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-

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

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.

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.

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

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

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

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