Step 1: Apply Bragg's law.
\[
2d\sin\theta = n\lambda
\]
For first order (\(n=1\)):
\[
d = \frac{\lambda}{2\sin\theta} = \frac{0.2}{2\sin21^\circ} = \frac{0.2}{0.716} = 0.279\, \text{nm}
\]
Step 2: Relate interplanar spacing to lattice constant.
For cubic crystals:
\[
d_{hkl} = \frac{a}{\sqrt{h^2 + k^2 + l^2}} = \frac{a}{\sqrt{4}}
\]
\[
a = 2d = 2(0.279) = 0.558 \, \text{nm} \approx 0.56\, \text{nm}
\]
Step 3: Conclusion.
Hence, unit cell size \(a = 0.56\, \text{nm}\).
The figure below shows a cubic unit cell with lattice constant \(a\). The shaded crystallographic plane intersects the x-axis at 0.5a. The Miller indices of the shaded plane are: 
Consider the crystal structure shown in the figure, where black and grey spheres represent atoms of two different elements and \(a\) denotes the lattice constant. The Bravais lattice for this structure is: 
Which one of the following crystallographic planes represent \( (101) \) Miller indices of a cubic unit cell? 
The location of Cs$^+$ and Cl$^-$ ions inside the unit cell of CsCl crystal is shown in the figure. The Bravais lattice of CsCl is 