Zinc sulfide, ZnS, exists in two main crystal forms. The more stable form, zinc blende, is...

Zinc sulfide, ZnS, exists in two main crystal forms. The more stable form, zinc blende, is face-centered cubic with tetrahedral coordination geometry and has density of 4.09 g/cm³. Use 184 pm for the ionic radius of S^2- to calculate the ionic radius of Zn²⁺.

Expert Solution

We know that density , d = (Z x atomic mass) / ( N_o x a³ x 10^-30 cm³ )

Where Z = No . of atoms in a unit cell = 4 Since it is a fcc structure

atomic mass of Zn = 65.4 g

N_o = avagadro number = 6.023x10²³

a = edge length = in pm

d = density = 4.09 g/cm³

Plug the values we get a³ = (Z x atomic mass) / ( N_o x d x 10^-30 cm³ )

= (4 x 65.4) / ( 6.023x10²³ x 4.09 x 10^-30 cm³ )

= 106.2 x10⁶

a = (106.2 x10⁶ )^1/3

= 473.5 pm

For fcc arrangement radius , r = (?2 / 4 ) a

= (?2 / 4 )x473.5

= 167.4 pm

queen_honey_blossom answered 1 hour ago

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Zinc sulfide, ZnS, exists in two main crystal forms. The more stable form, zinc blende, is...

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