Recall that for a** unit cell**:

$\overline{){\mathbf{\#}}{\mathbf{}}{\mathbf{atoms}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\mathbf{(}\mathbf{\#}\mathbf{}\mathbf{of}\mathbf{}\mathbf{corner}\mathbf{}\mathbf{atoms}\mathbf{}\mathbf{\times}\frac{\mathbf{1}}{\mathbf{8}}\mathbf{)}{\mathbf{+}}\mathbf{(}\mathbf{\#}\mathbf{}\mathbf{of}\mathbf{}\mathbf{face}\mathbf{}\mathbf{atoms}\mathbf{}\mathbf{\times}\frac{\mathbf{1}}{\mathbf{4}}\mathbf{)}\mathbf{+}\mathbf{(}\mathbf{\#}\mathbf{}\mathbf{of}\mathbf{}\mathbf{atoms}\mathbf{}\mathbf{at}\mathbf{}\mathbf{the}\mathbf{}\mathbf{center}\mathbf{\times}\mathbf{1}\mathbf{)}}$

***Atoms on the corner will have 1/8 of its volume on the unit cell *

***Atoms on the cube face will have 1/4 of its volume on the unit cell *

This means that:

An oxide of rhenium crystallizes with the unit cell depicted here (where rhenium = gray and oxygen = red)

.

What is the formula of the oxide?

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