Metallic Bonding and Properties

Metallic bonding creates unique material properties that make metals essential in everyday applications. This type of bonding differs significantly from covalent bonds in structure and characteristics.

Definition: Metallic bonding involves the attraction between positive metal ions arranged in a regular lattice and a sea of delocalized electrons.

Highlight: Key properties of metals include:

• Excellent electrical conductivity due to mobile electrons
• High melting points resulting from strong metallic bonds
• Malleability allowing shape changes without breaking
• Ductility enabling formation into wires

Example: The ability of metals to conduct electricity comes from their delocalized electrons, which can freely move throughout the material.

Vocabulary: Malleable means capable of being hammered into shape, while ductile refers to the ability to be drawn into wires.

Understanding Covalent Bonds

Covalent bonding forms the foundation of molecular structures in non-metallic compounds. These bonds create stable molecules through electron sharing between atoms.

Definition: A covalent bond is formed when two non-metal atoms share a pair of electrons, creating a strong connection that requires significant energy to break.

Example: Common molecules featuring covalent bonds include HCl (hydrogen chloride), NH₃ (ammonia), CO₂ (carbon dioxide), and H₂O (water).

Vocabulary: A lone pair refers to electrons that aren't involved in bonding but remain associated with a specific atom.

Highlight: Structural formulae, such as CH₄ (methane) and H₂O (water), show how atoms are arranged and bonded within molecules.

Definition: A molecule consists of two or more atoms joined by covalent bonds, while diatomic molecules specifically contain two covalently bonded atoms.