• Chapter -1 The Solid State Assignments 1

    (a) Explain the following phenomena with the help of Henry’s law.
    (i) Painful condition known as bends.
    (ii) Feeling of weakness and discomfort in breathing at high altitude.
    (b) Why soda water bottle kept at room temperature fizzes on opening?

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  • Chapter -1 The Solid State Assignments 2

    Why are aquatic species more comfortable in cold water in comparison to
    warm water?

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  • Chapter -1 The Solid State Assignments 3

    What is the significance of Henry’s Law constant KH?

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  • Chapter -1 The Solid State Assignments 4

    Concentration terms such as mass percentage, ppm, mole fraction and molality
    are independent of temperature, however molarity is a function of temperature.
    Explain.

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  • Chapter -1 The Solid State Assignments 5

    Explain the solubility rule “like dissolves like” in terms of intermolecular forces
    that exist in solutions.

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  • Chapter -1 The Solid State Assignments 6

    Explain why on addition of 1 mol of NaCl to 1 litre of water, the boiling point
    of water increases, while addition of 1 mol of methyl alcohol to one litre of
    water decreases its boiling point.

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  • Chapter -1 The Solid State Assignments 7

    Components of a binary mixture of two liquids A and B were being separated
    by distillation. After some time separation of components stopped and
    composition of vapour phase became same as that of liquid phase. Both the
    components started coming in the distillate. Explain why this happened.

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  • Chapter -1 The Solid State Assignments 8

    How does the doping increase the conductivity of semiconductors?

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  • Chapter -1 The Solid State Assignments 9

    Show that in a cubic close packed structure, eight tetrahedral voids are present
    per unit cell.

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  • Chapter -1 The Solid State Assignments 10

    With the help of a labelled diagram show that there are four octahedral voids
    per unit cell in a cubic close packed structure.

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  • Chapter -1 The Solid State Assignments 11

    Match the type of packing given in Column I with the items given in Column II.
    Column I                                                           Column II
    (i) Square close packing in                                      (a) Triangular voids
    two dimensions
    (ii) Hexagonal close packing                                    (b) Pattern of spheres is repeated in
    in two dimensions every fourth layer
    (iii) Hexagonal close packing in                                (c) Coordination number 4
    three dimensions 
    (iv) Cubic close packing in                                       (d) Pattern of sphere is repeated in
    three dimensions alternate layers

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  • Chapter -1 The Solid State Assignments 12

    Match the items given in Column I with the items given in Column II.
    Column I                                                                 Column II
    (i) Mg in solid state                                                   (a) p-Type semiconductor
    (ii) MgCl2 in molten state                                            (b) n-Type semiconductor
    (iii) Silicon with phosphorus                                          (c) Electrolytic conductors
    (iv) Germanium with boron                                         (d) Electronic conductors

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  • Chapter -1 The Solid State Assignments 13

    Match the type of unit cell given in Column I with the features given in
    Column II.
    Column I                                                     Column II
    (i) Primitive cubic unit cell                        (a) Each of the three perpendicular
    edges compulsorily have the different
    edge length i.e; a≠b≠c.
    (ii) Body centred cubic unit cell                    (b) Number of atoms per unit cell is one.
    (iii) Face centred cubic unit cell                    (c) Each of the three perpendicular
    edges compulsorily have the same
    edge length i.e; a = b = c
    (iv) End centred orthorhombic                        (d) In addition to the contribution from
    unit cell the corner atoms the number of atoms
    present in a unit cell is one.
                                                                 (e) In addition to the contribution from
    the corner atoms the number of
    atoms present in a unit cell is three.

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  • Chapter -1 The Solid State Assignments 14

    Note : In the following questions match the items given in Column I with
    the items given in Column II. In some questions more than one item of
    Column I and Column II may match.

     Match the defects given in Column I with the statements in given Column II.
    Column                                                          I Column II
    (i) Simple vacancy defect                                  (a) shown by non-ionic solids and
    increases density of the solid.
    (ii) Simple interstitial defect                            (b) shown by ionic solids and decreases
    density of the solid.
    (iii) Frenkel defect                                        (c) shown by non ionic solids and density
    of the solid decreases
    (iv) Schottky defect                                      (d) shown by ionic solids and density of
    the solid remains the same.

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  • Chapter -1 The Solid State Assignments 15

    Under which situations can an amorphous substance change to crystalline form?

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  • Chapter -1 The Solid State Assignments 16

    In a compound, nitrogen atoms (N) make cubic close packed lattice and metal
    atoms (M) occupy one-third of the tetrahedral voids present. Determine the
    formula of the compound formed by M and N?

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  • Chapter -1 The Solid State Assignments 17

    Explain why does conductivity of germanium crystals increase on doping
    with galium.

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  • Chapter -1 The Solid State Assignments 18

    Why does the electrical conductivity of semiconductors increase with rise in
    temperature?

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  • Chapter -1 The Solid State Assignments 19

    Why does white ZnO (s) becomes yellow upon heating?

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  • Chapter -1 The Solid State Assignments 20

    Why is FeO (s) not formed in stoichiometric composition?

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  • Chapter -1 The Solid State Assignments 21

    Why does table salt, NaCl, some times appear yellow in colour?

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  • Chapter -1 The Solid State Assignments 22

    Inspite of long range order in the arrangement of particles why are the crystals
    usually not perfect?

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  • Chapter -1 The Solid State Assignments 23

    Why are solids incompressible?

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  • Chapter -1 The Solid State Assignments 24

    Why are liquids and gases categorised as fluids?

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  • Chapter -1 The Solid State Assignments 25

    What do you mean by paramagnetic substance?

     

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  • Chapter -1 The Solid State Assignments 26

    Which substance exhibit schottky and Frenkel both defects. 

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  • Chapter -1 The Solid State Assignments 27

    Name a salt which is added to Agcl so as to produce cation vacancies. 

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  • Chapter -1 The Solid State Assignments 28

    Why Frenkel defects not found in pure Alkali metal halide. 

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  • Chapter -1 The Solid State Assignments 29

    What is the use of amorphous silica? 

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  • Chapter -1 The Solid State Assignments 30

    Analysis shows that a metal oxide has the empirical formula Mo.9801.00. Calculate the percentage of M2+ and M3+ ions in the crystal.

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  • Chapter -1 The Solid State Assignments 31

    What is the co‐ordination no. of cation in Antifluorite structure? 

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  • Chapter -1 The Solid State Assignments 32

    What is the Co.No. of cation and anion in Caesium Chloride. 

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  • Chapter -1 The Solid State Assignments 33

    What is F centre?

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  • Chapter -1 The Solid State Assignments 34

    How does amorphous silica differ from quartz?

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  • Chapter -1 The Solid State Assignments 35

    Which point defect lowers the density of a crystal?

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  • Chapter -1 The Solid State Assignments 36

    Why glass is called supper cooled liquids?

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  • Chapter -1 The Solid State Assignments 37

    Some of the very old glass objects appear slightly milky instead of being transparent why?

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  • Chapter -1 The Solid State Assignments 38

    What is anisotropy?

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  • Chapter -1 The Solid State Assignments 39

    What is the coordination number of atoms?

     

    a)   in fcc structure b) in bcc structure

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  • Chapter -1 The Solid State Assignments 40

     How many lattice points are there in one cell of ‐

     

    a)   fcc b) bcc c) simple cubic

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  • Chapter -1 The Solid State Assignments 41

    What are the co‐ordination numbers of octahedral voids and tetrahedral voids?

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  • Chapter -1 The Solid State Assignments 42

    Why common salt is sometimes yellow instead of being of being pure white?

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  • Chapter -1 The Solid State Assignments 43

    A compound is formed by two elements X and Y. The element Y forms ccp and atoms of X occupy octahedral voids. What is formula of the compound?

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  • Chapter -1 The Solid State Assignments 44

    Explain how electrical neutrality is maintained in compounds showing Frenkel and Schottky defect.

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  • Chapter -1 The Solid State Assignments 45

    Calculate the number of atoms in a cubic unit cell having one atom on each corner and two atoms on each body diagonal.

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  • Chapter -1 The Solid State Assignments 46

    Gold crystallizes in an FCC unit cell. What is the length of a side of the cell(r=0.144mm)

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  • Chapter -1 The Solid State Assignments 47

    Classify each of the following as either a p‐type or n‐type semi‐conductor. a) Ge doped with In

     

    b) B doped with Si

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  • Chapter -1 The Solid State Assignments 48

    In terms of band theory what is the difference between a conductor, an insulator and a semi‐

    conductor?

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  • Chapter -1 The Solid State Assignments 49

    CaCl2 will introduce Scotty defect if added to AgCl crystal. Explain

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  • Chapter -1 The Solid State Assignments 50

    The electrical conductivity of a metal decreases with rise in temperature while that of a semi‐

    conductor increases. Explain.

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  • Chapter -1 The Solid State Assignments 51

    What  type  of   substances  would  make  better   permanent  magnets,  ferromagnetic  or ferromagnetic, why?

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  • Chapter -1 The Solid State Assignments 52

    In a crystalline solid, the atoms A and B are arranged as follows:‐

    a.   Atoms A are arranged in ccp array.

    b.   Atoms B occupy all the octahedral voids and half of the tetrahedral voids. What is the

    formula of the compound?

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  • Chapter -1 The Solid State Assignments 53

    In compound atoms of element Y forms ccp lattice and those of element X occupy 2/3rd of tetrahedral voids. What is the formula of the compound?

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  • Chapter -1 The Solid State Assignments 54

    Explain the following with suitable examples:

    (i) Ferromagnetism

    (ii)Paramagnetism

    (iii)Ferrimagnetism

    (iv)Antiferromagnetism

    (v)12-16 and 13-15 group compounds.

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  • Chapter -1 The Solid State Assignments 55

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

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  • Chapter -1 The Solid State Assignments 56

    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 cm3of aluminium?

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  • Chapter -1 The Solid State Assignments 57

    Explain the following terms with suitable examples:

    (i) Schottky defect

    (ii) Frenkel defect

    (iii) Interstitials and

    (iv) F-centres

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  • Chapter -1 The Solid State Assignments 58

    In terms of band theory, what is the difference

    (i) Between a conductor and an insulator

    (ii) Between a conductor and a semiconductor

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  • Chapter -1 The Solid State Assignments 59

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

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  • Chapter -1 The Solid State Assignments 60

    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.

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  • Chapter -1 The Solid State Assignments 61

    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.

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  • Chapter -1 The Solid State Assignments 62

    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?

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  • Chapter -1 The Solid State Assignments 63

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

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  • Chapter -1 The Solid State Assignments 64

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

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  • Chapter -1 The Solid State Assignments 65

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

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  • Chapter -1 The Solid State Assignments 66

    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.

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  • Chapter -1 The Solid State Assignments 67

    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.

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  • Chapter -1 The Solid State Assignments 68

    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?

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  • Chapter -1 The Solid State Assignments 69

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

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  • Chapter -1 The Solid State Assignments 70

     

    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).

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  • Chapter -1 The Solid State Assignments 71

     

    Explain

    (i) The basis of similarities and differences between metallic and ionic crystals.

    (ii) Ionic solids are hard and brittle.

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  • Chapter -1 The Solid State Assignments 72

     

    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

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  • Chapter -1 The Solid State Assignments 73

     

    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?

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  • Chapter -1 The Solid State Assignments 74

    'Stability of a crystal is reflected in themagnitude 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?

     

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  • Chapter -1 The Solid State Assignments 75

     

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

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  • Chapter -1 The Solid State Assignments 76

     

    (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-centred cubic structure?

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  • Chapter -1 The Solid State Assignments 77

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

    (i) Tetra phosphorus decoxide (P4O10) (vii) Graphite

    (ii) Ammonium phosphate (NH4)3PO4 (viii) Brass

    (iii) SiC (ix) Rb

    (iv) I2 (x) LiBr

    (v) P4 (xi) Si

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  • Chapter -1 The Solid State Assignments 78

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

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  • Chapter -1 The Solid State Assignments 79

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

     

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  • Chapter -1 The Solid State Assignments 80

    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?

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  • Chapter -1 The Solid State Assignments 81

    Ionic solids, which have anionic vacancies due to metal excess defect, develop colour. Explain with the help of a suitable example.

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  • Chapter -1 The Solid State Assignments 82

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

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  • Chapter -1 The Solid State Assignments 83

    What type of stoichiometric defect is shown by:

    (i) ZnS (ii) AgBr

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  • Chapter -1 The Solid State Assignments 84

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

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  • Chapter -1 The Solid State Assignments 85

    An element with molar mass 2.7 x 10-2kg mol-1forms 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?

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  • Chapter -1 The Solid State Assignments 86

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

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  • Chapter -1 The Solid State Assignments 87

    A compound is formed by two elements M and N. The element N forms ccp and atoms of M occupy 1/3rdof tetrahedral voids. What is the formula of the compound?

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  • Chapter -1 The Solid State Assignments 88

    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?

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  • Chapter -1 The Solid State Assignments 89

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

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  • Chapter -1 The Solid State Assignments 90

    Explain how much portion of an atom located at (i)corner and (ii)body-centre of a cubic unit cell is part of its neighbouring unit cell.

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  • Chapter -1 The Solid State Assignments 91

    Distinguish between

    (i)Hexagonal and monoclinic unit cells

    (ii) Face-centred and end-centred unit cells.

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  • Chapter -1 The Solid State Assignments 92

    Distinguish between

    (i)Hexagonal and monoclinic unit cells

    (ii) Face-centred and end-centred unit cells.

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  • Chapter -1 The Solid State Assignments 93

    Name the parameters that characterize a unit cell.

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  • Chapter -1 The Solid State Assignments 94

     

    Give the significance of a 'lattice point'.

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  • Chapter -1 The Solid State Assignments 95

     What type of solids are electrical conductors, malleable and ductile?

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  • Chapter -1 The Solid State Assignments 96

     

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

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  • Chapter -1 The Solid State Assignments 97

    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?

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  • Chapter -1 The Solid State Assignments 98

    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.

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  • Chapter -1 The Solid State Assignments 99

     

    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?

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  • Chapter -1 The Solid State Assignments 100

     

    Why is glass considered a super cooled liquid?

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  • Chapter -1 The Solid State Assignments 101

    Classify the following as amorphous or crystalline solids:

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

     

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  • Chapter -1 The Solid State Assignments 102

    Why do solids have a definite volume?

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  • Chapter -1 The Solid State Assignments 103

     

    Why are solids rigid?

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    • Description:-

    Lecture 6: Revison
    In the last class, we had completed our Chapter -1 The Solid State. Now today, you are going to revise the whole chapter through summary of the chapter, key points and practice paper, HOTS 
    Please go through all the topics which we had studied till now, their notes. Properly do the assignments, watch videos of the concerned topics.
    If you have any doubt about any topic/point please submit it in the discussion section... it will be answered as soon as possible.
    Now ...you can attempt quiz given of this chapter to check your concept clearance about the chapter.

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