Question

Nickel crystallizes in a face-centered cubic lattice. If the density of the metal is 8.908 g/cm3, what is the unit cell edge length in pm?

Answer #1

1) Calculate the average mass of one atom of Ni:

58.6934 g mol¯^{1} ÷ 6.022 x 10^{23} atoms
mol¯^{1} = 9.746496 x 10¯^{23} g/atom

2) Calculate the mass of the 4 nickel atoms in the face-centered cubic unit cell:

9.746496 x 10¯^{23} g/atom times 4 atoms/unit cell =
3.898598 x 10¯^{22} g/unit cell

3) Use density to get the volume of the unit cell:

3.898598 x 10¯^{22} g ÷ 8.908 g/cm^{3} =
4.376514 x 10¯^{23} cm^{3}

4) Determine the edge length of the unit cell:

[cube root of] 4.376514 x 10¯^{23} cm^{3} =
3.524 x 10¯^{8} cm

5) Convert cm to pm:

cm = 10¯^{2} m; pm = 10¯^{12} m.

Consequently, there are 10^{10} pm/cm

(3.524 x 10¯^{8} cm) (10^{10} pm/cm) = 352.4
pm

Copper crystallizes with a face-centered cubic lattice and has a
density of 8.93 g/cm3.
a.) Calculate the mass of one unit cell of copper (in grams) b.)
Calculate the volume of the copper unit cell (in cm3). c.)
Calculate the edge length of the unit cell (in cm). d.) Calculate
the radius of a copper atom (in pm).

A metal crystallizes in a face-centered cubic cell and had a
density of 11.9 g/cm3. If the radius of the metal atom is 138 pm,
what is the molar mass of the metal? What metal is it?

1. Unit Cells
i. A certain metal crystallizes in a face-centered cubic unit
cell. If the atomic radius is 150 pm, calculate the edge length
(cm) and volume of the unit cell (cm3)?
ii. If said metal is Gold (Au), calculate the density.

They metal crystallizes in a face center cubic lattice. The radius
of the atom is 196 PM and the density of the element is 1.55 g/cm3.
How many atoms are there per unit cell?

A certain element crystallizes in a face-centered cubic lattice.
The density of the crystal is 22.67 g·cm–3, and the edge of the
unit cell is 383.3 pm. Calculate the atomic mass of the element.
(a) 192 g·mol–1 (b) 40 g·mol–1 (c) 183 g·mol–1 (d) 70 g·mol–1 (e)
None of the above

A hypothetical metal crystallizes with the face-centered cubic
unit cell. The radius of the metal atom is 184 picometers and its
molar mass is 195.08 g/mol. Calculate the density of the metal in
g/cm3.

Gold crystallizes is a face-centered cubic unit cell.
Its density is 19.3 g/cm3
. Calculate the atomic radius of
gold in picometer.

An element crystallizes in a body-centered cubic lattice. The
edge of the unit cell is 3.37 Å in length, and the density of the
crystal is 7.88 g/cm3 .
Calculate the atomic weight of the element.
Express the atomic weight in grams per mole to three significant
digits.

Chromium metal crystallizes as a body-centered cubic lattice. If
the atomic radius of Cr is 1.25 angstroms, what is the density of
Cr metal in g/cm3?

A certain metal crystallizes in a body centered cubic unit cell
with an edge length of 310 pm. What is the length in Angstroms of
the unit cell diagonal that passes through the atom?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 15 minutes ago

asked 15 minutes ago

asked 25 minutes ago

asked 30 minutes ago

asked 38 minutes ago

asked 38 minutes ago

asked 38 minutes ago

asked 38 minutes ago

asked 40 minutes ago

asked 46 minutes ago

asked 51 minutes ago

asked 1 hour ago