Pack Ionic
Pack Ionic
chem help wileyplus! solid structures ionic solids?
An element has ccp packing with a face-centered cubic unit cell. Its density is 12000 kg/m3 and the unit cell volume is 5.89 x 10-26 L. Calculate the molar mass (g/mol) of the element to three significant figures.
how it was done would be great, but just an answer is perfect too! thanks
just like your other two questions...
(g / cm³) x (cm³ / cell) x (cell / atoms) x (atoms / mole) = g/mole
you know the first two and the last one.. but what about atoms / cell?
*** atoms / cell ***
this is a face centered cubic cell.. it has 8 corner atoms and 6 face atoms.. each corner atom exists in 8 adjacent cells.. so 1/8 of each corner atom is in any given cell. each face atom exists in two adjacent cells. so 1/2 of each face atom is in any given cell.
8x1/8 + 6x1/2 = 4 atoms / cell
now we need to do some unit conversions...
12000 kg / m³ x (1 m / 100 cm)³ x (1000 g / 1 kg) = 1.2 g / cm³
and
5.89x10^-26 L x (1000 mL / 1 L) x (1 cm³ / 1 mL) = 5.89x10^-23 cm³
finally...
(1.2 g / cm³) x (5.89x10^-23 cm³ / cell) x (1 cell / 4 atoms) x (6.022x10^23 atoms / mole) = 10.6 g/mole
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