AP Nomenclature
Common Ions and Nomenclature
 Memorize the AP Common Ions Memorizing the list of ions is not difficult, but it does take
time. You are unlikely to pass the ion test if you wait until September to start memorizing.
Many people like using flash cards.
 Learn correct spellings, formulas and charges
 Be able to read charges for type I ions from the periodic table
 First test: Fri Sept 4. I will give you names of ions, you will write the formulas and charges.
 Second test: Fri Sept 11. I will give you compound names (you write the formulas) and
compound formulas (you write the names). Yes, spelling counts. Capitalization also counts.
1st year chemistry nomenclature notes [Summary is first, complete notes plus practice follow]
Compound Types
I.
II.
III.
Identify the type by looking at the first half of the compound
Ionic: metal (known charge) + nonmetal
 Name the metal, then the nonmetal
 Nonmetal has –ide ending.
CaCl2: calcium chloride
Ca3(PO4)2: calcium phosphate
Ca3P2: calcium phosphide
Ionic: metal (variable charge) + nonmetal
 Identify the charge of the metal
 Name the metal, put the charge in () as a Roman numeral
 Name the nonmetal (-ide ending).
Fe2O3: iron(III) oxide
CuO: copper(II) oxide
Cu2O: copper(I) oxide
Covalent: nonmetal + nonmetal
 Use prefixes to identify the relative number of atoms in the compound.
 First element: use element name; second: use –ide ending (like anions)
 ‘Mono’ is not used for the first element.
 Some names use contractions: monoxide, not monoxide.
1: mono
2: di
3: tri
4: tetra
5: penta
6: hexa
7: hepta
8: octa
9: nona
10: deca
BF3
N2O5
CCl4:
NO2:
IV.
boron trifluoride
dinitrogen pentoxide
carbon tetrachloride
nitrogen dioxide
Acids: H + anion
Without oxygen:
HCl: hydrochloric acid
H2S: hydrosulfuric acid
With oxygen:
H2SO4: sulfate ion  sulfuric acid;
H2SO3: sulfite ion  sulfurous acid
5 Nomenclature
Longer version
Early chemists made up names for compounds without a system:
sugar of lead; blue vitriol; quicklime; Epsom salts; milk of magnesia; gypsum; laughing gas
Nomenclature: naming system; name describes the composition of the compound
5.1 Naming Compounds
Binary compounds: compounds composed of two elements
Compound Types
I.
Ionic: metal (known charge) + nonmetal
Name the metal, then the nonmetal; nonmetal has –ide ending.
CaCl2: calcium chloride
Ca3(PO4)2: calcium phosphate
Ca3P2: calcium phosphide
CsF:
cesium chloride
AlCl3: aluminum chloride
MgI2: magnesium iodide
II.
Ionic: metal (variable charge) + nonmetal
Identify the charge of the metal; name the metal, put the charge in () as a Roman
numeral; name the nonmetal (-ide ending).
Copper has more than one possible charge. The charge must be added to the name.
CuO: copper(II) oxide
Cu2O: copper(I) oxide
Fe2O3: iron(III) oxide
5.2 Naming Binary Compounds that contain a Metal and a Nonmetal (Types I and II)
Some metal atoms can form two or more cations:.
Type I compounds: the metal present forms only one type of cation
Na is always 1+
Type II compounds: the metal present can from two (or more) cations that have different charges
Cr can form Cr2+ and Cr3+; Cu can form Cu+ and Cu2+
Naming Type I Ionic Compounds
1. Cation is first, then the anion.
2. Cations (except the polyatomic one) take their names from the element name.
3. Anions from a single atom are named by adding –ide to the root of the name.
Ex 5.1 Type I binary compounds
Compound formula
ions
CsF
Cs+
FAlCl3
Al3+
ClMgI2
Mg2+
I-
ion names
cesium
fluoride
aluminum
chloride
magnesium
iodide
compound name
cesium fluoride
aluminum chloride
magnesium iodide
Type II binary compounds
When a cation has variable charges, the specific charge needs to be in the compound name.
Use roman numerals to give the charge.
Fe2+ or Fe3+?
[charge on Fe?] + 2(1-) = 0
charge is 2+
+
Cl
2 + 2 = 0 [no net charge for compound]
Name: iron (II) chloride
Since there are two chloride ions, the iron must have a charge of 2 + to result in a neutral compound.
* Note that the II refers to the charge, not the subscript number*
FeCl3 = iron (III) chloride
Ex
FeCl2
Ex.
PbO2
Lead (IV) oxide
Alternate system:
O2-
Pb?+ + 2(2-) = 0; Pb4+
The ion with the higher charge has a name ending in –ic;
The ion with the lower charge has a name ending in –ous.
Fe3+ = ferric
Fe2+ = ferrous
Ex. 5.2 Type II binary
a.
CuCl
b.
HgO
c.
Fe2O3
d.
MnO2
e.
PbCl4
Cu?+
ClHg?+
O2Fe?+
O2Mn?+
O2Pb?+
Cl-
6+
64+
44+
4-
Cu+
copper (I) chloride
Hg2+
mercury (II) oxide
Fe3+
iron (III) oxide
Mn4+
manganese (IV) oxide
Pb4+
lead (IV) chloride
Rules: 1. Cation first, then anion 2. Because the cation can have more than one charge, specify the charge
with a roman numeral in parentheses.
5.3 Naming Binary Compounds that Contain Only Nonmetals (Type III)
Covalent: nonmetal + nonmetal
What would make good names for NO and NO2?  need a way to distinguish these two ‘nitrogen oxides’
Rules for Naming Type III Binary Compounds
1. The first element in the formula is named first (full element name).
2. The second element is named as though it were an anion.
3. Prefixes are used to denote the numbers of atoms present.
4. The prefix mono- is never used for naming the first element. For example, CO is called carbon
monoxide, not monocarbon monoxide.
BF3
NO
N2O5
CCl4:
NO2:
IF3:
boron trifluoride
nitrogen monoxide [aka nitric oxide]
dinitrogen pentoxide
carbon tetrachloride
nitrogen dioxide
iodine trifluoride
1: mono
2: di
6: hexa
7: hepta
3: tri
8: octa
4: tetra
9: nona
5: penta
10: deca
5.4 Naming Binary Compounds: Strategy / Review
* Use the periodic table to determine which elements are metals, nonmetals and transition metals.
5.5 Naming Compounds that Contain Polyatomic Ions
Polyatomic ions: several atoms bound together (covalently) that have a charge
Oxyanions
=Polyatomic ions that contains an atom of an element, and different numbers of oxygen
The ion with a smaller number of oxygen atoms has an –ite ending
The ion with a bigger number of oxygen atoms has an –ate ending
If there are more than 2 oxyanions in a series, hypo- (less than) and per- (more than) are used as
prefixes to indicate the ion with the fewest number of oxygen, and the one with the most
Ex.
ClOhypochlorite
ClO2- chlorite
ClO3- chlorate
ClO4- perchlorate
5.6 Naming Acids
Acids: compounds that produce H+ ions when dissolved in water (~ molecules with H+ attached to anions)
Rules for naming acids (depend on whether the anion contains oxygen)
1. If the anion does not contain oxygen, the acid is named with the prefex hydro- and the suffix –ic
attached to the root name for the element.
2.
a.
HCl (hydrogen chloride), when dissolved in water forms hydrochloric acid
b.
HCN (hydrogen cyanide), when dissolved in water forms hydrocyanic acid
c.
H2S (hydrogen sulfide), when dissolved in water forms hydrosulfuric acid
When the anion contains oxygen, the acid name is formed from the root name of the central
element of the anion or the anion name, with a suffix of –ic or –ous. When the anion name ends in
–ate, the suffix –ic is used; when the anion name ends in –ite, the suffix –ous is used.
a.
H2SO4
SO42- sulfate
sulfuric acid
b.
H3PO4
PO43- phosphate
phosphoric acid
c.
HC2H3O2
C2H3O2- acetate
acetic acid
d.
H2SO3
SO32- sulfite
sulfurous acid
e.
HNO2
NO2- nitrite
nitrous acid
Acids: starts with H
Without oxygen:
HCl: hydrochloric acid
H2S: hydrosulfuric acid
With oxygen:
H2SO4: sulfate ion  sulfuric acid;
H2SO3: sulfite ion  sulfurous acid
Nomenclature practice
Write the names for these compounds.
1.
I2O7
2.
CO2
3.
CF4
4.
NH3
5.
PCl3
6.
PCl5
7.
P4O6
8.
SF6
9.
SO3
10. SO2
11. N2O3
12. CO
13. NO2
14. SeF6
15. SiO2
16. H2O
17. CuO
18. SrO
19. B2O3
20. K2S
21. AsF3
22. Al2S3
23. SnBr4
24. CS2
25. CdS
26. AgCl
27. KI
28. NO
29. P2O5
30. FeCl3
31. ClF3
32. CuCl
33. MnO2
34. MgO
Naming Practice
1.
Ca(OH)2
2.
Na3PO4
3.
KMnO4
4.
(NH4)2Cr2O7
5.
Co(ClO4)2
6.
KClO3
7.
Cu(NO2)2
8.
PbCO3
9.
KHSO4
10. NH4I
11. NaCN
12. H3PO3
13. Na2CO3
14. FeBr3
15. HF
16. CsClO4
17. PCl3
18. H2S
19. CuSO4
20. Ca(HCO3)2
21. MgI2
22. KMnO4
23. HBrO4
24. Fe(OH)2
25. NaHCO3
26. BaSO4
27. HNO3
28. BrF5
29. NaBr
30. Zn3(PO4)2
Naming Practice
1.
Fe2O3
11. HF
2.
CsCl
12. MgCO3
3.
NaCN
13. PbO
4.
P2S3
14. NH4NO3
5.
H2S
15. BaSO4
6.
Cu(NO3)2
16. Li2CO3
7.
Ag2S
17. H3PO4
8.
SnBr4
18. K2Cr2O7
9.
Ca3(PO4)2
19. HNO3
10. Ba(OH)2
21. Diboron trioxide
22. Hydrochloric acid
23. Calcium acetate (calcium ethanoate)
24. Sodium hydroxide
25. Copper (II) permanganate
26. Aluminum phosphate
27. Silicon dioxide
28. Magnesium oxide
29. Ammonium hydroxide
30. Sodium carbonate
31. Cobalt (III) nitrate
32. Sulfuric acid
33. Calcium chloride
34. Lead (IV) oxide
35. Dinitrogen pentoxide
36. Silver chloride
37. Iron (II) oxide
38. Hydrosulfuric acid
39. Ammonium sulfate
40. Sulfur hexafluoride
20. MnSO4
Name Compound Types I, II, III and acids
1.
KClO3
7.
NH4I
2.
NaBr
8.
H2SO4
3.
SrO
9.
CuSO4
4.
B 2O 3
10. Ca(HCO3)2
5.
HBr
11. MgI2
6.
PbCO3
12. BrF5
Write formulas from names
For ionic compounds, write ions with charges, then combine, using subscripts and parentheses as
necessary.
13. barium carbonate
23. disulfur dichloride
14. hydrochloric acid
24. nitric acid
15. potassium hydroxide
25. lithium iodide
16. sodium carbonate
26. aluminum oxide
17. cobalt (III) nitrate
27. sodium nitrate
18. calcium chloride
28. ammonium hydroxide
19. lead (IV) oxide
29. magnesium bromide
20. dinitrogen pentoxide
30. carbon disulfide
21. ammonium phosphate
31. cobalt (II) chloride
22. ammonium sulfate
32. cesium fluoride
Nomenclature: Types I, II and III
Write the names for the following compounds.
1.
KCl
2.
CO2
3.
CoCl3
4.
CaO
5.
PbBr4
6.
CO
7.
CsCl
8.
PCl5
9.
CuI2
10. SF6
11. Fe2O3
12. PbS
13. FeO
14. SnBr4
15. LiH
16. SO3
17. CaI
18. NO
19. KI
20. P4O6
21. NaF
22. CuCl
23. BaCl
24. N2O3
25. Al2S3
ch 5
Nomenclature
ch 5
Write the names for the following compounds.
1.
Ca(OH)2
9.
HC2H3O2
2.
K2S
10. Al2S3
3.
MgO
11. PbBr4
4.
HBr
12. CuSO4
5.
P2O5
13. HCl
6.
NaCN
14. PCl3
7.
NO
15. CuNO3
8.
FePO4
Write the chemical formulas. (For types I and II, write the ions with charges first, then combine)
16. Sodium sulfide
17. Nitrogen monoxide
18. Dinitrogen trioxide
19. Copper (II) chloride
20. Aluminum bromide
21. Iron (III) hydroxide
22. Carbon tetrafluoride
23. Potassium nitrate