Imperfections or Defects in a Solid

When we talk about the structure of a solid, especially a crystalline solid, we talk about the uniformity of their structure and arrangement of atoms. However, there are certain defects in this structure, that give solids certain characteristic features. Here we will learn particularly about point defects.

Suggested Videos

 

Defects in a Solid

When we talk about crystalline solids, we say they have a definite structure. They have long term arrangement of their molecules. This means that they have repeated arrangement of a unit cell to form a space lattice structure. So the arrangement of molecules, in the long run, will remain the same.

However, these crystals are not perfect. They have defects or imperfections in their arrangement of constituent particles. These defects are a deviation from their uniform arrangement of particles. The defects are of two kinds

• Point Defects: When the deviation occurs around an atom/particle it is a point defect. It could be due to displacement, an extra particle or a missing particle.
• Line Defects: When there is an abnormality in the arrangement of an entire row, then it is a line defect.

Point Defects

Our main focus today will be to learn about point defects. Point defects usually occur when the crystallization has occurred very rapidly, not allowing a perfect crystal arrangement to form. Although it should be noted there are imperfections in even during a slow crystallization. There are mainly three different kinds of point defects. Let us study each of them.

Browse more Topics under The Solid State

• General Introduction
• Crystalline and Amorphous Solids
• Space Lattice or Crystal Lattice and Unit Cell
• Number of Particles in Unit Cells
• Close Packing in Crystals
• Tetrahedral and Octahedral Voids
• Radius Ratio Rules
• Density of a Cubic Crystal
• Electrical Properties of Solids
• Magnetic Properties of Solids

Stoichiometric Defects

Stoichiometric compounds are those who maintain their stoichiometry. That means they maintain their ratios of cations and anions as indicated by their chemical formula. The defects in the solid do not affect this ratio. They are of various kinds, such as

Vacancy Defect

Here the lattice site is simply vacant, which means there is a missing particle. In a perfect crystal, there would not be this vacancy. This defect will lead to a reduced density of the solid. Some surrounding particle may move to fill in the gap, but the vacancy will only shift in the opposite direction, Also the solid structure of the crystal will ensure that the particles surrounding the vacant spot do not collapse.

Interstitial Defect

There is an unoccupied space at the very center of the cube structure of the solid. When the eight spheres of a unit cell meet at the center they leave a little space, the interstitial site. Sometimes another particle will occupy this space. This is what we call an interstitial defect.

These are extra atoms or molecules or ions that occupy space which was supposed to be empty, which is why it is a defect. The density of the solid also increases due to such defects.

Schottky Defects

In this defect, more than one particle is missing. But the number of cations missing is equal to the number of anions missing. So the electrical composition remains the same.

Since more than one particle is missing, the mass of the structure will decrease. But since the volume remains the same, the density of the solid will also decrease. If there are too many particles missing, then the lattice structure may be compromised. this could mean the stability of the structure may suffer. An example of this defect is NaCl, KCl, and other such ionic compounds.

Frenkel Defects

When a cation is missing from its normal position and has instead occupied an interstitial site it is a Frenkel Defect. Here the electrical neutrality will be unaffected. Also, it is usually cations that cause this defect since they can easily fit in the interstitial site due to their small and compact size.

Here no particles are actually missing, only the position is wrong. So the density of the solid will not change. It usually occurs in compounds where there is a significant size difference between cations and anions. Some examples are AgCl, AgBr etc.

Non-Stoichiometric Defects

These defects will change the ration of ions in the solid. The number of cations and anions will not reflect as stated in their chemical formula. This imperfection is generally found in a large number of inorganic compounds. There are mainly two types of non-stoichiometry defects. Let us take a look.

Metal Excess Defects

Here there is a surplus of metal ions in the space lattice. This can happen in one of two ways;

• Anionic Vacancy: Sometimes an anion may be missing from its usual position in the unit cell. This empty space will be occupied by an electron to maintain the electric neutrality of the solid. This space that the electron invades, is known as the F-center. This F-center electron is what gives the compound a color, One common example is NaCl and the yellow color it obtains on being heated.
• Extra Cations: On being heated many compounds result in having extra cations. These cations fit into the interstitial sites. To balance the neutrality an equal number of electrons do the same. But the ultimate result is the excess of metal in the solid. An example of this is when Zinc Oxide is heated and it losses oxygen,

Metal Deficiency Defects

In such compounds, there is less metal than its ideal stoichiometric proportions. Sometimes a positive ion is missing from the lattice site, but the neutrality of the solid will remain same as a neighbouring ion will take up two charges. The metal deficiency defect is normally found in Transition Elements, that have the ability to have multiple valencies.

Solved Question for You

Q: Which defect in any crystal lowers its density?

1. Schottky
2. Interstitial
3. F-center
4. Frenkel

Ans: The correct answer is “A”. In Schottky defect, the same number of cations and anions are missing from the lattice. Hence this defect will decrease the density.