1. IONIC COMPOUNDS

2. STABILITY Relates to nobility Every element’s dream
They’ll do what they can to look like a noble gas…pseudo-noble gas configuration
Duet Rule
Octet Rule
Potential Energy

3. Bond Energy The energy required to break a bond
The energy is absorbed when the bond is broken, thus…released when formed
Stronger bonds are more stable
Require more energy to break them
i.e. ionic bonds
Weaker bonds are less stable
Require less energy to break them
i.e. molecular or covalent bonds

4. Achieving Stability Ionic bonds made by transferring electrons
Metals will do what?
Nonmetals will do what?
Once electrons are transferred, the atoms are converted to ions.
lose electron(s)
gain electron(s)

5. Ions Positively charged ions are called?
Negatively charged ions are called?
Bond to make an ionic compound or salt
cations
anions

6. Salts Made of metals and nonmetals or polyatomic ions Solid Brittle
Ordered arrangement called crystal lattice
Brittle
High melting point
Electrical conductors in aqueous and molten phases

7. More About Ions
Written as a symbol with superscript to the right indicating the charge
Charge is written as a number followed by a + or – sign
Monatomic ions— “one-atomed” ions
Polyatomic ions— “many-atomed” ions

8. Monatomic Ions
Use periodic table to determine charges of representative elements
Group 1…1+…element name + ion
Group 2…2+…element name + ion
Group 13…3+…element name + ion
Group 14…skip
Group 15…3-…ide ending + ion
Group 16…2-…ide ending + ion
Group 17…1-…ide ending + ion

9. Monatomic Ions
For the transition metals, you must memorize the possible charges of the common ions
Cr2+
Chromium (II) ion
Chromous ion
Cr3+
Chromium (III) ion
Chromic ion
Mn2+
Manganese (II) ion
Manganous ion
Mn3+
Manganese (III) ion
Manganic ion
Fe2+
Iron (II) ion
Ferrous ion
Fe3+
Iron (III) ion
Ferric ion

10. Monatomic Ions Co2+ Cobalt (II) ion Cobaltous ion Co3+
Cobalt (III) ion
Cobaltic ion
Ni2+
Nickel (II) ion
Nickelous ion
Ni3+
Nickel (III) ion
Nickelic ion
Cu1+
Copper (I) ion
Cuprous ion
Cu2+
Copper (II) ion
Cupric ion
Hg22+
Mercury (I) ion
Mercurous ion
Hg2+
Mercury (II) ion
Mercuric ion

11. Monatomic Ions Sn2+ Tin (II) ion Stannous ion Sn4+ Tin (IV) ion
Stannic ion
Pb2+
Lead (II) ion
Plumbous ion
Pb4+
Lead (IV) ion
Plumbic ion
Ag1+
Silver ion
Zn2+
Zinc ion
Cd2+
Cadmium ion

12. Polyatomic Ions Refer to handout
Know the formula (that means elements, subscripts, and charge) of each listed

13. Making Ionic Compounds
A cation and an anion will bond in order to bring the charge of the compound to zero.
A “criss-cross” method is used to determine the number of each ion necessary to balance the charges
Always reduce subscripts.

14. Making Ionic Compounds
Na1+
Cl1- 1
= NaCl
Mg2+
Cl1- 1 2
= MgCl2
Al3+
Cl1- 1 3
= AlCl3

15. Making Ionic Compounds
NaCl
sodium chloride
MgCl2
magnesium chloride
AlCl3
aluminum chloride

16. Making Ionic Compounds
Na1+
S 2- 2 1
= Na2S
Mg2+
O 2- 2
= MgO
Ca2+
P 3- 3 2
= Ca3P2

17. Making Ionic Compounds
Na2S
sodium sulfide
MgO
magnesium oxide
Ca3P2
calcium phosphide

18. Making Ionic Compounds
Pb4+
O 2- 2 4
= PbO2
Ag1+
I 1- 1
= AgI
Fe3+
O 2-
= Fe2O3 2 3

19. Making Ionic Compounds
PbO2
Lead (IV) oxide or
plumbic oxide
AgI
silver iodide
iron (III) oxide or
ferric oxide
Fe2O3

20. Making Ionic Compounds
Pb4+
(OH)1-
= Pb(OH)4 1 4
Mg2+
(SO4)2-
= MgSO4 2 2
Al3+
(C2O4)2-
= Al2(C2O4)3 2 3

21. Making Ionic Compounds
Pb(OH)4
lead (IV) hydroxide or
plumbic hydroxide
MgSO4
magnesium sulfate
Al2(C2O4)3
aluminum oxalate

22. Crystal Lattice 3-dimensional arrangement of atoms or ions in a solid
Simplest part is called a unit cell
There are six types of crystal systems
We will focus on the cubic unit cell

23. Cubic Unit Cells
Three types:
Simple
Body-centered
Face-centered

24. Simple Cubic Unit Cell P

25. Face-centered Cubic Unit Cell
NaCl
Cl- ions
Na+ ions

26. Body-centered Cubic Unit Cell
CsCl
Cs+ ion
Cl- ion

27. Now…
PRACTICE