Chemical Nomenclature

Basic Types of Compounds Ionic compound Binary ionic Polyatomic cation/anion Transition metals Molecular compounds Binary molecular Acid/Base compounds Binary acids Oxyacids

Ionic Compounds Cations – named first in compound Name as written on periodic table Group 1A -3A Metals + charge K+, Ca2+, Al3+ Name the above Transition Metals – named with roman number to represent charge Fe3+, Cu2+, Cr2+ Name the above (be careful!!)

Ionic Compounds (cont) Anions Non-metals ‘-’ charge Group 4A-7A Name element as is with ending of –ide Example – O-2 oxygen  oxide Br -, C -4, S-2 Name the above

Ionic and covalent compounds Polyatomic ions Combination of covalently bonding elements Combine with metal or nonmetal element or another polyatomic ion + polyatomic ion NH4+ - polyatomic ions Many – remember polyatomic ion sheet Name polyatomic ions as is – DO NOT CHANGE THEIR NAME

Common Polyatomic Ions ..\..\All Classes\Polyatomic Ion List.doc ..\..\All Classes\COMMON POLYATOMIC IONS.doc

Practice NH4NO3 Al(NO3)3 Mg3(PO4)2

Ionic Compounds (cont) Transition metals Groups 3-12 Name of metal + (roman numeral) Roman numeral Charge of metal Determine charge from non-metal and subscripts Example CrO  Chromium (II) oxide Oxygen charge -2 Name the following PbS, MnO2, Co2O3

Molecular Compounds Combination of two or more nonmetals or highly electronegative elements or group of elements Electrons are shared Types Binary molecular compound Polyatomic compound Acid/Base compound

Binary Covalently Bonded Compounds 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 9 Nona 10 Deca Use of prefixes

Molecular Compounds 2 non-metals Name 1st non-metal as is Name 2nd non-metal with –ide ending Prefixes indicate # of atoms of each element Example P2O5  Diphosphorus pentoxide Name the following CO2 , SO3 , XeF6 , N2O

Molecular Compounds Examples NH3  ammonia

hydrates

Single bonded carbon and hydrogen compounds Organic Compounds Meth- C Eth- C2 Prop- C3 But- C4 Pent- C5 Hex- C6 Hept- C7 Oct- C8 Non- C9 Dec- C10 Single bonded carbon and hydrogen compounds

Organic Compounds Single bonded ending Single bonded Double bonded -ane Ex: CH4 Methane Double bonded -ene Triple bonded -yne Single bonded CnH2n+2 Double bonded CnH2n Triple bonded CnHn

Examples

Acids and Bases Acids Binary Acids Hydrogen and one other element H  hydro Name other element ending –ic followed by acid Example HCl  Hydrochloric acid

Acids/Bases (cont) Oxyacids Acids containing oxyanion – a polyatomic ion containing oxygen Pay attention to ending of polyatomic ion Ending –ate  -ic acid -ite  -ous acid Examples HNO3  nitric acid Name the following H3 PO4 , HF, HClO3 , HClO2 , H2S

Common Acids

Bases No special naming rules Most end in –OH group Exception Name this polyatomic ion – Exception NH3  Organic bases  non covered except in lab