1. Ions and Ionic Compounds
Chapter 5
5-1 Simple Ions

2. Valence Electrons
Electrons in the outer energy level

3. The Octet Rule

4. Valence electrons and the Periodic Table

5. Chemical Reactivity How reactive an element is
Depends on the electron configuration
Notice the Noble gases

6. Noble Gases Filled s and p sublevels ns2 np6 Least Reactive elements
Filled outer energy levels
Noble Gases
Filled s and p sublevels
ns2 np6

7. Alkali Metals and Halogens
The most reactive elements
Alkali Metals,
1 valence electron
Halogens, seven valence electrons

8. Lewis Dot Diagram
Lewis Dot, or Electron Dot Diagram

9. Ions Atoms Gain or Lose Electrons to Form Stable Ions
(Have the same electron configuration of a noble gas)

10. Characteristics of Stable Ions
Some Ions have noble gas configurations, but are not like noble gases
Ions have a charge and so they form compounds
Noble gases are very unreactive

11. Some stable Ions do NOT have noble gas configurations
Mainly the transition metals
Lose valence electrons
Some form more than 1 stable ion

12. Ions have different properties from parent atoms
Sodium and Chlorine are both dangerous
But the ions together make table salt

13. Ions from metals and non-metals
Form cations (positive)
Form anions (negative)

14. Ionic Bonding and Salts
5-2

15. Ionic Bonding
Electrons are transferred
Ionic Compound

16. Ionic Bonding Ionic Bonds form between ions of opposite charge
Forms Salts

17. Ionic bonds from between metals and non-metals
Form cations (positive)
Form anions (negative)

18. Transferring electrons involves energy change
Removing an electron requires energy (ionization energy)
Adding an electron releases energy (electron affinity)

19. Ionic Bonding and Energy
The net result of ionic bond formation is the release of energy (exothermic)
Called Lattice Energy

20. Lattice Energy A measure of the strength of an ionic bond
The greater the lattice energy, the stronger the bond

21. Salt Crystals
The ions in a salt form a repeating pattern called a crystal lattice
The smallest repeating unit is called a unit cell

22. Ionic Compounds Do not consist of molecules
Each cation is surrounded by 6 anions and vise versa

23. Ionic Compound Crystals
In a ratio that results in the compound having no charge (electroneutral)

24. Ionic Bonds are Strong
Stronger than molecular (covalent) bonds (like water)
Takes more energy to break them
Results in high melting and boiling points

25. Names and Formulas of Ionic Compounds
Section 5-3

26. Ionic bonds from between metals and non-metals
Form cations (positive)
Form anions (negative)

27. Writing Ionic Formulas
Ionic compounds are always electroneutral
The formula for the compound is written thusly

28. Rules for Naming Simple (monatomic) Ions
Naming the cation
The name of the cation is the name of the element
Sodium atom makes a sodium ion
Some elements (transition metals) have more than 1 ion
Use roman numerals to indicate the charge
Copper (II) ion or Copper (I) ion have charge of Cu+2 or Cu+
Iron (II) ion or Iron (III) ion

29. Naming simple ionic compounds
The cation followed by the anion with –ide on the end

30. Naming Ionic Compounds
Say the names of these compounds

31. Polyatomic Ions
A charged group of two or more bonded atoms
Hydroxide

33. Names of Polyatomic Ions
The endings –ite and –ate indicate oxygen
If more than one, -ite is the lesser and –ate is more oxygen

34. Presence of Hydrogen
Name starts with hydrogen
Prefixes mono- and di-

35. Naming Compounds with Polyatomic Ions