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alpha polonium crystalizes in a simple cubic unit cell with an edge length of 336 pm. whatis the density of alpha polonium (in g/cm^3)?

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alpha polonium crystallizes in a simple cubic unit cell with an edge length of 336 pm, the density becomes 7.318 g/cm³.

What is unit cell?

The smallest repeating unit with complete crystal structural symmetry is designated as a unit cell. The unit cell geometry, sometimes referred to as a parallelepiped, provides six lattice parameters, which are the lengths of the cell edges (a, b, and c) and the angles at which they are spaced apart ( α,β,γ ).

Given that,

alpha polonium crystallizes in a simple cubic unit cell with an edge length (a) of 336 pm.

As we know, the relation between radius (r) and edge length (a) for simple cubic unit cell is: 2 r = a

Thus, r = a/2

r = 336/2   [ given a = 336 pm]

r = 168 pm

Now, density (d) = (Z × M) / a³ × [tex]N_A[/tex]

Here, Z = number of atom in a simple cubic unit cell = 1

M = molecular weight of polonium

[tex]N_A[/tex] = Avogadro's no.

d = ( 1  × 209) / (168 ×10⁻¹²)³ × (6.023 × 10²³)

d = 7.318 × 10⁷ g/m³

d =  7.318 g/cm³

So, the density of alpha polonium is 7.318 g/cm³.

To know more about unit cell refer to:

https://brainly.com/question/8305059

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