1. Chapter 7
Nomenclature
CHM130
GCC

2. Nomenclature
We will be presenting this chapter a bit different than the text book does. The information is the same, so reading the text is still a good idea. But take an especially careful look at the online notes for this chapter. Good luck! 

3. Terms Ionic compound = metal + nonmetals
Covalent compound = nonmetals only, (aka molecular)
Monoatomic ion = one atom w/charge
Na+, Cl-, Ca2+
Polyatomic ion = two or more atoms w/charge (listed on your Periodic Table – become familiar with them)
PO43-, OH-, CO32-

4. Element Names Know the names for elements 1-20 AND Barium Ba Silver Ag
Cobalt Co Gold Au
Iodine I Zinc Zn
Copper Cu Tin Sn
Iron Fe Strontium Sr
Lead Pb Nickel Ni
Mercury Hg Bromine Br

5. Ionic Compounds
We will begin by learning formulas and names for ionic compounds
Remember that ionic compounds are made of ions, and ions have a charge
The sum of the charges must = zero

6. Oxidation States Is a fancy name for charge
All elements have a charge of zero when they are alone (elemental state)
Elements have a charge when they have lost or gained electrons
Some elements have a fixed charge – only one possibility
Other elements have variable charge – several possibilities

7. Cations Metals lose electrons to be cations (+) Charges (learn these)
Column IA is always +1 (alkali metals)
Column IIA is always +2 (alkaline earth metals)
Column IIIA is often +3 (Al always)
Zn and Cd always +2
Silver always +1
Other metals can vary from +1 to +9 so use Roman Numeral to tell the difference like Cu+2 is copper(II), Fe+3 is iron(III), Pb+4 is lead(IV)

8. Anions Nonmetals gain electrons to be anions (-) Charges (learn these)
Column 5 is –3 usually
Column 6 is –2 usually
Column 7 is –1 usually (F always)
Column 8 is 0 Why???
Noble gases are already happy with 8 outer valence electrons (He has 2) so don’t need to form bonds – they don’t want to gain or lose electrons!!!

9. 7.3 Polyatomic Ions Check out information on your periodic table
Keep these atoms together as a group, think of them as a group, a single entity

10. Formulas of Ionic Compounds
Compounds MUST be neutral
Need enough cations and anions to = zero
Combine Na and N: Na is +1 and N is –3 so need three Na’s for one N so Na3N is the formula
What is the formula?
Na and S
Mg and O
K and Br
Ca and N
Al and Cl
Zn and I
Cu(II) and O
Na2S
MgO
KBr
Ca3N2
AlCl3
ZnI2
CuO

11. Formulas with Polyatomic Ions
What is the Formula?
Mg and OH-
K and PO43-
Ag and SO42-
Ca and NO3-
Cu(II) and CO32-
Pb(IV) and O
Mg(OH)2
K3PO4
Ag2SO4
Ca(NO3)2
CuCO3
PbO2

12. Naming Ionic Compounds
Now that you can write ionic compound formulas, we need to learn their names
The name depends on whether the metal has a fixed or variable charge
For a fixed charge metal, like Na, we KNOW the charge so don’t use Roman numerals
For a variable charge metal, like Cu, we don’t know the charge so we do use Roman numerals
Check it out…

13. Fixed charge metal ionic compound
Metal name + nonmetal + “ide”
NaCl sodium chloride
What is the name?
KBr
MgO
CaF2
Li2S
AgCl
Note the ionic name does NOT indicate how many atoms there are
Potassium bromide
Magnesium oxide
Calcium fluoride
Lithium sulfide
Silver Chloride

14. Names with Polyatomic Ions
Do NOT change the polyatomic ion name
NaNO3 sodium nitrate
What is the name?
K3PO4
Ca(OH)2
ZnSO4
Potassium phosphate
Calcium hydroxide
Zinc sulfate

15. Variable charge Metal Ionic Compound
Metal name (Roman #) + nonmetal + “ide”
YOU must figure out charge on Trans metal
CuCl2 copper(II) chloride (Cu must be +2 since Cl is –1 and there are two of them)
What is the name?
PbO2
FeBr3
CoSO4
HgNO3
CoN
Lead(IV) oxide
Iron(III) bromide
Cobalt(II) sulfate
Mercury(I) nitrate
Cobalt(III) nitride

16. YOU must figure out the formula AND the name for ionic compounds.
Name only for covalent compounds (Why? They don’t have ions so you can’t add to zero)
Example: K and O
You figure out formula:
You figure out name:
K2O
Potassium oxide

17. Covalent / Molecular Compounds
Compounds with only nonmetals
These are NOT ions, so no charges
Use prefixes
mono -penta
di -hexa
tri -hepta
tetra -octa
Prefix + nonmetal name + prefix + 2nd nonmetal name + “ide”
Don’t use mono for the 1st nonmetal

18. Examples CO2 is carbon dioxide What is the name? CO P2O5 PF3 IF7
Carbon monoxide
Diphosphorus pentoxide
Phosphorus trifluoride
Iodine heptafluoride

19. Given the formula, write the name and vice versa
Br3O8
P4S7
SO3
Iodine hexafluoride
Dichlorine pentaoxide
P2I4
Tribromine octaoxide
Tetraphosphorus heptasulfide
Sulfur trioxide
IF6
Cl2O5
Diphosphorus tetraiodide

20. Reminders Prefixes are ONLY with covalent compounds
Roman Numerals are ONLY with variable charged metal compounds
Polyatomic ions NEVER change their name

21. Acids Compounds that lower pH in water Have H+ ions in them
Dissolved in water = (aq)
You should memorize these 6 acids
HCl(aq) hydrochloric acid
HF(aq) hydrofluoric acid
H2SO4 (aq) sulfuric acid
H3PO4 (aq) phosphoric acid
HNO3 (aq) nitric acid
H2CO3 (aq) carbonic acid

22. What the heck is (aq)?

23. Write the formula or name for each – you have 3 minutes!
Barium chloride
Nitrogen dioxide
Iron(II) phosphate
I2O4
Ag2SO4
Ni2S3
BaCl2
NO2
Fe3(PO4)2
Diiodine tetraoxide
Silver sulfate
Nickel(III) sulfide

24. Do the chapter 7 worksheet posted on this practice problems web page
Seriously – JUST DO IT
Self Test
Page 196
Try 4, 6, 9, 11
Answers in Appendix J