1. IONIC COMPOUNDS

2. 12/9 Today you need… The paper from the side table
Your polyatomic/d-block chart
Quick review  Name the following on a clean sheet of paper (you have 10 minutes):
Li2O -C2S4
Be(NO3)2 -AlPO4
Co(OH)2

3. 12/1 Pre-AP Turn in your molecular geometry HW
Have a seat and clear your desk
Today you will take TWO quizzes. The first one will be another memorization quiz. If you already made an A on this quiz, you are exempted. The second quiz will be a simple one over covalent compounds. You will review on your own and then take the quiz.
Today we will continue with naming IONIC compounds. They are different then covalent, so you will need to pay attention when we are learning this.

4. On a clean piece of paper:
1. NAME : SO2, N2O5, SF6, CBr3
2. FORMULA: As2O5, XeF5, CCl4
3. What are the shapes of SO2, CCl4, CBr3, Br2, BF3
4. List the seven diatomic elements
5. What is another name for a covalent compound?
6. How are electrons BONDED in a covalent compound?
7. How do you think you will be able to tell the difference between covalent and ionic compounds?

5. 12/2 Pre-AP Pick up the paper from the side table and have a seat
Take out the periodic table you colored and took notes on yesterday.
I will quickly teach you to name and write formulas for binary ionic compounds and ionic compounds that have a d-block metal. HW: Naming Ionic Compounds Part 1 and Part 2

6. Ionic COMPOUNDS:
Compounds made up of a METAL (cation) and a nonmetal (anion).
Electrons are TRANSFERRED between the metal and the nonmetal to obtain a noble gas configuration.
There are THREE different types of ionic compounds you will learn to name and write formulas for:
1. Binary ionic
2. Ionic compounds containing polyatomics
3. Ionic compounds with the metal located in the d-Block

7. Monatomic Ions: need to know their trend on the periodic table
Ions formed from a single atom
Gain or lose electrons to attain a noble gas configuration

8. Monatomic Ions: Common Charges1+
Chart with charges of ions on page 205 2+ 3+ NA 3- 2- 1-

9. NAMING TYPE 1: Binary Ionic Compounds
Compounds composed of 2 different elements that are ionically bonded
Charges of ions must “cancel out” so the overall charge on the compound is 0.
Use the “crisscross method” to write the formula.

10. Binary Ionic Compunds: Crisscross method
Find the formula for a compound formed by the ions of aluminum and oxygen.
Write the symbols for the ions side by side, CATION FIRST.
Al3+ O2-
Cross over the charges by using the number only from each ions’ charge. Make this the subscript for the other ion.
Al2O3
Check the subscripts to make sure that they cannot be simplified.

11. Binary Ionic Compounds: Crisscross Method (swap and drop)
Write the formulas for the binary ionic compounds formed between the following elements:
Sodium and phosphorus
Gallium and nitrogen
Na3P
GaN

12. Naming Binary Ionics
Combine the names of the cation and anion, cation first.
Example: Al2O3
Cation: aluminum
Anion: oxide
Compound: Aluminum oxide
Most elements form only one ion, so you usually don’t have to indicate the charge in the name.

13. NAMING TYPE 2: ionic compounds with d-Block metals
Some elements can form more than one ion.
Example: Iron can form a +2 and +3 ion
When you name these compounds, you have to indicate which ion is present.
If I asked you to write the formula for iron oxide without telling you if it was Fe+2 or Fe+3, then you could write 2 different formulas
FeO Fe2O3
Use Roman numerals in parentheses in the name to indicate the charge on the ion.
FeO is Iron (II) oxide Fe2O3 is Iron (III) oxide

14. Pre-AP 12-1
Today you need the papers from the side table AND your answer document
We will quiz the last 10 minutes of class over bonding
We will review naming binary IONIC compounds and learn to name compounds with the metal in the d-block and compounds containing polyatomic ions

15. QUICK CHECK: Write the formula: NAME: Lithium flouride
Beryllium nitride
Strontium bromide
NAME:
CaCl2
MgO2
K2S
N5O10

16. D-Block ionic compounds
Use ROMAN NUMERALS to indicate the charge of the CATION when formula writing.
The roman numeral will be written between the cation and anion when naming a compound.

17. Naming Practice Write the formula Chromium (III) fluoride
Iron (III) oxide
Tin (II) sulfide
Lead (II) chloride

18. Naming Practice
Name the following compounds
Cr3N2
CuO
CoF3
Ag2S

19. NAMING TYPE 3: Compounds Containing Polyatomics
Chart of polyatomics on page 210.
Compounds containing polyatomics are named the same way at binary ionics.
Name the cation
Name the anion
Example: Name the compound AgNO3
Cation: silver
Anion: nitrate
Compound: silver nitrate

20. Polyatomic Examples Write the formula for tin (IV) sulfate
Cation: Sn+4
Anion: SO42-
Formula using crisscross method: Sn2(SO4)4
If you need more than one polyatomic ion, put it in parentheses to avoid confusion!
Wrong: Sn2SO44 Right: Sn2(SO4)4

21. Polyatomic Examples Write formulas for the following ionic compounds:
Sodium iodide
NaI
Calcium nitrite
Ca(NO3)2
Copper (II) sulfate
CuSO4

22. Polyatomic Examples Give the names for the following compounds Ag2O
Silver oxide
KClO3
Potassium chlorate
FeCrO4
Iron (II) chromate