List three kinds of crystalline solids, and give an example of each.

Verified step by step guidance

1. Identify the three main types of crystalline solids: ionic, covalent network, and metallic.
2. For ionic solids, consider the structure formed by the electrostatic attraction between cations and anions. An example is sodium chloride (NaCl).
3. For covalent network solids, recognize that atoms are bonded by covalent bonds in a continuous network. An example is diamond, which is a form of carbon.
4. For metallic solids, understand that metal atoms are surrounded by a sea of delocalized electrons. An example is copper (Cu).
5. Summarize the examples: Sodium chloride for ionic, diamond for covalent network, and copper for metallic solids.

Key Concepts

Ionic Crystalline Solids

Ionic crystalline solids are formed by the electrostatic attraction between positively and negatively charged ions. These solids typically have high melting and boiling points due to the strong ionic bonds. A common example is sodium chloride (NaCl), which forms a cubic lattice structure.

Covalent Network Solids

Covalent network solids consist of atoms connected by a network of covalent bonds, resulting in a rigid structure. These solids are characterized by their high melting points and hardness. An example is diamond, where each carbon atom is tetrahedrally bonded to four other carbon atoms.

Metallic Crystalline Solids

Metallic crystalline solids are composed of metal atoms that share a 'sea of electrons,' allowing for conductivity and malleability. The metallic bonds provide strength and flexibility, making these solids good conductors of heat and electricity. An example is copper, widely used in electrical wiring.