1. Names & Formulas
Nomenclature

2. Over 6 million compounds have been identified.
Each one has a unique name and formula.
All compounds are neutral.

3. I. 3 Categories of Compounds

4. Used to name ionically bonded atoms.
Made up of metals plus non-metals.

5. 2) Molecular:
Used to name covalently bonded atoms.
Made up of non-metals.

6. 3) Acids and Bases:
All traditional acids begin with the hydrogen ion (H+).
All traditional bases end with hydroxide ion (OH-).

7. II. Ionic Compounds Contain IONIC bonds.
Form between metals and non-metals.
Ions combine in small, whole number ratios.
They are ALWAYS NEUTRAL

8. A. Binary Ionic Compounds
“Binary” means two.
Binary ionic compounds contain only two elements.
Their names always end in “ide”.

9. Writing Formulas of Binary Ionic Compounds
Write + and - ions.
Reduce oxidation numbers if needed.
“Criss-cross” oxidation numbers (without signs) to become subscripts within the formula

10. Example #1
sodium chloride
1. Write the ions: Na+1 + Cl-1
2. Reduce as needed: OK
3. Write the formula by criss-crossing oxidation numbers so that they become the subscripts of the other ion: Na1Cl1
Formula is NaCl

11. Example #2
calcium chloride
Write ions: Ca+2 + Cl-1
Reduce as needed: OK
Criss cross oxidation numbers without signs to become subscripts within formula: Ca1Cl2
CaCl2

12. magnesium nitride 1. Write ions: Mg+2 + N-3 2. Reduce as needed: OK
Example #3
magnesium nitride
1. Write ions: Mg+2 + N-3
2. Reduce as needed: OK
3. Criss-cross
Mg3N2

13. Naming Binary Ionic Compounds
Cations (+) retain the name of the element.
Anions (-) keep the root name but add “ide” ending.

14. Example #1
LiF
lithium fluoride

15. Example #2
SrCl2
strontium chloride

16. Example #3
Al2O3
aluminum oxide

17. B. Multi-Charge Metals
Most of the transition metals have variable oxidation numbers.
Roman numerals are used to indicate charges of these elements.
First, look at the total negative charge of the anion (oxidation number x number of atoms).
Then, use this information to determine the oxidation number of the metallic cation.

18. Example #1
FeO
First, look at anion to determine total negative charge:
1 (# of atoms) x -2 (oxidation #) = -2
Total positive charge must be +2 because all molecules are neutral.
When you look at formula, you see the ratio of Fe to O is 1:1
Fe2+ + O2-
iron (II) oxide

19. Example #2
Fe2O3
Total charge on anion:
3(-2) = -6
Total charge on cation: +6
2(?) = +6 ? = +3
Fe3+ + O2-
iron(III) oxide

20. Example #3
Copper (I) Oxide
Cu1+ + O2-
Cu2O
These are easy because the Roman numeral in the name gives you the charge of the cation!

21. Example #4
Copper (II) Oxide
Cu2+ + O2-
CuO

22. IMPORTANT EXCEPTIONS to MEMORIZE!
Silver always forms a +1 ion.
Zinc always forms a +2 ion.
Cadmium always forms a +2 ion.
The oxidation numbers of lead and tin also vary.

23. Binary Ionic Compounds HW
STOP Do
Binary Ionic Compounds HW

24. Ternary Ionic Compounds

25. C. Ternary Ionic Compounds
Contain three or more elements
Contain at least one polyatomic ion

26. Follow the same rules and complete the same steps as for binary ionic compounds
Enclose PAI in parentheses when necessary

27. Example #1
Aluminum phosphate
Write ions: Al PO43-
Reduce oxidation numbers then criss-cross: Al1 (PO4 )1
AlPO4

28. Example #2
Sodium sulfate
Na 1+ + SO4 2-
Na2SO4

29. Example #3
Iron (II) bromate
Fe2+ + BrO3-
Fe(BrO3)2

30. Example #4
CaCO3
calcium carbonate

31. Example #5
Cu(NO3)2
Remember, copper is a transition metal and you will need parentheses in the name
copper(II) nitrate

32. Example #6
(NH4)3N
ammonium nitride

33. Ternary Ionic Compounds HW
STOP Do
Ternary Ionic Compounds HW

34. Molecular Compounds

35. III. Molecular Compounds
Contain COVALENT bonds.
The same elements can combine in various ways.
PREFIXES are used to tell them apart.

36. A. Binary Molecular Compounds
Binary compounds contain two different elements.
Binary compounds always end in “ide” .
We will only learn BINARY molecular compounds.

37. Prefixes: 1 = mono 6 = hexa 2 = di 7 = hepta 3 = tri 8 = octa
4 = tetra 9 = nona
5 = penta 10 = deca

38. To name: Use prefixes on first atom, except for “mono”.
Always use prefixes on the last atom.
Change ending to “ide”.

39. OF2 is oxygen difluoride
Examples
S2O3 is disulfur trioxide
CO is carbon monoxide
OF2 is oxygen difluoride

40. To write formulas:
Look at prefixes attached to each element to determine subscript.

41. Examples:
Arsenic pentiodide = ArI5
Carbon dioxide = CO2
Diphosphorus trioxide = P2O3

42. B. Hydrocarbons
Molecular compounds that contain only carbon and hydrogen

43. Alkanes have single bonds

44. Alkenes have double bonds

45. Alkynes have triple bonds

46. Alkanes carbon chain held together with single bonds.
Generic Formula: CxH(2x + 2)

47. Naming Alkanes
Based on number of carbons in molecule (prefixes indicate #)
All end in “ane”.

48. Prefixes for Alkanes Meth = 1 Hex = 6 Eth = 2 Hept = 7
Prop = 3 Oct = 8
But = 4 Non = 9
Pent = 5 Dec = 10

49. Mice Eat Peanut Butter
Meth
Eth
Prop
But

50. Examples
Ethane is C2H6
Heptane is C7H16

51. IV. Acids and Bases
Acids are easy to recognize because they begin with “H”.
Bases are easy to recognize because they end with “OH” .

52. A. Bases The anion in bases is always the hydroxide ion.
Because they are ionic, you already know how to name them (there are no special rules)

53. Examples
NaOH
sodium hydroxide

54. KOH
potassium hydroxide

55. B. Binary Acids
Have only two elements: hydrogen and a non-metal.

56. Naming Binary Acids
Use the prefix “hydro”
2) Add the suffix “ic”

57. Examples:
HCl is hydrochloric acid
H3N is hydronitric acid

58. To write formulas: 1) Start with H+1
2) End with negative ion (nonmetal) from periodic table
3) “Criss-Cross”

59. Examples:
Hydroiodic acid = HI
Hydrophosphoric acid = H3P

60. C. Ternary Acids
Have at least three elements:
H and a polyatomic ion

61. Naming Ternary Acids 1) DO NOT use “hydro” prefix! 2) Add suffix:
if “ate” ion, use “ic” suffix
if “ite” ion, “ous” suffix

62. Examples #1
HClO3
ClO31- is chlorate (ate = ic)
chloric acid

63. Example #2
H2SO3
SO32- is sulfite (ite = ous)
sulfurous acid

64. To write formulas: 1) Start with H 1+
2) End with negative polyatomic ion
3) “Criss-Cross”

65. Examples: perchloric acid (ic = ate) Perchlorate is ClO4-1
All acids start with H+1
HClO4

66. chlorous acid (ous = ite)
Chlorite is ClO2-1
All acids start with H+
HClO2

67. STOP Do
Names and Formulas
Of Acids HW