Aluminum (atomic radius = 1.43 Å) crystallizes in a cubic closely packed structure. Calculate the following:
a. The edge length of the face-centered cubic unit cell (in Angstroms).
b. The density of aluminum (in g/cm3).

nope

Explanation:

it's c. elements are placed in rows based on how may valencies electrons have.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.