Ionic Compounds
- Solid ionic compounds have no moving charged particles, they do not conduct
- Liquid and aqueous ionic compounds have free moving charged particles (ions) in solution which can carry charge under the influence of an electric
| Ionic Bond | Covalent Bond | |
| Bonding | – Results from the attraction between positive and negative ions
– Occurs when a metal reacts with a non-metal |
– Formed by the sharing of electrons between atoms
– Occurs when two non-metals react |
| Properties | – Does form ions so it will conduct electricity as liquid or aqueous
– Forms a crystal lattice structure – Has a high melting point |
– Does not form ions so does not conduct electricity
– Forms a shared electron structure – Has a low melting and boiling point |
Intermolecular – these are attractions between molecules when they are close together and are broken when substances melt or boil.
Intramolecular – this refers to the covalent bonding. These bonds are only broken during a chemical reactions and never when melting or boiling. There are three varying degrees of strength of these bonds that depend on the type of molecules:
- Temporary dipole attractions – the weakest attraction between non-polar molecules
- Permanent dipole attractions – the next strongest attraction between polar molecules
- Hydrogen bonding – strongest attraction between polar molecules and extremely reactive non- metals (like F, O, or N)
Physical Changes – when the appearance/form of the substance changes but the actual identity and characteristics of the substance remain the same
Chemical Change/Reaction – when substances chemically combine and alter one another forming new substances with different properties and characteristics.