Course Content
CHAPTER 10: HALOALKANES AND HALOARENES
Topic Name 10 Haloalkanes and Haloarenes 10.1 Classification 10.2 Nomenclature 10.3 Nature of C–X Bond 10.4 Methods of Preparation of Haloalkanes 10.5 Preparation of Haloarenes 10.6 Physical Properties 10.7 Chemical Reactions
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CHAPTER 11: ALCOHOLS, PHENOLS AND ETHERS
Topic Name 11 Alcohols, Phenols and Ethers 11.1 Classification 11.2 Nomenclature 11.3 Structures of Functional Groups 11.4 Alcohols and Phenols 11.5 Some Commercially Important Alcohols 11.6 Ethers
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CHAPTER 13: AMINES
Topic Name 13 Amines 13.1 Structure of Amines 13.2 Classification 13.3 Nomenclature 13.4 Preparation of Amines 13.5 Physical Properties 13.6 Chemical Reactions 13.7 Method of Preparation of Diazonium Salts 13.8 Physical Properties 13.9 Chemical Reactions 13.10 Importance of Diazonium Salts in Synthesis of Aromatic Compounds
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CHAPTER 14: BIOMOLECULES
Topic Name 14 Biomolecules 14.1 Carbohydrates 14.2 Proteins 14.3 Enzymes 14.4 Vitamins 14.5 Nucleic Acids 14.6 Hormones
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CHAPTER 15: POLYMERS
Topic Name 15 Polymers 15.1 Classification of Polymers 15.2 Types of Polymerisation Reactions 15.3 Molecular Mass of Polymers 15.4 Biodegradable Polymers 15.5 Polymers of Commercial Importance
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CHAPTER 16: CHEMISTRY IN EVERYDAY LIFE
Topic Name 16 Chemistry in Everyday Life 16.1 Drugs and their Classification 16.2 Drug-Target Interaction 16.3 Therapeutic Action of Different Classes of Drugs 16.4 Chemicals in Food 16.5 Cleansing Agents
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Class 12th Chemistry Online Class For 100% Result
About Lesson

No. Atoms in Unit Cell:-

The Solid State

The Solid State

Number of atoms per unit cell : Body Centered Cubic Unit Cell

In a body-centered cubic (bcc) unit cell, the atoms are present in the body-center besides the ones that are at its corners that wholly belongs to the unit cell in which it is present. Thus in a body-centered cubic (bcc) unit cell:

8 corners X 1/8 per corner atom =   8 * 1/8           = 1 atom

1 body center atom = 1 X 1                              = 1 atom

Total number of atoms per unit cell                   = 2 atoms

Number of atoms per unit cell : Face Centered Cubic Unit Cell

In a face-centered cubic (fcc) unit cell the atoms are present in the corners and at the center of all the faces of the cube.

Each atom present at the face-center is shared between two adjacent unit cells and only a ½ of each atom belongs to a unit cell.

Thus, in a face-centered cubic (fcc) unit cell:

8 corners X 1/8 per corner atom =      8 * 1/8                             = 1 atom

6 face-centered atoms X 1/2 per unit cell = 6 X  1/2                     = 3 atoms

Total number of atoms per unit cell                                             = 4 atoms

In solids, these constituent particles are closely-packed that leaves minimum vacant space.

Numerical on Packing efficiency

The Solid State Notes

Packing Efficiency in hcp and ccp Structures

let the unit cell edge length be ‘a’ and face diagonal AC = b.

The Solid State Notes
The Solid State Notes
The Solid State Notes
The Solid State Notes
The Solid State Notes
The Solid State Notes

Q.Find out the  no. of atoms in BCC (Body Centered Cubic Unit Cell)? [Delhi 2014/2015C]

Q. Find out the no. of atoms in FCC (Face Centered Cubic Unit Cell)? [Delhi 2008/2013/CBSE 2008/2009]

Q. Find out the packing efficiency in simple cubic lattice? [Delhi 2011C/CBSE2011/2009C]

Q. Calculation involving unit cell dimensions? {Relation} [Delhi 2011]

Q. Aluminium crystallises in FCC structure. Atomic radius of metal is 125 pm. what is the lenght of the side of unit cell of the metal? [CBSE 2013]

Ans. length of side (a) = 4r/√2    or [√2a = 4r] for FCC

= (4 x 125 pm)/√2 = 35.3.61 pm

Q. An element with density 11.2 gcm-3 form a fcc lattice with edge length of  4 x 10-8 cm. calculate the atomic mass of elements? [CBSE 2014]

Ans. Given data, d= 11.2 gcm-3 , a = 4 x 10-8 , N= 6.023 x 1023

For FCC, Z = 4

We know the relation,  d = Z M / aN

M = ?  , M = d x ax N/ Z

Put the values and Answer will be  107.9 gmol-1  or 108 gmol-1

NCERT Book Questions

Q 1.18. An element with molar mass 2:7 x 10-2 kg mol-1 forms a cubic unit cell with edge length 405 pm. If its density is 2:7 x 103 kg m-3, what is the nature of the cubic unit cell ? (C.B.S.E. Delhi 2015) (NCERT Book)
Ans: 

The Solid State NCERT Solution Class 12th Chemistry

The Solid State NCERT Solution Class 12th Chemistry

The Solid State NCERT Solution Class 12th Chemistry

The Solid State NCERT Solution Class 12th Chemistry
The Solid State NCERT Solution Class 12th Chemistry
The Solid State NCERT Solution Class 12th Chemistry
The Solid State NCERT Solution Class 12th Chemistry
The Solid State NCERT Solution Class 12th Chemistry

The Solid State NCERT Solution Class 12th Chemistry

The Solid State NCERT Solution Class 12th Chemistry

(i) In metals, conductivity strongly depends upon the number of valence electrons available in an atom. The atomic orbitals of metal atoms form molecular orbitals which are so close in energy to each other, as to form a band. If this band is partially filled or it overlaps with the higher energy unoccupied conduction band, then electrons can flow easily under an applied electric field and the metal behaves as a conductor.

If the gap between valence band and next higher unoccupied conduction band is large, electrons cannot jump into it and such a substance behaves as insulator.

(ii) If the gap between the valence band and conduction band is small, some electrons may jump from valence band to the conduction band. Such a substance shows some conductivity and it behaves as a semiconductor. Electrical conductivity of semiconductors increases with increase in temperature, since more electrons can jump to the conduction band. Silicon and germanium show this type of behaviour and are called intrinsic semiconductors. Conductors have no forbidden band.

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