Posted by Arnol on Sunday, November 13, 2011 at 8:57pm.
An estimation of the radius of a lead atom:
a. You are given a cube of lead that is 1.000 em on each side. The density of lead is
11.35 g/cm3. How many atoms of lead are contained in the sample.
b. Atoms are spherical; therefore, the lead atoms in this sample cannot fill all the
available space. As an approximation, assume that 60% of the space of the cube
is filled with spherical lead atoms. Calculate the volume of one lead atom from
this information. From the calculated volume (V), and the formula V = 47tr3/3, estimate the radius (r) of a lead atom.
c. Assume the lead atoms along each side of the cube touch one another. How many atoms lie along one edge of the cube?

Chemistry  Arnol, Sunday, November 13, 2011 at 9:02pm
is suppose to be V=4pir^3/3
sry. I get part A. but part B and C are confusing!

Chemistry  DrBob222, Sunday, November 13, 2011 at 9:20pm
a. density = 11.35 g/cc. volume = 1 cm^3. grams = volume x density = ?
Remember there are 6.022E23 atoms in a mole. You have ?g/atomic mass Pb moles Pb atoms.
b. If the volume is 1 cc, then the volume of the atom must be 0.60 if it occupies 60% of the volume. Then volume of 1 Pb atom is
1/# Pb atoms in the 1 cc = xx
I have no idea what 47tr3/3 means to you (nothing to me). You probably meant Volume of a sphere = (4/3)*pi*r^3 and you can use that to calculate the radius.
Post your work if you get stuck.
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