1. BELLWORK 11/29/16
All metals _______ electrons, and have a ________ charge.
All non-metals ________ electrons, and have a ________ charge.

2. WRITING IONIC FORMULAS

3. Label these charges on your Periodic Table
Cations and Anions
Label these charges on your Periodic Table +1 +2 +3 -3 -2 -1
Skip transition Metals
Skip

4. Writing Binary Ionic Compound Formulas
A Binary Ionic Compounds is composed of two elements.
Ionic Compounds have to have an overall neutral (zero) charge.
In order to achieve this, we must balance the charges on the cation and the anion to make sure the resulting compound formed has a neutral charge.

5. Example #1
What is the overall charge on the Ionic Compound formed between these two atoms?
Na and Cl-1

6. Example #2
What is the overall charge on the Ionic Compound formed between these two atoms?
Mg+2 and O-2

7. Example #3
What is the overall charge on the Ionic Compound formed between
Mg and Cl-1
Since this compound has an overall positive charge, we need to balance the positive and negative charges.
We use subscripts and multiply them by the charge to achieve an overall charge of of zero.

8. Example #4
What is the overall charge on the Ionic Compound formed between
Ca and P-3
Since this compound has an overall negative charge, we need to balance the charges

9. Writing Neutral Ionic Formulas
Sodium chloride
Metal Non-metal
Na Cl
Identify the chemicals as either a metal, transitional metal or non-metal
Write out the chemical symbols of each

10. Na Cl NaCl sodium chloride + 1 - 1 + 1 - 1 metal non-metal
1. Identify the metal and non-metal
2. Write the symbols
Write the charges
Swap-n-drop the charges and write them as subscripts.
A subscript of 1 is understood, and not written.
NaCl

11. metal
non-metal
Calcium oxide + 2 - 2 Ca O + 2 - 2 1 1
CaO

12. metal
non-metal
magnesium chloride + 2 - 1 Mg Cl - 1 + 2
MgCl2

13. metal
non-metal
calcium phosphide + 2 - 3 Ca P - 3 + 2
Ca3P2

14. PRACTICE QUESTIONS Beryllium fluoride Barium bromide Sodium nitride
Gallium sulfide
Calcium sulfide
Zinc bromide
Aluminum chloride
Cesium phosphide
Lithium phosphide
Germanium oxide
BeF2
BaBr2
Na3N
Ga2S3
CaS
ZnBr2
AlCl3
Cs3P
Li3P
GeO2

15. Writing Ionic Formulas Using Transitional Metals

16. Sometimes, the metal in your Ionic Compound is a Transitional Metal ( A metal found in group 3-12 on the periodic table).
When your metal is a transitional metal, it will be listed in the Left Column under Common Ions on your Chemistry Reference Page

17. How is A Transitional Metal Different from a Main group Metal?
A transitional metal can have more than one charge.
If we have a transition metal the charge will be shown in parentheses after the element name.

18. Examples: 1. Copper (II) and Bromine 2. Iron (II) and Oxygen
3. Lead (II) and chlorine
4. Mercury (II) and sulfur
5. Tin (II) and Fluorine
6. Iron (III) and Oxygen

19. BELLWORK 11/28/16 WHAT CHARGE DOES HYDROGEN HAVE? Ex: HBr - cation
NaH anion

20. Writing Ternary Ionic Formulas using Polyatomic Ions

21. Polyatomic Ions – Acts as the non-metal in an Ionic Compound
Sometimes a group of atoms are chemically bonded, and act as one anion with a negative charge.
A list of Polyatomic ions is listed in the two right-hand columns on your Chemistry Reference Page under Common Ions.
Exceptions: There are 2 polyatomic ions that have a positive charge. (NH4+(ammonium and Hg22+ (dimercury)

22. Examples:
Potassium sulfate-
Lithium Nitrate –
Copper (I) sulfate –

23. ANSWERS
K+SO  K2SO4
Li+NO  LiNO3
Cu+SO42-  Cu2SO4

24. Homework
Ch. 6 Worksheet #2