Advertisements
Advertisements
प्रश्न
Draw diagram of bcc unit cell.
Advertisements
उत्तर
APPEARS IN
संबंधित प्रश्न
In crystal lattice formed by primitive unit cell, the space occupied by particles is ______.
Write the effect on density of a substance in the Frenkel defect?
Name the bravais lattice in the triclinic system.
Which among the following crystal lattices occupies all of the cubic holes by cations?
If a metal crystallises in bcc structure with edge length of unit cell 4.29 × 10-8 cm the radius of metal atom is ______.
Which of the following crystal systems shows base-centred unit cell?
How many unit cells are present in 1.00 cm3 of of aluminum crystal, if edge length of unit cell is 3.54 × 10-8 cm?
What is the mass of unit cell of gold if it crystallises in fee structure?
(At mass of gold= 197 g mol-1)
The edge length of bcc type of unit cell of an element is 400 pm. Calculate the density of unit cell. (Molar mass of an element = 100 g mol-1)
How many lithium atoms are present in a unit cell with edge length 3.5 Å and density 0.53 g cm-3 (At. mass of Li= 6.94).
What is the mass of an fcc unit cell if mass of one atom of an element is 6 × 10-23 g?
What is the number of atoms present per unit cell of aluminium having edge length 4 Å?
Which is the number of atoms in 12.08 × 1023 unit cells if an element crystallizes in bcc structure?
A metallic element crystallizes to bcc type of crystal lattice, having edge length of unit cell 5 A. Calculate radius of its atom.
Bcc type of crystal lattice contains 1.208 × 1023 unit cells. How many atoms of the element are present in these unit cells?
An element crystallizes in fee lattice with cell edge 250 pm. Calculate the density of an element. (At. Mass = 90.3)
Xenon crystallizes in fee lattice and the edge length of unit cell is 620 pm. What is the radius of Xe atom?
The edge length of bcc type of unit cell of metal is 5 Å. What is the radius of metal atom if it's density is 2 glee?
Calculate the number of unit cells in 1 cm³ volume of metal if it forms сср structure
\[\begin{bmatrix} a=3.5\times10^{-8} & cm \end{bmatrix}\]
Calculate the molar mass of an element if it forms fee unit cell structure [mass of unit cell =1.8 × 10-22 g, NA = 6.022 × 1023 mol-1]
