Solid State
Number of atoms per unit cell in B.C.C. is:
The radius of the largest sphere which fits properly at the centre of the edge of body centred cubic unit cell is:(Edge length is represented by '$$a$$')
$$a = 2(R + r)$$
$$\dfrac{a}{2} = (R + r) $$
$$a \sqrt{3} = 4R$$
Using (1) & (2)
$$\dfrac{a}{2} = \dfrac{a \sqrt{3}}{4} +r$$
$$a \left(\dfrac{2 - \sqrt{3}}{4} \right) = r$$
$$r = 0.067 a$$
Number of atoms per unit cell in B.C.C. is:
If a is the edge length, In BCC, the distance between two nearest atoms will be:
CsBr crystallizes in a body-centered cubic lattice. The unit cell length is 436.6 pm. Given that the atomic mass of Cs = 133 and that of Br = 80 amu and Avogadro number being $$6.02\times 10^{23}$$ mol$$^{-1}$$, the density of CsBr is:
An element has a body centered cubic (bcc) structure with a cell edge of $$288 pm$$. The atomic radius is
Body centred cubic lattice has a co-ordination number of:
An example of a body cube is:
The intermetallic compound $$LiAg$$ crystallizes in a cubic lattice in which both $$Li$$ and $$Ag$$ atoms have coordination numbers of $$8$$. To what crystal class does the unit cell belong?
Packing fraction in BCC lattice is
The low density of alkali metals is due to
What is the theoretical density of crystalline $$K$$?