Question

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.

Answer #1

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.

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?

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.

iridium has a cubic closest packed structure with an edge length
of 385 pm. calculate the value of the atomic radius and the density
of iridium

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.

A metal crystallizes in a face-centered cubic closest packed
structure. The radius of the metal atom is 2.14x10^-8 cm. calculate
the density of solid metal if the atomic mass of the metal is known
to be 87.62 g/mol. Identify the metal.
Thank you!

what is the atomic mass of the metal?
The density of a sample of metal was measured to be 8.90 g/cm3 .
An X-ray diffraction experiment measures the edge of a
face-centered cubic cell as 352.4 pm .

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.

Aluminum metal crystallizes in a face-centered cubic unit cell.
If the atomic radius of an Al is 1.43Angstroms, what is the density
of aluminum (in g/cm^3)

Chromium crystallizes in a body-centered cubic unit cell with an
edge length of 2.885 Å.
(a) What is the atomic radius (in Å) of chromium in this
structure?
____ Å
(b) Calculate the density (in g/cm3) of chromium.
____ g/cm3

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