Meadock

Alright, first, thanks for answering. Next, why multiply by 1000cm cubed? by not 1cm cubed? It is 2.23 grams per cubic centimeter. So lets pretend we have only one cubic centimeter. Also, I do believe the grams cancel each other in the end of your calculations. So it should be a quantity of moles, not a mass. I plugged your calculations into my own and it decreased the size of the radius by a factor of 10:-\ Thanks. Andrew

Out of pure curiosity I decided to try to determine the radius of a Carbon atom plus the average distance between atoms in Graphite to give me the total distance between the center of two Carbon Atoms in Graphite. Here's my data: Graphite Sample Density: about 2.23 g/cm cubed. Carbon Atomic Weight: 12.0107 g/mol. Avogadro constant(L): 6.02214279(30)×10^23 Start by determining how many moles are in our sample: 2.23 g / 12.0107 g/mol = 0.187 mol Then multiply it by Avogadro constant to find how many molecules of carbon are in our sample. 0.187 mol * (6.02*10^3) = 1.13*10^23 molecules in 1cm cubed Find the cube root of this: = 4.817*10^7 molecules in 1cm Then convert it to pm = 0.04817 molecules per 1pm The inverse of this should be the radius of a Carbon Atom = 10.38pm but... Carbon Atomic Radius is actually about 70 pm. What did I do wrong?