Question

Iridium packs in a face centered cubic structure with a density of 22.43 g/cm3 . Calculate the following: (1) Volume of unit cell in pm3 . (2) cell length (3) radius of iridium.

Answer #1

The very dense metal iridium has a face centered cubic structure
and density of 22.56 g/cm3. use this information to calculate the
radius of an iridium atom.

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).

1. Rubidium metal has a
body-centered cubic structure. The density of the metal is 1.532
g/cm3. Calculate the radius of the rubidium atom. Assume
that rubidium atoms are spheres. Then note that each corner sphere
of the unit cell touches the body-centered sphere.
2. Copper metal has a face-centered
cubic structure. The density of the metal is 8.93 g/cm3.
Calculate the radius of the copper atom. Assume that copper atoms
are spheres. Then note that the spheres on any face...

Iridium metal crystalizes in a face-centered cubic structure.
The edge length of the unit cell was found by x-ray diffraction to
be 383.9 pm. The density of iridium is 22.42g/cm^3. Calculate the
mass of an iridium atom. Use Avogadro's number to calculate the
atomic mass of iridium.

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

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?

Niobium has a density of 8.57 g/cm3 and crystallizes
with the body-centered cubic unit cell. Calculate the radius of a
niobium atom.

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.

1) For a metal that has the face-centered cubic (FCC) crystal
structure, calculate the atomic radius if the metal has a density
of (8.000x10^0) g/cm3 and an atomic weight of
(5.80x10^1) g/mol. Express your answer in
nm.
2) Consider a copper-aluminum solid solution containing
(7.82x10^1) at% Al. How many atoms per cubic centimeter
(atoms/cm^3) of copper are there in this solution?
Take the density of copper to be 8.94 g/cm3 and the
density of aluminum to be 2.71 g/cm3.

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