1. After the test
Please fill out the following news letter: Topics Being Covered: The topics we have covered you should know. The upcoming topic is Nomenclature. This is a system of naming compounds and it is crucial to chemistry and the topics to follow. Important dates: Please indicate that you will be having a quiz during each class for the next four classes and after those quizzes are complete a unit 3 test. Also please indicate that PSAT testing is Oct. 14th. Grade Update: Write down your current grades in class and how you felt that you did on the test today in the Grade Update Section. If you need help on what your current grade is please come see me. You will need to take this home to your parents / guardians. Any student that brings it back signed by their parent or guardian will get 5 extra credit points on their Unit 2 Test.

2. College Preparatory Chemistry Unit 3
DO NOW:
Write the formula and name the following compounds produced from the listed ions:
Al O-2
Ca C-4
Cu O-2
Cu O-2
College Preparatory Chemistry Unit 3

3. Answers
Al+3 O-2 Al2O3 - aluminum oxide Ca+2 C-4 Ca2C - calcium carbide Cu+2 O-2 CuO - copper oxide Cu+1 O-2 Cu2O - copper oxide
Do They Look The Same Now?
How Do We Distinguish Between Them In Writing?
ARE THESE TWO THE SAME COMPOUND?
DO YOU THINK THEY HAVE THE SAME PROPERTIES?

4. Nomenclature
A system of naming compounds Why do we need a naming system? - Common names aren’t practical because they don’t give information about the composition of a substance (i.e. water)

5. Binary Compounds Compounds consisting of 2 elements
Ionic- made of __a metal__ and __a non-metal_
(held together with ionic bonds)
Molecular- made of a non-metal and a non-metal
(held together with covalent bonds)

6. Binary ionic compounds
Contain a cation and an anion
Type I (“Simple”)- contain a cation that only forms one type of cation
The ionic compounds we named last unit were this type.
Most simple cations are from metals that are NOT transition metals.
Ex. Na+
Ex. Mg+2
Ex. Al+3

8. Naming Type I (“Simple”)
Ex. NaCl = sodium chloride
Ex, Rb2O = rubidium oxide
Ex. K2S = potassium sulfide
Exceptions: Although they are transition metals, two elements always have the same charge (start to memorize this):
Cd+2 Ag+1
Zn+2

10. Type II (“Not so simple”)
Contain a cation that can form two or more cations with different charges
(truly called oxidation numbers)
Most transition metals form multiple cations
 Ex. Cu+1 and O formula __Cu2O__
Ex. Cu+2 and O formula __CuO___
Naming Type II (“Not so simple”) - use a Roman numeral to specify the charge of the cation (read this again and again!!)
 Ex. Cu2O is copper (I) oxide
and CuO is copper (II) oxide
NOTE: The Roman numeral represents the charge, not the subscript!

12. Example 1 Mn+2 and P-3 formula: Mn3P2 name: manganese (II) phosphide
NOTE:  Mn+2
Mn+4

13. Example 2
Ex. Name FeCl have to determine if cation is iron (II) or iron (III)
Work backwards to determine the charge on cation
Fe+? and Cl-1 ? + 2(-1) = 0 (remember, net charge must be zero)
? - 2 = 0
? = +2
Write name of cation followed by the Roman numeral in parentheses
Ex. iron (II)
Name anion
Ex. iron (II) chloride
NOTE: Fe+2
Fe+3

14. More Examples
Ex. CoS cobalt (II) sulfide Ex. Pb3P4 lead (IV) phosphide

15. NOTE:
Use the Roman numeral in names, NOT formulas!! (NEVER Cu(II)O !!)
Exceptions: Although they are not transition metals, two metals that do form multiple cations are lead and tin, so you must use Roman numerals when naming them (start to memorize this):
Sn+4 tin (IV) and Sn+2 tin (II)
Pb+4 lead (IV) and Pb+2 lead (II)

17. Old system of naming – not on test
Used the Latin name and suffix “-ic” for the cation with the higher charge or suffix “-ous” for cation with lower charge Ex. Fe+2 = ferrous, instead of iron (II) Ex. Fe+3 = ferric, instead of iron (III) Ex. Cu+1 and O-2 = Cu2O copper (I) oxide or cuprous oxide Ex. Cu+2 and O-2 = CuO copper (II) oxide or cupric oxide Ex. Sn+4 and Br-1 = SnBr4 tin (IV) bromide or stannic bromide

18. NOTE Do not mix and match the new system with the old system:
Ex. Do not say cuprous (I) oxide

19. Type III (“Molecular”) Binary Compounds
Contain two nonmetals
Naming Type III or Molecular Compounds
Remember these involve ONLY NONMETALS
State the name of the first element
Name the 2nd element as if it were an anion (“-ide”)
Use prefixes to indicate the number of atoms of each element
Do not use “mono” if it applies to the first element
Note: From now on check the first element and see it if is a transition metal, a fixed charge metal or a non-metal

21. Prefixes 1 = mono 6 = hexa 2 = di 7 = hepta 3 = tri 8 = octa
4 = tetra = nona
5 = penta = deca

22. Examples Ex. CO2 = carbon dioxide Ex. NO = nitrogen monoxide
dinitrogen pentoxide

23. NOTES
NOTE: IF there is a double vowel, often we drop the first vowel. The last example by the rules would be “pentaoxide”, but we usually say “pentoxide”.
NOTE: subscripts come after the formula, but prefixes come before the name. 

24. Common Names
Common Names of Molecular Compounds- these are not named according to the system above and you WILL have to MEMORIZE these!
H2O = Water
NH3 = Ammonia
CH4 = Methane
(actually is the base of a whole different form of nomenclature that we are not going to cover in this class)

25. Mixed Review of Binary Compounds
(both ionic and molecular)
Ex. SF6 =
sulfur hexafluoride
Ex. N2O3 =
dinitrogen trioxide
Ex. CaO =
calcium oxide
Ex. AuCl3 =
gold (III) chloride

27. Semi-metals
Helpful Hint: semi-metals/ metalloids are treated as nonmetals when naming usually unless it is bound to a polyatomic ion or contains an ionic bound.
(So usually name them like type III compounds)
Ex. BF3 = boron trifluoride
Ex. SiO2 =
silicon dioxide

28. How to approach the problem
A flow chart for naming binary compounds is provided in this section. These are the steps your BRAIN must take to properly name compounds, unless it is one of those 3 exceptions that you need to memorize.

29. Extra Practice: ionic molecular ionic molecular Compound
Ionic or Molecular?
Name
1. Al2S3
ionic 
aluminum sulfide 
2. B2F6
molecular
diboron hexafluoride
3. GaI3
 ionic
gallium iodide 
4. ZnS
zinc sulfide  
5. CuCl
 copper (I) chloride
6. CH4
methane 
7. BrF
molecular 
 bromine monofluoride
8. Ca3P2
calcium phosphide

30. Naming Compounds Containing Polyatomic Ions
Polyatomic ion- several atoms bonded together (with covalent bonds) that have a charge; their names and charges do not change when in compounds
Observations from Polyatomic Ion helper sheet:
Ammonium is the only positive ion
“-ite” vs “-ate” and “hypo-” vs “per-” depend on the amount of oxygen present in the polyatomic  

31. You MUST memorize the names, formulas and charges of these six polyatomic ions:
+1 ions NH4+ ammonium ion -1 ions OH- hydroxide ion NO2- nitrite ion NO3- nitrate ion HCO3- hydrogen carbonate ion (bicarbonate) C2H3O2- acetate ion CN- cyanide ion -2 ions SO3-2 sulfite ion SO4-2 sulfate ion CO3-2 carbonate ion -3 ions PO4-3 phosphate ion

32. Hints
Since polyatomic compounds are made of ions, our naming rules for ionic compounds still apply:   
Name cation (Remember to use a Roman numeral if it’s a transition metal; ammonium is the only polyatomic cation)
Name anion (usually everything AFTER the first element, since ammonium is the only polyatomic cation)
Do NOT use prefixes unless already part of a polyatomic ion’s name

33. Examples Ex. NaOH = sodium hydroxide Ex. NH4C2H3O2 = ammonium acetate
Ex. NH4C2H3O2 = ammonium acetate
Ex. CuSO4 = copper (II) sulfate
Ex. Al(H2PO4)3 = aluminum hydrogen phosphate
Ex. Na2SO3 = sodium sulfite
Ex. Mg(BrO4)2 = magnesium perbromate

34. Formula Writing
Naming acids will be covered later in the year. For now, you only need to know the formulas:
hydrochloric acid = HCl
sulfuric acid = H2SO4
nitric acid  = HNO3
acetic acid = HC2H3O2

35. Hydrates
Solid compounds that contain water in their crystalline structure
Ex. CuSO4  5H2O = copper (II) sulfate pentahydrate
They are easily named by naming the ionic compound part and then using a prefix for the number of water molecules that are present followed by the word “hydrate”
Ex. BaCl2  2H2O = barium chloride dihydrate

37. Ionic Compounds
Use the the periodic table to figure out the charges and/or names of ions. You must “zero out” the positive and negative charges. Once complete, use subscripts AFTER the ion to show how many of each ion are in the compound. Don’t write the charges since the chemical formula is now neutral.
a. Binary Ionic Compounds
Ex. lithium chloride = Li+1 and Cl-1 = LiCl 
Ex. sodium sulfide = Na+ and S-2 = Na2S
Ex. iron (III) oxide = Fe+3 and O-2 = Fe2O3

38. b. Polyatomic Ionic Compounds- You may NOT change the formula (internal subscripts) of polyatomic ions. If you need more than one of the entire polyatomic ion, put parentheses around the entire formula of the polyatomic ion. Do NOT “multiply through” by the subscript.
Ex. ammonium hydroxide = NH4+1 and OH-1 = NH4OH
 Ex. magnesium hydroxide = Mg+2 and OH-1 = Mg(OH)2

39. NOTE
AGAIN! You cannot change the name or formula (internal subscripts) of the polyatomic ion. It stays exactly the same – you just put parentheses around the formula and use subscripts to show how many of the whole ion you need. Summary on next page.