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

(a) The unit cells of three structural types of ionic solids are shown below (the anions appear light and the cations dark). The anions occupy the lattice positions. X (B) (A) (i) Name the common structural type for (A), (B) and (C). (Hint: a typical structural type is rutile (T1O₂).] (C) (ii) The structures (A), (B) and (C) can be considered as packing of anlons with the cations occupying specific types of hole. For each structure: state the unit cell that the packing of anions is based on. state which holes are occupied by the cations and what fraction of them are occupied. State the coordination numbers of the cations and anions for (A), (B) and (C).

(a) A hypothetical compound MB2 crystallises in the rutile lattice structure. (i) Draw the lattice structure of the unit cell MB2. (ii) Show by calculation that the stoichiometry of the formula is consistent with the structure. (iii) Determine the coordination number of the MB₂ unit cell.

At room temperature, F2 and Cl2 are gases, Br2 is a liquid, and I2 is solid. This is because of what?

A metal crystallizes in the face-centered cubic crystal structure with a unit cell edge of 3.52 x 10 -8 cm.The density of the metal is 8.90 g/cc. (a) What is the mass, in grams, of a single atom of this element? (b) What is the atomic weight of the element (g/mol). (c) What is the radius, in cm, of an atom of the element?

Titanium carbide, TiC, adopts the rock-salt (NaCl) crystal structure. (i) Draw the unit cell indicating clearly the position of all atoms.(ii) The unit cell parameter for TiC is 0.4329 nm. Calculate the C-Cdistance, the Ti-C bond length and the Ti-Ti  distance.