1. Chapter 4 Compounds and Their Bonds

2. 4.1 Octet Rule and Ions He 2 2 Ne 2, 8 8 Ar 2, 8, 8 8 An octet
is 8 valence electrons.
is associated with the stability of the noble gases.
He is stable with 2 valence electrons (duet).
valence electrons He
Ne 2,
Ar 2, 8,
Kr 2, 8, 14,

3. Ionic and Covalent Bonds
Atoms that are not noble gases form octets
to become more stable.
by losing, gaining, or sharing valence electrons.
by forming ionic bonds or covalent bonds.

4. Metals Form Positive Ions (Cations)
by a loss of their valence electrons.
with the electron configuration of the nearest noble gas.
that have fewer electrons than protons.
Called cations
Group 1A metals ion 1+
Group 2A metals ion 2+
Group 3A metals ion 3+

5. Formation of a Sodium Ion, Na+

6. Charge of Sodium Ion, Na+
With the loss of its valence electron,
the sodium ion has a 1+ charge.
Na atom Na+ ion
11p p+
11e e-
2, 8
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7. 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-

8. Examples
A. The number of valence electrons in aluminum is 1) 1e-. 2) 2e-. 3) 3e-. B. The change in electrons for octet requires a 1) loss of 3e-. 2) gain of 3e-. 3) a gain of 5e-. C. The ionic charge of aluminum is 1) 3-. 2) 5-. 3) 3+. D. The symbol for the aluminum ion is 1) Al3+. 2) Al3-. 3) Al+.

9. Formation of Negative Ions (Anions)
In ionic compounds, nonmetals in Groups 5A (15), 6A (16) and 7A (17)
achieve an octet arrangement by gaining electrons.
form negatively charged ions with 3-, 2-, or 1- charges.
called anions

10. Formation of a Chloride, Cl-
Chlorine achieves an octet by adding an electron to its valence electrons.

11. Charge of a Chloride Ion, Cl-
By gaining 1 electron, the chloride ion has a 1- charge.
Chlorine atom, Cl Chloride ion, Cl –
17p p+
17e e- –
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12. 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(3) = 3+
The charge of a negative ion is obtained by subtracting 8 or 18 from its Group number.
Group 6A(16) = = 2-
or = 2-

13. Some Ionic Charges
TABLE 4.2

14. Examples
A. The number of valence electrons in phosphorous is 1) 4e-. 2) 5e-. 3) 8e-. B. The change in electrons for octet requires a 1) loss of 2e-. 2) gain of 2e-. 3) a gain of 3e-. C. The ionic charge of sulfur is 1) 2+. 2) 3-. 3) 4-.

15. 4.2 Ionic Compounds Ionic compounds
Sodium chloride or “table salt” is an example of an ionic compound.
Ionic compounds
consist of positive and negative ions.
have attractions called ionic bonds between positively and negatively charged ions.
have high melting and boiling points.
are solid at room temperature.

16. Ionic Formulas An ionic formula
consists of positively and negatively charged ions.
is neutral.
has charge balance.
total positive charge = total negative charge
The symbol of the metal is written first, followed by the symbol of the nonmetal.

17. Charge Balance for NaCl, “Salt”
In NaCl,
a Na atom loses its valence electron.
a Cl atom gains an electron.
the symbol of the metal is written first, followed by the symbol of the nonmetal.

18. Charge Balance in MgCl2 In MgCl2, a Mg atom loses 2 valence electrons.
two Cl atoms each gain 1 electron.
subscripts indicate the number of ions needed to give charge balance.

19. Charge Balance in Na2S In Na2S,
two Na atoms lose 1 valence electron each.
one S atom gains 2 electrons.
subscripts show the number of ions needed to give charge balance.

20. 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-) =

21. 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

22. Examples
Select the correct formula for each of the following ionic compounds. A. Na+ and O2- 1) NaO 2) Na2O 3) NaO2 B. Mg2+ and Cl- 1) MgCl2 2) MgCl 3) Mg2Cl C. Al3+ and O2- 1) AlO 2) Al2O3 3) Al3O2

23. Naming Ionic Compounds with Two Elements
4.3 Naming and Writing Ionic Formulas
Naming Ionic Compounds with Two Elements
To name a compound that contains two elements,
identify the cation and anion.
name the cation first, followed by the name of the anion with an –ide ending.

24. Examples
Complete the names of the following ions: Ca2+ Al3+ Li+ _________ __________ _________ N3 Se2 F _________ __________ _________ P3 S2 Br

25. Examples of Ionic Compounds with Two Elements
Formula Ions Name
cation anion
NaCl Na Cl- sodium chloride
K2S K S2- potassium sulfide
MgO Mg O2- magnesium oxide
CaI2 Ca I- calcium iodide
Al2O3 Al O2- aluminum oxide

26. Examples
Write the formulas and names for compounds of the following ions:
Br− S2− N3−
Li+
Al3+

27. Example
Write the formula and names of the following compounds: 1) K+ and Br- 2) Ca2+ and O2- 3) Al3+ and S2- 4) Mg2+ and F-

28. Transition Metals Form Positive Ions
Most transition metals and Group 4 (14) metals form 2 or more positive ions. However, Zn2+, Ag+, and Cd2+ form only one ion.

29. Metals That Form More Than One Cation
The name of metals with two or more positive ions (cations) use a Roman numeral to identify ionic charge.

30. Naming FeCl2
To name FeCl2: 1. Determine the charge of the cation using the charge of the anion (Cl-). Fe ion + 2 Cl- = Fe ion + 2- = 0 Fe ion = Name the cation by the element name and add a Roman numeral in parentheses to show its charge. Fe2+ = iron(II) 3. Write the anion with an ide ending. FeCl2 = iron(II) chloride

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

32. Examples
Select the correct name for each. A. Fe2S3 1) iron sulfide 2) iron(II) sulfide 3) iron(III) sulfide B. CuO 1) copper oxide 2) copper(I) oxide 3) copper(II) oxide

33. Writing Formulas
Write a formula for potassium sulfide. 1. Identify the cation and anion. potassium = K+ sulfide = S2− 2. Balance the charges. K+ S2− K+ 2(1+) + 2(1-) = K+ and 1 S2− = K2S

34. Writing Formulas
Write a formula for iron(III) chloride. 1. Identify the cation and anion. iron (III) = Fe3+ (III = charge of 3+) chloride = Cl− 2. Balance the charges. Fe3+ Cl− Cl− = (3+) + 3(1-) = 0 Cl− 3. 1 Fe3+ and 3 Cl− = FeCl3

35. Examples
What is the correct formula for each of the following? A. Copper(I) nitride 1) CuN 2) CuN3 3) Cu3N B. Lead(IV) oxide 1) PbO2 2) PbO 3) Pb2O4

36. 4.4 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)

37. Some Compounds with Polyatomic Ions

38. Some 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 the prefix hydrogen (or bi).
HCO3− hydrogen carbonate (bicarbonate)
HSO3− hydrogen sulfite (bisulfite)

39. Names and Formulas of Common Polyatomic Ions
Memorize these ions

40. 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

41. Examples
Match each formula with the correct name. A. MgS 1) magnesium sulfite MgSO3 2) magnesium sulfate MgSO4 3) magnesium sulfide B. Ca(ClO3)2 1) calcium chlorate CaCl2 2) calcium chlorite Ca(ClO2)2 3) calcium chloride

42. Examples Name each of the following compounds: A. Mg(NO3)2
B. Cu(ClO3)2
C. PbO2
D. Fe2(SO4)3
E. Ba3(PO3)2

43. 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 has the polyatomic ions in parentheses.
Mg2+ and 2NO3− -> Mg(NO3)2
subscript 2 for charge balance

44. Examples
Select the correct formula for each. A. aluminum nitrate 1) AlNO3 2) Al(NO)3 3) Al(NO3)3 B. copper(II) nitrate 1) CuNO3 2) Cu(NO3)2 3) Cu2(NO3) C. iron(III) hydroxide 1) FeOH 2) Fe3OH 3) Fe(OH)3 D. tin(IV) hydroxide 1) Sn(OH)4 2) Sn(OH)2 3) Sn4(OH)

45. Examples Write the correct formula for each. A. potassium bromate
B. calcium carbonate
C. sodium phosphate
D. iron(II) nitrite

46. Flowchart for Naming Ionic Compounds

47. Examples
Name the following compounds: A. Ca3(PO4)2 B. FeBr3 C. Al2S3 D. NaHCO3

48. Examples
Write the formulas for the following: A. iron(II) hydroxide B. aluminum carbonate C. copper(II) bromide D. lithium phosphate