Key Terms
Representative elements
S and p orbitals are filling. Found in groups 1, 2, and 12-18.
Inner transition metals
F orbitals filling.
Passivation
A nonreactive oxide (or other compound) film forms on a metal surface and protects it from further reaction. Mg, Al, Zn,
Salt
Ionic compound of cations and anions. General rule - metal + nonmetal = salt.
All react vigorously with water
2M + 2H2O -> 2MOH + H2 (gas)
Zinc
Most reactive in group 12. Passivates via basic carbonate coating.
Sacrificial anode
A more active metal (more negative reduction potential) attached to the metal you want to protect. Corrosion happens at
Mercury
Only metal liquid at 25 C. Does NOT displace hydrogen from acids; it is less easily oxidized than most metals.
With acid
Al + HCl -> AlCl3 + H2 With base: Al + NaOH + H2O -> NaAlO2 + H2
Inert pair effect
Ga, In, Tl also exhibit 1+ oxidation state (two below expected 3+). The valence s orbital pair is unusually stable and r
Oxidation state
3+ in most stable compounds. sp2 hybridized in most compounds; trigonal planar geometry.
Purification for semiconductors
Zone refining - a thin molten zone is moved through a silicon rod; impurities dissolve in the melt and travel to one end
Silicates
Salts containing Si-O anions; sp3 Si at centers of tetrahedra; tetrahedra can share oxygen atoms in various ways to form
Example
N forms NF3 only; P forms both PF3 and PF5
Oxidation-reduction chemistry rules for nonmetals
1. Nonmetals oxidize most metals (metal -> positive oxidation state) 2.