1. Chemical Nomenclature
Section 2.2

2. -system used in chemistry to name compounds
Nomenclature
-system used in chemistry to name compounds
Ionic Compounds
Covalent Compounds

3. Naming Ionic Compounds
Binary compounds and
Polyatomic compounds

4. Binary Compounds
Binary Compounds- are inorganic compounds that contain elements
Write the full name of the cation (metal)
Write the root of the anion (non-metal) next to the cation
Write the ending –ide next to the root of the anion
Ex: AlCl3 = aluminum chlorine 
Aluminum chloride

5. Transition Metal Ions
Some elements may form more than one cation (ions with different charges), these are called multivalent ions.
You will indicate the charge of the ion by writing the charge in roman numerals after the cation name
Use the cross up rule to find charges!
Ex: Fe2O2 and Fe2O3
______________ and ______________

6. Multivalent (Two Valences)
Element
Ion
Stock System
Classical System
Copper
Cu+
Copper (I)
cuprous
Cu 2+
Copper (II)
cupric
Mercury
Hg+
mercury (I)
mercurous
Hg2+
mercury (II)
mercuric
Lead
Pb2+
lead (II)
plumbous
Pb4+
lead (IV)
plumbic

7. Example of Multivalents
Write the name using the classical system and the stock system for the following:
HgO PbO2
Write the chemical formula from the following names.
Cobaltic iodide stannous fluoride

8. Polyatomic Compounds Polyatomic Ions-
compounds that contains 3 elements (often called tertiary compounds).

9. Polyatomic Ions you should know!
Common Polyatomics
OH-  Hydroxide
NO2-  Nitrite
SO32-  Sulfite
ClO2 -  Chlorite
ClO3-  Chlorate
CO32-  Carbonate
NO3-  Nitrate
SO42-  Sulfate
PO43-  Phosphate
Weird Polyatomics
CN-  Cyanide
CH3COO-  Acetate
NH4+  Ammonium
Page 98 Table 3.4
MORE TO KNOW 

10. Naming Polyatomic Ionic Compounds
Naming a polyatomic ionic compound is a similar process to naming a binary compounds only the ending of the anion is given from the chart …and does not change!
Examples:
Ca(ClO2)2  Calcium Chlorite
Ca(ClO3)2  Calcium Chlorate

11. Naming Molecular Compounds

12. Molecular Compounds Molecular compounds= 2 non-metals
The system of naming molecular compounds is based on the use of prefixes

13. Pre-fixes you need to know
1  Mono-
2  Di-
3  Tri-
4  Tetra-
5  Penta-
6  Hexa-
7  Hepta-
8  Octa-
9  Nona-
10  Deca-

14. Naming Molecular Compounds
Prefixes are used to designate how many atoms of each element are present.
RULES:
NOTE: The prefix mono- is not used with the first elements name.
The first element is named with the appropriate prefix
The second element’s root name with the appropriate prefix and ending -ide

15. Examples Name the compound: N2O4 2 Nitrogens  Di-nitrogen
4 Oxygens  Tetra – oxy – ide
Dinitrogen Tetraoxide
Name the compound: SO2
1 Sulfur  Sulfur
2 Oxygens  Di – oxy – ide
Sulfur Dioxide

16. Naming Acids
(Chapter 10)

17. General Formula: HX (aq)
Naming Acids: Rules
There are 2 main kinds of acids:
1.binary acids
2. oxoacids
Binary Acids- composed of 2 elements
Hydrogen + non-metal
General Formula: HX (aq)
Examples: HF (aq) =hydrofluoric acid
HCl (aq) = hydrochloric acid

18. Naming Binary Acids
If the name of the anion ends in “–ide”, the acid name begins with the prefix “hydro-”, then the stem of the anion is given and finally the suffix “-ic” is added and is followed by the word “acid”.
Example: H2S (aq)
(anion: sulfide)  hydro + stem + ic + acid
Hydrosulfuric Acid

19. How do you know when to do this?
Naming Binary Acids
Every acid formula starts with “H”, as the cation. To name an acid, look at the anion the hydrogen is bonded to.
Name: HCl (aq) =hydrochloric acid
Prefix + root name of non-metal + suffix + “acid”
Hydro chlor ic + acid
How do you know when to do this?

20. General Formula: HXOn (aq)
What about these?
H2S anion = sulfide ion
H2SO anion = sulfite ion
H2SO anion = sulfate ion
Add one
more “O”
Oxoacids- an acid formed from a polyatomic ion.
Hydrogen + Oxygen +Element
General Formula: HXOn (aq)
Examples: HClO4 (aq)

21. “ITE”  “OUS” Naming Oxoacids
If the name of the anion ends in “–ite”, the acid name is the stem of the anion with the suffix “–ous” and is followed by the word “acid”.
H2SO3 (aq) Stop and think about the anion SO32-
(anion: sulfite)  stem + ous + acid
Sulfurous Acid

22. “ATE”  “IC” Naming Oxoacids
If the name of the anion ends in “–ate”, the acid name is the stem of the anion with the suffix “–ic” and is followed by the word “acid”.
H2SO4 (aq) Stop and think about the anion SO42-
(anion: sulfate)  stem + ic + acid)
Sulfuric Acid

23. Adding Oxygens Polyatomic Ion Prefix Suffix + acid hypo ous acid -
ClO-
hypo
ous acid
ClO2- -
ClO3-
ic acid
ClO4-
per

24. Writing Formulas/Naming Acids
Remember the following statements…
“I ate it and it was icky.”
-ate becomes -ic
“Rite ous” as (Righteous)
-ite becomes -ous

25. Naming Acids Flowchart Does the formula contain Oxygen?
No=Binary Acid
Yes=Oxoacid
Hydro “stem”ic acid
Anion end in __ ?
“ate”
“ite”
“stem”ic acid
“stem”ous acid

26. Writing Formulas for Acids
If the name starts with “hydro”
Hydroselenic Acid
Write the hydrogen ion with charge.
H+1
Write the anion with the proper charge.
Se-2
Balance the charges using subscripts.
H2Se (aq)

27. Writing Formulas for Acids
If the name contains the suffix “–ous”
Nitrous Acid
Write the hydrogen ion with charge. H+
Look up the polyatomic ion (nitrite) and write it with the correct charge.
NO2-
Balance the charges using subscripts.
HNO2

28. Writing Formulas for Acids
If the name contains the suffix “–ic” without the prefix “hydro”
Phosphoric Acid
Write the hydrogen ion with charge. H+
Look up the polyatomic ion (phosphate) and write it with the correct charge.
PO4-3
Balance the charges using subscripts.
H3PO4

29. Naming Bases
Bases are named using the traditional ionic naming system.
Metal name + polyatomic ion name
Examples:
Ca(OH)2 = calcium hydroxide
NaOH = sodium hydroxide
Al(OH)3 = aluminum hydroxide

30. Writing Base Formulas
Base formulas are written using the traditional ionic system.
Look up the metal ion. Write the symbol with the proper charge. Ca+2
Look up the polyatomic ion. With bases, this will always be hydroxide, OH-1.
Balance the charges using subscripts.
Ca(OH)2