1. Chapter 6 Ionic Compounds
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Ionic vs Covalent bonding
Formulas and Names of ionic and covalent compounds.
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2. Octet Rule An octet Contains 8 valence electrons.
Is associated with the stability of the noble gases.
Exception is He that is stable with 2 valence electrons (duet).
valence electrons He
Ne 2,
Ar 2, 8,
Kr 2, 8, 18,

3. Review: Valence Electrons
The valence electrons
Are the electrons in the s and p sublevels in the highest energy level.
Are related to the Group number of the element.
Determine the chemical properties of the elements.
Elements with similar properties have the same number of valence electrons!

4. Forming Octets Atoms acquire octets
By losing, gaining, or sharing valence electrons.
To form compounds.
To become more stable.

5. Atomic Size Atomic radius
Is the distance from the nucleus to the valence electrons.
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6. Sizes of Metal Atoms and Ions
A positive ion
Has lost its valence electrons.
Is smaller (about half the size) than its corresponding metal atom.
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7. Size of Sodium Ion The sodium ion Na+
Forms when the Na atom loses one electron from the 3rd energy level, its valence electron.
Is smaller than a Na atom.
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Octet

8. Sizes of Nonmetal Atoms and Ions
A negative ion
Has a complete octet.
Increases the number of valence electrons.
Is larger (about twice the size) than its corresponding metal atom.
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9. Size of Fluoride Ion The fluoride ion F-
Forms when a valence electron is added.
Has increased repulsions due to the added valence electron.
Is larger than F atom
Octet
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10. Ionic and Covalent Bonds
Ionic bonds involve
Loss of electrons by a metal.
Gain of electrons by a nonmetal.
Covalent bonds involve
A sharing of electrons by nonmetals.
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11. Metals Form Positive Ions
Octets by losing all of their valence electrons.
Positive ions with the electron configuration of the nearest noble gas.
Positive ions with fewer electrons than protons.
Group 1A(1) metals  ion 1+
Group 2A(2) metals  ion 2+
Group 3A(13) metals  ion 3+
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12. Formation of a Sodium Ion, Na+
Sodium achieves an octet by losing its one
valence electron.
2, 8, , 8
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13. Charge of Sodium Ion, Na+
With the loss of its valence
electron, the sodium ion has a
1+ charge.
Sodium atom Sodium ion
11p p+
11e e-
2, 8
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14. Formation of Mg2+
Magnesium achieves an octet by losing its two valence electrons.
2, 8, , 8
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15. Charge of Magnesium Ion Mg2+
With the loss of two valence
electrons, magnesium forms
a positive ion with a 2+ charge.
Mg atom Mg2+ ion
12p+ 12p+
12e e-
2, 8
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16. Formation of Negative Ions
In ionic compounds, nonmetals
Achieve an octet arrangement.
Gain electrons.
Form negatively charged ions with 3-, 2-, or 1- charges.

17. Formation of Chloride Ion, Cl-
Chlorine achieves an octet by adding an electron to its valence electrons.
2, 8, , 8, 8
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18. Charge of a Chloride Ion, Cl-
A chlorine ion forms
When Cl gains one electron
With a 1- charge.
Chlorine atom Chloride ion
17p p+
17e e- –
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19. Some Ionic Charges Copyright © 2008 by Pearson Education, Inc.
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20. Ionic Charge from Group Numbers
The charge of a positive ion is equal to its Group number.
Group 1A(1) = 1+
Group 2A(2) = 2+
Group 3A(13) = 3+
The charge of a negative ion is obtained by subtracting 8 or 18 from its Group number .
Group 6A(16) = = 2-
or = 2-

21. Upon loss or gain of electons, the electronic arrangement of the ion is “isoelectric” with its nearest noble gas.

22. Octet Rule - What is special about “8” ?
An octet
Is 8 valence electrons
Is associated with the stability of the noble gases
He is stable with two valence electrons (duet).
valence electrons
He 1s
Ne 1s2 2s2 2p
Ar 1s2 2s2 2p6 3s2 3p
Kr 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 8 Q►

23. Quiz Questions 1- 4 [30 seconds for each question]
Select the correct answer for aluminum 3A(13):
1. Number of valence electrons (1 pt)
A) 1 electron B) 2 electrons C) 3 electrons
2. Electron change to achieve octet (1 pt)
A) loss of 3e B) gain of 3e C) gain of 5e-
3. Ionic charge of aluminum ion (1 pt)
A) 3- B) C) 3+
4. The symbol for the aluminum ion (2 pt)
A) Al3+ B) Al C) Al+

24. Quiz Questions 5 - 8 [30 seconds for each question]
Select the correct answer for sulfur 6A(17):
5. Number of valence electrons (1 pt)
A) 4e B) 6e C) 8e-
6. Change in electrons for octet (1 pt)
A) loss of 2e B) gain of 2e C) gain of 8e-
7. Ionic charge of sulfide ion (1 pt)
A) 2+ B) C) 4-
8. The symbol for the sulfide ion (2 pt)
A) S1- B) S C) S2-

25. Compounds - Compounds result from the formation of chemical bonds between two or more different elements.

26. Chemical bond: attractive force holding two or more atoms together.

27. Ionic Bonds - electron transfer process
Ionic Bonds - electron transfer process. Typically between a metal and a nonmetals
Covalent Bonds - electrons shared. Typically involving nonmetals.

28. Ionic Compounds Ionic compounds Consist of positive and negative ions.
Have ionic bonds between positively and negatively charged ions.
Have high melting and boiling points.
Are solid at room temperature.

29. Salt is An Ionic Compound
Sodium chloride (table salt) is an example of an ionic compound.
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30. Ionic Formulas An ionic formula
Consists of positively and negatively charged ions.
Is neutral.
Has charge balance.
total positive charge = total negative charge
Uses subscripts to indicate the number of ions needed to give charge balance.

31. Ionic Formula of NaCl In an ionic formula
The symbol of the metal is written first followed by the symbol of the nonmetal.
The charges of the ions in the compound are not shown.
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32. Charge Balance in NaF
The formulas of ionic compounds are determined from the charges on the ions.
atoms ions
    –
Na   F :  Na+ : F :  NaF
   
sodium fluorine sodium fluoride
The overall charge of NaF is zero (0).
Na F- = NaF
(1+ ) + (1-) = 0

33. Charge Balance In MgCl2 In forming MgCl2
A Mg atom loses two valence electrons.
Two Cl atoms each gain one electron.
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34. Using Lewis Electron Dot SymbolsBr
Ca →

35. Using Lewis Electron Dot Symbols
Al N →

36. Writing Ionic Formulas from Charges
Charge balance is used to write the formula for
sodium nitride, a compound containing Na+ and
N3−.
Na+
3 Na N3− = Na3N
3(+1) (3-) =
Note: the subscript 3 for three sodium ions.

37. Formula from Ionic Charges
Write the ionic formula of the compound with Ba2+
and Cl.
Write the symbols of the ions.
Ba2+ Cl
Balance the charges.
Ba2+ Cl two Cl- needed Cl
Write the ionic formula using a subscript 2 for two chloride ions.
BaCl2

38. Learning Check Write the correct formula for the ionic compounds
formed by the following ions:
1. Na+ and S2-
A) NaS B) Na2S C) NaS2
2. Al3+ and Cl-
A) AlCl3 B) AlCl C) Al3Cl
3. Mg2+ and N3-
A) MgN B) Mg2N3 C) Mg3N2

39. Naming and Writing Ionic Formulas
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40. Naming of Ionic Compounds
In the name of an ionic compound
The positive ion (first ion) is named as the element.
The negative ion (second ion) is named by changing the end of the element name to –ide.

41. Names of Some Common Ions
Table 6.3
3A (13)
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42. Learning Check Complete the names of the following ions: Ba2+ Al3+ K+
_________ __________ _________
N3 O2 F
_________ __________ _________
P3 S2 Cl
_________ __________ _________
barium
aluminum
potassium
nitride
oxide
fluoride
phosphide
sulfide
chloride

43. Naming Ionic Compounds with Two Elements
To name a compound that contains two elements
Identify the cation and anion.
Name the positive metal ion (cation) as the element.
Name the anion by changing the ending to ide.
Name the cation first followed by the name of the anion.

44. Charges of Representative Elements
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45. Some Ionic Compounds with Two Elements
Formula Ions Name
NaCl Na+ Cl- sodium chloride
K2S K+ S2- potassium sulfide
MgO Mg2+ O2- magnesium oxide
CaI2 Ca2+ I- calcium iodide
Al2O3 Al O2- aluminum oxide

46. More Ionic Compounds
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47. Homework Assignment: Your Name:________________________
Write the formulas and names for compounds of the following ions:
N3− Br− S2−
Na+
Al3+

48. Homework Assignment: Name:________________________
Write the names of the following compounds:
1) CaO ___________
2) KBr ___________
3) Al2O3 ___________
4) MgCl2 ___________

49. Most Transition Metals form Two or More Positive Ions
Most of the transition metals
Form 2 or more positive ions.
For example,
Copper forms Cu+ and Cu2+
Iron forms Fe2+ and Fe3+
Gold form Au+ and Au3+

50. Metals that form more than One Cation
Table Some Metals That Form More Than One Positive Ion
Lead Pb lead(II)
Pb lead(IV)
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51. Periodic Table and Some Ions
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52. Naming Variable Charge Metals
Transition metals
With two different ions use a Roman numeral after the name of the metal to indicate ionic charge.
Only zinc, silver, and cadmium form one ion (Zn2+, Ag+, and Cd2+)
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53. Naming FeCl2 To name FeCl2 [ 1 Iron ion + 2 chloride ions ]
1. Determine the charge of the cation using the charge of the anion (Cl-).
Fe ion Cl- = 1(?) (1-) = 0
Fe ion = Fe2+
2. Name the cation by the element name and a Roman numeral in parenthesis to show charge.
Fe2+ = iron(II)
3. Write the name of the anion with an ide ending.
iron(II) chloride = FeCl2

54. Naming Cr2O3
To name Cr2O3
1. Determine the charge of cation from the anion (O2-).
2Cr ions O2- = ? (2-) = ? - 6 = 0
? = / 2Cr ions = +3
Cr ion = Cr3+
2. Name the cation by the element name and use a
Roman numeral in parenthesis to show its charge.
Cr3+ = chromium(III)
3. Write the name of the anion with -ide ending.
chromium (III) oxide = Cr2O3

55. Learning Check Select the correct name for each. 1. Fe2S3
P - 1
Select the correct name for each.
1. Fe2S3
A) iron sulfide
B) iron(II) sulfide
C) iron (III) sulfide
2. CuO
A) copper oxide
B) copper(I) oxide
C) copper (II) oxide

56. Writing Formulas Write the formula of potassium sulfide.
STEP 1 Identify the cation and anion.
potassium = K+
sulfide = S2−
STEP 2. Balance the charges.
K S2− K+
2(1+) + 2(1-) = 0
STEP K+ and 1 S2− = K2S

57. Writing Formulas Write the formula of cobalt(III) chloride.
STEP 1. Identify the cation and anion.
cobalt (III) = Co3+ (III = charge of 3+)
chloride = Cl−
STEP 2. Balance the charges.
Co Cl−
Cl− = (3+) + 3(1-) = 0
Cl−
STEP Co3+ and 3 Cl− = CoCl3

58. Learning Check The correct formula for each of the following is:
1. Copper (I) nitride
A) CuN B) CuN3 C) Cu3N
2. Lead (IV) oxide
A) PbO2 B) PbO C) Pb2O4

59. Polyatomic Ions Copyright © 2008 by Pearson Education, Inc.
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60. Polyatomic Ions A polyatomic ion Is a group of atoms.
Has an overall ionic charge.
Some examples of polyatomic ions are
NH4+ ammonium OH− hydroxide
NO3− nitrate NO2− nitrite
CO32− carbonate PO43− phosphate
HCO3− hydrogen carbonate
(bicarbonate)

61. Some Compounds with Polyatomic Ions
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62. More Names of Polyatomic Ions
The names of common polyatomic anions
End in ate.
NO3− nitrate PO43− phosphate
With one oxygen less end in ite.
NO2− nitrite PO33− phosphite
With hydrogen attached use prefix hydrogen (or bi).
HCO3− hydrogen carbonate (bicarbonate)
HSO3− hydrogen sulfite (bisulfite)

63. Names and Formulas of Common Polyatomic Ions
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64. Names and Formulas of Common Polyatomic Ions
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65. Prefixes for Names of Polyatomic Ions of Halogens
Polyatomic ions of the halogens require prefixes.
ClO4− perchlorate one oxygen more
ClO3− chlorate most common form
ClO2− chlorite one oxygen less
ClO− hypochlorite two oxygens less

66. Naming Compounds with Polyatomic Ions
The positive ion is named first followed by the name of the polyatomic ion.
NaNO3 sodium nitrate
K2SO4 potassium sulfate
Fe(HCO3)3 iron(III) bicarbonate or
iron(III) hydrogen carbonate
(NH4)3PO3 ammonium phosphite

67. Some Compounds with Polyatomic Ions
Table 5.7
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68. Learning Check Select the correct formula for each: P - 2
1. aluminum nitrate
A) AlNO B) Al(NO)3 C) Al(NO3)3
2. copper(II) nitrate
A) CuNO3 B) Cu(NO3)2 C) Cu2(NO3)
3. iron (III) hydroxide
A) FeOH B) Fe3OH C) Fe(OH)3
4. tin(IV) hydroxide
A) Sn(OH)4 B) Sn(OH) C) Sn4(OH)

69. Learning Check Match each formula with the correct name:
1. MgS A) magnesium sulfite
B) magnesium sulfate
C) magnesium sulfide
D) calcium chlorate
E) calcium chlorite
F) calcium hypochlorite 2
2. MgSO3 3
3. MgSO4 1
4. Ca(ClO3)2 4
5. Ca(ClO)2 6
6. Ca(ClO2)2 5

70. Learning Check Name each of the following compounds: 1. Mg(NO3)2
2. Cu(ClO3)2
3. PbO2
4. Fe2(SO4)3
5. Ba3(PO3)2
magnesium nitrate
copper(II) chlorate
lead (IV) oxide
iron(III) sulfate
barium phosphite

71. Writing Formulas with Polyatomic Ions
The formula of an ionic compound
Containing a polyatomic ion must have a charge balance that equals zero(0).
Na+ and NO3− → NaNO3
With two or more polyatomic ions encloses the polyatomic ions in parentheses.
Mg2+ and 2NO3− → Mg(NO3)2
subscript 2 for charge balance

72. Learning Check Write the correct formula for each:
1. potassium bromate
2. calcium carbonate
3. sodium phosphate
4. iron(III) oxide
5. iron (II) nitrite

73. Naming Ionic Compounds Review:
Table 5.8
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74. Flowchart for Naming
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75. Learning Check Name the following compounds: A. Ca3(PO4)2 B. FeBr3
C. Al2S3
D. Mn(NO2)2
E. NaHCO3
calcium phosphate
iron(III) bromide
aluminum sulfide
manganese(II) nitrite
sodium hydrogen carbonate

76. Learning Check Write the formulas for the following:
A. calcium nitrate
B. iron(II) hydroxide
C. aluminum carbonate
D. copper(II) hypobromite
E. lithium phosphate

77. Covalent Compounds and Their Names
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78. Forming a H2 Molecule Copyright © 2008 by Pearson Education, Inc.
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79. H2, A Covalent Molecule In a hydrogen (H2) molecule
Two hydrogen atoms share electrons to form a covalent single bond.
Each H atom acquires two (2) electrons.
Each H becomes stable like helium (He).
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80. Diatomic Elements
These elements share electrons to form diatomic, covalent molecules.
Table 6.9
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81. Electron-Dot Formulas
Electron-dot formulas show
The order of bonded atoms in a covalent compound.
The bonding pairs of electrons between atoms.
The unshared (lone) valence electrons if they exist.
A central atom with an octet.
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82. Electron-Dot Formulas and Models of Some Covalent Compounds
Table 5.10
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83. Names of Covalent Compounds
Prefixes are used
In the names of covalent compounds.
Because typically two nonmetals can form two or more different compounds.
Examples of compounds of N and O:
NO nitrogen oxide
NO2 nitrogen dioxide
N2O dinitrogen oxide
N2O4 dinitrogen tetroxide
N2O5 dinitrogen pentoxide

84. Naming Covalent Compounds
STEP 1 Name the first nonmetal as the element.
STEP 2 End the name of the
second nonmetal
with -ide
STEP 3 Use prefixes to show the number of atoms
(subscripts).
Mono is usually omitted.
Table 6.11
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85. Naming Covalent Compounds
What is the name of SO3?
STEP 1 The first nonmetal is S sulfur.
STEP 2 The second nonmetal is O named oxide.
STEP 3 The subscript 3 of O is shown as
the prefix tri.
SO3 → sulfur trioxide
The subscript 1(for S) or mono is
understood.

86. Naming Covalent Compounds
Name P4S3
STEP 1 The first nonmetal P is phosphorus.
STEP 2 The second nonmetal S is sulfide.
STEP 3 The subscript 4 of P is shown as tetra.
The subscript 3 of O is shown as tri.
P4S3 → tetraphosphorus trisulfide

87. Formulas and Names of Some Covalent Compounds
TABLE 6.12
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88. Learning Check Select the correct name for each compound.
A. SiCl4 1) silicon chloride
2) tetrasilicon chloride
3) silicon tetrachloride
B. P2O5 1) phosphorus oxide
2) phosphorus pentoxide
3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide
2) dichlorine oxide
3) chlorine heptoxide

89. Learning Check Write the name of each covalent compound: CO CO2 PCl3
CCl4
N2O
carbon monoxide
carbon dioxide
phosphorus trichloride
carbon tetrachloride
dinitrogen oxide

90. Guide to Writing Formulas
STEP 1 Write the symbols in the order of the
elements in the name.
STEP 2 Write any prefixes as subscripts.
Example: Write the formula for carbon disulfide.
STEP 1 Elements are C and S
STEP 2 No prefix for carbon means 1 C
Prefix di = 2
Formula: CS2

91. Learning Check Write the correct formula for each of the following:
A. phosphorus pentachloride
B. dinitrogen trioxide
C. sulfur hexafluoride

92. Learning Check Identify each compound as ionic or covalent and
give its correct name.
1. SO3
2. MnCl2
3. (NH4)3PO3
4. Cu2CO3
5. N2O4
covalent - sulfur trioxide
ionic - manganese(II) chloride
ionic - ammonium phosphite
ionic – copper(I) carbonate
covalent – dinitrogen tetroxide

93. Learning Check Identify each compound as ionic or covalent and
give its correct name.
Ca3(PO4)2
FeBr3
SCl2
Cl2O
ionic – calcium phosphate
ionic – iron(III) bromide
covalent – sulfur dichloride
covalent – dichlorine oxide