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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? 

Option: 1

9.03\times 10^{23},6.022\times 10^{23}

Option: 2

8.26\times 10^{23},6.022\times 10^{23}

Option: 3

9.03\times 10^{23},6.022\times 10^{22}

Option: 4

9.03\times 10^{23},5.34\times 10^{23}

Answers (1)


Given, the number of atoms in close packaging = 0.5 moles

\therefore Number of close-packed particles =0.5\times6.022\times10^{23}=3.011\times10^{23}

Now, we know the ?number of tetrahedral voids 

= 2 X number of atoms in close-packed structures.

Therefore, the number of tetrahedral voids =2\times 0.311\times10^{23}    


Again, the number of octahedral voids = number of atoms in close packaging

Thus, the number of octahedral voids = 3.011\times10^{23}

Now, the Total number of voids

= Tetrahedral voids + octahedral voids
                                        =6.022\times10^{23}+3.011\times10^{23} =9.03\times10^{23}

Therefore, Option(1) is correct 

Posted by

Suraj Bhandari

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