Classify each of the following solids as an metallic, molecular, network or ionic solids :

Silver (Ag), Silicon Carbide (SiC), Silicon (Si), white phosphorous (P₄) Glucose (C₆H₁₂O₆), naphthalene (C₁₀H₈), Na₂SO₄, SiO₂, Se, S₈, Sn.

2. Compare what happens when crystalline and amorphous solids are broken into pieces.

3. Answer the following questions :

(i) Write two examples of amorphous solids.

(ii) Name the type of solids which have long range orders.

(iii) Write down the difference between isotropy and anisotropy.

4. Which of the following do you expect to be molecular solids?

(a) Sodium hydroxide

(b) Solid ethane

(c) Nickel

(d) Solid silane

(e) Dry ice

5. Which network solid is an exceptionally good conductor of electricity?

6. A compound is formed by two elements 'P' and 'Q'. The compound crystallizes in cubic arrangement in which 'P' atoms occupy the corners of a cube and 'Q' atoms are present at face-centres. What is the formula of the compound?

7. In a face-centred cubic arrangement of 'A' and 'B' atoms, 'A' atoms occupy the corners and 'B' atoms occupy the face-centres of the unit cell. One of the corners in each unit cell remains vacant. What is the simplest formula of the compound?

8. A unit cell consists of a cube in which there are anions 'Y' at each corner and cations 'X' at the centre of alternate faces of a unit cell. What is the simplest formula of the compound?

9. A unit cell consists of a cube in which the atoms of A are occupying the corners while the atoms of B are occupying the centre of each face. If the atoms of A are missing from two corners, what is the simplest formula of the compound?

10. CsCl has bcc arrangement and its unit cell edge length is 400 pm. Calculate interionic distance in CsCl.