8. The density of nickel is 8.908 g/cm3. If the metallic radius of nickel is 125 pm, what is the structure of metallic nickel?

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8. The density of nickel is 8.908 g/cm3. If the metallic radius of nickel is 125 pm, what is the
structure of metallic nickel?
9. An element has a density of 10.25 g/cm3 and a metallic radius of 136.3 pm. The metal
crystallizes in a bcc lattice. Identify the element.
10. A 21.64 g sample of a nonreactive metal is placed in a flask containing 12.00 mL of water; the
final volume is 13.81 mL. If the length of the edge of the unit cell is 387 pm and the metallic radius
is 137 pm, determine the packing arrangement and identify the element.
11. Lithium crystallizes in a bcc structure with an edge length of 3.509 Å. Calculate its density.
What is the approximate metallic radius of lithium in picometers?
12. A simple cubic cell contains one metal atom with a metallic radius of 100 pm:
a. Determine the volume of the atom(s) contained in one unit cell
[the volume of a sphere = (4/3)Tr°].
b. What is the length of one edge of the unit cell?
c. Calculate the volume of the unit cell.
d. Determine the packing efficiency for this structure.
e. Use the steps in Problem 11 to calculate the packing efficiency for a bcc unit cell with a
metallic radius of 1.00 Å.
Transcribed Image Text:8. The density of nickel is 8.908 g/cm3. If the metallic radius of nickel is 125 pm, what is the structure of metallic nickel? 9. An element has a density of 10.25 g/cm3 and a metallic radius of 136.3 pm. The metal crystallizes in a bcc lattice. Identify the element. 10. A 21.64 g sample of a nonreactive metal is placed in a flask containing 12.00 mL of water; the final volume is 13.81 mL. If the length of the edge of the unit cell is 387 pm and the metallic radius is 137 pm, determine the packing arrangement and identify the element. 11. Lithium crystallizes in a bcc structure with an edge length of 3.509 Å. Calculate its density. What is the approximate metallic radius of lithium in picometers? 12. A simple cubic cell contains one metal atom with a metallic radius of 100 pm: a. Determine the volume of the atom(s) contained in one unit cell [the volume of a sphere = (4/3)Tr°]. b. What is the length of one edge of the unit cell? c. Calculate the volume of the unit cell. d. Determine the packing efficiency for this structure. e. Use the steps in Problem 11 to calculate the packing efficiency for a bcc unit cell with a metallic radius of 1.00 Å.
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