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Solid State Test - 16

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Solid State Test - 16
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  • Question 1
    1 / -0

    How many number of atoms are there in a cube based unit cell having one atom on each corner and two atoms on each body diagonal of cube -

    Solution

    Total body diagonal = 4
    two atoms in each body diagonal so total number of atoms = 4×2=8 and 8 atom on each corner, So its contribution will be

    so total number of atoms = 8+1=9

  • Question 2
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    A metal crystallizes with a face-centered cubic lattice. The edge of the unit cell is 408 pm. The diameter of the metal atom is

    Solution

  • Question 3
    1 / -0

    The number of atoms/molecules contained in one face centred cubic unit cell of a mono atomic substance is-

    Solution

    In Fcc
    Face contribution 1/2
    total 6 faces so its contribution  atom and contribution by its corner will be

    So total number of atom in F.C.C will be 4.

  • Question 4
    1 / -0

    In a face centred cubic arrangement of A & B atoms whose A atoms are at the corner of the unit cell & B atoms at the face centres. One of the A atom is missing from one corner in unit cell. The simplest formula of compound is-

    Solution

    There are 7 atoms at the corner. so contribution by 7 atoms form corner will be

    B will be at face so total contribution by it will be 3.

  • Question 5
    1 / -0

    Which is/are amorphous solids-

    Solution

    Rubber, P lastics and glass, all are amorphous solids so

  • Question 6
    1 / -0

    A solid has a b.c.c. structure. If the distance of closest approach between the two atoms is 1.73 Å. The edge length of the cell is-

    Solution

    In B.C.C
    4r = a √3
    2r = 1.73.
    2×1.73 = a √3
    Q = 200×10–12 m = 200 pm

  • Question 7
    1 / -0

    In a close packed array of N spheres, the number of tetrahedral holes are-

    Solution

    For N spheres, the number of tetrahedral holes is  2N

  • Question 8
    1 / -0

    In a face centred cubic cell, an atom at the face centre is shared by-

    Solution

  • Question 9
    1 / -0

    A solid XY has NaCl structure. If radius of X+ is 100 pm. What is the radius of Y- ion-

    Solution

    NaCl has octahredral structure


  • Question 10
    1 / -0

    How many atoms are there in a unit cell of Mg which forms hexagonal crystals, there being a face-centred atom in each end of the unit cell and 3 completely enclosed atoms within the unit cell-

    Solution

    6 face centred atom contbriution

    and 3 atom and 3 atoms are enclosed so total number of enclosed atom in the unit cell = 3 +3 = 6 atom

  • Question 11
    1 / -0

    A solid is made of two elements X and Z. The atoms Z are in c.c.p. arrangement while atoms X occupy all the tetrahedral sites. What is the formula of the compound-

    Solution

    Z is ccp so its total number 4.
    X atom occupy tetrahedral void so its total number will be 8
    X8Z4 = X2Z

  • Question 12
    1 / -0

    Close packing is maximum in the crystal-

    Solution

    Close packing is maximum in either face centrered ork in hexagonal

  • Question 13
    1 / -0

    The vacant space in b.c.c. unit cell is-

    Solution

    B.C.C. has the packing efficieny is 68%
    so the vacant space in BCCk is 32%

  • Question 14
    1 / -0

    AB crystallizes in a body centred cubic lattice with edge length 'a' equal to 387 pm. The distance between two oppositely charged ions in the lattice is

    Solution

    option B 

  • Question 15
    1 / -0

    The unit cell cube length for LiCl (just like NaCl structure) is 5.14 Å. Assuming anion-anion contact, the ionic radius for chloride ion is-

    Solution

    a = 5.14 A°
    structure is like NaCl

    r– = 1.815 A°

  • Question 16
    1 / -0

    At room temperature, sodium crystallizes in a body centred cubic lattice with a = 4.24 Å. The theoretical density of sodium (At. wt. of Na = 23) is-

    Solution


  • Question 17
    1 / -0

    The number of octahedral void(s) per atom present in a cubic close-packed structure is   

     [CBSE AIPMT 2012]

    Solution

    The total number of octahedral void(s) per atom present in a cubic close packed structure is 4. Besides the body centre, there is one octahedral void at the centre of each of the 12 edges. It is surrounded by six atoms, four belonging to the same unit cell (2 on the corners and 2 on face centres) and two belonging to two adjacent unit cells. Since each edge of the cube is shared between four adjacent unit cells, so is the octahedral void located on it. Only 1/4​th of each void belongs to a particular unit cell. Thus, in cubic close packed structure, octahedral void at the body-centre of the cube is 1.
    12 octahedral voids located at each edge and shared between four unit cells= 
    Total number of octahedral voids =4
    We know that in ccp structure, each unit cell has 4 atoms. Thus, the number of octahedral voids is equal to 4/4=1.

  • Question 18
    1 / -0

    In a face centred cubic lattice the number of nearest neighbour for a given lattice point are-

    Solution

    In a face centred cubic lattice the number of nearest neighour for a given lattice point 12

  • Question 19
    1 / -0

    AB crystallizes in a body centred cubic lattice with edge length 'a' equal to 387 pm. The distance between two oppositively charged ions in the lattice is   

    Solution

    Distance between two oppositely charge ions for BCC

    = 335.15 pm

  • Question 20
    1 / -0

    A solid AB has rock salt structure. If the edge length is 520 pm and radius of A+ is 80 pm, the radius of anion B- would be -

    Solution


    putting the value we get 180 pm

  • Question 21
    1 / -0

    A binary solid (A+ B-) has a zinc blende structure with B¯ ions constituting the lattice and A+ ions occupying 25% tetrahedral holes. The formula of solid is-

    Solution

    Zns - Zinc blende structure
    B- ions consisting the lattice so 4
    A here will be 2
    A2 B4 = AB2.

  • Question 22
    1 / -0

    A certain metal crystallises in a simple cubic structure. At a certain temperature, it arranges to give a body centred structure. In this transition, the density of the metal-

    Solution

    Simple cubic lattice → B.C.C
    So the Z will increase
    so density will increase

  • Question 23
    1 / -0

    For the structure given below the site marked as S is a-

                

    Solution

    Centre of edge is octehedral vold so

  • Question 24
    1 / -0

    ZnS is-

    Solution

    Zns is ionic erystal

  • Question 25
    1 / -0

    LiF is a/an-

    Solution

    LiF iso an ionic crstal

  • Question 26
    1 / -0

    A solid having no definite shape is called-

    Solution

    A solid having no definite shape is called Amorphous

  • Question 27
    1 / -0

    The mass of a unit cell of CsCl corresponds to-

    Solution

    CsCl has b.c.c. structure
    CS+ will be at the centre of the cente of the and 8 Cl— will occupy at the corner whch contribution will be 
    lhus, 1 CS+ & 1 Cl—

  • Question 28
    1 / -0

    Close packing is maximum in the crystal lattice of-

    Solution

    Close packing is maximum in F.C.C.

  • Question 29
    1 / -0

    The structure of MgO is similar to NaCl. The coordination number of Mg is-

    Solution

    The correct answer is Option C.

    For sodium chloride, there are 6 anions around each cation (coordination number of Na=6) because of the 1:1 stoichiometry, there must also be 6 cations around each Cl-  ion.
    Similarly, Mg2+O2- also has the octahedral structure and follows NaCl type geometry. 
    Therefore, the coordination number of Mg is also 6.
     

  • Question 30
    1 / -0

    Each unit cell of NaCl consists of 14 chlorine atoms and-

    Solution

    12 Na+ will find at centre of the edge and one will at centre of body so 13 Na atoms.

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