1. Chemical Nomenclature

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

3. 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!!)

4. 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

5. 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

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

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

8. 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

9. 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

10. Binary Covalently Bonded Compounds1
Mono 2 Di 3
Tri 4
Tetra 5
Penta 6
Hexa 7
Hepta 8
Octa 9
Nona 10
Deca
Use of prefixes

11. 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

12. Molecular Compounds
Examples
NH3  ammonia

13. hydrates

14. 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

15. 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

16. Examples

17. 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

18. 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

19. Common Acids

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