1. BEWARE!!! There is a lot memorization involved with this chapter.
Chapter 4 Nomenclature
BEWARE!!!
There is a lot memorization involved
with this chapter.

2. In the old days compounds had common names like: water, milk of magnesia, gypsum, quicklime, etc.
Today we know of over 4 million compounds. Common names won’t work
Therefore we have a system!
First we will learn about binary compounds, compounds made of two elements
There are two classes:
1) metal/nonmetal (ionic)
2) nonmetal/nonmetal (covalent)

3. 4.1 Naming Compounds that Contain a metal and a Nonmetal
Metals tend to lose electrons e-,
Nonmetals gain electrons e-
Metals like to be positive +
Nonmetals like to be negative -
These get together to form binary ionic (M with NM) compounds

4. When writing the
formula the cation is
first, anion second
When naming just say their names
Some cations have only one charge ever (called Type I ion)
Some have more than one charge (Type II ion)
There are also Type I compounds and Type II compounds
KNOW YOUR IONS!!!

5. Type I Binary ionic compounds
Reviewing the rules:

6. Type II binary ionic compounds
Some cations can form more than one charge!!!
(Type II ion!)
Let’s look at an example….
iron can form 2+ and 3+ ions
so what is the iron in iron chloride? Fe2+ or Fe3+?
must be a way to distinguish the two!
use Roman numerals…

7. So what is the name of FeCl2?
Chloride always has a 1- charge, and there are two, so…
The positive guy must have a total 2+ charge, and…
There is only one cation so it get the whole 2+ charge all to itself, so…
It must be iron(II), so…
It is iron(II) chloride
Know Table 4.2 (the systematic is emphasized in this class!!)

8. examples CuCl copper(I) chloride HgO mercury(II) oxide Fe2O3
iron(III) oxide
Mn2O4
manganese(IV) oxide
PbCl4
lead(IV) chloride

9. summary of Type I and Type II

10. summary examples CoBr2 cobalt(II) bromide CaCl2 calcium chloride Al2O3
aluminum oxide
CrCl3
chromium(III) chloride
summary examples

11. 4.2 Naming Binary Compounds that Contain only Nonmetals (Type III)
Type III contain only NM!
think prefixes!
(note: water and ammonia are Type III but always keep their common names)

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

14. 4.3 naming binary compounds: a review

15. 4.4 Naming Compounds that contain Polyatomic Ions
There is another(!) type of compound, one that involves…
Polyatomic ions. Ions with more than one type of atom in it
gotta know Table 4.4

16. Notice many have O in them Called oxyanions
Most common is called root-ate (e.g. sulfate)
One less O than most common?
root-ite (nitrite)
One less than that?
hypo-root-ite (hypochlorite)
One more than most common?
per-root-ate (perchlorate)
Must be able to recognize Polyatomic ions!!!

17. examples Na2SO4 sodium sulfate Fe(NO3)3 iron(III) nitrate Mn(OH)2
parentheses here mean there are 3 of what’s inside. “NO33” is nonsense!
iron(III) nitrate
Mn(OH)2
manganese(II) hydroxide
examples

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

19. 4.5 Naming Acids
Some things when dissolved in water can lose an H+ right off them
called acids
taste sour
know these!
have their own name system…

21. 4.6 Writing Formulas from Names
so far we’ve done formulas to names…
now we do reverse! yippee!
you HAVE TO KNOW all the names I warned you about!!!

22. examples potassium hydroxide KOH sodium carbonate Na2CO3 nitric acid
HNO3
calcium chloride
CaCl2
dinitrogen pentoxide
N2O5
ammonium perchlorate
NH4ClO4
examples

23. if this helps, use it. if it doesn’t, don’t!