1. Ionic, Metallic, and Covalent
Ch. 7 Chemical Bonds
Ionic, Metallic, and Covalent

2. Bonding Ionic, metallic, and covalent.
Use Lewis Dot structures for ease.

3. Ionic Bonds STEAL electrons
Ions’ +/- charge creates a bond.
Recognized by Metal with a Nonmetal
Ex: NaCl AlBr3 MgSO4
Ionic Compounds are also called salts

4. Ionic Compounds Properties
Most are solids at room temp.
High melting and boiling points
Conduct electricity when dissolved in water.
Brittle and hard.

5. Drawing Ionic Compounds

6. Learning Check
-With your group, correctly draw the following ionic compounds using Lewis Dot Structures.
1. LiCl KCl
3. NaCl NaBr
5. MgO CaS
7. LiF

7. Metallic Bonds Metal + Metal
-In metallic bonds valence electrons are mobile like a “sea” of electrons.
-Energy in all forms can easily move through this “sea.”
-This explains why metals are good conductors and malleable.

8. Metal Properties -Various melting points. -Do not dissolve in water.
-Solids at room temperature.

9. Covalent Bonds SHARE electrons
Atoms share valence electrons to obtain a full 8.
Use single, double, and triple bonds to do so.
Can be solids, liquids or gases at room temp.
Lower melting/boiling points.
Nonmetal and Nonmetal (NM/NM)
Ex: NH3 CO H2O

10. Learning Check
-With your group, correctly draw the following ionic compounds using Lewis Dot Structures.
1. H2O HCl
3. CH NH3
5. CO H2
7. H2O2

11. Covalent Properties
Don’t dissolve in water.
Soft.
Non-conductive.

12. Covalent Bonds

13. Diatomic Atoms Horses H2 Need N2 Oats O2 For F2 Clear Cl2 Brown Br2
-Atoms that covalently bond with itself.
***Easy way to remember them all***
Horses H2
Need N2
Oats O2
For F2
Clear Cl2
Brown Br2
I’s I2