1. Ionic Compound Naming
Taking electrons, not sharing them

2. Thumbs up = got it!, In the middle = okay with concept, thumbs down = not good (go over)
Lets do a quick review!

3. An atom losses 2 electrons
Cation or Anion
An atom losses 2 electrons
An atom gains 1 electron
Cation
Anion

4. Metals for ______ ions and nonmetals for ______ ions.
Negative Ions
Positive Ions
Metals for ______ ions and nonmetals for ______ ions.

5. Which is an Ion? Which is an Atom?

6. Forming an Ionic Compound
1st Ion
2nd Ion
Metal
Positive Ion
Cation
Non-metal
Negative Ion
Anion

7. So how do you name these things?!

8. Rules for naming binary ionic compounds
The positively charged ion must always be written first
The negatively charged ion must always be written second
The end of the negative ion’s name must be changed to ‘ide’ to indicate it is a compound

9. Examples of ionic compounds
Sodium and chlorine
Sodium has one valence electron  𝑁𝑎 1+
Chlorine has seven valence electrons  𝐶𝑙 1−

10. Examples of ionic compounds
Sodium and chlorine
Sodium has one valence electron  𝑁𝑎 1+
Chlorine has seven valence electrons  𝐶𝑙 1−
The electron that sodium wants to give up is accepted by chlorine, resulting in ionization

11. Examples of ionic compounds
Sodium and chlorine
Sodium has one valence electron  𝑁𝑎 1+
Chlorine has seven valence electrons  𝐶𝑙 1−
The positively charged sodium will be attracted to the negatively charged chlorine, creating an ionic bond, forming an ionic compound
This ionic compound is called sodium chloride
The electron that sodium wants to give up is accepted by chlorine, resulting in ionization

12. Rule Example 1 K3P Example 2 MgS Example 3 Al2O3
1. Name the metal ion.
2. Name the non-metal ion with the ending "-ide".
3. Write the name of the compound.

13. Phosphorus  Phosphide
Rule
Example 1
K3P
Example 2
MgS
Example 3
Al2O3
1. Name the metal ion.
 Potassium
2. Name the non-metal ion with the ending "-ide".
Phosphorus  Phosphide 
3. Write the name of the compound.
Potassium phosphide

14. Potassium phosphide Magnesium sulphide
Rule
Example 1
K3P
Example 2
MgS
Example 3
Al2O3
1. Name the metal ion.
 Potassium
Magnesium
2. Name the non-metal ion with the ending "-ide".
Phosphorus  Phosphide 
Sulphur  Sulphide
3. Write the name of the compound.
Potassium phosphide
Magnesium sulphide

15. Potassium phosphide Magnesium sulphide Aluminum oxide
Rule
Example 1
K3P
Example 2
MgS
Example 3
Al2O3
1. Name the metal ion.
 Potassium
Magnesium
Aluminum
2. Name the non-metal ion with the ending "-ide".
Phosphorus  Phosphide 
Sulphur  Sulphide
Oxygen  Oxide
3. Write the name of the compound.
Potassium phosphide
Magnesium sulphide
Aluminum oxide

16. On a separate piece of paper…
Example: name the ionic compound formed between the following elements
Potassium and fluorine
Calcium and oxygen
Nitrogen and beryllium
Phosphorous and lithium

17. How did you do?
Example: name the binary ionic compound formed between the following elements
Potassium and fluorine potassium fluoride
Calcium and oxygen calcium oxide
Nitrogen and beryllium beryllium nitride
Phosphorous and lithium lithium phosphide

18. Writing Formulas for Ionic Compounds
positive charges balance negative charges.
use this to find the ratio of positive ions to negative ions.
use the ratio to write subscripts in the formula.
Final formula must represent the smallest whole number ratio.

19. Example: Sodium fluroide
Rule
Example: Sodium fluroide
1. Identify each ion and its charge.
2. Determine the total charges needed to balance positive with negative.
3. Note the ratio of positive ions to negative ions (or swap and drop)
4. Use subscripts to write formula.
Na+ F-
1 Na + = +1
1 F- = -1
Ratio = 1:1
NaF

20. Example: Calcium oxide
Rule
Example: Calcium oxide
1. Identify each ion and its charge.
2. Determine the total charges needed to balance positive with negative.
3. Note the ratio of positive ions to negative ions (or swap and drop)
4. Use subscripts to write formula.
Ca2+ O2-
Ca2+ = +2
O2- = -2
Ratio = 1:1
CaO

21. Example: Magnesium phosphide
Rule
Example: Magnesium phosphide
1. Identify each ion and its charge.
2. Determine the total charges needed to balance positive with negative.
3. Note the ratio of positive ions to negative ions (or swap and drop)
4. Use subscripts to write formula.
Mg2+ P3-
Mg2+ x 3 = +6
P3- x 2 = -6
Ratio = 3:2
Mg3P2

22. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−

23. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
Fluorine can only accept one of magnesium’s electrons

24. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
Fluorine can only accept one of magnesium’s electrons, where does the other go?

25. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
Fluorine can only accept one of magnesium’s electrons, where does the other go? We need a second fluorine

26. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound 1- 2+ 1-

27. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound
This ionic compound is called magnesium fluoride 1- 2+ 1-

28. Examples of ionic compounds
Magnesium and fluorine
Magnesium has two valence electrons  𝑀𝑔 2+
Fluorine has seven valence electrons  𝐹 1−
The positively charged magnesium will be attracted to the two negatively charged fluorines, creating ionic bonds, forming an ionic compound
This ionic compound is called magnesium fluoride
The chemical formula of magnesium fluoride is: MgF2 1- 2+ 1-

29. Cross and drop
Ca2+ N3-

30. Cross and drop
Ca2+ N3- Ca3N2

31. Cross and drop
Ca2+ N3- Ca3N2

32. Cross and drop
Ca2+ N3- Ca3N2

33. Cross and drop
Ca2+ N3-
Ca3N2
Will this method always work?

34. Cross and drop Ca2+ N3- Ca3N2
Will this method always work? Yes, but you may have to reduce – Always want it in the LOWEST ratio
Ti4+ O2-  Ti2O4  TiO2

35. Let’s pull it all together!