NCERT solutions for Chemistry Class 12 chapter 1 - The Solid State [Latest edition]

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Solutions for Chapter 1: The Solid State

Below listed, you can find solutions for Chapter 1 of CBSE, Karnataka Board PUC NCERT for Chemistry Class 12.


Intext QuestionsExercises
Intext Questions [Pages 4 - 29]

NCERT solutions for Chemistry Class 12 Chapter 1 The Solid State Intext Questions [Pages 4 - 29]

Intext Questions | Q 1 | Page 4

Why are solids rigid?

Intext Questions | Q 2 | Page 4

Why do solids have a definite volume?

Intext Questions | Q 3 | Page 4

Classify the following as amorphous or crystalline solids:

Polyurethane, naphthalene, benzoic acid, teflon, potassium nitrate, cellophane, polyvinyl chloride, fibre glass, copper.

Intext Questions | Q 4 | Page 4

Why is glass considered a super cooled liquid?

Intext Questions | Q 5 | Page 4

Refractive index of a solid is observed to have the same value along all directions. Comment on the nature of this solid. Would it show cleavage property?

Intext Questions | Q 6 | Page 6

Classify the following solids in different categories based on the nature of intermolecular forces operating in them:

Potassium sulphate, tin, benzene, urea, ammonia, water, zinc sulphide, graphite, rubidium, argon, silicon carbide.

Intext Questions | Q 7 | Page 6

Solid A is a very hard electrical insulator in solid as well as in molten state and melts at extremely high temperature. What type of solid is it?

Intext Questions | Q 8 | Page 6

Ionic solids conduct electricity in molten state but not in solid state. Explain

Intext Questions | Q 10 | Page 12

Give the significance of a ‘lattice point’.

Intext Questions | Q 14 | Page 21

What is the two dimensional coordination number of a molecule in square close packed layer?

Intext Questions | Q 15 | Page 21

A compound forms hexagonal close-packed structure. What is the total number of voids in 0.5 mol of it? How many of these are tetrahedral voids?

Intext Questions | Q 17 | Page 22

Which of the following lattices has the highest packing efficiency (i) simple cubic (ii) body-centred cubic and (iii) hexagonal close-packed lattice?

Intext Questions | Q 18 | Page 22

An element with molar mass 2.7 × 10-2 kg mol-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7 × 103 kg m−3, what is the nature of the cubic unit cell?

Intext Questions | Q 19 | Page 29

What type of defect can arise when a solid is heated? Which physical property is affected by it and in what way?

Intext Questions | Q 20 | Page 29

What type of stoichiometric defect is shown by:

(i) ZnS 

(ii) AgBr

Intext Questions | Q 21 | Page 29

Explain how vacancies are introduced in an ionic solid when a cation of higher valence is added as an impurity in it.

Intext Questions | Q 23 | Page 29

A group 14 element is to be converted into n-type semiconductor by doping it with a suitable impurity. To which group should this impurity belong?

Intext Questions | Q 24 | Page 29

What type of substances would make better permanent magnets, ferromagnetic or ferrimagnetic. Justify your answer.

Exercises [Pages 30 - 32]

NCERT solutions for Chemistry Class 12 Chapter 1 The Solid State Exercises [Pages 30 - 32]

Exercises | Q 1 | Page 30

Define the term 'amorphous'. Give a few examples of amorphous solids.

Exercises | Q 2 | Page 30

What makes a glass different from a solid such as quartz? Under what conditions could quartz be converted into glass?

Exercises | Q 3 | Page 30

Classify each of the following solids as ionic, metallic, molecular, network (covalent) or amorphous.

(i) Tetra phosphorus decoxide (P4O10

(ii) Ammonium phosphate (NH4)3PO4 

(iii) SiC 

(iv) I2 

(v) P4 

(vii) Graphite

(viii) Brass

(ix) Rb

(x) LiBr

(xi) Si

 

Exercises | Q 4.1 | Page 30

What is meant by the term 'coordination number'?

Exercises | Q 4.2 | Page 30

What is the coordination number of atoms:

(a) in a cubic close-packed structure?

(b) in a body-centred cubic structure?

Exercises | Q 5 | Page 30

How can you determine the atomic mass of an unknown metal if you know its density and the dimension of its unit cell? Explain.

Exercises | Q 6 | Page 30

'Stability of a crystal is reflected in the magnitude of its melting point'. Comment. Collect melting points of solid water, ethyl alcohol, diethyl ether and methane from a data book. What can you say about the intermolecular forces between these molecules?

Exercises | Q 8 | Page 31

How many lattice points are there in one unit cell of each of the following lattice?

(i) Face-centred cubic

(ii) Face-centred tetragonal

(iii) Body-centred

Exercises | Q 9.1 | Page 31

Explain The basis of similarities and differences between metallic and ionic crystals.

Exercises | Q 9.2 | Page 31

Explain Ionic solids are hard and brittle.

Exercises | Q 10.1 | Page 31

Calculate the efficiency of packing in case of a metal crystal for simple cubic

Exercises | Q 10.2 | Page 31

Calculate the efficiency of packing in case of a metal crystal for body-centred cubic

Exercises | Q 10.3 | Page 31

Calculate the efficiency of packing in case of a metal crystal for face-centred cubic (with the assumptions that atoms are touching each other).

Exercises | Q 11 | Page 31

Silver crystallises in fcc lattice. If edge length of the cell is 4.07 × 10−8 cm and density is 10.5 g cm−3, calculate the atomic mass of silver

Exercises | Q 12 | Page 31

A cubic solid is made of two elements P and Q. Atoms of Q are at the corners of the cube and P at the body-centre. What is the formula of the compound? What are the coordination numbers of P and Q?

Exercises | Q 13 | Page 31

Niobium crystallises in body-centred cubic structure. If density is 8.55 g cm−3, calculate atomic radius of niobium using its atomic mass 93 u.

Exercises | Q 14 | Page 31

If the radius of the octachedral void is r and radius of the atoms in close packing is R, derive relation between r and R.

Exercises | Q 15 | Page 31

Copper crystallises into a fcc lattice with edge length 3.61 × 10−8 cm. Show that the calculated density is in agreement with its measured value of 8.92 g cm−3.

Exercises | Q 16 | Page 31

Analysis shows that nickel oxide has the formula Ni0.98O1.00. What fractions of nickel exist as Ni2+ and Ni3+ ions?

Exercises | Q 17.1 | Page 31

What is a semiconductor

Exercises | Q 17.2 | Page 31

Describe the two main types of semiconductors and contrast their conduction mechanism.

Exercises | Q 19 | Page 31

Ferric oxide crystallises in a hexagonal close-packed array of oxide ions with two out of every three octahedral holes occupied by ferric ions. Derive the formula of the ferric oxide.

Exercises | Q 20.1 | Page 31

Classify the following as being either a p-type or an n-type semiconductor:

Ge doped with In

Exercises | Q 20.2 | Page 31

Classify the following as being either a p-type or an n-type semiconductor:

B doped with Si.

Exercises | Q 21 | Page 32

Gold (atomic radius = 0.144 nm) crystallises in a face-centred unit cell. What is the length of a side of the cell?

Exercises | Q 22.1 | Page 32

In terms of band theory, what is the difference Between a conductor and an insulator

Exercises | Q 22.2 | Page 32

In terms of band theory, what is the difference Between a conductor and a semiconductor

Exercises | Q 23.1 | Page 32

Define the following term

Schottky defect

Exercises | Q 23.2 | Page 32

Explain the following terms with suitable examples: Frenkel defect

Exercises | Q 23.3 | Page 32

Explain the following terms with suitable examples : Interstitials

Exercises | Q 23.4 | Page 32

Explain the following terms with suitable examples: F-centres

Exercises | Q 24 | Page 32

Aluminium crystallises in a cubic close-packed structure. Its metallic radius is 125 pm.

(i) What is the length of the side of the unit cell?

(ii) How many unit cells are there in 1.00 cm3 of aluminium?

Exercises | Q 25 | Page 32

If NaCl is doped with 10−3 mol % of SrCl2, what is the concentration of cation vacancies?

Exercises | Q 26.1 | Page 32

What is ferromagnetism?

Exercises | Q 26.2 | Page 32

Explain the following with suitable examples: Paramagnetism

Exercises | Q 26.3 | Page 32

Explain the following with suitable examples: Ferrimagnetism

Exercises | Q 26.4 | Page 32

Explain the following with suitable examples: Antiferromagnetism

Exercises | Q 26.5 | Page 32

Explain the following with suitable examples:

12-16 and 13-15 group compounds.

Solutions for Chapter 1: The Solid State

Intext QuestionsExercises

NCERT solutions for Chemistry Class 12 chapter 1 - The Solid State

Shaalaa.com has the CBSE, Karnataka Board PUC Mathematics Chemistry Class 12 CBSE, Karnataka Board PUC solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. NCERT solutions for Mathematics Chemistry Class 12 CBSE, Karnataka Board PUC 1 (The Solid State) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.

Further, we at Shaalaa.com provide such solutions so students can prepare for written exams. NCERT textbook solutions can be a core help for self-study and provide excellent self-help guidance for students.

Concepts covered in Chemistry Class 12 chapter 1 The Solid State are Classification of Crystalline Solids, Amorphous and Crystalline Solids, Crystal Lattices and Unit Cells, Calculations Involving Unit Cell Dimensions, Close Packed Structures of Solids, Efficiency of Packing in Body-centred Cubic Structures, Close Packed Structures - Formula of a Compound and Number of Voids Filled, Number of Atoms in a Unit Cell, Imperfections in Solids - Introduction, Magnetic Properties, Band Theory of Metals, Electrical Properties - Introduction, Applications of n-type and p-type Semiconductors, General Characteristics of Solid State, Crystal Lattices and Unit Cells - Primitive and Centred Unit Cells, Packing Efficiency in hcp and ccp Structures, Packing Efficiency in Simple Cubic Lattice, Types of Point Defects - Stoichiometric Defects, Types of Point Defects - Impurity Defects, Types of Point Defects - Non-stoichiometric Defects, Conduction of Electricity in Metals, Conduction of Electricity in Semiconductors, Solid State Numericals.

Using NCERT Chemistry Class 12 solutions The Solid State exercise by students is an easy way to prepare for the exams, as they involve solutions arranged chapter-wise and also page-wise. The questions involved in NCERT Solutions are essential questions that can be asked in the final exam. Maximum CBSE, Karnataka Board PUC Chemistry Class 12 students prefer NCERT Textbook Solutions to score more in exams.

Get the free view of Chapter 1, The Solid State Chemistry Class 12 additional questions for Mathematics Chemistry Class 12 CBSE, Karnataka Board PUC, and you can use Shaalaa.com to keep it handy for your exam preparation.

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