1. Chapter 4 Nomenclature

2. In the old days compounds had common names like: water, milk of magnesia, gypsum, quicklime, blue vitriol
Today we know of over 4 million compounds. Common names
won’t work
binary compounds are compounds made of two elements
There are two classes:
1) metal & nonmetal
2)nonmetal & nonmetal

3. 4.1 Naming Compounds that Contain a metal and a Nonmetal
Metals tend to… (electrons)
lose electrons
Nonmetals tend to… (electrons)
gain electrons
Metals will have a ______ charge
Nonmetals will be ________
These get together to form neutral
binary ionic compounds
There are 2 Types…
positive
negative

4. Type I Binary ionic compounds
The metals must be from Group 1, 2, or Al3+, Ga3+, In3+, Zn2+, Cd2+, Ag+
The cation (usually a metal) is listed first
and the anion (usually a nonmetal) second
The subscripts in the formula must produce an electrically neutral formula unit.
3. The subscripts are the smallest whole numbers possible.
4. The cation takes the name of its element
(e.g. Li+ would be called "Lithium“)
5. The anion name uses the first part of its elemental name, and subsequently adding the suffix "-ide".
(e.g. Br- would be called "Bromide“)

5. Anion
Name H-
Hydride F-
Fluoride
Cl-
Chloride
Br-
Bromide I-
Iodide
O2-
Oxide
S2-
Sulfide
Se2-
Selenide
N3-
Nitride
P3-
Phosphide
As3-
Arsenide
C4-
Carbide

6. Example
Cation
Anion
Formula Na Cl

7. Example
Cation
Anion
Formula
Na+
Cl-

8. Example
Cation
Anion
Formula
Na+
Cl-
NaCl

9. Example
Cation
Anion
Formula Ca Br

10. Example
Cation
Anion
Formula
Ca2+
Br-

11. Example
Cation
Anion
Formula
Ca2+
Br-
CaBr2

12. Example
Cation
Anion
Formula Na S

13. Example
Cation
Anion
Formula
Na+
S2-

14. Example
Cation
Anion
Formula
Na+
S2-
Na2S

15. Example
Cation
Anion
Formula Mg O

16. Example
Cation
Anion
Formula
Mg2+
O2-

17. Example
Cation
Anion
Formula
Mg2+
O2-
MgO

18. Example
Cation
Anion
Formula Al O

19. Example
Cation
Anion
Formula
Al3+
O2-

20. Example
Cation
Anion
Formula
Al3+
O2-
Al2O3

21. Questions? 21

22. Type II binary ionic compounds
Type II ions can form more than one cation
The substance on the right is iron chloride
iron canform either 2+ or 3+ ions
“but Mr. Farrin, how do we know
which iron is in iron chloride?
Fe2+ or Fe3+?”
“By the use of Roman numerals”
e.g. iron (III) chloride

23. Type II binary ionic compounds
Write the formula for iron (III) chloride
Fe3+ Cl1-
FeCl3 23

24. what is the name of FeCl2? Which iron is it?
Chloride always has a 1- charge, and there are two of them
To balance that, the positive ion must have a total charge of… 2+
There is only one cation so it must have the whole 2+ charge all to itself
Therefore it must be…
iron(II) chloride

25. Common Type II Cations Ion Systematic Name Fe3+ iron(III)
Cu2+ copper(II)
Cu+ copper(I)
Co3+ cobalt(III)
Co2+ cobalt(II)
Sn4+ tin(IV)
Sn2+ tin(II)
Pb4+ lead(IV)
Pb2+ lead(II)
Hg2+ mercury(II)
Hg22+ mercury(I)

26. examples CuCl copper(I) chloride mercury(II) oxide HgO
(what would mercury (I) oxide look like?)
Hg2O
Fe2O3
iron(III) oxide
Mn2O4
manganese(IV) oxide
lead(IV) chloride
PbCl4

27. Questions?

28. 4.2 Naming Binary Compounds that Contain only Nonmetals (Type III)
Type III contain only nonmetals
Prefixes are used to show how many atoms of each element are in each molecule
Number of Atoms
Prefix 1
mono 6
hexa 2 di 7
hepta 3
tri 8
octa 4
tetra 9
nona 5
penta 10
deca

30. examples BF3 boron trifluoride NO nitrogen monoxide
dinitrogen pentoxide
N2O5
PCl5
phosphorus pentachloride
sulfur hexafluoride
SF6
SO2
sulfur dioxide
examples

31. 4.3 naming binary compounds: a review

32. Questions? 32

33. 4.4 Naming Compounds that contain Polyatomic Ions
There is another type of compound, that involves ions
Polyatomic ions: ions with more than one type of atom
Notice many have O in them, they are called oxyanions

34. In order to recognize that polyatomic ions are present (when given names), look for the following:
root-ate
root-ite
hypo-root-ite
per-root-ate

35. examples Na2SO4 sodium sulfate Fe(NO3)3 iron(III) nitrate
manganese(II) hydroxide Mn2+ (OH)-
Mn(OH)2

36. examples Na2CO3 sodium carbonate iron(III) bromide FeBr3 PCl3
phosphorus trichloride
cesium perchlorate
CsClO4
CuSO4
copper(II) sulfate
examples 36

38. Nomenclature Flowchart

39. 4.5 Naming Acids What do we know about acids? taste sour pH below 7
react with most metals
turn blue litmus paper red
H+ donor
Acetic acid, (HC2H3O2)
Hypochlorous acid (HClO)
hydrochloric acid (HCl)

40. 4.5 Naming Acids When the anion does NOT contain Oxygen:
Acetic acid, (HC2H3O2)
Hypochlorous acid (HClO)
hydrochloric acid (HCl)
When the anion does NOT contain Oxygen:
Use the prefix hydro + root of the anion’s name – ic + the word acid
Example: HCl - hydrochloric acid

41. 4.5 Naming Acids When the anion contains Oxygen:
Acetic acid, (HC2H3O2)
Hypochlorous acid (HClO)
hydrochloric acid (HCl)
When the anion contains Oxygen:
The name will depend on the name of the polyatomic anion.
-ate → -ic + the word acid
-ite → -ous + the word acid

42. 4.5 Naming Acids Examples HBr hydrobromic acid H2SO4 sulfuric acid
sulfurous acid
Examples
hydroflouric acid HF
phosphoric acid
H3PO4
nitrous acid
HNO2

43. 4.5 Naming Acids
Questions?