1. Unit 6: Chemical Nomenclature - Ionic Compounds with Transition Metals and Polyatomic Ions

2. Write the formula for these:
Sodium Chloride
Calcium nitride
Barium oxide
Iron (III) oxide
Sodium phosphate

3. Transition Metals
Where are they found?

4. Why are they called transition?
Have multiple oxidation numbers they transition in between
Example:
Iron (II) and Iron (III)
Fe+2 and Fe+3

5. Transition metals oxidation numbers:
Iron (II) and Iron (III)
Fe+2 and Fe+3
The oxidation number is represented by the roman numeral next to the elements name.
Number
Roman Numeral 1 I 6 VI 2 II 7
VII 3
III 8
VIII 4 IV 9 IX 5 V 10 X

6. Identify the oxidation numbers of the transition metals:
Lead (IV) oxide
Cobalt (II) chloride
Silver (I) oxide
Chromium (VI) nitride
Gold (III) sulfide

7. Writing Formulas for Transition Metals:
Manganese (VII) sulfide
Cation symbol: _____ Anion symbol:_____

8. Practice:
Gold (III) Oxide
Titanium (IV) sulfide
Zinc (I) chloride

9. Writing the names of Ionic Compounds with Transition Metals
Just like you write the names of any ionic compound, but you MUST include the OXIDATION NUMBER of the transition metal.
This is completed using a roman numeral
Iron (III) oxide

10. Identifying the oxidation number
Most of the time it is easily identified, other times it is not.
To get the oxidation numbers you simply undrop and unswap
Fe2O3
Iron (III) Oxide
Use the oxidation number of the nonmetal to check your work.
Does it match the periodic table?
If yes, you are good to go
If no, you will need to unsimplify

11. MnO2 Example: MnO2 Begin by unswapping and dropping Mn +2 and O -1
What is the oxidation number of oxygen? _____ (according to the periodic table)
Does it match (yes or no)? ______
What do we need to do to unsimplify it?

12. Practice:
TiO AgI
ZnCl Sn3N2
CrS2

13. Ionic Compounds with Polyatomic Ions
A polyatomic ion is simply a compound with a charge.
Poly = many or more than 1
Atomic = atoms
Ion = charged atom(s)

14. Where can I find these?
Take a look at the back of your periodic table…
Those are you polyatomic ions

16. Looking at your polyatomic ions what do you notice?

17. Polyatomics Are treated as single units instead of individual elements
The charge of the ion is the oxidation number
We cage the beasts
Polyatomic ions keep their names
The rest of the ionic compound naming rules apply

18. Can you identify the compounds with polyatomics?
Circle the polyatomic ion in the compounds
NaCl
Co(CO3)2
Li2SO4
CsNO3
MgO
Cr3(PO4)2

19. Naming compounds with polyatomic ions
Name the cation
*If there is a transition metal make sure to include its oxidation number
Name the anion
*If it is NOT a polyatomic don’t forget to change the ending to –ide.

20. Example:
Na2(CO3)
Mg3(PO4)2
Pb(NO3)2

21. Writing formulas for compounds with polyatomic ions
Calcium Carbonate
Ca+2 (CO3)-2
Ca2(CO3)2
Don’t forget to round it to the simplest whole number ratio
________________________

22. Practice Sodium Chlorate Ammonia phosphate
Aluminum Nitrate Chromium (III) cyanide
Silver (I) phosphate Ammonia chloride