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Nomenclature of Inorganic Compounds

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Presentation on theme: "Nomenclature of Inorganic Compounds"— Presentation transcript:

1 Nomenclature of Inorganic Compounds

2 0. review

3 Diatomic Molecules Hydrogen H2 Nitrogen N2 Oxygen O2 Fluorine F2
Chlorine Cl2 Bromine Br2 Iodine I2

4 Polyatomic Molecules Sulfur S8 Phosphorous P4

5 Outline 1. Common Names 2. Ions 3. Ionic Formulas 4. Polyatomic Ions
5. Halogen Compounds 6. Acids 7. Covalent Compounds

6 Chemical names are either:
common or systematic Common names are inconsistent but often come from stories, people’s names, important characteristics of a compound, history. They continue to be used in spite of their lack of consistency. Systemic names are regulated by the IUPAC: International Union of Pure and Applied Chemistry

7 1. common names

8 Common Name Chemical Name acetone
dimethyl ketone; 2-propanone (usually known as acetone) alcohol, grain ethyl alcohol alcohol, wood methyl alcohol aqua regia A mixture of nitric acid and hydrochloric acid aspirin acetylsalicylic acid baking soda sodium bicarbonate pencil lead graphite (carbon) bone ash crude calcium phosphate brimstone sulfur brine aqueous sodium chloride solution Calamine lotion zinc oxide and iron (III) oxide caustic lime calcium hydroxide Epsom salts magnesium sulfate laughing gas nitrous oxide lye sodium hydroxide milk of magnesium magnesium hydroxide quicksilver mercury rubbing alcohol isopropyl alcohol salt, table sodium chloride sugar, table sucrose vinegar impure dilute acetic acid vitamin C ascorbic acid

9 2. ions

10 If one or more electrons are removed from a neutral atom a positive ion is formed. A positive ion is called a cation. remove e- neutral atom cation

11 The charge of a cation depends on the atom.
Na  Na e- Ca  Ca e- Al  Al e-

12

13 cations have the same name as their parent atoms

14 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- neutral atom anion

15 anions made from one element have names that end in -ide

16

17 Ions are always formed by adding or removing electrons from an atom
Ions are always formed by adding or removing electrons from an atom. Protons are NOT added or removed except in NUCLEAR reactions.

18 elements of Group 6A have a -2 charge
6.2

19 Chemical compounds have a NET charge of zero
Chemical compounds have a NET charge of zero. The charge of all the cations must be equal to the charge of all the anions.

20 Write the formula of calcium chloride.
Step 1. Write down the formulas of the ions. Ca2+ Cl- Step 2. Combine the smallest numbers of Ca2+ and Cl- so that the sum of the charges equals zero. (Ca2+) + 2(Cl-) = 0 (2+) (1-) = 0 The correct formula is CaCl2

21 Write the formula of barium phosphide.
Step 1. Write down the formulas of the ions. Ba2+ P3- Step 2. Combine the smallest numbers of Ba2+ and P3- so that the sum of the charges equals zero. 3(Ba2+) + 2(P3-) = 0 3(2+) (3-) = 0 The correct formula is Ba3P2

22 Write the formula of magnesium oxide.
Step 1. Write down the formulas of the ions. Mg2+ O2- Step 2. Combine the smallest numbers of Mg2+ and O2- so that the sum of the charges equals zero. (Mg2+) + (O2-) = 0 (2+) (2-) = 0 The correct formula is MgO

23 3. ionic formulas

24 Binary compounds contain only two different elements
Binary compounds contain only two different elements. Binary ionic compounds consist of a metal combined with a non-metal.

25

26

27 NaCl name of metal sodium chloride nonmetal stem

28 MgCl2 name of metal magnesiumchloride nonmetal stem

29 K2O potassium oxide

30 Na3P sodium phosphide

31 Some metals form more than one type of cation.
These metals are said to have variable oxidation states. 6.2

32 Different compounds are formed with different oxidation states of the cation.
FeS Fe3+ Fe2S3 6.2

33 In the Stock System the charge on a cation with variable oxidations states is designated by a Roman numeral placed in parentheses immediately following the name of the metal. Cation Charge +1 +2 +3 +4 +5 Roman Numeral (I) (II) (III) (IV) (V)

34 Stock System Copper Cu+ copper (I) Cu2+ copper (II)
Iron Fe2+ iron(II) Fe3+ iron(III) Lead Pb2+ lead (II) Pb4+ lead(IV) Mercury Hg22+ mercury(I) Hg2+ mercury(II) Tin Sn2+ tin(II) Sn4+ tin (IV)

35 +2 -1 -1 +3 iron(II) chloride FeCl2 chloride iron(II) compound name
ion charge ion name iron(III) chloride FeCl3 -1 +3 iron(III) chloride

36 +2 -1 -1 +4 tin(II) bromide SnBr2 bromide tin(II) compound name
ion charge ion name tin(IV) bromide SnBr4 -1 +4 tin(IV) bromide

37 Classical System Cu+ Cu2+ Fe2+ Fe3+ Pb2+ Pb4+ Hg Hg2+ Sn2+ Sn4+ 2+ 2
Element Formula Name Copper Cu+ cuprous Cu2+ cupric Iron Fe2+ ferrous Fe3+ ferric Lead Pb2+ plumbous Pb4+ plumbic Mercury Hg mercurous Hg2+ mercuric Tin Sn2+ stannous Sn4+ stannic 2+ 2

38 4. polyatomic ions

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

40

41 The names, formulas and charges of polyatomic ions must be committed to memory.

42 hydroxide OH1-

43 cyanide CN1-

44 thiocyanate SCN1-

45 carbonate CO32-

46 bicarbonate HCO31-

47 sulfate SO42-

48 sulfite SO32-

49 phosphate PO43-

50 phosphite PO33-

51 nitrate NO31-

52 nitrite NO21-

53 ammonium NH41+

54 acetate C2H3O21-

55 chromate CrO42-

56 dichromate Cr2O72-

57 There are three common positively charged polyatomic ions.
mercury(I) ammonium hydronium

58 When naming a compound containing a polyatomic ion, name the cation first and then name the anion. The cations must neutralize the charge on the anions. sodium carbonate

59 sodium carbonate

60 potassium permanganate

61 Anions ending in -ate always contain more oxygen than ions ending in -ite.
nitrate nitrite

62 -ate and –ite do not indicate the number of oxygen atoms.
sulfate sulfite -ate and –ite do not indicate the number of oxygen atoms.

63 phosphate phosphite

64 Ba(OH)2 barium hydroxide

65 MgCO3 magnesium carbonate

66 K2SO3 potassium sulfite

67 NaSCN sodium thiocyanate

68 Al2(CrO4)3 aluminum chromate

69 aluminum phosphate AlPO4

70 sodium sulfate Na2SO4

71 magnesium nitrate Mg(NO3)2

72 calcium cyanide Ca(CN)2

73 ammonium nitrate NH4NO3

74 5. halogen compounds

75

76 per is a short form of hyper, meaning more
Per- denotes anions with more oxygen than the -ate form. chlorate perchlorate per is a short form of hyper, meaning more

77 hypo- denotes anions with less oxygen than the -ite form.
hypochlorite chlorite -hypo means less

78 Ba(ClO3)2 barium chlorate

79 Ca(ClO2)2 calcium chlorite

80 KIO4 potassium periodate

81 NaClO4 sodium perchlorate

82 Al(BrO4)3 aluminum perbromate

83 lithium bromate LiBrO3

84 sodium hypoiodite NaIO

85 magnesium chlorite Mg(ClO2)2

86 calcium perchlorate Ca(ClO4)2

87 ammonium chlorite NH4ClO2

88 6. acids

89 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 and only apply to the compounds when they are in the aqueous solution. Hydrogen is typically the first element of a binary acid formula.

90 HCl HCl(aq) The pure compound hydrogen chloride
dissolved in water becomes hydrochloric acid HCl(aq)

91 For binary acid formulas write the symbol of hydrogen first.
After hydrogen write the symbol of the second element. HCl To assign a name to the acid place the prefix hydro- in front of the stem of the nonmetal name. hydrochlor- Place the suffix –ic acid after the stem of the nonmetal name. hydrochloric acid

92 HI hydrogen iodide Pure Compound

93 HI(aq) hydroiodic acid Dissolved in Water

94 H2S hydrogen sulfide Pure Compound

95 H2S(aq) hydrosulfuric acid Dissolved in Water

96 H2Se hydrogen selenide Pure Compound

97 H2Se(aq) hydroselenic acid Dissolved in Water

98 Oxy-acids contain hydrogen, oxygen and one other element.

99 sulfuric acid indicates hydrogen contains hydrogen contains sulfur
contains oxygen sulfuric acid

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

101 sulfite sulfurous acid

102 sulfate sulfuric acid

103 nitrite nitrous acid

104 nitrate nitric acid

105

106 7. covalent compounds

107 Compounds between nonmetals are molecular, not ionic.

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

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

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

111 N2O3 dinitrogen trioxide indicates two nitrogen atoms
indicates three oxygen atoms

112 PCl5 phosphorous pentachloride indicates one phosphorous atom
indicates five chlorine atoms

113 Cl2O7 dichlorine heptaoxide indicates two chlorine atoms
indicates seven oxygen atoms

114 Determine the Name of PCl5
Analysis There are 2 elements present. The compound is binary. Phosphorous and chlorine are nonmetals so the rules for naming binary compounds of two nonmetals apply. Phosphorous is named first. Therefore the compound is a chloride.

115 Determine the Name of PCl5
No prefix is needed for phosphorous because each molecule of PCl5 has only one phosphorous atom. The prefix penta- is used with chloride because there are 5 chlorine atoms present in one molecule. The name is phosphorous pentachloride.

116 Cl2O3 dichlorine trioxide

117 N2O3 dinitrogen trioxide

118 CCl4 carbon tetrachloride

119 CO carbon monoxide

120 CO2 carbon dioxide

121 phosphorous triiodide
PI3 phosphorous triiodide

122 summary

123 6.5

124

125 Fe(NO3)2 iron (II) nitrate

126 CuCl2 copper (II) chloride

127 N2O5 dinitrogen pentoxide

128 NH4ClO4 ammonium perchlorate

129 AgNO2 silver nitrite

130 tin(IV) bromate Sn(BrO3)4

131 hydrosulfuric acid H2S(aq)

132 nitric acid HNO3(aq)

133 hypochlorous acid HClO(aq)

134 mercury (I) chlorite Hg2(ClO2)2


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