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The Solid State

Short Answer Type

11. Name the parameters that characterize a unit cell.

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12. Distinguish between Hexagonal and monoclinic unit cells.

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13. Distinguish between Face-centred and end-centred unit cells.

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

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

Number of closed packed particeles =

0.5 \times 6.022 \times 10^{23} = 3.011 \times 10^{23}

therefore number of octhahedral voids = 3.011

\times 10^{23}

and number oftetrahedral voids =

2 \times 3.011 \times 10^{23} = 6.022 \times 10^{23}

therefore total number of voids=

3.011 \times 10^{23} + 6.022 \times 10^{23} = 9.033 \times 10^{23}

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

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Multiple Choice Questions

18. Which of the following lattices has the highest packing efficiency:

simple cubic
body-centred cubic
hexagonal close packed lattice

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Short Answer Type

19. An element with molar mass 2.7 x 10^–2kg mol^–1 form 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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20. 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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