An imaginary element with BCC structure and has an atomic radius of 0.17 nm, with a molar mass of 56.08 g/mol. What is the density of this element in g/cc? hint: you will need Avogadro's number and you will need to convert the given radius to cm.

The density of the given element is

Explanation:

To calculate the edge length, we use the relation between the radius and edge length for BCC lattice:

where,

R = radius of the lattice = 0.17 nm

a = edge length = ?

Putting values in above equation, we get:

To calculate the density of metal, we use the equation:

where,

= density

Z = number of atom in unit cell = 2  (BCC)

M = atomic mass of metal = 56.08 g/mol

= Avogadro's number =

a = edge length of unit cell =    (Conversion factor:    )

Putting values in above equation, we get:

Hence, the density of the given element is

14 days is the half-life of phosphorus-32