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<u>Answer:</u>
<u>For a:</u> The edge length of the unit cell is 314 pm
<u>For b:</u> The radius of the molybdenum atom is 135.9 pm
<u>Explanation:</u>
- <u>For a:</u>
To calculate the edge length for given density of metal, we use the equation:
where,
= density =
Z = number of atom in unit cell = 2 (BCC)
M = atomic mass of metal (molybdenum) = 95.94 g/mol
= Avogadro's number =
a = edge length of unit cell =?
Putting values in above equation, we get:
Conversion factor used:
Hence, the edge length of the unit cell is 314 pm
- <u>For b:</u>
To calculate the edge length, we use the relation between the radius and edge length for BCC lattice:
where,
R = radius of the lattice = ?
a = edge length = 314 pm
Putting values in above equation, we get:
Hence, the radius of the molybdenum atom is 135.9 pm