1. Chapter 5.4, 6.3, 6.4, 15.1-2 IONS AND IONIC COMPOUNDS

2. Recap of Key Words Ions – Charged atoms Anions – negative charge
Either positive or Negative
Anions – negative charge
________________________________
Cations – positive charge

3. Chemical Reactivity
Some elements are more reactive than others. How much an element reacts depends on the electron configuration.
The noble gases are the least reactive.
Which do you think are the most reactive?
Non-metals-_________________
Metals-_________________

4. Why Bond? Atoms bond to increase stability.
Which electrons determine stability?
Stability is based on valence electrons.
What is the definition of a chemical bond
A chemical bond is a force that holds two atoms together and makes them behave like a unit.

5. Valence electrons Recap
How many valence electrons are the elements trying to achieve?
Group 1: 1
Group 2: 2
Group 13: 3
Group 14: 4
Group 15: 5
Group 16: 6
Group 17: 7 8

6. Charges to Find on Periodic Table
Atoms Gain or Lose electrons to form stable ions.
Charges to Find on Periodic Table

7. Na + Cl Na + Cl The Formation of NaCl -1 +1
The electron from Na moves over to
the Cl. Now both satisfy the octet rule.
Na becomes Na+1 - a cation
Cl becomes Cl an anion
The + and - charges attract each other
and form an ionic bond.

8. NaCl

9. To make an ionic bond, the following must take place.
1. Metal atom(s) must donate valence electrons to nonmetal atom(s).
2. This electron exchange creates cations and anions.
3. Opposites attract! = ionic bond

11. Facts about Ionic Compounds
The ratio of cations to anions in an ionic bond has NO overall charge.
Ionic bonds are strong.
Have distinctive properties (high boiling and melting points)
Conduct electric current.
Hard and brittle.

12. Structure of an ionic compound

13. Structure of an ionic compound

14. Using what you know about the crystal structure of ionic compounds, explain why they would be brittle. Use pictures if necessary (I did).