Chemical Bonding Types and Properties
This comprehensive page explores the fundamental differences between ionic and covalent bonds, their formation processes, and characteristic properties. The content details how these bonds influence material behavior and chemical reactions.
Definition: Ionic bonds are chemical bonds formed between two ions with opposite charges through electron transfer, while covalent bonds involve the sharing of electron pairs between atoms.
Example: Sodium chloride (NaCl) demonstrates ionic bonding where sodium (Na) loses an electron to become Na+ and chlorine (Cl) gains an electron to become Cl-, forming an ionic lattice structure.
Highlight: Ionic compounds conduct electricity when molten or in aqueous solutions but not in solid state, whereas covalent compounds typically don't conduct electricity at all.
Vocabulary:
- Cations: Positively charged ions formed when atoms lose electrons
- Anions: Negatively charged ions formed when atoms gain electrons
- Giant lattice: A three-dimensional structural arrangement of ions in ionic compounds
The page illustrates different types of covalent bonds:
- Single bonds (H-H): Share 2 electrons
- Double bonds (O=O): Share 4 electrons
- Triple bonds (N≡N): Share 6 electrons
Key property comparisons are made between ionic and covalent compounds:
- Ionic compounds have high melting and boiling points due to strong electrostatic forces
- Covalent compounds typically have lower melting and boiling points due to weaker intermolecular forces
- Ionic compounds are usually water-soluble while covalent compounds tend to be insoluble
