Based on the number of atoms per unit cell and the mass of the atom, the mass of the unit cell can be calculated. The density of the unit cell and the material as a whole can be determined from the mass and the volume of the unit cell as.

D= M/V


The usual units of density are grams per cubic centimeter or .
Part A
Nickel, , has a face-centered cubic structure (Part A figure) with an edge length of 352 . What is the density of this metal? Use the periodic table as needed.
Express your answer numerically in grams per cubic centimeter.

I need to know two things.

1. 352 what? meters, cm, pm?
2. What do you know about this problem? How much can you do and what don't you understand.

its pm

i guess we have to multipy by 10^-12

thn i don't knw abt mass

d=m/v
since i don't even knw the units too hw to cont

density = mass/volume.

First, calculate volume.
You know the edge length is 352 pm. Convert that to cm (since the problem wants the density in g/cc), then length^3 = volume (in cubic centimeters).
Now for mass.
A face centered cubic unit cell contains 4 particles so the mass of the unit cell contents is the mass of the Ni atom.
4*atomic mass Ni/6.022 x 10^23 = ?? grams of one unit cell.
Density, then, is ??grams/volume in cc.
Post your work if you get stuck.

In this case, the answer is 8.94 g/cm^3

To calculate the density of nickel, we need to determine the mass and volume of the unit cell.

1. Determine the volume of the unit cell:
In a face-centered cubic structure, there are four atoms located at each corner of the unit cell and one additional atom at the center of each face. This means there are a total of 14 atoms per unit cell (4 from each corner and 1 from each face).

Since nickel has a face-centered cubic structure, the edge length of the unit cell (a) is given as 352 pm (picometers).

The volume of the unit cell (V) can be calculated using the formula:
V = a^3

Substituting the given value of a:
V = (352 pm)^3

Note: To proceed with the calculations, it's important to convert picometers to centimeters since the density is usually expressed in grams per cubic centimeter. 1 picometer (pm) is equal to 1e-12 centimeters.

Therefore,
V = (352e-12 cm)^3

2. Calculate the mass of the unit cell:
To calculate the mass of the unit cell, we need to know the number of atoms per unit cell and the mass of each atom.

The number of atoms per unit cell for a face-centered cubic structure is given as 4.

The molar mass of nickel (Ni) can be found on the periodic table and is approximately 58.6934 grams per mole.

The mass of each atom (m) can be calculated using the formula:
m = molar mass / Avogadro's number

Avogadro's number is approximately 6.022 x 10^23 atoms per mole.

Therefore,
m = 58.6934 g/mol / (6.022 x 10^23 atoms/mol)

3. Calculate the mass of the unit cell (M):
Since there are 14 atoms per unit cell (as determined earlier), we can calculate the mass of the unit cell (M) using the formula:
M = 14 * m

4. Calculate the density (D):
Finally, we can calculate the density of the unit cell and the material as a whole using the formula:
D = M / V

Substitute the values of M and V calculated earlier to find the density of nickel in grams per cubic centimeter (g/cm^3).

By following these steps, you should be able to calculate the density of nickel based on the given information.