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 :
1.70-0
Practice:
Bigger Electronegtivity Value – Smaller Electronegitivity Value
Na-Cl : K-Br:
3.0 – 0.9 : 2.1 ( ionic) – 0.8 = 2.0 ( ionic)
Try…P-Cl, Li-F, Mg-O, & I-Br
P-Cl: 3.0 – 2.1 = 0.9 ( covalent) Li-F: 4.0 – 1.0: 3.0 (ionic)
Mg-O: 3.5 – 1.2 = 2.3 (ionic) I-Br: = 0.3 (covalent)
Description
●Cation electrically attracted anion
●Metal (+) gives its valence electrons to nonmetal(-)
●Share of electrons;
●Nonmetal shares electrons w/ another Nonmetal

6. Type
Ionic
Covalent
Structure
VSEPR: see later notes

7. 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.

9. Single: Cl Cl : Cl-Cl Mg S Double: O O : O=O Mg Cl Triple: Al S
Type
Ionic
Covalent
Bonding
Na Cl
Mg S
Mg Cl
Al S
Single:
Cl Cl : Cl-Cl
Double:
O O : O=O
Triple:
N N : NN

10. F & Cl Li & O 2. O & S 2. Ca & N 3. N & P 3. K & Br Type Ionic
Covalent
Bonding
Practice
Li & O
2. Ca & N
3. K & Br
F & Cl
2. O & S
3. N & P