1. E29: Inorganic Nomenclature
(Naming ionic compounds)

2. You should know…
The oxidation numbers, names, & symbols for the ions on pg. 16 in your WB (test tomorrow)
Cations are positive (tend to LOSE e-)
Anions are negative (tend to GAIN e-)
Opposites attract!
Cations will be attracted to anions in such a way that together their net charge is ZERO (balanced).
Monoatomic = single element (like H+)
Polyatomic = multiple elements bonded (like SO3 -2)

3. Periodic Table so far… Elements in the same group share properties +1
(do not bond, no charge)
Noble gasses= stable
Periodic Table so far…
Elements in the same group share properties +1
Zig zag “staircase” separates metals from nonmetals +2 -2 -1
Transition metals (Roman numerals)
Metals | Nonmetals
(+) (-)

4. (do not bond, no charge)
Noble gasses= stable
More Periodic Table
Group charges tend to continue as we go inward, skipping over the transition metals trench. +1 +2 +3 ±4 -3 -2 -1
Transition metals (Roman numerals)

5. Formula writing for Ionic Compounds
Start with the POSITIVE
Write the symbol for the cation first (on left), followed by the anion (on right) Ex: NaCl
Make the charges balance with subscripts.
Make the net ionic charge equal zero by adding subscripts as needed to each ion. Ex: CaBr2
Keep your polyatomics together.
Treat a polyatomic ion as a package deal, put parentheses around it before doing subscripts if needed. Ex: Ba(NO2)2 / Ba=+2 & NO2= - 1

6. Formula writing for Ionic Compounds
TRY IT!
Potassium bromide = _______________
Calcium chloride = _________________
Iron (III) oxide = ____________________
Barium chlorate = __________________
Magnesium phosphate = _____________

7. Naming Ionic Compounds
Start with the POSITIVE
Write the cation exactly as it appears on the oxidation list.
Don’t forget Roman numerals! Some math may be needed to determine the charge ex: Fe(OH)2
Negative comes last.
Monoatomics change the ending to –ide. ex: oxide, fluoride
Many polyatomics end in –ite or –ate.
ates have 1 more oxygen that ites do ex: nitrite/nitrate
Balancing subscripts do NOT affect the name.

8. Naming Ionic Compounds
TRY IT!
Li2S = ___________________________
AlBr3 = ___________________________
KMnO4 = _________________________
NH4OH = _________________________
CuO = ___________________________

9. Homework: start now!
WB pg 21: Do all multiples of 5 (5, 10, 15…), both columns
Check answers at front if finished during class.
E28 test is tomorrow! Study!
Check your p.18 practice test answers at the front
Check answers on blog at home(MHSchemistry.wordpress.com)
Extra time? Read E29 p22

10. Check p21 answers
5) Li2S 5) Potassium sulfide 10) Ag2O 10) Lead (II) iodide 15) FeCl3 15) Iron (II) bromide 20) Al2(SO4)3 20) Strontium sulfite 25) Hg3(PO4)2 25) Copper (II) phosphate 30) NaMnO4 30) Tin (II) chromate

11. E29 Day 2: Hydrated Ionic compounds
Remember that hydrates are ions which tend to have a certain amount of WATER attached to their crystalline structure.
Written _____ • H2O
Example: CuSO4• 5 H2O
Each CuSO4 molecule bonds to 5 water molecules.

12. Naming Hydrated Ionic compounds
Name the first part just like we did yesterday, leaving a space afterward.
Example: CuSO4 • 5 H2O
SO4 is -2, so it must be: Copper (II) sulfate
Look at the coefficient for the water- write THE GREEK PREFIX to match that number, followed by the word “hydrate.” That’s it!
CuSO4 • 5 H2O =
Copper (II) sulfate pentahydrate
GREEK PREFIXES:
1= mono
2= di
3= tri
4= tetra
5= penta
6= hexa
7= hepta
8= octa
9= nona
10= deca

13. Naming Hydrated Ionic compounds
TRY IT!
Fe(NO3)3 • 9 H2O =
_______________________________
2. BaCl2 • 2 H2O =
Magnesium sulfate heptahydrate =
__________________
GREEK PREFIXES:
1= mono
2= di
3= tri
4= tetra
5= penta
6= hexa
7= hepta
8= octa
9= nona
10= deca

14. HOMEWORK
WB page 22 all ODD practice problems (under Hydrated Ionic Compounds)
ANSWERS:
Copper chloride dihydrate 1) CaCl2 • 2H2O
3) Iron (III) chloride trihydrate 3) BaI2 • H2O
5) Nickel (II) chloride hexahydrate 5) FeCl3• 4H2O

15. Naming Acids All acid formulas start with hydrogen (H). ex: HCl
There are 2 types of acids: binary acids & oxyacids.
BINARY acids:
Have just hydrogen & a monoatomic anion (2 elements total)
Are usually aqueous (aq) = dissolved in water.
NAMES: ex: HCl
Start with “hydro” hydro
Write the ROOT for the anion hydrochlor
Add suffix “-ic” hydrochloric
Leave a space, then write “acid” hydrochloric acid

16. Naming Binary Acids TRY IT! H2S = __________________________________
Hydro-
root
-ic
acid
Naming Binary Acids
TRY IT!
H2S = __________________________________
HI = ___________________________________
H3P = __________________________________

17. Naming Oxyacids
Oxyacids contain hydrogen and a polyatomic ion containing oxygen. Ex: H2SO4
When naming oxyacids, follow these steps:
Determine the name of the anion.
Write the root word for the anion.
If the anion’s name ends with “–ate” change to the suffix “ic”. If the anion’s name ends with “–ite” change to the suffix “ous”
Leave a space, then write the word “acid”

18. Naming Oxyacids: Example 1: H2SO4 = sulfuric acid (ate ic)
but H2SO3 = sulfurous acid (ite ous)
Example 2: HNO3 = ________________________
but HNO2 = ________________________
But wait, there’s more! ….

19. Naming Oxyacids:
There is a pattern to the prefixes and suffixes of oxyanions!
Anion Corresponding Acid
ClO41- = perchlorate HClO4 = perchloric acid
ClO31- = chlorate HClO3 = chloric acid
ClO21- = chlorite HClO2 = chlorous acid
ClO1- = hypochlorite HClO = hypochlorous acid
Cl = chloride HCl = hydrochloric acid
When writing the formulas for acids, follow the same rules for writing the formulas of ionic compounds!
* Hint: Find the “ate” anion FIRST (ex. NO31-, ClO31-, C2H3O21-…)
**Remember to balance charges!!!

20. Naming Oxyacids
Per___ic acid
ate _____ ic acid
ite _____ ous acid
Hypo ____ ous acid
No O Hydro____ic acid
= a binary acid
TRY IT! The ion MnO4 = HMnO4 = HMnO3 = HMnO2 = HMnO = HMn=

21. Binary Molecular Compounds
These have two nonmetals. ex: CO These aren’t really ions, so they have different rules.
Names tell number of each element, using Greek prefixes to describe subscripts.
Write prefix matching the subscript of 1st nonmetal (if just 1, mono is usually left out), followed by full name of the 1st element.
Write prefix matching the subscript the 2nd element mono IS usually written for the 2nd if there’s 1, followed by ROOT for the name of 2nd element.
Add suffix “ide”. ex: CO2 = carbon dioxide
GREEK PREFIXES:
1= mono
2= di
3= tri
4= tetra
5= penta
6= hexa
7= hepta
8= octa
9= nona
10= deca

22. Binary Molecular Compounds
TRY IT!
CO = ___________________________
SO3 = __________________________
N2O4 = __________________________
Nitrogen trihydride= _______________
Diphosphorous hexoxide = ____________
GREEK PREFIXES:
1= mono
2= di
3= tri
4= tetra
5= penta
6= hexa
7= hepta
8= octa
9= nona
10= deca

23. HOMEWORK for Monday WBpg 23 ALL odd practice problems (acids)
WB pg 24 #1 & 10 both columns
MEET IN COMPUTER LAB B325 MON & TUES!