Comparison of Chemical Bonding Types
This page provides a comprehensive overview of the three main types of chemical bonding: metallic, covalent, and ionic. Understanding these bonding types is essential for grasping the behavior of different materials.
Metallic Bonding
Metallic bonding occurs in metals and is characterized by the following:
- Positive metal ions in a lattice structure
- Delocalized negative electrons moving freely within the lattice
Definition: Delocalized electrons are electrons that are not associated with any specific atom or bond in a molecule or crystal structure.
The electrostatic force of attraction between the positive ions and the delocalized electrons occurs in all directions, giving metals their unique properties.
Covalent Bonding
Covalent bonding, as discussed in the previous page, occurs between non-metals. Key points include:
- Sharing of electrons between atoms
- Formation of molecules or large structures
Example: The dot and cross diagram shows electron sharing in molecules like hydrogen H2, oxygen O2, nitrogen N2, and methane CH4.
Ionic Bonding
Ionic bonding typically occurs between metals and non-metals. While not extensively covered in this image, it's important to note its existence for a complete understanding of bonding types.
Highlight: The difference between ionic, covalent and metallic bonds lies in how electrons are shared or transferred between atoms.
Comparison of Bonding Types
Understanding the differences and similarities between these bonding types is crucial for predicting material properties:
- Metallic: Delocalized electrons, strong in all directions
- Covalent: Shared electrons, directional bonds
- Ionic: Transfer of electrons, strong electrostatic attraction
Vocabulary: Electrostatic force is the attractive or repulsive force between electrically charged particles.
Each bonding type results in materials with distinct physical and chemical properties, influencing their behavior in various applications and reactions.