We are being asked to calculate the edge length and density of the face-centered cubic unit cell of aluminum (atomic radius = 1.43 Å)
Recall that the face-centered cubic lattice contains an atom in each of the face of the cube and an atom in each of the corners. It looks like this:
We are going to do the following steps:
Step 1: Calculate the edge length of the aluminum unit cell
Step 2: Determine the volume of Al atoms in 1 unit cell
Step 3: Determine the mass of Al atoms in 1 unit cell
Step 4: Calculate the density of the aluminum unit cell
Aluminum (atomic radius = 1.43 Å) crystallizes in a cubic closely packed structure. Calculate the edge length of the face-centered cubic unit cell and the density of aluminum.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Unit Cell concept. You can view video lessons to learn Unit Cell. Or if you need more Unit Cell practice, you can also practice Unit Cell practice problems.
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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.