Net # Aton/Unit Cell # of DirT. Cubic Type: C Net #Atom/Unit Cell Cubic Type Net #Atom/Unit Cell #of Dir. AtoindUnit Cen /2 U C.Lt Alors Unit Cell Y Packing Efficiency 5 /4 of Dir. Ato11 s/Unit Cell L L1 . 3000 , Packing Efficiency고 互6 2.459 Packing Efficieney 2. The most stable solid form of phosphorus arranges itseif in a simple cubic crystalline lattice. If al the P atoms, each of radius 1.100 x 10 em n contact with each other, what is the density of the nonmetal phosphorus (g/cm? (atoms on the corners touch) 3. In metallic silver, silver atoms (Ag) are packed in a face-centered cubic arrangement. If a unit cell's edge length is 4.078 x I0 em, calculate the density of metallie silver (gJlem). (atoms on a face diagonal touch) 4. Sodium (Na) metal atoms crystallize in a body-centered cubic arrangement. If the sodium's unit cell length (cm) is 4.24 x 10-8 cm, what is metallic sodium's density (g/cm)? (atoms on the front to back diagonal of the cube touch)

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