Define the term 'amorphous'. Give a few examples of amorphous solids.

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

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

(I) What is meant by the term 'coordinationnumber'? (II) What is the coordination number ofatoms: (III) in a cubic close-packedstructure? (IV) in a body-centred cubicstructure?

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

'Stability of a crystal is reflected in the magnitude 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?

How will you distinguish between the following pairs of terms: (I) Hexagonal close-packing and cubicclose-packing? (II) Crystal lattice and unitcell? (III) Tetrahedral void and octahedralvoid?

How many lattice points are there in one unit cell of each of the following lattice? (I) Face-centredcubic (II) Face-centredtetragonal (III) Body-centred

Explain (I) The basis of similarities and differences between metallic and ioniccrystals. (II) Ionic solids are hard andbrittle.

Calculate the efficiency of packing in case of a metal crystal for (I) simplecubic (II) body-centredcubic (III) face-centred cubic (with the assumptions that atoms are touching eachother).

Silver crystallises in fcc lattice. If edge length of the cell is 4.07 × 10^-8 cm and density is10.5 g cm-3, calculate the atomic mass of silver.

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?

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.

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.

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.

Analysis shows that nickel oxide has the formula Ni_0.98O_1.00. What fractions of nickel exist as Ni²⁺ and Ni³⁺ ions?

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

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?

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.

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.

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

In terms of band theory, what is the difference (I) Between a conductor and aninsulator (II) Between a conductor and a semiconductor

Explain the following terms with suitable examples: (I) Schottkydefect (II) Frenkeldefect (III) Interstitialsand (IV) F-centres

Aluminium crystallises in a cubic close-packed structure. Its metallic radius is 125 pm. (I) What is the length of the side of the unitcell? (II) How many unit cells are there in 1.00 cm³ ofaluminium?

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

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

Why are solids rigid?

Why do solids have a definite volume?

Classify the following as amorphous or crystalline solids: Polyurethane, naphthalene, benzoic acid, teflon, potassium nitrate, cellophane, polyvinyl chloride, fibre glass, copper.

Why is glass considered a super cooled liquid?

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?

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.

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?

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

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

Give the significance of a ‘lattice point’.

Name the parameters that characterize a unit cell.

Distinguish between (I) Hexagonal and monoclinic unitcells (II) Face-centred and end-centred unitcells.

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 unitcell.

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

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?

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

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

An element with molar mass 2.7 × 10^-2 kg mol^-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7 × 103 kg m^-3, what is the nature of the cubic unit cell?

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

What type of stoichiometric defect is shown by:(i) ZnS (ii) AgBr

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

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

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?

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