NCERT Exemplar Class 12 Chemistry solutions Chapter 1 deals with the solid-state of matter with a detailed insight on its properties, study of its constituent particles, and the binding forces among such particles holding the shape. This NCERT lesson is a straightforward lesson which gives a brief description of solids and reflects upon various different factors responsible for the existence of such shapes. NCERT Exemplar Class 12 Chemistry Chapter 1 solutions also introduces various different terms that help solids to contain their shape such as intermolecular distance, intermolecular force, different constituent particles, etc. that further help in understanding the properties of solid-state. Class 12 Chemistry NCERT exemplar solutions Chapter 1 includes all the factors that are responsible for the solids to exist and help in distinguishing solids from liquid and gases at a molecular level.
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NCERT exemplar class 12 Chemistry solutions chapter 1: MCQ (Type 1)
Which of the following conditions favours the existence of a substance in the solid state?
(i) High temperature
(ii) Low temperature
(iii) High thermal energy
(iv) Weak cohesive forces
The answer is the option (ii) At low temperature, substance exists in solid state due to low thermal energy and hence decreased molecular motion, which in turn leads to strong intermolecular cohesive i.e., forces, which hold the constituent particles together. Hence, option b is correct.
Which of the following is not a characteristic of a crystalline solid?
(i) Definite and characteristic heat of fusion.
(ii) Isotropic nature.
(iii) A regular periodically repeated pattern of arrangement of constituent particles in the entire crystal.
(iv) A true solid
The answer is the option (ii) Anisotropy: Crystalline solids are anisotropic in nature. In Anisotropic substances, physical properties like electrical resistance or refractive index show different values when measured along different directions in the same crystal. This is primarily due to different arrangement of particles in different directions arrangement of particles along different directions
Isotropy: In isotropic substances, physical properties like electrical conductivity, refractive index etc. show the same value when measured in different directions just like in glass or liquid. Amorphous substances exhibit Isotropy.
Which of the following is an amorphous solid?
(i) Graphite (C)
(ii) Quartz glass
(iii) Chrome alum
(iv) Silicon carbide (SiC)
The answer is the option (ii)
Crystalline Silica (Quartz)
Amorphous silica (Glass)
They are crystalline in nature.
Light white powder appearance
All the 4 corners of silica tetrahedron are shared by others to give a solid network.
The silica tetrahedron are randomly joined giving rise to polymeric chains, sheets or 3-Dimensional units.
It has high melting point
It does not have any sharp melting point and softens gradually to liquid on heating.
Which of the following statement is not true about amorphous solids?
(i) On heating, they may become crystalline at a certain temperature.
(ii) They may become crystalline on keeping for a long time.
(iii) Amorphous solids can be moulded by heating.
(iv) They are anisotropic in nature.
The answer is the option (iv) Amorphous solids are isotropic because they show physical, thermal and optical properties that are identical in all directions.
The sharp melting point of crystalline solids is due to ___________.
(i) a regular arrangement of constituent particles observed over a short distance in the crystal lattice.
(ii) a regular arrangement of constituent particles observed over a long distance in the crystal lattice.
(iii) same arrangement of constituent particles in different directions.
(iv) different arrangement of constituent particles in different directions.
The answer is the option (ii) A solid is said to be crystalline whose constituents such as atoms, molecules or ions are arranged in highly ordered microscopic structure.
Crystalline solids have sharp melting point is due to this regular arrangement of constituent particles over a long distance in crystal lattice.
Iodine molecules are held in the crystals lattice by ____________.
(i) London forces
(ii) Dipole-dipole interactions
(iii) Covalent bonds
(iv) Coulombic forces
The answer is the option (i) is a molecular solid. Molecular solids are held together by the Dispersion or London forces and have very low melting point. Some other examples are
Which of the following is a network solid?
The answer is the option (iii) Diamond has a 3 dimensional tetrahedral arrangement of carbon atoms. Every carbon atom is bonded to 4 other carbon atoms.
Which of the following solids is not an electrical conductor?
(A) Mg (s) (B) TiO (s) (C) (s) (D) (s)
(i) (A) only
(ii) (B) Only
(iii) (C) and (D)
(iv) (B), (C) and (D)
The answer is the option (iii) (C) and (D)
In molecules are soft and non-conductor of electricity.
Hydrogen is covalently bonded to more electronegative oxygen atom in water. Due to non-ionic nature, they do not dissociate in ions and cannot conduct electricity.
Which of the following is not the characteristic of ionic solids?
(i) A very low value of electrical conductivity in the molten state.
(ii) Brittle nature.
(iii) Very strong forces of interactions.
(iv) Anisotropic nature.
The answer is the option (i) A very low value of electrical conductivity in the molten state. Ionic solids are hard but brittle in appearance. They have high melting point and act as insulators in solid state but conductors in molten state or aqueous solutions. They have very strong forces of attraction. Hence, option A is incorrect.
Graphite is a good conductor of electricity due to the presence of __________.
(i) lone pair of electrons
(ii) free valence electrons
The answer is the option (ii) Every carbon atom is bonded to 3 other carbon atoms in graphite by covalent bonds. One valence electron of each carbon atom is free. Graphite is a good conductor of electricity due to the presence of this free electron.
The lattice site in a pure crystal cannot be occupied by _________.
The answer is the option (iii) electron
Pure crystals have constituents i.e., atoms, molecules, or ions arranged in a highly ordered microscopic structure in fixed stoichiometric ratio. Lattice sites can be occupied by electron only when there is imperfection in solid. They do not occur in pure crystals. Hence, the lattice site in a pure crystal cannot be occupied by electron. It is feasible only in case of imperfection giving rise to Crystal defects.
Graphite cannot be classified as __________.
(i) conducting solid
(ii) network solid
(iii) covalent solid
(iv) ionic solid
The answer is the option (iv) Graphite has a covalent structure wherein each C atom is bonded to the 3 remaining Carbon atoms by covalent bonds. Despite being a covalent solid, its electrical conductivity is very high.
Cations are present in the interstitial sites in __________.
(i) Frenkel defect
(ii) Schottky defect
(iii) Vacancy defect
(iv) Metal deficiency defect
The answer is the option (i) Frenkel defect
Frenkel effect is when a cation is missing from the normal lattice position and is occupying interstitial site. It generally occurs in Ionic solids where the anion is larger than the cation.
Schottky defect is observed in crystals when __________.
(i) some cations move from their lattice site to interstitial sites.
(ii) the equal number of cations and anions are missing from the lattice.
(iii) some lattice sites are occupied by electrons.
(iv) some impurity is present in the lattice.
The answer is the option (ii) the equal number of cations and anions are missing from the lattice.
Schottky defect is when a crystal has equal number of cations and anions missing from their normal lattice site by creating vacancies or holes. In this case, the electrical neutrality is maintained.
Which of the following point defects are shown by AgBr(s) crystals?
(A) Schottky defect
(B) Frenkel defect
(C) Metal excess defect
(D) Metal deficiency defect
(i) (A) and (B)
(ii) (C) and (D)
(iii) (A) and (C)
(iv) (B) and (D)
The answer is the option (i).
Silver bromide shows Schottky as well as Frenkel defects. In AgBr, both the silver cation and bromide ion are absent from the lattice causing Schottky defect. But the silver ions are smaller in size and mobile, so they have a tendency to occupy interstitial sites when removed from lattice point. Hence cause Frenkel defect. ‘
In which pair most efficient packing is present?
(i) hcp and bcc
(ii) hcp and ccp
(iii) bcc and ccp
(iv) bcc and simple cubic cell
The answer is the option (ii)
Packing efficiency is defined as the percentage of space occupied by constituent particles in a unit cell.
Packing efficiency of various types of unit cell are:
simple cubic cell - 52.4% .
body centred cubic cell- 68
cubic closed packing- 74%
Which of the following statement is not true about the hexagonal close packing?
(i) The coordination number is 12.
(ii) It has 74% packing efficiency.
(iii) Tetrahedral voids of the second layer are covered by the spheres of the third layer.
(iv) In this arrangement spheres of the fourth layer are exactly aligned with those of the first layer.
The answer is the option (iv).
Hexagonal packing has layers arranged in ABAB pattern. The spheres of first layer are aligned with the third layer and not the fourth layer.
The 1st layer and 4th layer are not exactly aligned. Thus, statement (d) is not correct while other statements (a), (b) and (c) are true.
Which kind of defects are introduced by doping?
(i) Dislocation defect
(ii) Schottky defect
(iii) Frenkel defects
(iv) Electronic defects
The answer is the option (iv).
Doping introduces electronic defect. Electronic defect occurs due to the addition of electron rich or electron deficient impurity to a perfect crystal. There are 2 types of dopants- n-type and p-type.
Silicon doped with electron-rich impurity forms ________.
(i) p-type semiconductor
(ii) n-type semiconductor
(iii) intrinsic semiconductor
The answer is the option (ii) Silicon has four valence electrons. The conductivity increases on doping with an electron rich impurity as the extra electron becomes delocalised. The increase in conductivity is due to negatively charged electron. That is why silicon doped with electron-rich impurity is called n-type semiconductor.
Which of the following statements is not true?
(i) Paramagnetic substances are weakly attracted by the magnetic field.
(ii) Ferromagnetic substances cannot be magnetised permanently.
(iii) The domains in antiferromagnetic substances are oppositely oriented with respect to each other.
(iv) The pairing of electrons cancels their magnetic moment in the diamagnetic substances.
The answer is the option (ii).
Ferromagnetic materials such as iron are strongly attracted in the magnetic field and can be permanently magnetised. Hence, choice (ii) is not true while other three choices are correct.
Which of the following is not true about the ionic solids?
(i) Bigger ions form the close-packed structure.
(ii) Smaller ions occupy either the tetrahedral or the octahedral voids depending upon their size.
(iii) Occupation of all the voids is not necessary.
(iv) The fraction of octahedral or tetrahedral voids occupied depends upon the radii of the ions occupying the voids.
The answer is the option (iv) The fraction of Octahedral or tetrahedral voids is dependent on the radii of the ions occupying the voids. Hence, option (iv) is not true about ionic solids.
A ferromagnetic substance becomes a permanent magnet when it is placed in a magnetic field because ________.
(i) all the domains get oriented in the direction of the magnetic field.
(ii) all the domains get oriented in the direction opposite to the direction of the magnetic field.
(iii) domains get oriented randomly.
(iv) domains are not affected by the magnetic field.
The answer is the option (i).
Ferromagnetic substance becomes a permanent magnet when placed in a magnetic field as the domains get aligned in the direction of applied external magnetic field.
Which of the following defects is also known as dislocation defect?
(i) Frenkel defect
(ii) Schottky defect
(iii) Non-stoichiometric defect
(iv) Simple interstitial defect
The answer is the option (i).
In Frenkel defect, some cations create a vacancy and occupy interstitial site. That is why it is also called dislocation defect.
In the cubic close packing, the unit cell has ________.
(i) 4 tetrahedral voids each of which is shared by four adjacent unit cells.
(ii) 4 tetrahedral voids within the unit cell.
(iii) 8 tetrahedral voids each of them which are shared by four adjacent unit cells.
(iv) 8 tetrahedral voids within the unit cells.
The answer is the option (iv) In the cubic close packing the unit cell has 8 tetrahedral voids within the unit cells.
Which of the following represents correct order of conductivity in solids?
(i) κ metals >> κ insulators< κsemiconductors
(ii) κ metals << κ insulators < κsemiconductors
(iii) κ metals κsemiconductors> κ insulators = zero
(iv) κ metals < κsemiconductors >κ insulators ≠ zero
The answer is the option (i).
The relative values of conductivity of solid is represented in terms of k. The value for k for metals >> semiconductor>> Insulator
NCERT exemplar class 12 Chemistry solutions chapter 1: MCQ (Type 2)
Which of the following is not true about the voids formed in 3-dimensional hexagonal close-packed structure?
(i) A tetrahedral void is formed when a sphere of the second layer is present above triangular void in the first layer.
(ii) All the triangular voids are not covered by the spheres of the second layer.
(iii) Tetrahedral voids are formed when the triangular voids in the second layer lie above the triangular voids in the first layer and the triangular shapes of these voids do not overlap.
(iv) Octahedral voids are formed when the triangular voids in the second layer exactly overlap with similar voids in the first layer
The answer is the option (iii, iv) Tetrahedral voids are formed when the triangular void in the second layer lie exactly above the triangular voids in the first layer and the triangular shape of these voids oppositely overlap.
Octahedral voids are formed when triangular void of second layer is not exactly overlapping with similar void in first layer.
The value of the magnetic moment is zero in the case of antiferromagnetic substances because the domains ________.
(i) get oriented in the direction of the applied magnetic field.
(ii) get oriented opposite to the direction of the applied magnetic field.
(iii) are oppositely oriented with respect to each other without the application of the magnetic field.
(iv) cancel out each other’s magnetic moment.
The answer is the option (iii, iv) In the case of antiferromagnetic substances like manganese oxide, the magnetic moment becomes zero because the magnetic moments of atoms align in a pattern with neighbouring spins pointing in opposite directions which cancel out each other resulting in 0 net dipole moment.
Which of the following statements are not true?
(i) Vacancy defect results in a decrease in the density of the substance.
(ii) Interstitial defects increase the density of the substance.
(iii) Impurity defect does not affect the density of the substance.
(iv) Frankel defect results in an increase in the density of the substance.
The answer is the option (iii, iv)
Impurity defect involves the replacement of ions by an impurity which may have a different density than the ion present on perfect crystal. Frenkel defect results in neither decrease nor increase in density of substance as it involves only the migration of ions within the crystal.
Which of the following statements are true about metals?
(i) Valence band overlaps with conduction band.
(ii) The gap between the valence band and the conduction band is negligible.
(iii) The gap between the valence band and the conduction band cannot be determined.
(iv) Valence band may remain partially filled.
The answer is the option (i, ii, iv) The electrical conduction through metals is dependent on the type of valence band and its gap with the conduction band. This gap determines the conducting property of metal.
Which of the following statements are true about semiconductors?
(i) Silicon doped with an electron-rich impurity is a p-type semiconductor.
(ii) Silicon doped with an electron-rich impurity is an n-type semiconductor.
(iii) Delocalised electrons increase the conductivity of doped silicon.
(iv) An electron vacancy increases the conductivity of the n-type semiconductor.
The answer is the option (ii, iii) Silicon (valence electron – 4) doped with electron rich impurity is an n-type semiconductor due to extra electron. The conductivity of doped siliconis increased by the delocalised electrons.
An excess of potassium ions makes KCl crystals appear violet or lilac in colour since ________.
(i) some of the anionic sites are occupied by an unpaired electron.
(ii) some of the anionic sites are occupied by a pair of electrons.
(iii) there are vacancies at some anionic sites.
(iv) F-centres are created which impart colour to the crystals.
The answer is the option (i, iv).
When KCl is heated in vapour of K, anionic vacancies are created as some of the ions leave their lattice site. This chloride ion wants to combine with K vapour to form KCl. For this to happen, loss of electron by potassium atom to form potassium ion occurs. The unpaired free electron gets entrapped in the anion vacancy called F-centre that are responsible for imparting color to crystals. This entrapped electron gains energy due to the visible light falling on the crystal goes to the higher level and when it comes back to the ground state, energy is released in the form of light.
The number of tetrahedral voids per unit cell in NaCl crystal is ________.
(iii) twice the number of octahedral voids.
(iv) four times the number of octahedral voids.
The answer is the option (ii, iii) NaCl has fcc arrangement
Number of atoms in packing per unit cell = 4
Number of tetrahedral voids per unit cell = 2 No. of particles present in close packing
Number of tetrahedral voids per unit cell = 2 No. of octahedral voids
Hence, option ii and iii are correct.
Amorphous solid can also be called ________.
(i) pseudo solids
(ii) true solids
(iii) supercooled liquids
(iv) supercooled solids
The answer is the option (i, iii) Amorphous solid has short-range order which has a tendency to flow very slowly. Thus, although they are solids, they resemble liquid in many respects. Therefore amorphous solid can also be called as pseudo solids or super cooled liquids. Some examples of amorphous solid includes rubber, glass, plastic and gels.The Solid State Excercise: 1.2
Which of the following statements are correct?
(i) Ferrimagnetic substances lose ferrimagnetism on heating and become paramagnetic.
(ii) Ferrimagnetic substances do not lose ferrimagnetism on heating and remain ferrimagnetic.
(iii) Antiferromagnetic substances have domain structures similar to ferromagnetic substances and their magnetic moments are not cancelled by each other.
(iv) In ferromagnetic substances, all the domains get oriented in the direction of the magnetic field and remain as such even after removing magnetic field.
The answer is the option (i, iv) There is a loss of ferrimagnetism of Ferrimagnetic substances on heating changing them into paramagnetic.
All the domains get oriented in the direction of magnetic field in ferromagnetic substances and remain as such even on removal of the magnetic field.
Which of the following features are not shown by quartz glass?
(i) This is a crystalline solid.
(ii) Refractive index is the same in all the directions.
(iii) This has a definite heat of fusion.
(iv) This is also called supercooled liquid
The answer is the option (i, iii) Since quartz glass is an amorphous solid, it has no definite heat of fusion. This is due to short-range order of molecule. Also known as super cooled liquid, quartz glass is isotropic in nature.
Which of the following cannot be regarded as molecular solid?
(i) SiC (Silicon carbide)
The answer is the option (i, ii, iii) Silicon carbide, AIN and diamond are examples of network solid instead of molecular solids as they have three-dimensional structure while; is a molecular solid, because such solid particles are held together by dipole-dipole interactions. SiC and AIN are interstitial solids.
In which of the following arrangements octahedral voids are formed?
(iii) simple cubic
The answer is the option (i, iv) In hcp and fcc arrangement, octahedral voids are formed. In an fcc unit cell, the octahedral voids are observed at edge centre and body centre whereas in bcc and simple cubic, no octahedral voids are observed. Cubic voids are formed in bcc arrangement.
Frenkel defect is also known as ________.
(i) stoichiometric defect
(ii) dislocation defect
(iii) impurity defect
(iv) non-stoichiometric defect
The answer is the option (i, ii) Dislocation of cations takes place from one place to another in frenkel defect and the stoichiometry of the crystal remains unchanged.
Which of the following defects decrease the density?
(i) Interstitial defect
(ii) Vacancy defect
(iii) Frankel defect
(iv) Schottky defect
The answer is the option (ii, iv) Vacancy and Schottky defect lead to decrease the density. In Vacancy defect, an atom goes missing from one of the lattice site thus decreasing the density. In Schottky defect, an atom moves from inside of crystal to its surface. The density remains the same in case of Frenkel defect and interstitial defect.
NCERT Exemplar Class 12 Chemistry Solutions Chapter 1: Short answer type
Why are liquids and gases categorised as fluids?
The liquids and gases have an ability to flow. Liquid and gas molecules can easily move fast and tumble over one another freely. These have been categorized as fluids because of their tendency to flow.
Why are solids incompressible?
The particles in solid are already packed closely together. There will be a large repulsive force between electron clouds of these particles if brought closer. Therefore, solids are incompressible.
Why does table salt, NaCl, sometimes appear yellow in colour ?
The yellow colour of NaCl crystals can be attributed to metal excess defect as some chlorine ions leave their lattice sites and are occupied by unpaired electrons. These sites are called F-centres. On absorption of energy, electrons gets excited and falls on the crystals imparting yellow color.
Why does white ZnO (s) become yellow upon heating?
On heating, ZnO gives , electrons and colour.
The excess Zn ions thus formed move to the interstitial sites and electron in the neighbourhood vacant interstitial sites for neutralisation. This electron is responsible for the yellow colour and electrical conductivity in crystals. The color reverts back to white on cooling.
Why does the electrical conductivity of semiconductors increase with a rise in temperature?
The energy gap between valence and conduction band is small in semiconductors. Thus, they do not conduct electricity at normal temperature but with a rise in temperature large number of electrons get sufficient energy to jump from valence band to conduction band. Therefore, the electrical conductivity of a semi-conductor will increase exponentially with an increase in temperature.
Explain why does conductivity of germanium crystals increase on doping with gallium?
When germanium is doped with gallium or any other group 13 elements ,some of the positions of lattice of germanium atom are occupied by gallium. Gallium contains only 3 valence electrons. Thus the 4th valency of nearby germanium atom is not satisfied leaving this place vacant. Electron from neighbouring atom comes and fills the gap and creates a hole in its original position.
The electrons move towards positively charged plates through these under the influence of electric field for conduction of electricity. The holes appear to move towards negatively charged plates.
NCERT Exemplar Class 12 Chemistry Solutions Chapter 1: Matching Type
Match the defects given in Column I with the statements given in Column II.
(i) -> (c); (ii) -> (a); (iii) ->(d); (iv) ->(b)
Vacancy defect occurs when some of the lattice sites are vacant resulting in decrease in density. In case of schottky defect, an equal number of cations and anions are missing from their normal lattice site by creating vacancies or holes.
In case of frenkel defect, the density remains same as the cation missing from the normal lattice position occupies interstitial site. Thus, maintaining the same density. In Interstitial defect, some of the constituent atoms occupy the interstitial site. Hence, no change in density.
Match the type of unit cell given in Column I with the features given in Column II.
(i) —>(b, c); (ii) —>(c, d); (iii) —>(c, e); (iv) —> (a, d)
(i) In primitive unit cell each of the 8 corners contribute 1/8th to the unit cell
Total number of atoms per unit cell =
(ii) Body centered cubic unit cell contains atoms at corner as well as body centre.
each of the 8 corners contribute 1/8th to the unit cell and the contribution due to the atom at the centre of the body=1
(iii) In face centred unit cell, total constituent ions per unit cell present at corners
Total contribution of atoms per unit cell present at face centre
(iv) For end centred orthorhombic unit cell
each of the 8 corners contribute 1/8th to the unit cell
whereas at end centre the total contribution is
Thus, other than corner it contains total one atom per unit cell.
Match the types of defect given in Column I with the statement given in Column II.
i) —>(c); (ii) —>(a); (iii) —> (b)
(A) (i) Impurity defects: The defects introduced in the crystal lattice due to presence of the certain impurity are called impurity defects.
Example: Substitution of ions in NaCl by ions.
Structure with defect:
Impurity defect due to substitution of ions in NaCl by ions (Cation vacancy) ‘Schottky Defect’
(B) On heating NaCl in vapour of sodium, some of the Cl ions leave their lattice site and create anion vacancies. For chloride ions to combine with sodium vapour to form sodium chloride, sodium atom loses electrons to form ions. This released electron on diffusion into the crystal gets entrapped in the anion vacancy called F-centre.
(C) Metal deficiency is caused when a cation is missing from its lattice site and a nearby metal ion acquires 2 positive charge to maintain electrical neutrality.
This type of defect can be seen in compounds where metal exhibit variable valency.
Example: FeO, FeS, NiO
Match the items given in Column I with the items given in Column II.
(i) electronic conductivity is shown by Mg in solid state due to presence of free electrons.
(ii) electrolytic conductivity is shown by in molten state due to the presence of electrolytes in molten state.
(iii) Silicon doped with phosphorus is p-type semiconductor. It contain one extra electron due to which it shows conductivity under the influence of electric field.
(iv) Germanium doped with boron is p-type semiconductor. It shows conductivity under the influence of electric field due to the presence of a hole.
Match the type of packing given in Column I with the items given in Column II.
(i) —> (c); (ii) —> (a); (iii) —>(d); (iv) —> (b)
(i) In Square close packing in two dimensions, each sphere has coordination number 4, as shown in the diagram below.
(ii)In hexagonal close packing, in two dimensions, each sphere has coordination number 6 and a triangular void is created.
(iii) hcp in 3 dimensions is a repetitive pattern of ABAB…..
(iv) In ccp spheres are repeated at every 4th layer as in ABCABCA….
How does the doping increase the conductivity of semiconductors?
Conductivity of semiconductors are exceptionally low for practical use. Semiconductors are doped to generate either a surplus or deficiency in valence electrons depending on whether n-type semiconductors are required or p-type. An electron rich or electron deficient impurity as compared to the intrinsic semiconductor, silicon or germanium is used for doping. Electronic defects are introduced in them by such impurities.
On doping silicon with electron rich impurities, the extra electron becomes delocalized increasing the conductivity of doped silicon. Hence silicon doped with electron-rich impurity is called n-type semiconductor due to the negatively charged electron. For ex. When group 15 elements are added to silicon
When silicon is doped with electron-deficit impurities to increase the conductivity through positive holes, this type of semiconductors are called p-type semiconductors. Ex. Addition of group 13 elements to group 14 element
NCERT Exemplar solutions for Class 12 Chemistry Chapter 1 also helps in correlating different nature of particles, creating different properties of solid and also studies various arrangements of particles resulting in distinguished structures of solid. NCERT Exemplar Class 12 Chemistry solutions Chapter 1 Solid State deals with two different types of solid, namely crystalline and amorphous solids along with the further classification of crystalline solids into various other categories based on intermolecular forces along with examples. Students can make use of NCERT Exemplar Class 12 Chemistry solutions Chapter 1 PDF download prepared by experts. The topics included are as follows:
NCERT Exemplar Class 12 Chemistry solutions Chapter 1 Solid State -Main subtopics
1.1 General Characteristics of Solid State
1.2 Amorphous and Crystalline Solids
1.3 Classification of Crystalline Solids
1.3.1 Molecular Solids
1.3.2 Ionic Solids
1.3.3 Metallic Solids
1.3.4 Covalent or Network Solids
1.4 Crystal Lattices and Unit Cells
1.4.1 Primitive and Centred Unit Cells
1.5 Number of Atoms in a Unit Cell
1.5.1 Primitive Cubic Unit Cell
1.5.2 Body-Centred Cubic Unit Cell
1.5.3 Face-Centred Cubic Unit Cell
1.6 Close-Packed Structures
1.6.1 The formula of a Compound and Number of Voids Filled
1.7 Packing Efficiency
1.7.1 Packing Efficiency in HCP and CCP Structures
1.7.2 The efficiency of Packing in Body-Center Cubic Structures
1.7.3 Packing Efficiency in Simple Cubic Lattice
1.8 Calculations Involving Unit Cell Dimensions
1.9 Imperfections in Solids
1.9.1 Types of Point Defects
1.10 Electrical Properties
1.10.1 Conduction of Electricity in Metals
1.10.2 Conduction of Electricity in Semiconductors
1.11 Magnetic Properties
NCERT Exemplar Class 12 Chemistry Solutions
Chapter 2 Solutions
Chapter 3 Electrochemistry
Chapter 4 Chemical Kinetics
Chapter 5 Surface Chemistry
Chapter 6 General Principles and Processes of Isolation of Elements
Chapter 7 The p-Block Elements
Chapter 8 The d & f Block Elements
Chapter 9 Coordination Compounds
Chapter 10 Haloalkanes and Haloarenes
Chapter 11 Alcohols, Phenols, and Ethers
Chapter 12 Aldehydes, Ketones, and Carboxylic Acids
Chapter 13 Amines
Chapter 14 Biomolecules
Chapter 15 Polymers
Chapter 16 Chemistry in Everyday Life
Important topics to cover for exams from class 12 chemistry chapter 1 solid state
· NCERT Exemplar Class 12 Chemistry solutions Chapter 1 covers the diagrammatic representation of the regular and repeating pattern of crystalline solid in three-dimensional spaces with reference to fourteen possible arrangements known as Bravais Lattices.
· NCERT Exemplar solutions for Class 12 Chemistry Chapter 1 also includes questions related to the formation of the crystal lattice at the molecular level for defining various arrangements along with the study of unit cells and its types that make up the crystal lattice.
· Class 12 Chemistry NCERT exemplar solutions Chapter 1 also provides understanding and different methods for calculating the number of atoms combined to form a unit cell.
· NCERT Exemplar Class 12 Chemistry solutions Chapter 1 also explains different types of packing of constituent particles in solid in different dimensions, provides the formula for a compound made of different particles based on its arrangement of constituent particles and packing efficiencies of different types of structures.
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