**Calculate the number of atoms in the unit cell.**

The unit cell of polonium is a simple cube:

It has a #"Po"# atom at each corner.

But how many #"Po"# atoms are actually **inside** the cube?

Here's a cutaway diagram of the cube itself.

We see that there is only one-eighth of a Po atom at each corner.

Since there are 8 corners,

#"Number of Po atoms" = 8 color(red)(cancel(color(black)("corners"))) × ("⅛ Po atom")/(1 color(red)(cancel(color(black)("corner")))) = "1 Po atom"#

**Calculate the mass of the unit cell**

#"Mass of unit cell" = 1 color(red)(cancel(color(black)("atom Po"))) × (1 color(red)(cancel(color(black)("mol Po"))))/(6.022 × 10^23 color(red)(cancel(color(black)("Po atoms")))) × "209 g"/(1 color(red)(cancel(color(black)("mol Po"))))#

#= 3.471 × 10^"-22" color(white)(l)"g"#

**Calculate the volume of the unit cell.**

The formula for the volume of a cube is #V = l^3#, where #l# is the length of an edge of the cube.

#V = l^3 = (0.335 × 10^"-9" color(red)(cancel(color(black)("m"))))^3 × ("100 cm"/(1 color(red)(cancel(color(black)("m")))))^3 = 3.760 × 10^"-23"color(white)(l) "cm"^3#

**Calculate the density of the unit cell**

#ρ = m/V = (3.471 × 10^"-22" color(white)(l)"g")/(3.760 × 10^"-23" color(white)(l)"cm"^3) = "9.23 g/cm"^3#

Since density is an **intensive property**, this is also the density of the bulk metal.