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Chapter 1 the Solid State Class 12 Chemistry NCERT Solutions

Class 12 Chemistry NCERT Solutions Chapter 1: the Solid State is developed and witten by our expert teachers. Students can study our solutions of Chapter 1: the Solid State class 12 Chemistry, Question 1:Define the term ’amorphous’. Give a few examples of amorphous solids., Question 2. What makes a glass different from a solid such as quartz?, Question 3. Classify each of the following solids as ionic, metallic, molecular, network (covalent) or amorphous., Question 4. (i) What is meant by the term ’coordination number’ ? (ii) What is the coordination number of atoms (a) in a cubic close packed structure? (b) in a body–centered cubic structure? , Question 5. How can you determine the atomic mass of an unknown metal if you know its density?, Question 6. ’Stability of a crystal is reflected in the magnitude of its melting points’. 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?, Question 7. How will you distinguish between the following pairs of terms (i) Hexagonal close packing and cubic close packing (ii) Crystal lattice and unit cell (iii) Tetrahedral void and octahedral void. , Question 8 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, Question 9. Explain (i) The basis of similarities

NCERT Solutions Class 12 Chemistry
Chapter 1: the Solid State
Exercise Answers

=Question 1:Define the term ’amorphous’. Give a few examples of amorphous solids.

Question 1:Define the term ’amorphous’.

=Question 2. What makes a glass different from a solid such as quartz?

Question 2. What makes a glass

=Question 3. Classify each of the following solids as ionic, metallic, molecular, network (covalent) or amorphous.

Question 3. Classify each of the

=Question 4. (i) What is meant by the term ’coordination number’ ? (ii) What is the coordination number of atoms (a) in a cubic close packed structure? (b) in a body–centered cubic structure?

Question 4. (i) What is meant by the

=Question 5. How can you determine the atomic mass of an unknown metal if you know its density?

Question 5. How can you determine the

=Question 6. ’Stability of a crystal is reflected in the magnitude of its melting points’. 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?

Question 6. ’Stability of a crystal is

=Question 7. How will you distinguish between the following pairs of terms (i) Hexagonal close packing and cubic close packing (ii) Crystal lattice and unit cell (iii) Tetrahedral void and octahedral void.

Question 7. How will you distinguish

=Question 8 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

Question 8 How many lattice points are

=Question 9. Explain (i) The basis of similarities and differences between metallic and ionic crystals. (ii) Ionic solids are hard and brittle.

Question 9. Explain (i) The basis of

=Question 10 Calculate the efficiency of packing in case of a metal crystal for (i) simple cubic (ii) body–centred cubic (iii) face–centred cubic (with the assumptions that atoms are touching each other).

Question 10 Calculate the efficiency of

=Question 11 Silver crystallises in fcc lattice. If edge length of the cell is 4.07 × 10-8 cm and density is  0.5 g cm3, calculate the atomic mass of silver.

Question 11 Silver crystallises in fcc

=Question 12 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?

Question 12 A cubic solid is made of

=Question 13 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.

Question 13 Niobium  crystallises in

=Question 14 If the radius of the octahedral void is r and radius of the atoms in closepacking is R, derive relation between r and R.

Question 14 If the radius of the

=Question 15 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.

Question 15 Copper crystallises into a

=Question 16 Analysis shows that nickel oxide has the formula Ni0.98O1.00. What fractions of nickel exist as Ni2+ and Ni3+ ions?

Question 16 Analysis shows that nickel

=Question 17 What is a semiconductor? Describe the two main types of semiconductors and contrast their conduction mechanism.

Question 17 What is a semiconductor?

=Question 18: Non–stoichiometric cuprous oxide, Cu2O can be prepared in laboratory. In this oxide, copper to oxygen ratio is slightly less than 2:1. Can you account for the fact that this substance is a p–type semiconductor?

Question 18: Non–stoichiometric

=Question 19: 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.

Question 19: Ferric oxide crystallises

=Question 20: Classify each of the following as being either a p–type or an n–type semiconductor: (i) Ge doped with In (ii) B doped with Si.

Question 20: Classify each of the

=Question 21: Gold (atomic radius = 0.144 nm) crystallises in a face–centred unit cell. What is the length of a side of the cell?

Question 21: Gold (atomic radius =

=Question 22: In terms of band theory, what is the difference (i) Between a conductor and an insulator (ii) Between a conductor and a semiconductor

Question 22: In terms of band theory,

=Question 23: Explain the following terms with suitable examples: (i) Schottky defect (ii) Frenkel defect (iii) Interstitials and (iv) F–centres

Question 23: Explain the following

=Question 24: 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 aluminum?

Question 24: Aluminium crystallises in

=Question 25: If NaCl is doped with 10−3 mol % of SrCl2, what is the concentration of cation vacancies?

Question 25: If NaCl is doped with

=Question 26: Explain the following with suitable examples: (i) Ferromagnetism (ii)Paramagnetism (iii)Ferrimagnetism (iv)Antiferromagnetism (v)12–16 and 13–15 group compounds.

Question 26: Explain the following with

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