1. Naming ionic compounds

2. Chemical names Always has 2 parts
The first part is a POSITIVE ion and is always a metal
An example is Sodium (Na)
The second part is a NEGATIVE ion and is always a non-metal
An example is Chlorine (Cl)

3. Chemical names We always have to change the non-metal’s name
We change the ending from
“ine” to “ide”
Example: Chlorine becomes Chloride
Table salt is then called Sodium Chloride, not Sodium Chlorine)

4. Calcium and Nitrogen Potassium and Oxygen Lithium and Chlorine
Practice
Calcium and Nitrogen
Potassium and Oxygen
Lithium and Chlorine
Magnesium and sulphur
Silver and Fluorine

5. Why? Chemical formula We write sodium chloride as NaCl
We write aluminum chloride as AlCl3
Why?

6. Chemical formula We must examine that charges that each ion has.
Na has a charge of +1
Cl has a charge of -1
Together, they cancel each other out, and can be NaCl

7. Chemical formula Al has a charge of +3 Cl has a charge of -1
If these are going to bond properly, we will need 3 Cl to match the Al
So 1 Al and 3 Cl
We write this as:
AlCl3

8. Chemical formula Practice with Zinc and Nitrogen (Zn and N) Zn is +2
How can we make these equal?
We need 3 Zn and 2 N
We write this as Zn3N2

9. Practice
In pairs, complete the practice problems on pages 86 and 87. Work with another team. After every 5 questions, switch, and mark the other teams answers.
Tell the other team if they are on the wrong track. Help them correct errors.

10. Multivalent ions
As you have noticed, some ions have more than one charge!
Example: Iron can be +2 or +3
If we use the +2 charge, we say “iron two”
Iron (II) Oxide is said “Iron two oxide”
How would you say
Iron (III) Oxide?

11. Practice Chromium (II) chloride Copper (I) sulphide
Iron (III) phosphide
Tin (IV) nitride
How do you write these as formulas?

12. Multivalent formulas Identify each ion’s charge
Make each ion’s charge equal
Use subscripts to write the formula
Example: Iron (III) sulphide
Iron is +3
Sulphur is -2
We need 2 Iron and 3 Sulphur (totals 6)
We write Fe2S3

13. Practice
In pairs, complete the practice problems on page 89. Work with another team. After every 3 questions, switch, and mark the other teams answers.
Tell the other team if they are on the wrong track. Help them correct errors.
Remember to use the positive ion charge that is in the roman numerals!

14. Multivalent ions
If we see Fe0, how do we know which iron was used? Iron (III) or Iron (II)?
O is -2
Since there are no subscripts, in order to be balanced, that Fe must be +2!
So the answer is Iron (II)

15. Multivalent ions
If we see Fe203, how do we know which iron was used? Iron (III) or Iron (II)?
O is -2 x 3 = -6
There are 2 irons…if they are going to equal 6, they MUST each have a charge of +3
So the answer is Iron (III)

16. Practice
In pairs, complete the practice problems on pages 90. Work with another team. After every 3 questions, switch, and mark the other teams answers.
Tell the other team if they are on the wrong track. Help them correct errors.

17. questions
Complete questions 4 and 5 on page 95.
Remember to check if the metal is multivalent.
If it is multivalent, you must use the correct charge! Look closely, and make sure things balance.
You must also use roman numerals if you are writing out the name!

18. Next day
Bring any products from home…shampoo, deodarant, hairspray, cologne, food, etc.
Whatever you bring, make sure it has labels!

19. Polyatomic ions Polyatmoic ions do not exist on their own.
They are ALWAYS paired up with an opposite charge
Each polyatomic ion has a charge…so you can balance it the same way you were doing the others!
Example: Iron (III) hydroxide is Fe(OH)3
Look at the charge of OH on page 92.
Put brackets around it!
Say it just like it says on page 92.

20. Two polyatomic ions
Instead of using a metal and a polyatomic ion, you can link 2 polyatomic ions together
Ammonium (NH4) is +1
Carbonate (CO3) is -2
You will need 2 ammonium ions and 1 carbonate ion.
(NH4)2CO3

21. Practice
In pairs, complete the practice problems on pages 91. Work with another team. After every 3 questions, switch, and mark the other teams answers.
Tell the other team if they are on the wrong track. Help them correct errors.

22. questions
On page 95, complete questions 3 and 5

23. Build a compound With clay, build a compound.
Tell you partner what elements are in your compound, and see if they can write out the chemical name and the chemical formula.
Use the internet to help you if you need to look at where electrons are shared, or gained or lost.
Use polyatomic ions to make it harder!
Destroy, and try another one!

25. Products
Find a chemical listed on a container, and see if you can model it with clay.
If it’s a complicated chemical, you may need to use the internet for help.
See if you partner can guess the chemical model you made.