Q 1.15: A
compound forms hexagonal close−packed structure.
What is the total number of voids in 0.5 mol of it? How many of these are
tetrahedral voids?
Solution:
Number of atoms in close packaging = 0.5 mol
1 has 6.022 ×10 23 particles
So that
Number of close−packed particles
= 0.5 × 6.022 × 1023 = 3.011 × 1023
Number of tetrahedral voids = 2 × number of atoms in close
packaging
Plug the values we get
Number of tetrahedral voids = 2 × 3.011 × 1023
= 6.022 × 1023
Number of octahedral
voids = number of atoms in close packaging
So that
Number of octahedral voids = 3.011 × 1023
Total number of voids = Tetrahedral void + octahedral void
= 6.022
× 1023 + 3.011 × 1023
= 9.03 × 1023
why is the voids in a hcp structure not called 'hexagonal' void rather than octahedral void?because its little confusing.please help
ReplyDeleteits called octahedral due to the shape of the void.
Deletethe void is similar to a octagon
It is called octahedral because around the void the arrangement of atom is octahedral. Shape of the void is not octahedral
DeleteIn the above question they mentioned a compound so u cannot tell how many atoms are there. Then how can I assume it to be 6.023*10^23
ReplyDeleteI think each particle in above question is considered as an atom.so it can be assumed to be 6.022×10^23.
ReplyDeleteHow many of these are tetrahedral voids???
Delete6.032*10^230
DeleteQu ye duniya he..... Muze pats Nani and eska ans. de ke bata
ReplyDelete