Study Notes
Chemical bonding involves the interaction of atoms to form compounds, with different types of bonds affecting the properties of substances.
- Ionic Bonding — involves the transfer of electrons from metals to non-metals, forming cations and anions. Example: Sodium chloride (NaCl) forms from sodium donating an electron to chlorine.
- Covalent Bonding — involves the sharing of electrons between non-metal atoms to achieve a full outer shell. Example: Water (H2O) has covalent bonds between hydrogen and oxygen.
- Metallic Bonding — involves a lattice of metal cations surrounded by a sea of delocalized electrons. Example: Copper (Cu) exhibits metallic bonding, allowing it to conduct electricity.
Exam Tips
Key Definitions to Remember
- Ionic bonding involves electron transfer from metals to non-metals.
- Covalent bonding involves electron sharing between non-metals.
- Metallic bonding involves a lattice of cations and delocalized electrons.
Common Confusions
- Confusing ionic and covalent bonding due to electron transfer vs. sharing.
- Misunderstanding the role of delocalized electrons in metallic bonding.
Typical Exam Questions
- What is ionic bonding? Ionic bonding is the transfer of electrons from metals to non-metals.
- How do covalent bonds form? Covalent bonds form by sharing electrons between non-metal atoms.
- Why do metals conduct electricity? Metals conduct electricity due to the presence of delocalized electrons.
What Examiners Usually Test
- Understanding of electron transfer in ionic bonding.
- Ability to explain electron sharing in covalent bonds.
- Knowledge of the properties of metallic bonds and their effects on conductivity.