1. Types of Bonding Chemical Bond: Chemical Formula:
attraction b/w the nuclei & valence e- of different atoms thus binding atoms together.
Chemical Formula:
represents #s of atoms of each kind in
compound by using symbols & # subscripts.

2. What does electronegativity mean again?

4. What group is the most stable?

5. Bigger Electronegtivity Value – Smaller Electronegitivity Value
Type
Ionic
Covalent
Determine
Electronegitivity Difference of :
1.71 +
0-1.70
Practice:
Bigger Electronegtivity Value – Smaller Electronegitivity Value
Na-Cl= K-Br=
P-Cl= Li-F=
Mg-O= I-Br=
Description
Transfer of electrons;
Cation(+) is then electrically attracted to the anion(-)
Usually between a metal & non-metal
Sharing of electrons;
Always between non-metals
Structure
VSEPR: see later notes

6. Type Ionic Covalent Beaker A: Table Salt ( NaCl)
Properties
Strong Electrical Attraction
High Melting & Boiling Point
Hard but Brittle
Dissolve in H2O: ions break apart
Conductors: only in liquid state
- Melted or dissolved
- Need FREE metal ions
Strong Bond
Interaction between 2 or more molecules is weaker than ionic
Low Melting Point
Low Boiling Point
Demo
Beaker A: Table Salt ( NaCl)
Beaker B: Table Salt (NaCl) dissolved in H2O
Beaker C: Sugar (C6H12O6)
Beaker D: Sugar (C6H12O6) dissolved in H2O
Questions:
What did you observe for each beaker?
Explain why these observations make sense.