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CUET Chemistry Study Materials The Solid State Notes AMBIPi

Hi CUET aspirants, Welcome to Amans Maths Blogs (AMBIPi). In this post, you will get CUET Chemistry Study Materials The Solid State Notes AMBIPi. This CUET Chemistry Notes are designed by analyzing to the CUET Syllabus and CUET Previous Years Questions Papers.

CUET Chemistry Notes

CUET Chemistry The Solid States: Important Points to Remember

There are following important points in this chapter of The Solid States. 

CUET Chemistry: Types of Solids

Depending on three dimension arrangement:

Amorphous Solids :Amorphous (mean – omorphe – shapeless) solids are with irregular arrangement without any shape and geometry.

Crystalline: Solids with ordered arrangement of molecules with regular three-dimensional arrangement.

Classification of Crystalline Solids:

Depending upon the nature of bonding, the crystalline solids have been classified into four types as given in the table below:

CUET Chemistry: Crystal System

On basis of geometrical consideration, main seven crystal system are present also known as even primitive unit cells, which differ three-dimensionally in axial edge length (a, b and c) and axial angles (α, β, γ).

Crystalline solids have definite shape and volume. They are rigid, incompressible, anisotropic, i.e. their mechanical, electrical properties depend on their direction along which these are measured. Amorphous solids (like plastic,, glass) however, are isotropic.

CUET Chemistry: Number of Particles Per Unit Cell

CUET Chemistry: Radio Ratio Rules for AB Type Structure

CUET Chemistry: Defects or Imperfections in Solids

Stoichiometric Defect: The defects do not disturb the stoichiometry (the ratio of numbers of positive and negative ions) are called stoichiometric defects.

Interstitial defect : This type of defect is caused due to the presence of ions in the normally vacant interstitial sites in the

Schottky Defect : When equal number of cation and anion are missing from its normal site Schottky defect is created.

Frenkel Defect : Found mostly in ionic solids. The ion leaves its position in the lattice and occupies an interstitial void.

Frenkel = Interstitial + Schottky 

CUET Chemistry: Packing Fraction

Bragg’s equation: nλ = 2dsinθ, Where, λ = Wave length of X-rays, n = order of reflection, θ = Angle of reflection, d = Distance between two parallel surfaces.

Interstitial sites in close packing: Trigonal void: r = 0.155 R, r = Radius of the spherical trigonal void, R = Radius of closely packed spheres.

Tetrahedral void: r/R = 0.225, Where, r is the radius of the tetrahedral void or atom occupying tetrahedral void, R is the radius of spheres forming tetrahedral void.

Octahedral: The number of octahedral voids is equal to the number of spheres. r/R = 0.414, Cubic void: r/R = 0.732.

Density of Unit Cell: How closely the atoms are packed in a unit cell is shown by the density of packing. Cubic crystal system follows the order : FCC > BCC > SC 

CUET Chemistry: Magnetic Properties of Solids

Type of crystal defect in which an ion is missing from its lattice site, leaves a hole that is occupied by unpaired electrons.
They are responsible for imparting color to the crystals.

CUET Chemistry Mock Test

Now, you have revised the this CUET Chemistry chapter. So, you must need to practice CUET Chemistry Sample Papers. By solving these CUET Chemistry questions, you will be more confident about your CUET preparations.

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