2. Binary Compound A compound made up of two parts, a positive part and a negative part H2OH2O

3. The positive part is always written first Binary Compound H2OH2O

4. The negative part is always written second Binary Compound H2OH2O

5. Examples: NH 4 OHNaCl CO 2 H 2 SO 4 Mg(OH) 2 Binary Compound

6. Chemical Formula A shorthand method of representing the makeup of chemicals... H2OH2O

7. using chemical symbols and oxidation numbers. Chemical Formula H2OH2O

8. C 6 H 12 O 6 Chemical Formula

9. (NH 4 ) 2 SO 4 Chemical Formula

10. Oxidation Number The apparent charge on an atom. The charge on an ion.

11. Tells the number of electrons gained or lost when forming compounds. Oxidation Number

12. Atoms with positive oxidation numbers lose electrons. Oxidation Number Na +

13. Metals commonly have positive oxidation numbers. Oxidation Number Na +

14. Atoms with negative oxidation numbers gain electrons. Oxidation Number Cl -

15. Nonmetals commonly have negative oxidation numbers. Oxidation Number Cl -

16. The sum of the oxidation numbers in a chemical formula is equal to zero. Oxidation Number Na + Cl -

17. Subscripts Small numbers to the lower right of a chemical symbol. H2OH2O

18. Represent the number of atoms of the element in the compound. H2OH2O Subscripts

19. Subscripts of 1 are never used, they are understood. H2OH2O Subscripts

20. Multiply the subscript by the oxidation number. H2OH2O Subscripts

21. H2OH2O Hydrogen: Oxidation # X Subscript + 1 X 2 = + 2

22. H2OH2O Oxygen: Oxidation # X Subscript - 2 X 1 = - 2

23. H2OH2O Total Oxidation Number: ( + 2 ) + ( - 2 ) = 0

24. A Simplification Make the oxidation of one element the subscript of the other element.

25. There is one possible problem! CaO +2 -2 Ca 2 O 2 A Simplification

26. There is one possible problem! These subscripts will reduce... CaO +2 -2 Ca 2 O 2 A Simplification

27. Subscripts MUST be written in their lowest form. CaO A Simplification

28. What is the formula of the compound formed when magnesium and chlorine combine? Example:

29. What is the formula of the compound formed when magnesium and chlorine combine? Example: MgCl 2

30. What is the formula of the compound formed when sulfur and potassium combine? Example:

31. What is the formula of the compound formed when sulfur and potassium combine? Example: K2SK2S

32. What is the formula of the compound formed when oxygen and aluminum combine? Example:

33. What is the formula of the compound formed when oxygen and aluminum combine? Al 2 O 3 Example:

34. Ion An atom (or atoms) with a charge.

35. Ion Meaning the number of protons and electrons is no longer the same.

36. Ion Chemists cannot change an atom's protons, so it must be the electrons that change.

37. H + O -2 Mg +2 P -3 Ion This atom has lost __ e -

38. H + O -2 Mg +2 P -3 Ion This atom has gained __ e -

39. H + O -2 Mg +2 P -3 Ion This atom has lost __ e -

40. H + O -2 Mg +2 P -3 Ion This atom has gained __ e -

41. A group of covalently bonded atoms with an overall charge. Polyatomic Ion

42. NEVER change the subscripts in a polyatomic ion. Polyatomic Ion

43. If more than one is needed in a formula, put parenthesis around the ion... Polyatomic Ion

44. and add the subscript outside the parenthesis. Polyatomic Ion

45. ( NH 4 ) 2 SO 4 Polyatomic Ion

46. What is the formula of the compound formed when calcium combines with the nitrate ion? Example:

47. What is the formula of the compound formed when calcium combines with the nitrate ion? Example: Ca(NO 3 ) 2

48. What is the formula of the compound formed when zinc combines with the sulfate ion? Example:

49. What is the formula of the compound formed when zinc combines with the sulfate ion? Example: ZnSO 4

50. What is the formula of the compound formed when the ammonium and phosphate ions combine? Example:

51. What is the formula of the compound formed when the ammonium and phosphate ions combine? Example: (NH 4 ) 3 PO 4

52. The sum of the oxidation numbers in a polyatomic ion is equal to the charge on the ion. Polyatomic Ion

53. What is the formula for the sulfate ion?

54. SO 4 -2 Polyatomic Ion The Sulfate Ion

55. SO 4 -2 Polyatomic Ion This oxidation number must be positive.

56. SO 4 -2 Polyatomic Ion This oxidation number must be negative.

57. SO 4 -2 Polyatomic Ion The total of the oxidation numbers must equal this charge.

58. SO 4 -2 oxygen -2 X 4 = -8 + sulfur = ? = -2 Polyatomic Ion

59. SO 4 -2 oxygen -2 X 4 = -8 + sulfur = +6 = -2 Polyatomic Ion

60. What is the formula for the compound formed when zinc combines with the perchlorate ion?

61. Zn(ClO 4 ) 2

62. What is the oxidation number of chlorine in this compound?

63. Zn(ClO 4 ) 2 Zn is +2 X 1 = +2

64. Zn(ClO 4 ) 2 Zn is +2 X 1 = +2 O is -2 X 4 X 2 = -16

65. Zn(ClO 4 ) 2 Zn is +2 X 1 = +2 O is -2 X 4 X 2 = -16 Cl's total must be +14

66. Zn(ClO 4 ) 2 Zn is +2 X 1 = +2 O is -2 X 4 X 2 = -16 Cl's total must be +14 There are 2 Cl's, each one = +7

68. Lab Question: Does steel wool weigh more or less after burning.

69. A combustion reaction is defined as a hydrocarbon combining with oxygen to produce carbon dioxide and water. Combustion CH 4 + 2O 2 CO 2 + 2H 2 O

70. Metallic substances combine with oxygen in oxidation-reduction reactions, such as the rusting of iron. Combustion 4Fe + 3O 2 2Fe 2 O 3

71. Do these two reactions suggest that anything that burns is actually combining with oxygen in the atmosphere? Combustion 4Fe + 3O 2 2Fe 2 O 3 CH 4 + 2O 2 CO 2 + 2H 2 O

72. Steel wool is commonly purchased as pads formed from very thin metal threads. These pads are used as abrasives. Combustion coarse - medium - fine

73. Is it possible that these metal threads would burn? Combustion coarse - medium - fine

74. An impressive pyrotechnic display using steel wool.

76. Naming Binary Compounds Chemical Names

77. First: Write the name of the positive element. Chemical Names

78. Then: Write the name of the negative element... Chemical Names

79. with an ide ending. Chemical Names

80. Examples: NaCl CaI 2 Li 4 C Chemical Names

81. Examples: NaCl Sodium chloride CaI 2 Li 4 C Chemical Names

82. Examples: NaCl Sodium chloride CaI 2 Calcium iodide Li 4 C Chemical Names

83. Examples: NaCl Sodium chloride CaI 2 Calcium iodide Li 4 C Lithium carbide Chemical Names

84. Compounds Containing Polyatomic Ions Chemical Names

85. First: Write the name of the positive element or ion. Chemical Names

86. Then: Write the name of the negative part... Chemical Names

87. Then: If the negative part is a polyatomic ion, write the name with no changes... Chemical Names

88. Then: If the negative part is an element, write the name with an ide ending as usual. Chemical Names

89. Examples: MgSO 4 CaCO 3 NH 4 Cl Chemical Names

90. Examples: MgSO 4 Magnesium sulfate CaCO 3 NH 4 Cl Chemical Names

91. Examples: MgSO 4 Magnesium sulfate CaCO 3 Calcium carbonate NH 4 Cl Chemical Names

92. Examples: MgSO 4 Magnesium sulfate CaCO 3 Calcium carbonate NH 4 Cl Ammonium chloride Chemical Names

93. With Roman Numerals Chemical Names

94. If the positive element has more than one possible oxidation number... Chemical Names

95. or if it is out of character, its oxidation number is shown... Chemical Names

96. with a Roman numeral in parenthesis after its name. Chemical Names

97. Examples: lead (IV) oxide nitrogen (III) fluoride copper (I) chloride Chemical Names

98. Examples: lead (IV) oxide PbO 2 nitrogen (III) fluoride copper (I) chloride Chemical Names

99. Examples: lead (IV) oxide PbO 2 nitrogen (III) fluorideNF 3 copper (I) chloride Chemical Names

100. Examples: lead (IV) oxide PbO 2 nitrogen (III) fluorideNF 3 copper (I) chlorideCuCl Chemical Names

101. The "Big 3" industrial acids: Chemical Names

102. The "Big 3" industrial acids: Chemical Names

103. The "Big 3" industrial acids: Chemical Names