1. “How Do We Name Compounds?”
Nomenclature
“How Do We Name Compounds?”

2. Systematic Naming Compounds are made up of two or more elements
Name should tell us how many and what type of atoms
Too many compounds to remember all the names

3. Metals

4. Metals Qualities of Metals Luster – shiny
Ductile – think making it into wires
Malleable – hammer it into sheets
Good conductors of heat and electricity

5. Transition Metals

6. Non-metals

7. Metalloids or Semimetals

8. Cation Anion Positive ion Formed by losing electrons
Metals form cations
Anion
Negative ion
Has gained electrons
Non metals form anions

9. Ionic Compounds Made of cations and anions Metals and nonmetals
Electrons lost by the cation are gained by the anion

10. Ionic Compounds Cl Na + Na + Cl Sodium is cation Chlorine is anion 1-1+
Na +
Na + Cl
Chlorine is anion

11. Charges on Ions

12. Naming Ions Metal ion is written first in both name and formula
It is named directly from element which formed the ion.
Will nearly always be the positive ion or “cation”
Transition metals can have more than one type of charge
Indicate the charge with roman numerals in parenthesis. Iron(II) or Iron(III)
Exceptions:
Silver always +1
Cadmium and Zinc always +2

13. Name these Na 1+ Ca 2+ Al 3+ Fe 3+ Fe 2+ Pb 2+ Li 1+ Sodium Calcium
Aluminum
Iron (III)
Iron (II)
Lead (II)
Lithium

14. Write Formulas for these
Potassium ion
Magnesium ion
Copper (II) ion
Chromium (VI) ion
Barium ion
Mercury (II) ion
K1+
Mg2+
Cu2+
Cr4+
Ba2+
Hg2+

15. Naming Anions Anions are always the same.
Change the element ending to -- ide
F1- Fluorine to Fluoride

16. Name These Chloride Cl1- Nitride N3- Bromide Br 1- Oxide O2- Iodide
Strontium
Cl1-
N3-
Br 1-
O2-
I1-
Sr2+

17. Write These Sulfide ion Iodide ion Phosphide ion Strontium ion S2- I1-
Sr2+

18. Polyatomic Ions Tightly bound groups of atoms acting as a single ion.
Names given in table in book. (pg 123)
Most are anions that contain oxygen. Names end in –ate (one more O), or –ite (one less O).
SO32- = sulfite; SO42- = sulfate
Exceptions: Ammonium cation NH4+, Cyanide CN-, and hydroxide OH-

19. Naming Binary Ionic Compounds
2 elements involved
Ionic – metal (cation) and a non-metal (anion)
Naming is easy with representative elements in A groups
NaCl = Na+ Cl- = sodium chloride
MgBr2 = Mg2+Br- = magnesium bromide

20. Naming Binary Ionic Compounds
The problem comes with the transition metals.
Need to figure out their charges
All ionic compounds will have a neutral charge
Same number of + and – charges
Use the anion to determine the charge on the positive ion.

21. Naming Binary Ionic Compounds
Try naming these
KCl
Na3N
CrN
ScP
PbO
PbO2
Na2Se
Potassium chloride
Sodium nitride
Chromium (III) nitride
Scandium (III) phosphide
Lead (II) oxide
Lead (IV) oxide
Sodium selenide

22. Ternary Ionic Compounds
Will have polyatomic ions
At least 3 elements
Use blue sheet
Name these ions
NaNO3
CaSO4
CuSO3
(NH4)2O
LiCN
Fe(OH)3
(NH4)2CO3
NiPO4
Sodium nitrate
Calcium sulfate
Copper (II) sulfite
Ammonium oxide
Lithium cyanide
Iron (III) hydroxide
Ammonium carbonate
Nickel (III) phosphate

23. Writing Formulas Net charge must add to zero.
Get charges of cation/anion
Balance the charges
Put polyatomics in parenthesis

24. Writing Formulas Write formula for calcium chloride Calcium is Ca2+
Chloride is Cl1-
Ca+2Cl-1 would have a +1 charge
Need another Cl1-
Ca+2Cl2-1 = CaCl2

25. CaCl2 Ca2+ Cl1- Fe 3+ S2- Fe 2 S3 Writing Formulas Fe2S3
Crisscross method
Calcium chloride
CaCl2
Ca2+ Cl1-
No need to write the one
Iron (III) sulfide
Fe 3+ S2-
Fe 2 S3
Fe2S3

26. Write Formulas for These
Lithium sulfide
Tin (II) oxide
Tin (IV) oxide
Magnesium fluoride
Copper (II) sulfate
Iron (III) phosphide
Iron (III) sulfide
Ammonium chloride
Ammonium sulfide
Li2S
SnO
SnO2
MgF2
CuSO4
FeP
Fe2S3
(NH4)Cl
(NH4)2S

27. Things to Look For
If cations have ( ), the roman numeral is their charge.
If anions end in –ide they probably are off the periodic table (monoatomic)
If anion ends in –ate or –ite it is a polyatomic ion