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Problem: Iron has a density of 7.86 g/cm3 and crystallizes in a body-centered cubic lattice. Show that only 68% of a body-centered lattice is actually occupied by atoms, and determine the atomic radius of iron.

FREE Expert Solution

This problem involves a series of calculations to obtain the answers. We will first solve for the atomic radius for a body-centered cubic cell. Through explanation and calculations below we'll know why we need to answer this first in order to prove that only 68% of a body-centered cubic (BCC) lattice is actually occupied by atoms.

We don't have an equation that directly relates the radius to any of the given information so we solve this through multiple steps.


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Problem Details

Iron has a density of 7.86 g/cm3 and crystallizes in a body-centered cubic lattice. Show that only 68% of a body-centered lattice is actually occupied by atoms, and determine the atomic radius of iron.

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Khatiwada's class at Abraham Baldwin Agricultural College.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.