Question

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?

Answer #1

The calculated Atomic mass of metal is 106.56 g/mol that is
nearly Atomic mass of **Palladium.**

**therefore, the metal is Palladium.**

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.

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?

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).

Rhodium crystallizes in a face-centered cubic unit cell. The
radius of a rhodium atom is 135 pm.
Determine the density of rhodium in g/cm3.
please show all work and units!

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

Rhodium crystallizes in a face-centered cubic unit cell. The
radius of a rhodium atom is 135 pm.
Determine the density of rhodium in g/cm3. Which of the below is
the correct answer?
12.4 g/cm3
3.07 g/cm3
278 g/cm3
0.337 g/cm3

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.

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?

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...

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