Suppose the mass of a single Ag-atom is $m$. Ag metal crystallises in fcc lattice with unit cell of length $a$. The density of $Ag$ metal in terms of $a$ and $m$ is
- $\frac{4m}{a^{3}}$
- $\frac{2m}{a^{3}}$
- $\frac{m}{a^{3}}$
- $\frac{m}{4a^{3}}$
The Correct Option is A
Solution and Explanation
Mass of single Ag-atom $=m$
Unit cell length $=a$
Total atoms present per unit cell of fcc lattice $=4$
Therefore, mass of unit cell becomes $4 m$.
Volume of unit cell $=a^{3}$
Density( $\rho)=\frac{\text { Mass of unit cell }}{\text { Volume of unit cell }}$
$=\frac{4 m}{a^{3}}$
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Concepts Used:
Unit Cells
The smallest portion of a crystal lattice which repeats in different directions to form the entire lattice is known as Unit cell.
The characteristics of a unit cell are:
- The dimensions are measured along the three edges, a, b and c. These edges can form different angles, they may be mutually perpendicular or may not.
- The angles held by the edges are α (between b and c) β (between a and c) and γ (between a and b).
Therefore, a unit cell is characterised by six parameters such as a, b, c and α, β, γ.
Types of Unit Cell:
Numerous unit cells together make a crystal lattice. Constituent particles like atoms, molecules are also present. Each lattice point is occupied by one such particle.
- Primitive Unit Cells: In a primitive unit cell constituent particles are present only on the corner positions of a unit cell.
- Centred Unit Cells: A centred unit cell contains one or more constituent particles which are present at positions besides the corners.
- Body-Centered Unit Cell: Such a unit cell contains one constituent particle (atom, molecule or ion) at its body-centre as well as its every corners.
- Face Centered Unit Cell: Such a unit cell contains one constituent particle present at the centre of each face, as well as its corners.
- End-Centred Unit Cells: In such a unit cell, one constituent particle is present at the centre of any two opposite faces, as well as its corners.