1. Chapter 9 Chemical Names and
Formulas
Ionic Compounds

2. Learning Targets:
I can …
identify the charge of ions
calculate the amounts of electrons being transferred in an ionic bond
explain the ratio between cations and anions in an ionic compound

3. Vocabulary Terms
Monatomic ion- a single ion, Ca2+ or Cl1-
Binary Compound – made of two different elements bonded together

4. Death due to accidental inhalation of DHMO, even in small quantities.
Why learning chemical nomenclature is important!
Death due to accidental inhalation of DHMO, even in small quantities.
Prolonged exposure to solid DHMO causes severe tissue damage.
Excessive ingestion produces a number of unpleasant though not typically life-threatening side-effects.
DHMO is a major component of acid rain.
Gaseous DHMO can cause severe burns.
Contributes to soil erosion.
Leads to corrosion and oxidation of many metals.
Contamination of electrical systems often causes short-circuits.
Exposure decreases effectiveness of automobile brakes.
Found in biopsies of pre-cancerous tumors and lesions.
Given to vicious dogs involved in recent deadly attacks.
Often associated with killer cyclones in the U.S. Midwest and elsewhere, and in hurricanes including deadly storms in Florida, New Orleans and other areas of the southeastern U.S.
Thermal variations in DHMO are a suspected contributor to the El Nino weather effect.

5. Chemical reactions occur and bonds form if stability can be increased.

6. Bonding
All of the elements on the periodic table will try and achieve a stable arrangement of electrons like the noble gases.

7. Bonding
All of the elements on the periodic table will try and achieve a stable arrangement of electrons like the noble gases.
They will do this by undergoing chemical reactions and forming bonds with other elements in order to gain or lose or share electrons

8. AlCl3 C6H12O NaCl CO2 H2O Chemical Formulas
Show the kinds and numbers of atoms present
AlCl3 C6H12O NaCl
CO2
H2O

9. Ionic Compounds
Ionic bonds form between metals and nonmetals by a transfer of electrons

10. Ionic Bonding
The electron moves from the metal atom to the nonmetal atom
Opposite charges hold the ions together ­-
Nonmetal +
Metal

11. Ionic compound:
A compound that results when a metal reacts with a nonmetal to form ions called cations and anions.

12. Ion:
Atoms that have gained or lost one or more electrons to acquire a net positive or negative electric charge
Na+1 11 p+
10 e-­
Na 11 p+
11 e­-
Lose 1 e-­

13. Cation name = name of metal atom
Cations –
Positive ions formed when metal atoms lose electrons
Ca+2 Na+1 Al+3
Cation name = name of metal atom

14. Anions –
Negative ions formed when nonmetal atoms gain electrons
Cl-1 S­-2 N­-3
Anion names end in -­ide

15. Properties of Ionic Compounds
Metal + nonmetal atoms
Crystalline structure – Crystal lattice
Ions are strongly bonded to each other

16. Ionic compounds are called salts (ex/ NaCl)
Simplest ratio of ions is called the formula unit
The formula unit shows the lowest whole number ratio of the ions.

17. Na Cl Ionic Bonding The dots around the element
symbol are called Lewis Dots
and represent the VALENCE
electrons for the atom

18. Na Cl Ionic Bonding Sodium (Na) transfers its ONE valence electron to
Chlorine (Cl) and gives
Chlorine a full octet

19. Na+1 Cl -1 ­ Ionic Bonding Result is a positive Na ion
and a negative Cl ion that are
attracted to each other
(opposite charges)

20. NaCl
Formula Unit

21. Nomenclature of Ionic Compounds
metal + nonmetal with “ide” ending

22. Why do elements gain or lose electrons?
(2) 8
1 outer e­
2 outer e­
Various #’s of outer e­

23. How do we know the charges?
Group 1 elements – lose 1e­ = +1 charge
Group 2 elements – lose 2e­ = +2 charge
Group 13 elements – lose 3e­ = +3 charge
Group 14 elements – gain/lose 4­ = +4/-­4
Group 15 elements – gain 3e­ = ­-3 charge
Group 16 elements – gain 2e­ = -­2 charge
Group 17 elements – gain 1e­ = -­1 charge
Group 18 elements do not gain or lose electrons!

24. Charges on monoatomic ions
+4/­-4 +1
Transition metals can have a variety of charges +2
+3 ­-3 ­-2 ­-1

25. Transition Metal Ions ­Stock System – use roman numerals to denote charge
Fe Iron (II)
Fe3+ Iron (III)
Cu+ Copper (I)
Cu2+ Copper (II)
Au+ Gold (I)
Au3+ Gold (III)

26. Special exceptions Regular (non-transition) metals with multiple charges
Sn2+ Tin (II)
Sn4+ Tin (IV)
Pb2+ Lead (II)
Pb4+ Lead (IV)
You MUST write roman numerals for these elements
Memory aide- Roman soldiers carry tin(Sn) and lead (Pb) shields.

27. Special exceptions Transition metals with single charges
Silver (Ag +)
Zinc (Zn 2+)
Do not write roman numerals for these elements

28. Polyatomic Ions Ions that contain 2 or more nonmetal elements
Groups of nonmetal atoms that carry a charge

29. SO4-2­
sulfate ion

30. contain oxygen atoms and are named in a special way
Some polyatomic ions
contain oxygen atoms and are named in a special way
ate – 1 more oxygen atom
ite – 1 fewer oxygen atom
NO3-1­
NO2-1­
nitrate
nitrite

31. Hypochlorite ClO -1­ Chlorite ClO2 -1­ ClO3 -1­ ClO4 -1­ Chlorate
The prefix hypo – means under or too little
Hypochlorite
ClO -1­
Chlorite
ClO2 -1­
ClO3 -1­
ClO4 -1­
Chlorate
Perchlorate
He prefix per means hyper – means above or too much

32. Some polyatomic ions end in -­ide
cyanide hydroxide
CN -1­
OH -1­

33. NH4 1+
Ammonium ion
The only + polyatomic ion The only polyatomic cation

34. Writing Formulas for
Binary Ionic Compounds
2 elements only
(Type I)

35. Na Cl Ionic compounds are neutral. Equal
#’s of electrons­ have been transferred.
Na Cl

36. Ionic compounds are neutral. Equal #’s of e­ have been transferred.
Na Cl

37. Ionic compounds are neutral. Equal #’s of e­ have been transferred.
Na+1 Cl -1­

38. NaCl Formula Unit Ionic Compounds have zero net charge Na+1 x 1
Cl-1 x 1 +1 -1

39. Br Al

40. Br Al

41. Br -1 Al

42. -1
Br -1 Al

43. -1
Br -1 Al

44. -1
Br -1
Al+3 -1

45. AlBr3 Br-1 ­x Formula Unit +3 ­-3 3:1 Ratio between Al and Br
Creates a neutral compound
Formula Unit
AlBr3
Br-1 ­x
Al3+ x 1 3 +3
­-3

46. P Ca

47. P Ca

48. P
Ca+2

49. P
Ca+2 Ca

50. P -3­
Ca+2 Ca

51. P­ P
Ca+2 Ca

52. P­ P
Ca+2 Ca+2

53. Ca Ca+2
Ca+2 P­ P

54. Ca Ca+2
Ca+2 P­ P

55. Ca2+ Ca2+ Ca2+ P­

56. Ca3P2 P3-­ x Formula Unit +6 ­-6 3:2 Ratio between Ca and P
Creates a neutral compound
Formula Unit
Ca3P2
P3-­ x
Ca2+ x 3 2 +6
­-6

57. AlBr3 Al Br Writing a binary chemical formula 3+ 1-
Metal ion is always written first
AlBr3

58. Ca3P2 Ca P Writing a binary chemical formula 2+ ­3-
Metal ion is always written first
Ca3P2

59. Potassium and nitrogen Aluminum and Oxygen Strontium and Phosphorous
More Practice
Magnesium and Sulfur
Calcium and Bromine
Potassium and nitrogen
Aluminum and Oxygen
Strontium and Phosphorous

60. Naming Binary Ionic Compounds
Type I
Name the metal ion (same as metal atom)
Name the nonmetal ion (by changing the ending and adding ­-ide)

61. For cations (metal ions) simply
name the metal as usual:
Na+1
Al+3

62. For anions (nonmetal ions) –
change the ending to ­-ide
(may need to drop part of element name) •
N­-3
• O­-2 •
P­-3

63. Binary ionic naming examples:
CaBr2
K3N
Sr3P2 ­

64. calcium chloride barium oxide aluminum sulfide lithium selenide CaCl2
BaO
barium oxide
aluminum sulfide
lithium selenide

65. Naming Type II Compounds
Stock system (Roman Numerals) for Transition metals
Determine if 1st element is a transition metal
If yes, use roman numerals when naming

66. Don’t Forget the Exceptions!
Silver (Ag) and Zinc (Zn) do not get a roman numeral
Lead (Pb) and Tin (Sn) must have roman numerals

67. Stock System (for transition metals)
Copper (II) chloride =
Copper (I) chloride =
Iron (III) chloride =
Iron (II) chloride =
Tin (IV) chloride =
Tin (II) chloride =

68. Ternary Compounds: (w/ polyatomic ions) (Type I or II)
Formed from a metal cation and a polyatomic anion
Contain 3 or more different elements in the formula
Use ( ) around polyatomic ions if
there is more than 1.
Al(NO3)3

69. Na 1+ OH 1­
Not Na(OH)
NaOH
Mg 2+ OH 1­
Mg(OH)2
Not MgOH2

70. Naming Ternary compounds:
Name the metal cation
Name the polyatomic ion

71. K +1
NO3-1­
KNO3

72. K +1
NO3-1­
KNO3
Potassium nitrate

73. Ca 2+
PO4 3­
Ca3(PO4)2

74. Ca 2+
PO4 3­
Ca3(PO4)2

75. NH SO3 2-­
(NH4)2SO3

76. NH SO3 2-­
(NH4)2SO3
Ammonium sulfite

77. Cu2+ SO42-­
CuSO4

78. Cu2+ SO42-­
CuSO4
Copper (II) sulfate

79. Fe2+
NO2-1

80. Reviewing Ionic Formulas
In an ionic formula the net charge is zero
An –ide ending usually indicates a binary compound (two elements – metal and nonmetal)
Exceptions: cyanide, peroxide, hydroxide
An –ate or – ite ending indicates a polyatomic ion that has oxygen in the formula
ate = more oxygens ­ ite = fewer oxygens

81. Reviewing Ionic Formulas
A roman numeral after the name of a cation shows the ionic charge on the transition metal cation
Ions in the same group have similar formulas (due to the same number of valence electrons)
­ ­
Use ( ) around polyatomic ions if there is more than one*
* if there is only one, do not use ( )
Ca3(PO4)2

82. Naming Molecular Compounds (Covalent) Type III Nonmetal + Nonmetal

83. The Covalent Bond Sharing of electrons

84. Properties of Molecular or Covalent Compounds
Made from 2 or more non­metals
Consist of molecules not ions

85. Molecular Formulas
Show the kinds and numbers of atoms present in a molecule of a compound.
Molecular Formula = H2O

86. Structural formula
H N H H
NH3
Molecular formula

87. Molecular Formulas
Examples
CO2
SO3
N2O5

88. Rules for Naming Molecular compounds
The most “metallic” nonmetal element is written first (the one that is furthest left)
The most non­metallic of the two nonmetals is written last in the formula
NO2 not O2N
All molecular compounds end in -­ide

89. Molecular compounds
Ionic compounds use charges to determine the chemical formula
The name of the molecular compound indicates the chemical formula.
Uses prefixes to tell you the quantity of each element.
You need to memorize the prefixes !

90. Prefixes Memorize! 1 mono­ 2 di­ 3 tri­ 4 tetra­ 5 penta­ 6 hexa­
7 hepta­
8 octa­
9 nona­
10 deca­
Memorize!

91. More Molecular Compound Rules
If there is only one of the first element do not put mono­
Example: carbon monoxide (not monocarbon monoxide)
If the nonmetal starts with a vowel, drop the vowel ending from all prefixes except di and tri
monoxide not monooxide
tetroxide not tetraoxide

92. Molecular compounds
N2O5

93. Molecular compounds
N2O5 di

94. Molecular compounds
N2O5
dinitrogen

95. Molecular compounds
N2O5
dinitrogen
penta

96. Molecular compounds
N2O5
dinitrogen
pentaoxide

97. Molecular compounds
N2O5
dinitrogen
pentaoxide

98. Molecular compounds
N2O5
dinitrogen pentoxide
dinitrogen pentoxide

99. Molecular compounds Sulfur trioxide

100. Molecular compounds
Sulfur trioxide S

101. Molecular compounds
Sulfur trioxide S

102. Molecular compounds
Sulfur trioxide S O3

103. Molecular compounds Sulfur trioxide
SO3

104. Molecular compounds
CCl4

105. Molecular compounds
CCl4
monocarbon

106. Molecular compounds
CCl4
monocarbon

107. Molecular compounds
CCl4
carbon

108. Molecular compounds
CCl4
tetra
carbon

109. Molecular compounds
CCl4
tetrachloride
carbon

110. Molecular compounds
CCl4
tetrachloride
carbon
Carbon tetrachloride

111. Write molecular formulas for these
diphosphorus pentoxide
trisulfur hexaflouride
nitrogen triiodide

112. Common Names
H2O NH3

113. Common Names
H2O
Water
NH3
Ammonia

114. Names and Formulas for Common Acids (memorize these)
HCl Hydrochloric Acid
HNO3 Nitric Acid
H2SO4 Sulfuric Acid
H3PO4 Phosphoric Acid