🤓 Based on our data, we think this question is relevant for Professor Halpin's class at NYU.

**Step 1: Calculate the volume of the unit cell in cm ^{3}.**

**Given:** **edge length (a) = 392.0 pm**

$\mathbf{volume}\mathbf{}\mathbf{of}\mathbf{}\mathbf{unit}\mathbf{}\mathbf{cell}\mathbf{=}\mathbf{volume}\mathbf{}\mathbf{of}\mathbf{}\mathbf{cube}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{volume}}{\mathbf{}}{\mathbf{of}}{\mathbf{}}{\mathbf{unit}}{\mathbf{}}{\mathbf{cell}}{\mathbf{=}}{{\mathbf{a}}}^{{\mathbf{3}}}}\phantom{\rule{0ex}{0ex}}\mathbf{volume}\mathbf{}\mathbf{of}\mathbf{}\mathbf{unit}\mathbf{}\mathbf{cell}\mathbf{}\mathbf{=}{\left(\mathbf{392}\mathbf{}\overline{)\mathbf{pm}}\right)}^{\mathbf{3}}\mathbf{\times}{\left(\frac{{\mathbf{10}}^{\mathbf{-}\mathbf{12}}\mathbf{}\overline{)\mathbf{m}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{pm}}}\right)}^{\mathbf{3}}\mathbf{\times}{\left(\frac{\mathbf{1}\mathbf{}\mathbf{cm}}{{\mathbf{10}}^{\mathbf{-}\mathbf{2}}\mathbf{}\overline{)\mathbf{m}}}\right)}^{\mathbf{3}}$

**volume of unit cell = 6.0236x 10 ^{-23} cm^{3}**

A metallic solid with atoms in a face-centered cubic unit cell with an edge length of 392 pm has a density of 21.45 g/cm^{3}. Calculate the atomic mass and the atomic radius of the metal. Identify the metal.

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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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Based on our data, we think this problem is relevant for Professor Halpin's class at NYU.

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 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.