2How much an element reacts depends on… Electron ConfigurationOxygen vs. NeonElectron Configuration: 1s22s22p4Orbital Diagram for NeonElectron Configuration: 1s22s22p6Oxygen: 2p orbital only has 4 electrons can hold 6 electronsNeon: Has a full 2p electron orbital or shell with 6 electrons
3Octet RuleA concept of chemical bonding theory that atoms tend to have either an empty valence shell or full valence shell of 8 electrons. All atoms try to get an octet, 8 electrons in their outermost shell by either losing or gaining electrons. This is an attempt to have the electron configuration of a noble gas.*Valence shell: the electrons found in the outermost shell of an atom.OrbitalElectronss2p6d10f14
4Alkali Metals and Halogens Most reactive elementsOuter s and p orbital that do not match the Noble gases will react to lose or gain an electron…so the outer orbital will be full.
5Cations and Anions Cation: atoms lose electrons Usually metalsAnion: atom gains electronsUsually non-metalsIons form in order to achieve an octet (or as close as possible).Ions have different properties than their parent atoms.
17Ionic compounds Do not consist of molecules Bonds are strong, multiple attractionsHigh melting point and boiling pointHard and BrittleConduct electricity (if ions are mobile, in other words melted or dissolved in water)