1. Writing & Naming Formulas of Ionic & Covalent Compounds1

2. Bonding Types

3. Ionic, Covalent, or Metallic
Review

4. Ionic Compounds
Crystalline Lattice

5. Ionic Compounds Contains a metal and nonmetal
The valence electrons from the metal are transferred to the nonmetal.
Metal is listed first, followed by the nonmetal.
Change the name of the nonmetal to ~ide.
Examples: sulfide, oxide, phosphide.
Ionic Example: NaCl
Sodium Chloride

6. Ionic Binary Compound Naming Practice
Al2S3
Ba3P2
BaO
CaBr2
CsI
Aluminum Sulfide

7. More Ionic Binary Compounds Naming Practice
Fr2Cl
FrF
Sr3N2
K2O
Mg3P2
Francium Chloride

8. The 5 steps for writing a binary ionic compound formula
Write the symbols of the two elements
Write the oxidation number of each as superscripts.
Drop the positive and negative signs
Crisscross the superscripts so they become subscripts.
Reduce when possible

9. Formula for Aluminum Oxide
Write the symbols of the elements Al O

10. Formula for Aluminum Oxide
Write the oxidation numbers for each element +3 -2 Al O

11. Formula for Aluminum Oxide
Drop the positive & negative sign. 3 2 Al O

12. Formula for Aluminum Oxide
Crisscross the superscripts so they become subscripts 3 2 Al O

13. Formula for Aluminum Oxide
Reduce subscripts when possible. (not possible here) Al O 3 2

14. Examples of Reduction of Subscripts
Sr2O2 Al3P3 Pb2O4 Ba3N2
SrO

15. Ionic Binary Compound Formula Practice
Potassium iodide
Lithium bromide
Magnesium oxide
Sodium nitride
Radium phosphide KI

16. More Ionic Binary Compound Formula Practice
Gallium Fluoride
Strontium chloride
Cesium sulfide
Aluminum bromide
Barium Phosphide
GaF3

17. Polyatomic Ions
Polyatomic (many atoms) ions are covalent molecules with a charge. They behave as if they were one-atom ion.

18. Note: Ammonium is the only polyatomic ion with a + charge.
Polyatomic Ions
Use your reference sheets to determine the name of the following polyatomics.
NH4+1 C2H3O2-1 ClO3-1 NO3-1
OH-1 CO3-2 SO4-2 PO4-3
Note: Ammonium is the only polyatomic ion with a + charge.
Treat polyatomic ions as you would an ion – crisscross to determine the formula.
The only difference is that when you have more than one of a Specific polyatomic ion in a formula you must encase it in parenthesis.

19. Writing Names with Polyatomics
Ca3(PO4)2
NH4Br
NaNO3
K2SO4
Mg(ClO3)2
Calcium Phosphate
As in all ionic compounds you must reduce subscripts, but you cannot change the formula of the polyatomic ion. You can only reduce subscripts outside the parenthesis.

20. Writing Names with Polyatomics
Lithium Hydroxide
Potassium Carbonate
Barium Acetate
Ammonium Sulfide
Strontium Sulfate
LiOH

21. Rolling Atoms Instructions: Obtain a yellow cube and a blue cube
Roll the dice and using the elements that appear on the tope face, write it’s name, ion, along with the correct formula and name for the compound in the template provided
Use the dice to write 30 different compound formulas and names. You must have 30 different compounds!! After you reach 15, you will need to come up and get a new set
When finished, you need to turn in your template and get a molecular naming review half sheet
Metal
Nonmetal
Metal Ion
NM Ion
Cmpd. Name
Cmpd. Formula 1.

22. Covalent Compounds Water Molecule Hydrogen Atom Oxygen Atom

23. Covalent Compounds Contains 2 or more nonmetals
The valence electrons are shared between the nonmetals.
Must use prefixes in the name.
Name tells you the formula.
Example: N2O4 – dinitrogen tetroxide
You CANNOT reduce the formulas

24. Mono -1 Di – 2 Tri – 3 Tetra – 4 Penta – 5
Covalent Prefixes
Mono -1 Di – 2 Tri – 3 Tetra – 4 Penta – 5
Hexa – 6
Hepta – 7
Octa – 8
Non – 9
Deca -10
A prefix tells you the number of atoms of that element in the compound.

25. Naming Covalent Compounds
N2O3
CH4
PO5
S2F4
P4O10
Dinitrogen trioxide

26. Writing Formulas for Covalent Compounds
Carbon Monoxide
Phosphorus Pentachloride
Sulfur hexafluoride
Dinitrogen trioxide
Sulfur dioxide CO

27. Ionic & Covalent Structure
Water
Ionic Compounds form a crystalline lattice – repeating pattern of ions.
Covalent compounds form individual molecules that are not connected to each other.
Na+1 Ions
Cl-1 Ions
Sodium Chloride

28. Name These Compounds
PCl3
Sr3N2
KOH
NO2
MgCO3
Phosphorus trichloride

29. Write formulas for these compounds
Calcium Chlorate
Sodium Bromide
Sulfur hexafluoride
Carbon tetrachloride
Potassium Phosphate
Ca(ClO3)2

30. Review of Ionic Compounds
Include Metals & Nonmetals You need oxidation numbers Name the metal Change the Nonmetal to –ide ….Unless it has a polyatomic and you give it it’s name…

31. Summing up: Ionic
Ionic bonding occurs between a metal and a nonmetal. Metals lose all their valence electrons and become cations. Nonmetals gain enough electrons to fill their valence level and become anions.
Always crisscross oxidation numbers and reduce to determine the formulas of ionic compounds
Do not use prefixes in the names.
Ions form a crystalline lattice.

32. Summing up: Covalent
Covalent bonding occurs when two nonmetals share electrons to fill their valence energy level.
Never use oxidation numbers to determine the formula. There aren’t any since the two atoms share electrons, they do not take on a charge.
Always use prefixes in the names.
Atoms combine to form individual molecules.

33. WarmUp What is necessary to write ionic compounds?
Which elements are involve d in ionic compounds?
When writing names for covalent compounds what must be included?
Which elements are involved in covalent compounds?

34. Chemical Formulas Vocab
Ionic Compounds Valence Electrons Polyatomic Ions Covalent Compounds Prefixes Crystalline Lattice Structure Molecules

35. Remember Covalent Bonds – Molecules 2 or more nonmetals
prefixes Phosphorus Pentachloride PCl5
name it with prefixes CO Carbon Monoxide
Ionic Bonds-
crystalline lattice
metal & nonmetal
criss cross oxidation numbers: Al+3O-2  Al2O3
name as you see it Aluminum Oxide