1. 1

2. 2 Common and Systematic Names

3. 3 Chemical nomenclature is the system of names that chemists use to identify compounds. Two classes of names exist: common names and systematic names.

4. 4 –They are not based on the composition of the compound. –They are based on an outstanding chemical or physical property. Chemists prefer systematic names. –Systematic names precisely identify the chemical composition of the compound. –The present system of inorganic chemical nomenclature was devised by the International Union of Pure and Applied Chemistry (IUPAC). Common names are arbitrary names.

5. 5

6. 6 Elements and Ions

7. 7 The formula for most elements is the symbol of the element. SodiumNa PotassiumK ZincZn ArgonAr MercuryHg LeadPb CalciumCa

8. 8 HydrogenH 2 NitrogenN 2 OxygenO 2 Fluorine F 2 ChlorineCl 2 BromineBr 2 Iodine I 2 These 7 elements are found in nature as diatomic molecules.

9. 9Ions

10. 10 → remove e - neutral atom A charged particle known as an ion can be produced by adding or removing one or more electrons from a neutral atom. If one or more electrons are removed from a neutral atom a positive ion is formed. A positive ion is called a cation.

11. 11 Na  Na + + e - Ca  Ca 2+ + 2e - Al  Al 3+ + 3e - Positive Ion Formation: Loss of Electrons From a Neutral Atom

12. 12 Naming Cations

13. 13 Cations are named the same as their parent atoms

14. 14 Atom Cation Name of Cation sodium (Na) Na + sodium ion

15. 15 Atom Cation Name of Cation calcium (Ca) Ca 2+ calcium ion

16. 16 Atom Cation Name of Cation lithium (Li) Li + lithium ion

17. 17 Atom Cation Name of Cation magnesium (Mg) Mg 2+ magnesium ion

18. 18 Atom Cation Name of Cation strontium (Sr) Sr 2+ strontium ion

19. 19 → neutral atom A charged particle known as an ion can be produced by adding or removing one or more electrons from a neutral atom. If one or more electrons are added to a neutral atom a negative ion is formed. A negative ion is called an anion. add e -

20. 20 Naming Anions

21. 21 An anion consisting of one element has the stem of the parent element and an – ide ending

22. 22 Atom Anion Name of Anion fluorine (F) F-F- fluoride ion stem

23. 23 Atom Anion Name of Anion chlorine (Cl) Cl - chloride ion stem

24. 24 Atom Anion Name of Anion bromine (Br) Br - bromide ion stem

25. 25 Atom Anion Name of Anion nitrogen (N) N 3- nitride ion stem

26. 26 Atom Anion Name of Anion phosphorous (P) P 3- phosphide ion stem

27. 27 Atom Anion Name of Anion oxygen (O) O 2- oxide ion stem

28. 28 Ions are always formed by adding or removing electrons from an atom.

29. 29 Most often ions are formed when metals combine with nonmetals.

30. 30 The charge on an ion can be predicted from its position in the periodic table.

31. 31 elements of Group IIA have a +2 charge elements of Group IA have a +1 charge elements of Group VA have a -3 charge elements of Group VIA have a -2 charge elements of Group VIIA have a -1 charge

32. 32 Writing Formulas From Names of Compounds

33. 33 A chemical compound must have a net charge of zero.

34. 34 If the compound contains ions, then the charges on all of the ions must add to zero.

35. 35 Write the formula of calcium chloride. Step 1. Write down the formulas of the ions. Ca 2+ Cl - Step 2. Combine the smallest numbers of Ca 2+ and Cl - so that the sum of the charges equals zero. (2+) + 2(1-) = 0 The correct formula is CaCl 2 The lowest common multiple of +2 and –1 is 2 The cation is written first. The anion is written second. (Ca 2+ ) + 2(Cl - ) = 0

36. 36 Write the formula of barium phosphide. Step 1. Write down the formulas of the ions. Ba 2+ P 3- Step 2. Combine the smallest numbers of Ba 2+ and P 3- so that the sum of the charges equals zero. 3(2+) + 2(3-) = 0 The correct formula is Ba 3 P 2 The lowest common multiple of +2 and –3 is 6 3(Ba 2+ ) + 2(P 3- ) = 0 The cation is written first. The anion is written second.

37. 37 Write the formula of magnesium oxide. Step 1. Write down the formulas of the ions. Mg 2+ O 2- Step 2. Combine the smallest numbers of Mg 2+ and O 2- so that the sum of the charges equals zero. (2+) + (2-) = 0 The correct formula is MgO The lowest common multiple of +2 and –2 is 1 ( Mg 2+ ) + (O 2- ) = 0

38. 38 Binary Compounds

39. 39 Binary compounds contain only two different elements.

40. 40 Binary ionic compounds consist of a metal combined with a non-metal.

41. 41 A. Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation (one charge)

42. 42 Type I Cations include: the Group A metals Hydrogen B metals with one charge: Zn +2, Cd +2, Ag + The polyatomic ion NH 4 +

43. 43 The chemical name is composed of the name of the metal followed by the name of the nonmetal which has been modified to an identifying stem plus the suffix –ide. Using this system the number of atoms of each element present is not expressed in the name.

44. 44 Name of Metal + Stem of Nonmetal plus -ide ending

45. 45 (ur)

46. 46 If hydrogen is written first in the formula, it is treated as if it were a group IA metal.

47. 47 Step 1 From the formula it is a two-element compound and follows the rules for binary compounds. Name the Compound CaF 2

48. 48 Name the Compound CaF 2 Step 2 The compound is composed of Ca, a metal and F, a nonmetal. Ca forms only a +2 cation. Thus, call the positive part of the compound calcium.

49. 49 Step 3 Modify the name of the second element to the stem fluor- and add the binary ending –ide to form the name of the negative part, fluoride. Name the Compound CaF 2

50. 50 Step 4 The name of the compound is therefore calcium fluoride. Name the Compound CaF 2

51. 51Examples

52. 52 Compound Name sodium chloride NaCl nonmetal stem name of metal

53. 53 Compound Name hydrogen chloride HCl ( g ) nonmetal stem name of metal For naming purposes only, hydrogen is treated as if it were a group IA metal.

54. 54 Compound Name magnesium chloride MgCl 2 nonmetal stem name of metal

55. 55 Compound Name potassium oxide K2OK2O nonmetal stem name of metal

56. 56 Compound Name sodium phosphide Na 3 P nonmetal stem name of metal

57. 57 B. Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations (two or more charges)

58. 58 Type II Cations include: B metals with two charges Zn +2, Cd +2, Ag + are excluded

59. 59 Name the Compound FeS Step 1 This compound follows the rules for a binary compound.

60. 60 Step 2 It is a compound of Fe, a metal, and S, a nonmetal, and Fe is a transition metal that has more than one type of cation. Name the Compound FeS Step 2 In sulfides, the charge on S is –2. Therefore the charge on Fe must be +2, and the name of the positive part of the compound is iron (II).(or ferrous)

61. 61 Step 3 We have already determined that the name of the negative part of the compound will be sulfide. Name the Compound FeS

62. 62 Step 4 The name of FeS is iron(II) sulfide.(or ferrous sulfide) Name the Compound FeS

63. 63 The IUPAC (Stock) System

64. 64 The metals in the center of the periodic table (including the transition metals) often form more than one type of cation.

65. 65 Each ion of iron forms a different compound with the same anion. Fe 2+ Fe 3+ FeS Fe 2 S 3

66. 66 IUPAC devised the Stock System of nomenclature to name compounds of metals that have more than one type of cation. Cation Charge +1+2+3+4+5 Roman Numeral IIIIIIIVV In the IUPAC System the charge on the cation is designated by a Roman numeral placed in parentheses immediately following the name of the metal. The nonmetal name ends in -ide.

67. 67 Stock System Lower Charge Higher Charge ElementFormulaNameFormulaName Copper Cu + copper(I) Cu 2+ copper(II) Iron Fe 2+ iron(II) Fe 3+ iron(III) Lead Pb 2+ lead(II) Pb 4+ lead(IV) Mercury Hg 2 2+ mercury(I) Hg 2+ mercury(II) Tin Sn 2+ tin(II) Sn 4+ tin(IV) IUPAC System Higher Charge ElementFormulaNameFormulaName Lower Charge

68. 68Examples

69. 69 ion chargeion name FeCl 2 iron(II) chloride +2 chlorideiron(II) FeCl 3 iron(III) chloride +3 iron(III)chloride compound name

70. 70 ion chargeion name SnBr 2 tin(II) bromide +2 bromidetin(II) SnBr 4 tin(IV) bromide +4 tin(IV)bromide compound name

71. 71 The Classical System

72. 72 In the Classical System the name of the metal (usually the Latin name) is modified with the suffixes -ous and ic.

73. 73 -ous lower charge - ic higher charge Metal name ends in nonmetal name ends in -ide

74. 74 Examples

75. 75 ion chargeion name FeCl 2 ferrous chloride +2 chlorideferrous FeCl 3 ferric chloride +3 ferricchloride compound name

76. 76 ion chargeion name SnBr 2 stannous bromide +2 bromidestannous SnBr 4 stannic bromide +4 stannicbromide compound name

77. 77 Lower Charge Higher Charge ElementFormulaNameFormulaName CopperCu + cuprousCu 2+ cupric IronFe 2+ ferrousFe 3+ ferric LeadPb 2+ plumbousPb 4+ plumbic MercuryHg 2 2+ mercurousHg 2+ mercuric TinSn 2+ stannousSn 4+ stannic Ion Names: Classical System

78. 78 Binary Compounds Containing Two Nonmetals

79. 79 Compounds between nonmetals are molecular, not ionic.

80. 80 In a compound formed between two nonmetals, the element that occurs first in this series is named first. Si B P H C S I Br N Cl O F

81. 81Prefixes

82. 82 A Greek prefix is placed before the name of each element to indicate the number of atoms of the element that are present.

83. 83 di = 2 tri = 3 tetra = 4 penta = 5 hexa = 6 hepta = 7 octa = 8 nona = 9 deca = 10 mono = 1 Mono is rarely used when naming the first element.

84. 84Examples

85. 85 N2O3N2O3 dinitrogen trioxide indicates two nitrogen atoms indicates three oxygen atoms

86. 86 PCl 5 phosphorous pentachloride indicates one phosphorous atom indicates five chlorine atoms

87. 87 Cl 2 O 7 dichlorine heptaoxide indicates two chlorine atoms indicates seven oxygen atoms

88. 88 Step 1 There are 2 elements present. The compound is binary. Phosphorous and chlorine are nonmetals so the rules for naming binary compounds of 2 nonmetals apply. Phosphorous is named first. Therefore the compound is a chloride. Determine the Name of PCl 5

89. 89 Step 2 No prefix is needed for phosphorous because each molecule of PCl 5 has only one phosphorous atom. The prefix penta- is used with chloride because there are 5 chlorine atoms present in one molecule. Step 3 The name is phosphorous pentachloride. Determine the Name of PCl 5

90. 90Examples

91. 91 dichlorine trioxide Cl 2 O 3

92. 92 dinitrogen trioxide N2O3N2O3

93. 93 carbon tetrachloride CCl 4

94. 94 carbon monoxide CO

95. 95 carbon dioxide Name CO 2

96. 96 phosphorous triiodide Name PI 3

97. 97 D. Acids Derived from Binary Compounds

98. 98 Certain binary hydrogen compounds, when dissolved in water, form solutions that have acid properties. The aqueous solutions of these compounds are given acid names. The acid names are in addition to their –ide names. Hydrogen is typically the first element of a binary acid formula.

99. 99 Acid Formation water binary hydrogen compound (not an acid). acid

100. 100 Dissolved in water acid HCl Pure compound HCl -ide

101. 101 To name binary acids write the symbol of hydrogen first. After hydrogen write the symbol of the second element. Place the prefix hydro- in front of the stem of the nonmetal name. Place the suffix -ic after the stem of the nonmetal name.

102. 102Examples

103. 103 HCl (g) hydrogen chloride Pure Compound

104. 104 HCl (aq) hydrochloric acid Dissolved in Water

105. 105 HI (g) hydrogen iodide Pure Compound

106. 106 HI (aq) hydroiodic acid Dissolved in Water

107. 107 H 2 S (g) hydrogen sulfide Pure Compound

108. 108 H 2 S (aq) hydrosulfuric acid Dissolved in Water

109. 109 H 2 Se (g) hydrogen selenide Pure Compound

110. 110 H 2 Se (aq) hydroselenic acid Dissolved in Water

111. 111

112. 112 Naming Compounds Containing Polyatomic Ions

113. 113 A polyatomic ion is an ion that contains two or more elements.

114. 114 They usually consist of one or more cations combined with a negative polyatomic ion. Compounds containing polyatomic ions are composed of three or more elements.

115. 115 When naming a compound containing a polyatomic ion, name the cation first and then name the anion.

116. 116 The ions are what is actually present. This is the way the formula is written.

117. 117 This is the way the formula is written. The ions are what is actually present.

118. 118 Prefixes and Suffixes Elements that Form More than One Polyatomic Ion with Oxygen

119. 119 Anions ending in -ate always contain more oxygen than ions ending in -ite. nitratenitrite

120. 120 Anions ending in -ate always contain more oxygen than ions ending in -ite. phosphatephosphite

121. 121 Anions ending in -ate always contain more oxygen than ions ending in -ite. sulfatesulfite -ate and –ite do not indicate the number of oxygen atoms.

122. 122 perper- (short form of hyper) denotes anions with more oxygen than the -ate form. perchloratechlorate

123. 123 hypohypo- denotes anions with less oxygen than the -ite form. chloritehypochlorite

124. 124 Oxy-Anions and Oxy-Acids of Chlorine (also Bromine and Iodine) AnionAnion NameAcidAcid Name ClO – hypochloriteHClOhypochlorous acid ClO 2 – chloriteHClO 2 chlorous acid ClO 3 – chlorateHClO 3 chloric acid ClO 4 – perchlorateHClO 4 perchloric acid

125. 125 Four ions do not use the –ate/ite system. hydroxide hydrogen sulfide cyanide peroxide

126. 126 There are three common positively charged polyatomic ions. ammoniumhydronium mercury(I)

127. 127

128. 128 Names of Selected Compounds That Contain More Than One Kind of Positive Ion FormulaName of compound KHSO 4 potassium hydrogen sulfate Ca(HSO 3 ) 2 calcium hydrogen sulfite NH 4 HSammonium hydrogen sulfide MgNH 4 PO 4 magnesium ammonium phosphate NaH 2 PO 4 sodium dihydrogen phosphate Na 2 HPO 4 disodium hydrogen phosphate KHC 2 O 4 potassium hydrogen oxalate KAl(SO 4 ) 2 potassium aluminum sulfate Al(HCO 3 ) 3 aluminum hydrogen carbonate

129. 129AcidsAcids

130. 130 The other element is usually a nonmetal, but it can be a metal. Its first element is hydrogen. Its remaining elements include oxygen and form a polyatomic ion. Oxy-acids contain hydrogen, oxygen and one other element.

131. 131 Hydrogen in an oxy-acid is not expressed in the acid name. The word acid in the name indicates the presence of hydrogen.

132. 132 contains oxygen contains sulfur contains hydrogen indicates hydrogen sulfuric acid

133. 133 Anions ending in -ate always contain more oxygen than ions ending in -ite. phosphatephosphite

134. 134 Naming the Acid Based on the Name of the Polyatomic Ion Ending of Polyatomic Ion more oxygen less oxygen ite ate Ending of Acid ous ic

135. 135Examples

136. 136 sulfite sulfurous acid

137. 137 sulfate sulfuric acid

138. 138 nitrite nitrous acid

139. 139 nitrate nitric acid

140. 140

141. 141

142. 142