Study Notes
Molecules are formed when atoms share or transfer electrons to achieve a stable electronic configuration. Covalent Bond — a bond formed by the sharing of electron pairs between atoms. Example: Water (H2O) has covalent bonds between hydrogen and oxygen atoms. Ionic Bond — a bond formed by the electrostatic attraction between oppositely charged ions. Example: Sodium chloride (NaCl) is formed by the transfer of electrons from sodium to chlorine. Metallic Bond — a bond formed by the attraction between positively charged metal ions and delocalized electrons. Example: Copper (Cu) exhibits metallic bonding, allowing it to conduct electricity.
Exam Tips
Key Definitions to Remember
- Covalent Bond: Sharing of electron pairs between atoms.
- Ionic Bond: Electrostatic attraction between oppositely charged ions.
- Metallic Bond: Attraction between metal ions and delocalized electrons.
Common Confusions
- Confusing covalent bonds with ionic bonds due to both involving electrons.
- Mistaking metallic bonds for ionic bonds because both involve charged particles.
Typical Exam Questions
- What is a covalent bond? A covalent bond is the sharing of electron pairs between atoms.
- How do ionic bonds form? Ionic bonds form through the transfer of electrons from one atom to another, creating charged ions.
- Why do metals conduct electricity? Metals conduct electricity due to the presence of free-moving delocalized electrons.
What Examiners Usually Test
- Understanding of how different types of bonds form.
- Ability to distinguish between covalent, ionic, and metallic bonds.
- Knowledge of properties resulting from different types of bonding.