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. SHORT CHAPTER
VERY IMPORTANT CHAPTER
THE REST OF THE YEAR YOU WILL BE EXPECTED TO KNOW THE CHEMICAL NAMES!
If you have a photographic memory this chapter will be a breeze
BUY FLASHCARDS!!

3. 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
2) nonmetal/nonmetal

4. 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 compounds

5. Type I Compounds Type I & Type II is referring to the cation
Type I cations only have 1 charge!
First 2 rows of the periodic table
NOTE – ALUMINUM(+3) AND SILVER(+1)

6. Questions
Aluminum is a group 3A metal. Which ion does Al typically form?
a. Al3- c. Al5-
b. Al3+ d. Al5+

7. Type I Examples CsF Cesium Fluoride AlCl3 Aluminum Chloride MgI2
Magnesium Iodide
CaS
Calcium Sulfide KI
Potassium Iodide
Sodium Iodide
NaI
Calcium Fluoride
CaF2
Lithium Oxide
Li2O
Aluminum Sulfide
Al2S3
Strontium Oxide
SrO

8. Type I Binary ionic compounds
Reviewing the rules:

9. Question What type of ions have names ending in -ide?
a. only cations c. only metal ions
b. only anions d. only gaseous ions

10. Questions What is the correct name for the N3- ion?
a. nitrate ion c. nitride ion
b. nitrogen ion d. nitrite ion

11. Questions
Which of the following formulas represents an ionic compound?
a. CS c. NO
b. BaI d. PCl

12. Questions
Which element, when combined with fluorine, would most likely form an ionic compound?
lithium c. phosphorus
b. carbon d. chlorine

13. 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…

14. 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!!)

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

16. examples FeI3 iron(III) iodide MnCl2 manganese(II) chloride HgO
mercury(II) oxide
Cu2O
copper(I) oxide
CuO
copper(II) oxide

17. summary of Type I and Type II

18. Questions What is the correct name for the compound CoCl?
a. cobalt(I) chlorate c. cobalt(II) chlorate
b. cobalt(I) chloride d. cobalt(II) chloride

19. Questions
 In which of the following is the name and formula given correctly?
a. sodium oxide, NaO c. cobalt (I) chloride, CoCl
b. barium nitride, BaN d. tin (IV) fluoride, SnF4

20. Questions Which of the following compounds contains the Mn3+ ion?
a. MnS c. Mn2O3
b. MnBr2 d. MnO

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

22. 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)

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

25. examples sulfur trioxide SO3 dinitrogen trioxide N2O3 silicon dioxide
SiO2
dioxygen diflouride
O2F2
tetraphosphorus hexoxide
P4O6
xenon hexaflouride
XeF6
examples

26. Questions
Which of the following formulas represents a molecular compound (molecular means between two non-metals)?
a. ZnO c. SO
b. Xe d. BeF

27. Questions Select the correct formula for sulfur hexafluoride.
a. S2F6 c. F6S2
b. FSO d. SF6

28. 4.3 naming binary compounds: a review

29. 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

30. -ate ClO3- SO42- PO43- NO3- CO32- THE ROOT, MOST IMPORTANT!
chlorate
SO42-
sulfate
PO43-
phosphate
NO3-
nitrate
CO32-
carbonate
THE ROOT, MOST IMPORTANT!
NOTICE TRENDS ON THE PT
Subtle but helpful
Charge
Oxygens

31. -ite ClO3-  ClO2- chlorite Minus 1 Oxygen SO42-  SO32- Same Charge
sulfite
NO3-  NO2-
nitrite
Minus 1 Oxygen
Same Charge

32. Hypo- ClO3-  ClO2-  ClO- hypochlorite
Minus one more oxygen from the –ite
Charge still the same
Think hypo is the opposite of hyper
Hyper = more
Hypo = less

33. per- ClO4-  ClO3-  ClO2-  ClO- perchlorate MnO4- permanganate O22-
peroxide
Per means we add an oxygen
Bottom two just need to memorize

34. hydrogen ___ HPO42- hydrogen phosphate H2PO4- dihydrogen phosphate
HCO3-
hydrogen carbonate
HSO4-
hydrogen sulfate
Just add the name hydrogen to the beginning of the name
Adding hydrogen decreases the overall charge by 1

35. Some more -ates CrO42- chromate Cr2O72- dichromate C2H3O2- Acetate
aka CH3COO-
There is no rhyme or reason to these. You just have to know them.

36. Few More Outliers OH- hydroxide (VERY IMPORTANT!!!) CN- cyanide NH4+
ammonium

37. 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

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

39. 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…
All acids are named
based on their anion
ending.

40. When dissolved in water, acids produce ____.
a. negative ions c. hydrogen ions
b. polyatomic ions d. oxide ions

41. -ide ending(no oxygen) Hydro – root – icHF
hydrofluoric acid
HCl
hydrochloric acid
HBr
hydrobromic acid HI
hydroiodic acid
HCN
hydrocyanic acid
H2S
hydrosulfuric acid

42. -ate ending root-ic (with oxygen)
ClO3-  HClO3
chlorate  chloric acid
SO42-  H2SO4
sulfate  sulfuric acid
PO43-  H3PO4
phosphate  phosphoric acid
NO3-  HNO3
nitrate  nitric acid
CO32-  H2CO3
carbonate  carbonic acid
Notice, the number of hydrogens added is the same as the number of the charge.

43. -ite ending root-ous ClO2-  HClO2 chlorite  chlorous acid
SO32-  H2SO3
sulfite  sulfurous acid
NO2-  HNO2
nitrite  nitrous acid
Once again, notice the charges balance out with the Hydrogens

44. Questions
Compared with acids that have the suffix -ic, acids that have the suffix -ous contain
a. more hydrogen. c. less oxygen.
b. more oxygen. d. the same amount of oxygen.

46. 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!!!

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

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