| A | B |
|---|
| Three Main Types of Bonding | Ionic, metallic, covalent |
| Occurs when a metal will lose an electron to a nonmetal, results in a cation and an anion, held together by electrostatic attraction | Ionic Bonding |
| What hold together the ion of a cation and anion | Electrostatic Attraction |
| Characteristics of Ionic Compounds | Solid crystals, brittle, high melting points, high boiling points, water soluble, electrolytes |
| Can conduct electricity when molten or dissolved in water | Electrolytes |
| The charge of the cation must balance out the charge of the anion to determine the formula unit | Formation of an ionic compound |
| Indicates the ratio of cation to anion in any ionic compound | Formula Unit |
| Groups of atoms that are covalently bonded, but carry an overall net charge | Polyatomic Ions |
| NO3^-1 | Nitrate |
| CO3^-2 | Carbonate |
| OH- | Hydroxide |
| SO4^-2 | Sulfate |
| PO4^-3 | Phosphate |
| The energy released when one mole of an ionic crystalline compound is formed from gaseous ions | Lattice Energy |
| Consists of positively charged metallic cations that donate electrons to the "sea" | Metallic Bonding(Electron Sea Model) |
| Are shared by all atoms and can move throughout the structure | The "sea" of electrons |
| Thermal conductivity, electrical conductivity, malleability, ductility | Properties of metals |
| Matter, lower melting and boiling points | Properties of covalent compounds |
| Occurs when atoms are bound together to form a discrete molecule, have lower melting points and are nonconducters | Molecular Covalent Bonding |
| Occurs when atoms are bound to multiple atoms to form a complex structure | Network Covalent Bonding |
| The distance between two bonded atoms at the minimum potential energy | Bond Length |
| The energy required to break a chemical bond | Bond Energy |
| Occurs when there is more than one valid Lewis Structure | Resonance |
| Compounds with the same molecular formula but different structural formulas | Isomers |
