1. Ions Continued
Unit 3 Topic 2

2. Charges
Because elements in the same group (column) of the Periodic Table have the same number of valence electrons
They also tend to form ions with the same charge

3. Oxidize (lose electrons) to form Positive Ions
Charges
Elements in columns 1-13 tend to undergo Oxidation (lose electrons) and form Positive ions.
Oxidize (lose electrons) to form Positive Ions

4. Reduces (gains electrons) to form Negative Ions
Charges
Elements in columns tend to undergo Reduction (gain electrons) and form Negative ions.
Reduces (gains electrons) to form Negative Ions

5. Oxidation vs Reduction
How am I going to remember these terms?
O -Oxidation
I -Is
L -Loss
R -Reduction
G -Gain

6. Oxidation States
The common oxidation state (ion charge) for elements can be predicted by their position on the Periodic Table

7. Common Oxidation States (Charges)+1 +2 +3
+ or -4 -3 -2 -1
~Charges Vary~
Color Page 2 of your PT Coloring book.

8. Octet Rule
When elements react by losing or gaining electrons, they will lose or gain the number of electrons needed to become more stable
The most stable electron configuration is a completely filled energy level
Which means you have a filled valence shell of 8 valence electrons known as the octet rule (except Hydrogen and Helium)

9. 8 is Great
Which means you have a filled valence shell of 8 valence electrons known as the octet rule
Or in the case of Hydrogen and Helium
2 electrons or zero electrons

10. Bonding
Positive and negative ions are attracted to each other (because of their opposite charges) and combine to form ionic compounds.
When ions combine to form compounds they must balance out their charges so that the compound ends up with no charge (electrically neutral)

11. The POSTIVE ion (cation) always goes FIRST!
Predicting…
We can predict the formulas for ionic compounds by determining the number of each ion (cation and anion) that is needed to cancel each other’s charges
Note:
The POSTIVE ion (cation) always goes FIRST!

12. Cl Na IONIC bond is formed Valence Electrons? Valence Electrons? 7 1
How many does it want to gain or lose?
GAIN 1
What’s the charge? -1
Valence Electrons? 1
How many does it want to gain or lose?
LOSE 1
What’s the charge? +1

13. Sodium Chloride
Na+1 + Cl-1  NaCl
(+1) + (-1) = 0

14. O Li IONIC bond is formed Valence Electrons? Valence Electrons? 6 1
NEEDS ONE MORE!
Valence Electrons? 6
How many does it want to gain or lose?
GAIN 2
What’s the charge? -2
Valence Electrons? 1
How many does it want to gain or lose?
LOSE 1
What’s the charge? +1

15. Lithium oxide
Li+1 + O-2 
Li2O
2(+1) + 1(-2) = 0
CrissCross Method

16. Barium Iodide
Ba+2 + I-1  BaI2
(+2) + 2(-1) = 0

17. Magnesium phosphide
Mg+2 + P-3 
Mg3P2
3(+2) + 2(-3) = 0

18. Magnesium phosphide
Mg+2 + P-3  Mg3P2
3(+2) + 2(-3) = 0

19. Ionic Bonding Na Cl Cl Ca Cl
Ionic bonding occurs when a metal transfers one or more electrons to a nonmetal in an effort to attain a stable octet of electrons. For example, the transfer of an electron from sodium to chlorine can be depicted by a LDD. Na Cl Cl Ca Cl

20. O Cl P Na Ca Li Al Na+1 O-2 Na2O Anion Cation Valence 1Valence Lose 1
And Charge
6 valence
Gain – 2 Na
1Valence
Lose 1 +1
Na+1 O-2
Na2O Ca Li Al

21. O Cl P Na Ca Li Al Na2O Anion Cation Valence 1Valence Lose 1 +1
And Charge
6 valance
Gain – 2 Na
1Valence
Lose 1 +1
Na2O Ca Li Al

22. Naming Ionic Compounds
What is an Ionic Compound?
Positive Metal + Negative Nonmetal
To name compounds:
Positive Metal name + Negative nonmetal name (drop ending and add “ide”
NaCl = sodium chloride
Ba3P2 = barium phosphide

23. O Cl P F Na
Sodium oxide Ca Li Al Ba
Barium phosphide