Summary
Covalent bonding involves the sharing of electrons between non-metal atoms to form stable compounds. The strength of these bonds comes from the electrostatic attraction between the nuclei and shared electrons.
- Covalent Bonding — a type of chemical bonding where electrons are shared between atoms. Example: Water (H2O) has covalent bonds between hydrogen and oxygen.
- Coordinate (Dative) Bonding — a covalent bond where one atom provides both electrons. Example: In ammonium ion (NH4+), nitrogen donates a pair of electrons to hydrogen.
- Giant Covalent Structures — large networks of atoms bonded covalently. Example: Diamond and graphite are both giant covalent structures of carbon.
- Electronegativity — the ability of an atom to attract electrons in a bond. Example: Fluorine has a high electronegativity, attracting electrons strongly.
- Bond Polarity — occurs when there is a difference in electronegativity between bonded atoms. Example: In HCl, chlorine is more electronegative, creating a polar bond.
- Permanent Dipole-Permanent Dipole Forces — attractions between molecules with permanent dipoles. Example: Water molecules attract each other through these forces.
Exam Tips
Key Definitions to Remember
- Covalent Bonding: Sharing of electrons between non-metal atoms.
- Coordinate Bonding: A covalent bond where one atom provides both electrons.
- Electronegativity: The ability of an atom to attract electrons.
- Bond Polarity: A difference in electronegativity between bonded atoms.
Common Confusions
- Confusing covalent bonds with ionic bonds, which involve electron transfer.
- Misunderstanding that coordinate bonds are a type of covalent bond.
Typical Exam Questions
- What is covalent bonding? Covalent bonding is the sharing of electrons between non-metal atoms.
- How does electronegativity affect bond polarity? Differences in electronegativity create polar bonds with dipole moments.
- Describe a giant covalent structure. A giant covalent structure is a large network of atoms bonded covalently, like diamond.
What Examiners Usually Test
- Understanding of how covalent bonds form and their properties.
- Ability to explain the concept of electronegativity and its effects.
- Knowledge of examples of giant covalent structures and their uses.