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The Solid State

Short Answer Type

171. Explain the following with suitable examples:
Ferrimagnetism

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172. Explain the following with suitable examples:
Piezoelectric effect (or pressure electricity)

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173. Explain the following with suitable examples:
Antifluorite structure

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174. Give reasons for the following:
Molecular solids are generally soft and easily compressible.

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175. Give reasons for the following:
The energy required to vapourise one mole of copper is smaller than that of energy required to vapourise one mole of diamond.

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176. Give reasons for the following:
All metals have metallic bonds but some metals are soft and having low melting points and some are hard and having high melting points.

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177. Give reasons for the following:
Covalent crystals like diamond and silicon carbide are quite hard and difficult to break.

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178. Give reasons for the following:
Ionic solids, inspite of being made up of ions, do not conduct electricity.

Solid ionic compounds do not conduct electricity because the ions (charged particles) are locked into a rigid lattice or array. The ions cannot move out of the lattice, so the solid cannot conduct electricity.

When molten, the ions are free to move out of the lattice structure.

Cations (positive ions) move towards the negative electrode (cathode)
M⁺ + e -----> M
Anions (negative ions) move towards the positive electrode (anode)
X^- -----> X + e

When an ionic solid is dissolved in water to form an aqueous solution, the ions are released from the lattice structure and are free to move so the solution conducts electricity just like the molten (liquid) ionic compound.

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