1. nomenclature

2. Writing a molecular formula
The oxidation numbers of the elements or polyatomic molecules involved must add up to zero
Review pg. 221 if you can’t remember oxidation numbers.
You must know the polyatomic ions on THE HANDOUT I GAVE YOU

3. Formation of Ionic Compounds
Remember that objects with opposite charges attract each other.
The strong attractive force between ions of opposite charge is called an ionic bond.
Don’t forget that even though the ions have charges, the overall charge of the compound will be …
ZERO!

4. Polyatomic Ions
Polyatomic ions are groups of covalently bonded atoms that have a charge
For example:
SO4 -2
NO3 –1
ClO3 –1
NH4 +1

5. Polyatomic Ions Writing formulas with polyatomic ions is the same.
You just have to keep the polyatomic ions grouped together
The charges need to cancel out, so you’re going to have to do a little multiplication.
you MUST use parentheses with polyatomics!

6. Formula writing with polyatomic Ions
Write the formula for the compound formed between sodium and nitrate
Na +1 NO3 -1 (the charges cancel so….)
Na(NO3)

7. Formula writing with polyatomic Ions
Write the formula between ammonium and sulfate
NH SO4 -2 (charges don’t cancel….)
So multiply by the smallest common factor to get the charges to cancel.
(NH4)2 (SO4)

8. Formation of Ionic Compounds
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9. Don’t Forget! Some elements oxidation numbers can not be predicted
elements can form multiple charges
Roman numerals will tell you the charge!
For example: Copper (II)  Cu +2

10. More examples Copper (II) and chlorine Silver and Nitrate CuCl2
Magnesium and sulfite
Calcium and sulfur
Potassium and oxygen
Ammonium and phosphate
Ammonium and chlorine
CuCl2
AgNO3
MgSO3
CaS
K2O
(NH4)3PO4
NH4Cl

11. Multiple Charges to Remember
Copper
Iron
Lead
Tin
Manganese
Gold
Cobalt
+1 and +2
+2 and +3
+2 and +4
+2, +4, and +7
+1 and +3

12. Mg+2 combined with PO4-3 =
Mg3(PO4)2
K+1 combined with SO4-2 =
K2SO4

13. Write the molecular formulas for : Ammonium nitrate Iron (III) oxide
NH4NO3
Iron (III) oxide
Fe2O3
Barium hydroxide
Ba(OH)2

14. Nomenclature- The scientific process of naming compounds in chemistry.
Ionic compounds- are composed of ions combined so that the net charge equals zero. The positive ion is always named first. These are usually found in a one to one ratio.

15. Naming ionic compounds
In naming ionic compounds, name the cation first, then the anion.
Monatomic cations use the element name.
Monatomic anions use the root of the element name plus the suffix -ide.
(This means 1 element with a negative charge will end in –ide).

16. Naming ionic compounds
If an element can have more than one oxidation number, use a Roman numeral in parentheses after the element name, for example, iron(II) to indicate the Fe 2+ ion.
For polyatomic ions, use the name of the ion.

17. Oxyanions
Certain polyatomic ions, called oxyanions, contain oxygen and another element.
If two different oxyanions can be formed by an element, the suffix -ate is used for the oxyanion containing more oxygen atoms, and the suffix -ite for the oxyanion containing fewer oxygens.

18. Examples NaCl MgSO4 K3PO4 Ca(ClO3)2 NH4NO2 Al(ClO)3 CuSO3 Fe(NO3)2
Sodium chloride
Magnesium sulfate
Potassium phosphate
Calcium chlorate
Ammonium nitrite
Aluminum hypochlorite
Copper (II) sulfite
Iron (II) nitrate

19. Molecules Molecule – two or more atoms covalently bound together
Diatomic molecule – two of the same atom bound together

20. Diatomic Molecules Br I N Cl H O F or the Magnificent 7
These atoms never exist alone.
They always come in pairs
For example:
Br  Br2
I  I2
N  N2
Cl  Cl2
H  H2
O  O2
F  F2

21. Naming Binary Covalent Compounds
Before you can name binary covalent compounds, you MUST know the prefixes!

22. Prefixes Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 67 8 9 10

23. Rules for naming Binary Covalent Compounds
Name the prefix for the number of atoms of the first element
Then name the first element
Name the prefix for the number of atoms of the second element
Than name the root of the second element with the ending -ide

24. Note… No charges are used in Binary Covalent Compounds
If the 1st prefix is mono….DROP IT!
When the prefix ends in an o or a, and the name of the element begins with a vowel, the o or a is often dropped

25. Examples What is the name of N2O4? N2  di nitrogen O4  tetra oxide
Since oxide begins with a vowel, we will
drop the a in tetra
Dinitrogen tetroxide

26. More examples Name SO2 S  mono sulfur
But mono is with the 1st element, so it will be dropped  sulfur
O2  dioxide
Sulfur dioxide

27. More examples Write the formula for dichlorine monoxide
Dichlorine  Cl2
Monoxide  O
Cl2O

28. More examples Write the formula for disulfur dichloride Disulfur  S2
Dichloride  Cl2
S2Cl2

29. Acids Acids can be recognized because the start with H Examples HCl
H2SO4 HI

30. Acids - Follow their own rules. Most if not all acids contain H.
The binary acids always begin with the prefix hydro.
The stem comes from the other atom involved.
They always end in ic.

31. Rule #1 - naming acids
If the anion ends in –ide, the acid will be named…
Hydro (root) – ic acid
This is usually for H plus one element

32. For example HCl Hydrochloric acid HI Hydroiodic acid H2S
Hydrosulfuric acid

33. Complex Acids or Oxyacids- do not ever have a prefix.
Formed from polyatomic ions that have an O in them.
ate polyatomics form acids and their ending changes to ic
ite polyatomic ions end in ous

34. Rule #2 – naming acids
If you have an H plus an anion ending in –ate, the acid will be named…
(root) – ic acid

35. Examples
H2SO4
Sulfuric acid
HNO3
Nitric acid
H3PO4
Phosphoric acid

36. Rule # 3 – naming acids
If you have an H plus an anion ending in –ite, the acid will be named…
(root) – ous acid

37. Examples
H2SO3
Sulfurous acid
HNO2
Nitrous acid
H3PO3
Phosphorous acid

38. Remember…
ate  ic
ite - ous

39. Mixed examples (remember to figure out what type of compound it is 1st
KClO2
CO2
H2SO4
NH4Br
CuCO3
Fe2O3
HClO
Potassium chlorite
Carbon dioxide
Sulfuric acid
Ammonium bromide
Copper (II) carbonate
Iron (III) oxide
Hypochlorous acid

40. More Mixed Examples Carbon tetrachloride Phosphorous pentachloride
Aluminum oxide
Copper (II) nitrate
Chlorous acid
Hydrophosphoric acid
Iron (III) hydroxide
CCl4
PCl5
Al2O3
Cu(NO3)2
HClO2
H3P
Fe(OH)3

41. More examples H2SO3 H2CO3 HF Nitrous acid Perchloric acid Iodic acid
Phosphorous acid
Sulfurous acid
Carbonic acid
Hydrofluoric acid
HNO2
HClO4
HIO3
H3PO3

42. Organic Notes Nomenclature- a system used to name compounds
Hydrocarbons-
Organic chemistry uses prefixes and suffixes to name compounds
Prefixes tell how many carbons are in the chain

43. Ex; meth = 1
Eth = 2
Prop = 3
But = 4
Pent = 5
Hex = 6
Hept = 7
Oct = 8
Non = 9
Dec = 10

44. Suffixes tell what type of bond the compound has
Ane = single bond
Ene = double bond
Yne = triple bond
There will be only one of these bonds in the compound.

45. Cyclo = when the the carbon chain forms a ring
Ex; cyclopropane is 

46. Branched Chain Alkanes-
When all the carbons in the hydrocarbon molecule are not bonded in a straight line they are called branched chains. They are named based on the following rules:

47. Determine the longest continuous chain of carbon atoms = parent chain.
Number thru parent chain so that the first branch is closest to the lowest number.
Name the branched groups by changing the ane ending to yl.
Use the prefixes di and tri for multiple branched groups.

48. EX:
CH2CH3 CH2CH3
CH3CH2CHCH2CHCHCH3
CH2CH3

49. Concept 7 organic notes
A conjugated system is when multiple p orbitals overlap, see pg These are very stable systems, much more stable than other unsaturated systems.
Isomers- two or more compounds with the same molecular formula. See. Pg 718
Structural isomers – a re-arrangement of the carbon chain.

50. Positional isomers – when an atom other than C or H can occupy more than 1 position.
Functional isomers- when a functional group can occupy more than one position.
Geometric isomers- when the arrangement of atoms on either side of a multiple bond can be altered.