1. Ionic vs Molecular Compounds
Pages 56-64
Questions page 69, #1, 5, 6

2. Ionic Compounds Made up of a ______ and a __________ Hard or soft?
High or low melting and boiling points?
Conduct electricity? When?

3. Forming Ionic Compounds

4. Forming Ionic Solids Crystal lattice structure: In an ionic crystal,
it minimizes repulsions
from same charges
and maximizes
attraction between
like charges
Can you put this in
your own words?

5. Explaining ionic properties
Why do they have high melting and boiling points?

6. Explaining ionic properties
Hard and brittle because crystal lattice structure prevents the crystal from changing shape
Providing enough physical force will crack or fracture the crystal into smaller pieces

7. Explaining ionic properties
Dissolving/dissociation?
NaCl(s)  Na+(aq) + Cl-(aq)

8. Molecular compounds
Generally between __________ although could be a __________ and a __________

9. Molecular compounds Otherwise, they have a wide range of properties
At ambient temperature, some are gases, liquids or solids
Some a malleable while others are brittle
Relatively low melting and boiling points
Many do not dissolve in water
Most do not conduct electricity well

10. Molecular compounds
Some elements are only found in nature as a diatomic molecular compound
HOBrFINCl

11. Forming a covalent bond

12. Bonding capacity
Definition?

13. Lewis Structure Model showing covalent bonding using Lewis symbols
Bond pairs of electrons can be shown or represented by a line
Lone pairs are shown in a Lewis structure but omitted in a structural formula

14. Lewis Structure
Double bonds
Triple bonds