Question

Explain the basis of differences between metallic and ionic crystals.

Answer 1

1. The primary differences between ionic and metallic crystals are brittleness, hardness, and electrical conductivity.
2. The characteristics of electrostatic attraction and electron mobility in the metals serve as the foundation for these variations.
3. Electrostatic forces between oppositely charged ions that are fixed at the lattice sites are present in ionic solids.
4. They can’t conduct currents because of this. Kernels and mobile valence electrons in metallic materials are electrically attracted to one another.
5. Metals are excellent electrical conductors because of the mobility of their valence electrons.

Answer 2

	Property	Metallic Crystals	Ionic Crystals
1.	Constituents	These are composed of positive metal ions immersed in a sea of delocalised electrons.	These consist of both positive and negative ions held together by strong electrostatic forces.
2.	Bonding	The atoms are bonded through metallic bonding, which involves a lattice of positive ions surrounded by free-moving electrons.	The ions are held together by strong ionic (Coulombic) attraction between oppositely charged ions.
3.	Electrical Conductivity	They are good conductors of electricity due to the presence of free-moving electrons.	They conduct electricity only in the molten state or when dissolved in water, as the ions are free to move.
4.	Malleability & Ductility	They are highly malleable and ductile and can be hammered or drawn into wires without breaking.	They are brittle and tend to shatter when subjected to stress due to repulsion between like-charged ions on displacement.
5.	Melting & Boiling Points	These generally have high melting and boiling points, although the values may vary depending on the metal.	They usually have high melting and boiling points due to strong ionic bonds, not conductivity (the original line had an error).