A. The atomic radius of sodium can be estimated using the equation for the volume of a cube, V = a3, where a is the length of one side of the cube. Since the density of sodium is 0.97 g/cm3, we can calculate the volume of one mole of sodium atoms as 0.97 cm3/mol. Using Avogadro's number (6.022 x 1023 atoms/mol), we can calculate the length of one side of the cube as 0.282 nm. The atomic radius of sodium is therefore 0.141 nm.
B. The density of sodium if its structure were that of a cubic close-packed metal would be 2.27 g/cm3. This is much higher than the density of water (1 g/cm3), so sodium would not float on water.
Sodium metal adopts a body-centered cubic structure with a density of 0.97g/cm3. A. Use this information and Avogadro's number to estimate the atomic radius of sodium. B. If it didn't react so vigorously, sodium could float on water. Use the answer from part a to estimate the density of Na if its structure were that of a cubic close-packed metal. Would it still float on water?
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