Aluminium crystallizes in a cubic closed pack structure. Its metallic radius is 125pm. Calculate the edge length of unit cell.
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It is given that aluminum crystallises in a cubic closed packed structure.
Its metallic radius is 125 pm.
(i) For cubic close-packed structure
a=2√2r
r=2 √2×125=354 pm
Here, a is the edge length of the unit cell and r is the atomic radius.
Explanation:
It is @Suyash01
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Solution : For a, c.c.p length of the side of unit cell is related to radius `r=(sqrt(2)a)/(4)` <br> `a=(4r)/(sqrt(2))=(4xx125)/(1.414)=353.5` pm <br> `therefore` Volume of unit cell `= a^(3)=(353.3xx10^(-10))^(3)cm^(3)=4.42xx10^(-23)cm^(3)` <br> Number of unit cells in `1cm^(3)=(1)/(4.42xx10^(-23))=2.26xx10^(22)` unit .
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