The density of Nickel that crystallizes in FCC lattice structure has to be calculated. Concept Introduction: In crystalline solids , the components are packed in regular pattern and neatly stacked. The components are imagined as spheres and closely packed. This phenomenon is called “close packing” in crystals. The two major types of close packing of the spheres in the crystal are – hexagonal close packing and cubic close packing. Cubic close packing structure has face-centered cubic (FCC) unit cell. In face-centered cubic unit cell, each of the six corners is occupied by every single atom. Each face of the cube is occupied by one atom. Each atom in the corner is shared by eight unit cells and each atom in the face is shared by two unit cells. Thus the number of atoms per unit cell in FCC unit cell is, 8 × 1 8 atoms in corners + 6 × 1 2 atoms in faces = 1 + 3 = 4 atoms

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Chapter 12.3, Problem 12.3.1SR

Interpretation Introduction

Interpretation:

The density of Nickel that crystallizes in FCC lattice structure has to be calculated.

Concept Introduction:

In crystalline solids, the components are packed in regular pattern and neatly stacked. The components are imagined as spheres and closely packed. This phenomenon is called “close packing” in crystals. The two major types of close packing of the spheres in the crystal are – hexagonal close packing and cubic close packing. Cubic close packing structure has face-centered cubic (FCC) unit cell.

In face-centered cubic unit cell, each of the six corners is occupied by every single atom. Each face of the cube is occupied by one atom. Each atom in the corner is shared by eight unit cells and each atom in the face is shared by two unit cells. Thus the number of atoms per unit cell in FCC unit cell is,

8 × 18 atoms in corners + 6 × 12 atoms in faces = 1 + 3 = 4 atoms

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