1. Chemical Nomenclature
A system of naming compounds.

2. Section 1 Binary Compounds
Chapter 4
Section 1
Binary Compounds

3. Binary Compounds Binary means 2.
Binary Cmpds are cmpds containing only 2 elements.

4. 2 Types of Binary Compounds
Binary Covalent Compounds
Binary Ionic Compounds

5. 2 Types of Binary Cmpds Binary Ionic Cmpds
Cmpds containing 1 metal and 1 nonmetal.
Formed when electrons are transferred from the metal to the nonmetal.
Formed by the electrostatic attraction between cations and anions.

6. Binary Covalent (Molecular) Cmpds
Cmpds containing 2 nonmetals.
Formed by the sharing of electrons between the nonmetals.
There are no ions present in these cmpds.

7. Binary Covalent Compounds
Cmpds containing only 2 nonmetals

8. The first element in the formula is named first, and the full element name is used.
The second element is named as though it were an anion (with –ide suffix).
Prefixes are used to denote the numbers of atoms present.
The prefix mono- is never used on the first element.

9. Prefixes
Hexa-
Hepta-
Octa-
Nona-
Deca-
Mono-
Di-
Tri-
Tetra-
Penta-

10. Anion Names C N O F P S Cl As Se Br Te I At

11. BF3

12. NO

13. N2O5

14. PCl5

15. P4O6

16. SF6

17. H2O
You can no longer name this water.

18. Writing Chemical Formulas
The prefixes tell you the subscripts to write in the chemical formula.

19. Sulfur trioxide

20. Disulfur tetroxide

21. Dinitrogen trioxide

22. Selenium hexabromide

23. Binary Ionic Cmpds Cmpds containing 1 metal and 1 nonmetal.
Formed when electrons are transferred from the metal to the nonmetal.
Formed by the electrostatic attraction between cations and anions.

24. Binary Ionic Cmpds Contain only 2 elements (metal and nonmetal)
Metal Cation – Always written 1st in formula
Nonmetal Anion – Always written last

25. Type I Ionic Cmpds The metal present forms only one type of cation.
These are considered true metals because they have a constant charge.

26. Remember Charges Alkali Metals Alkaline Earth Metals
Nitrogen Family Nonmetals
Oxygen Family Nonmetals
Halogens
Noble Gases
Special Ions (Transition Metals)

29. Naming Type I Cmpds Name cation first
Name anion last (with -ide ending)

30. NaCl Na + is the sodium ion Cl – is the chloride ion Sodium chloride
You may capitalize the first letter of the first name only. You never capitalize the first letter of the second name.

31. MgO

32. CsF

33. AlF3

34. MgI2

35. Rb2O

36. SrBr2

37. Cd3As2

38. BaH2

39. ZnS

40. Al2S3

41. Write the correct chemical formula for each Type I ionic compound.↓

42. Write the correct symbol for each ion.
The algebraic sum of all positive and negative charges must equal zero.
Simply “cross” the charges.

43. Calcium chloride
Aluminum oxide
Potassium bromide

44. Calcium oxide
Magnesium nitride
Strontium bromide

45. Sodium sulfide
Lithium arsenide

46. Type II Ionic Cmpds
The metal present can form two or more cations that have different charges.
Contain a transition metal with variable charges.

47. Copper
Cu + or Cu 2+
Chromium
Cr 2+ or Cr 3+

48. AuCl and AuCl3 We can’t name both cmpds gold chloride.
We use (Roman Numerals) to specify the charge on the metal cation (not the number of ions present in the cmpd).

50. AuCl and AuCl3

51. FeCl2 and FeCl3

52. PbO2

53. CuCl

54. HgO

55. Fe2O3

56. MnO2

57. PbCl4

58. CoCl3

59. CuI

60. SnBr4

61. PbS

62. Be Familiar with these names:
Stock name
Common Name
Copper I
Cuprous
Copper II
Cupric
Iron II
Ferrous
Iron III
Ferric
Lead (II)
Plumbous
Lead (IV)
Plumbic

63. Mercury
Mercury (I)
Hg2 2+
Mercury (II)
Hg 2+

64. Mercury (I) chloride and Mercury (II) chloride

65. Name Each Binary Ionic Cmpd (they’re mixed up)
CoBr2
CaCl2
Al2O3
CrCl3

66. Give Correct Chemical Formula
Tin (IV) iodide
Potassium nitride
Mercury (II) oxide
Rubidium fluoride
Sodium hydride
Chromium (II) fluoride
Magnesium sulfide
Lithium phosphide

68. Section 2 Polyatomic Ions and Acids!
Chapter 4
Section 2
Polyatomic Ions and Acids!

69. Polyatomic Ions
Charged units composed of several atoms bound together covalently.

71. Polyatomic ions are found only in ionic cmpds.
These cmpds are not binary because they contain more than two elements.

72. Oxyanions
Polyatomic anions that contain a given element (usually a halogen) and different numbers of oxygen atoms.

74. FO 1-
FO2 1-
FO3 1-
FO4 1-

75. Second Category of compounds – Ternary Ionic Compounds
Second Category of compounds – Ternary Ionic Compounds. These compounds contain at least one polyatomic ion.
What is a polyatomic ion?
Let’s look at the name to try to understands.
It is an ion – that means it has a charge.
It is polyatomic – that means it is made of more than one atom.
Simple as that!!
Let’s look at some examples of polyatomic ions.

76. CO32-
carbonate
This ion is composed of one carbon and three oxygens and the entire group has a charge of 2-.
Polyatomic ion – Group of atoms that act as a unit and carry a charge.
More examples:
PO43-
Phosphate
C2H3O21-
Acetate
SO42-
Sulfate
OH1-
Hydroxide
SO32-
Sulfite
NO31-
Nitrate
ClO41-
Perchlorate
NO21-
Nitrite
ClO31-
Chlorate
NH41+
Ammonium
ClO21-
Chlorite
ClO1-
Hypochlorite
You need to learn these!!!

77. Polyatomic Ion How do you recognize Ternary Ionic Cmpds?
Composed of 2 ions in which at least one is a polyatomic ion.
There is only one positive polyatomic ion (NH41+)
Three possible types of Ternary Ionic Compounds:
Ammonium + negative ion (nonmetal)
Metal (positive ion) + negative polyatomic ion
Ammonium + negative polyatomic ion
Polyatomic Ion

78. How do you name Ternary Ionic Compounds?
EASY! PIECE OF CAKE! NO PROBLEM!
Name the first ion.
Name the second ion. Isn’t that simple??!!
Examples:
When you look at this compound you should recognize that this is NOT binary. There are THREE elements present. When you see this, immediately look for a polyatomic ion. Carbonate is present here.
Na2CO3
Sodium
carbonate
Notice that you do NOT change the suffix – just name the polyatomic ion
Name the first ion.
Name the second ion.

79. A few more examples:
Fe(OH)3
Name the first ion.
Iron
(III)
hydroxide
Remember that iron requires a Roman Numeral since it is a transition element. What Roman Numeral should be used?
Since there are 3 OH groups, each with a 1- charge, the charge of the iron must be 3+ for the compound to be neutral
The Roman Numeral comes from the charge of the ion. How do you find the charge of the iron?
You know two things:
All compounds are neutral.
You know the charge of OH (1-)
Name the polyatomic ion.

80. NH4Cl
Name the first ion.
Ammonium
chloride
Name the second ion.
Notice that since the second ion is a nonmetal, like binary ionic compounds, the suffix of the nonmetal changes to –ide.
Name the first ion.
(NH4)3PO4
Ammonium
phosphate
Name the second ion.
Looks like a monster, but it’s really a kitty cat.

81. ONE more example:
Cu2SO4
Name the first ion.
You should realize that you need a Roman Numeral since copper is a transition metal.
Copper
(I)
sulfate
The Roman Numeral is the same as the charge.
What is the charge?
The charge of sulfate is 2-.
Since there are two coppers, the charge of the copper must be 1+.
Name the second ion.

82. How do you write formulas for Ternary Ionic Compounds?
Very much like writing formulas for Binary Ionic Compounds.
Two steps:
Write the formulas/symbols of each ion.
Balance the charges by supplying subscripts.
If a subscript is needed for a polyatomic ion, it must be put in parentheses with the subscript on the outside.
Let’s do some!!

83. Al(NO3)3 Aluminum nitrate
First, you can tell from the name that there is a polyatomic ion present (nitrate). All binary ionic compounds have suffixes of –ide.
Al NO31-
Al(NO3)3
Write the formula/symbol and charge of each ion.
Balance the charges by supplying subscripts.
Since Al is 3+ and NO3 is 1-, you need a total of 3NO31- to balance one Al3+
Since you will need a subscript of 3 for NO31-, you need to put this in parentheses with the 3 outside.

84. Ca3(PO4)2 Pb(C2H3O2)4 Lead (IV) acetate
Write the formula/symbol and charge of each ion.
Pb C2H3O21-
Balance the charges by supplying subscripts. Since Pb is 4+ and C2H3O2 is 1-, you will need 4 C2H3O21- to balance 1 Pb4+
Pb(C2H3O2)4
Write the formula/symbol and charge of each ion.
Calcium phosphate
Ca PO43-
Balance the charges by supplying subscripts. Since Ca is 2+ and PO4 is 3-, you will need 3 Ca2+ to balance 2 PO43-
Ca3(PO4)2

85. Use the same rules as before when naming ionic compounds containing polyatomic ions.

86. Na2SO4
KH2PO4
Fe(NO3)3
Mn(OH)2
Na2SO3

87. Give the correct chemical formula.
Copper (II) nitrate
Lead (II) carbonate
Potassium hydrgen sulfate
Ammonium iodide
Sodium cyanide

88. KH2PO4

89. Fe(NO3)3

90. Mn(OH)2

91. Na2SO3

92. Page 111 Practice Problems

93. Use the same rules as before when writing formulas of ionic compounds containing polyatomic ions. Remember to “cross” the charges.

94. Give the correct chemical formula.
Copper (II) nitrate
Lead (II) carbonate
Potassium hydrgen sulfate
Ammonium iodide
Sodium cyanide

95. Page 112 Practice Problems

97. Acids
An acid is a substance that produces hydrogen ions (H+) in solution (when dissolved in water).
Also called proton donors.

98. Acids
Have one or more hydrogen ions attached to an anion.

99. If the anion does not contain oxygen…
Use the prefix hydro- and the suffix
–ic attached to the root name for the
element.

100. HCl HF
HBr HI
H2S
H2Se
H2Te
H3N
H3P
H3As

101. If the anion does contain oxygen…
If the anion name ends in –ate, the suffix –ic is used.
H2SO4
HC2H3O2

102. Nitric acid
Tartric acid
Boric acid

103. If the anion ends in –ite, the suffix –ous is used.
H2SO3
HNO2

104. Phosphorous acid
Hypochlorous acid

106. Homework Notebook
Page 118 # 14-16
Page 119 # , 27-29

107. And Lastly…
We need to name hydrates.

108. Hydrates
Ionic cmpds that have water chemically attached.

109. Magnesium sulfate tetrahydrate
MgSO4 · 4H2O
Name the ionic cmpd
Name the hydrate using the prefixes.
Magnesium sulfate tetrahydrate

110. If no water is attached to the cmpd, we say the cmpd is anhydrous.