Problem: Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, calculate the density of solid calcium.

FREE Expert Solution

Step 1 Determine mass

$mass = \frac{4 Ca atoms}{1 unit cell} \times \frac{1 mol Ca}{6.022 \times 10^{23} Ca atoms} \times \frac{40.078 g Ca}{1 mol Ca}$

mass = 2.6621x10^-22 g/unit cell

Step 2 Determine volume

$volume = a^{3} a = 2 \sqrt{2} \cdot r volume = {(2 \sqrt{2} \cdot r)}^{3} volume = {(2 \sqrt{2} \times 197 pm \times \frac{10^{- 12} m}{1 pm} \times \frac{1 cm}{10^{- 2} m})}^{3} volume = {(5.572 \times 10^{- 8} cm)}^{3}$

volume = 1.723x10^-22 cm³

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Problem Details

Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, calculate the density of solid calcium.

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Problem: Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, calculate the density of solid calcium.

FREE Expert Solution

Problem Details

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