1. Ionic and molecular bonding
Lesson 9 and 10

2. reminders - Lab was due YESTERDAY - Creative project due TOMORROW
- If you will be away hand it in in the morning or after school
- Unit test next TUESDAY
- Unit Outline, Test Outline and vocabulary online
- Practice problems in textbook
- Extra help hmu PERIOD 4

3. IF YOU LOSE YOUR PERIODIC TABLE

4. Ion review Ions are atoms with a charge
The number of protons does not equal the number of electrons
They have lost/gained/shared ELECTRONS (protons never change)
They do this because of the octet rule
Atoms are most stable with a full valence shell

5. Complete the table Group Valence Electrons Lose or Gain e- How many?
New Charge
Cation or Anion 1
Lose +1
Cation 2 13 3 +3 14 15 5
Gain -3
Anion 16 17 7 -1 18 2
Lose 2 +2
Cation 4
Can do both 4
-4 or +4
Can be both 6
Gain 6 -2
Anion 8
Neutral

6. Where do the lost electrons go?

7. Bonding
Occurs when atoms combine to make a molecule, usually to get a full valence shell
Two main types: ionic and molecular bonds

8. Ionic bonds Bond between METAL and NON-METAL Creates IONIC bond
Electrons are TRANSFERRED to get a full valence shell
Because atoms are gaining and losing electrons they become IONS

9. Foldable note
Foldable time
So much excitement!

10. Ionic bonds Bond between METAL and NON-METAL Creates IONIC bond
Electrons are TRANSFERRED to get a full valence shell
Because atoms are gaining and losing electrons they become IONS

11. Properties of ionic bonds
Transfer of electrons (gain/lost)
Solid
Crystal lattice structure
High melting point
Soluble in water? Yes
Ions dissociate
Conduct electricity
In solution
As liquid

12. How do ionic bonds happen
Lithium chloride
Calcium oxide
Potassium oxide
Aluminum chloride

13. Steps for bonding Draw the Lewis structures of each element
Connect the diagrams with arrows
Draw the ions that were made
New number of electrons
Brackets
Charge
Write the new charges and cross down
Write chemical formula
Write name with non-metal ending in ”ide” instead of “ine” or “gen”
Make foldable

14. Examples Sodium and chlorine Magnesium and fluorine
Potassium and oxygen
Aluminum and sulfur

15. Foldable note
Foldable time
So much excitement!

16. Foldable note
Practice time
Complete the worksheet

17. reminders Unit Test next TUESDAY Test and unit outline online
Practice problems in textbook
Extra help every day PERIOD 4

18. Molecular bonds Electrons are SHARED between atoms Between NON-METALS
Bond is called COVALENT bond

19. properties OF MOLECULAR COMPOUNDS
2 or more non-metals
Electrons are shared
State is often liquid or gas
Low melting point
Soluble in water? Usually no
Conduct electricity? Usually no

20. Diatomic elements F H H O O F N N O O F H F H N N H2 O2 F2 N2
H O F Br I N Cl
Atoms that always travel in pairs
Example of covalent bonds F H H O O F N N O O F H F H N N H2 O2 F2 N2
same as Br2, I2, Cl2

21. Steps for bonding Draw the Lewis structures of each element
Determine the bonding capacity of each atom
Circle shared electrons. Check for full octet.
Redraw structural diagram with lines.
Write molecular formula based on structural diagram.
You will not have to name the compound in Grade 9 (but your foldable will tell you how)
Make foldable

22. More examples hydrogen and chlorine oxygen and hydrogen
nitrogen and iodine

23. Building molecular compounds with models

24. Metallic bonding Between METALS Electrons delocalize
Have positive ions in a sea of electrons

25. Electrical Conductivity
BONDING OVERVIEW
Compound
Ionic
Molecular
Metallic
Atoms
Metal and non metal
Non metals
Metals
Type of Bond
Covalent
Electron are
Transferred, Gain/Lost
Shared
Delocalized
Structure
Crystal lattice
True molecules
Electron sea
Physical State
Solid
Liquid or gas
Melting Point
High
Low
Very high
Soluble in Water
Yes
Usually no No
Electrical Conductivity
In solution or liquid
Ions are formed