1. IONIC COMPOUNDS

2. IN ORDER TO BE SUCCESSFUL:
1. Must memorize the D-block ions AND the polyatomic ions
2. Know the names and symbols of the elements

3. Significance of a Chemical Formula
Ionic formula-represents one formula unit
The simplest whole number ratio of cations to anions in the compound
CaBr2
No subscript=implied “1”
For every calcium ion in the compound, there are 2 bromide ions

4. TYPES OF IONIC COMPOUNDS:
1. monatomic (1 atom that has formed it’s cation or anion)
2. Binary (composed of one NONMETAL and one METAL)
3. ionic compounds with D BLOCK metals
4. Ionic compounds containing polyatomic

5. Monatomic Ions Ions formed from a single atom
Gain or lose electrons to attain a noble gas configuration

6. IONIC COMPOUNDS METAL (CATION +) and NONMETAL (ANION -)
Use the crisscross method.

7. Monatomic Ions: Common Charges1+ 2+ 3+ NA 3- 2- 1-

8. Naming Monatomic Ions Cations-same as element’s name
Example- Li+ is a lithium cation
Anions-drop the ending of the element’s name and at –ide
Example- F- is a fluoride anion

9. 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
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. D-BLOCK AND GROUP 14 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. Naming Practice
Write the formula and give the name for the compound formed by the ions:
Cr3+ and F-
CrF3, Chromium (III) fluoride
Na+ and S2-
Na2S, Sodium sulfide
Sn2+ and S2-
SnS, Tin (II) sulfide
Pb2+ and Cl-
PbCl2, Lead (II) chloride

15. Naming Practice Name the following compounds CuO LiBr CoF3
Copper (II) oxide
LiBr
Lithium bromide
CoF3
Cobalt (III) fluoride

16. Compounds Containing Polyatomics
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

17. 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

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

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

20. Let’s Play GO FISH!!! Directions:
potassium, magnesium, aluminum, germanium, indium, lithium, sodium, sodium, Fe+2, Ag+1, Cd+2, Zn+2, Ni+2, Cu+2, nitrate, sulfate, sulfite, sulfur, chlorine, nitrogen, hydroxide, phosphate, phosphorus, fluorine, oxygen, iodine, oxygen, calcium, Zn+1, bromine, Cu+1