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Standard XII

Physics

Energy Band Diagrams

Metallic magn...

Question

Metallic magnesium has a hexagonal close-packed structure and a density of 1.74 $g / c m^{2}$ . Assume magnesium atoms to be spheres of radius r. 74.1% of the space is occupied by atoms. Calculate the volume of each atom and the atomic radius r. (Mg=24.31)

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Solution

Atomic mass $= 54.94$
density $= 7.42 g / c c$
Apparent volume occupied by one atom $= ?$
$v o l u m e = \frac{m a s s}{d e n s i t y} = \frac{54.94}{7.42} = 7.40 c m^{3}$ (volume of one mole)
volume of one atom $= \frac{v o l u m e o f o n e m o l e}{6.022 \times 10^{- 23}}$
$= \frac{7.40}{6.022 \times 10^{- 23}}$
$= 1.23 \times 10^{- 23} c m^{3}$

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Metallic magnesium has a hexagonal close-packed structure and a density of 1.74 g/cm2. Assume magnesium atoms to be spheres of radius r. 74.1% of the space is occupied by atoms. Calculate the volume of each atom and the atomic radius r. (Mg=24.31)

Atomic mass =54.94density =7.42g/ccApparent volume occupied by one atom =?volume=massdensity=54.947.42=7.40cm3 (volume of one mole)volume of one atom =volume of one mole6.022×10−23=7.406.022×10−23=1.23×10−23cm3

Metallic magnesium has a hexagonal close-packed structure and a density of 1.74 $g / c m^{2}$ . Assume magnesium atoms to be spheres of radius r. 74.1% of the space is occupied by atoms. Calculate the volume of each atom and the atomic radius r. (Mg=24.31)