1. Naming Compounds
Chemical Bonding

2. Review of the Periodic Table
Each row is called a period.
All elements in a period have the same number of atomic orbitals (or shells)
Each column is called a group or family.
All elements in a group have the same number of valence electrons

3. Lewis Dot Diagrams Discovered by Gilbert N. Lewis
Method of representing valence electrons
Discovered by Gilbert N. Lewis
Several examples include:
Sodium – 1 valence electron: Na
Nitrogen – 5 valence electrons: N
Bromine – 7 valence electron: Br

4. Lewis Structures
Ionic – show transfer of e-

5. Things to know about Ionic
Lewis Dot Diagrams represent?
Ionic compounds are made up of?
The electrons are being?
What is written first?
Opposite charges will?

6. S.O.X’S. How to write a formula Overall net charge must equal zero.
Ionic Formulas
Overall net charge must equal zero.
S.O.X’S.
Symbols-> Oxidation # -> Crisscross -> Simplify
Don’t show charges in the final formula.

7. Writing Formula Practice
Potassium Chloride
K+ Cl-
 KCl
Aluminum Bromide
Al+3 Br-
 AlBr3
Beryllium Sulfide
Be+2 S-2
 BeS = Reduce

8. How to Name an Ionic Compound
Ionic Nomenclature
How to Name an Ionic Compound
Write the name of the Cation (Metal) first. It comes straight off the periodic table.
Change ending of the Anion (Nonmetal) to end in -ide.

9. Naming Practice Al2O3 CaS Na3P Aluminum Oxide Calcium Sulfide
Sodium Phosphide

10. Polyatomic Ions
When you have a compound that involves more than 2 elements, you must look at a Polyatomic Chart for help.
When writing formulas, keep these ions in parentheses.
These ions will also have different endings (- ate) (-ite)
Helpful for determining between individual atoms and polyatomic ions

11. Writing a Formula Look at the ending of the name (-ATE) or (-ITE)
You need to determine if a Polyatomic Ion is present!
Look at the ending of the name
(-ATE) or (-ITE)
What are some exceptions???
What if the ending is (-IDE)?
What will you do then?

12. Writing Polyatomics KNO3 Aluminum Sulfide Al2S3 Barium Phosphite
Potassium Nitrate
KNO3
Aluminum Sulfide
Al2S3
Barium Phosphite
Ba3(PO3)2

13. Naming Polyatomics
Look for more than two elements. That’s means a Polyatomic is present.
Match up the polyatomics and write the correct names and ending straight from the chart.

14. Practice w/ Polyatomics
CaSO4
Calcium Sulfate
Ga(IO3)3
Gallium Iodate

15. Writing with Transitions
When a Transition metal is involved in the bond, you must identify which form of the atom is bonding.
These atoms can have different oxidation numbers.
Look for the Roman Numeral in the name when writing the formula. The Roman numeral is the oxidation number of the transition metal.

16. Practice Writing Transitions
Copper (II) Fluoride
CuF2
Zinc (I) Phosphate
Zn3PO4
Nickel (IV) Oxide
NiO2 (Simplified formula)

17. Naming Transitions
When Naming the compound, you must balance the total charge, it has to be zero!
Look at the Anion. Determine the total sum of the charges provided by the Anion.
Look at the Cation. Remembering that the sum of the ionic compound must equal zero, determine the positive charge, and roman numeral.

18. Practice Naming Transitions
Au2S
Gold (I) Sulfide
Co2O3
Cobalt (III) Oxide
FeN
Iron (III) Nitride

19. C. Molecular Nomenclature
Prefix System (binary compounds)
How do we recognize these?
Where are nonmetals found???
Add prefixes to indicate # of atoms. Omit mono- prefix on first element.
3. Change the ending of the second element to -ide.

20. C. Molecular Nomenclature
PREFIX
mono-
di-
tri-
tetra-
penta-
hexa-
hepta-
octa-
nona-
deca-
NUMBER 1 2 3 4 5 6 7 8 9 10

21. Special Rules with Mono
If there is only one of the first element, then the prefix mono is not used.
If there is only one of the second element, then the prefix mono is necessary.
Ex.
CO – Carbon Monoxide
CO2 – Carbon Dioxide
C2O – Dicarbon Monoxide

22. N3O6 - Trinitrogen Hexaoxide NO2 - Nitrogen Dioxide
Also….
There is no reducing for covalent compounds. What you see is what you get. If you reduced, you would change the chemical formula and ratio of the elements in the bond….Not good….
C2H4 - Dicarbon Tetrahydride
CH2 - Carbon Dihydride
N3O6 - Trinitrogen Hexaoxide
NO2 - Nitrogen Dioxide

23. You Try CCl4 carbon tetrachloride N2O SF6 dinitrogen monoxide
sulfur hexafluoride

24. Try some more arsenic trichloride AsCl3 dinitrogen pentoxide
tetraphosphorus decoxide
AsCl3
N2O5
P4O10

25. C. Molecular Nomenclature
The Seven Diatomic Elements
I2 Br2 Cl2 F2 O2 N2 H2 H N O F Cl Br I

26. Acids All acids will end in the word “acid”. (ex. Hydrochloric acid)
You will know a compound is an acid because the formula ALWAYS STARTS WITH a H
- (ex. H2S.)
*(Not always true in real life, but it will be for us!)
All acids will end in the word “acid”. (ex. Hydrochloric acid)

27. When to include prefix “Hydro”
You use the “Hydro” only when the formula includes hydrogen and one other element. (no polyatomic)
HCl = hydrochloric acid
Short Formula = Long Name
Always “Hydro(Insert element here)-ic Acid

28. When Not to Include Hydro
No Hydro prefix is used if there is a polyatomic Ion Present
If the acid has a polyatomic ion in it, then “hydro” will not be at the beginning of the name.
HClO3 = chloric acid
Long Formula = Short Name

29. One last thing….
When naming acids with polyatomics, sometimes there are two ions with similar names: Ex) Nitrate and Nitrite
If the polyatomic ion ends in “–ate”, then the suffix “-ic” will be added.
Example – Nitrate  HNO3  Nitric Acid
If the polyatomic ion ends in “–ite”, then the suffix “- ous” will be added.
Example – Nitrite  HNO2  Nitrous Acid

30. Examples: H2S Polyatomic Ion?
the formula is “short”, so the name is long , hydro is needed.
What is the ending?
Name: Hydrosulfuric acid

31. More Examples… HNO2 Polyatomic ion?
The formula is long, so the name is short, hydro is not needed
What is the correct ending?
Name: Nitrous acid

32. Last Example H2SO4 Polyatomic ion?
The formula is long, so the name is short, hydro is not needed
What is the ending?
Name: Sulfuric acid

33. Writing Formula Help SOCS!
Find oxidation numbers (charges) and criss cross as you would with ionic compounds.
If name is long (includes Hydro) then it is the element hydrogen and another element from periodic table.
If the name is short, you have a polyatomic ion. Look for “ –ic” or “-ous” to determine which polyatomic ion to use.

34. Short name  Long formula (Polyatomic) Formula: H3PO3
Phosphoric acid
Short name- long formula (polyatomic)
use oxidation numbers to get the formula
Formula: H3PO4
Hydrophosphoric acid
long name- short formula – (not a polyatomic)
criss cross ox #
Formula: H3P
Phosphorous acid
Short name  Long formula (Polyatomic)
Formula: H3PO3

35. Practice Naming! HF
HBrO3
H2CrO4
H3P
HClO2

36. Hydrosulfuric Acid Acetic Acid Hydroiodic Acid Phosphoric Acid
Practice Writing!
Hydrosulfuric Acid
Acetic Acid
Hydroiodic Acid
Phosphoric Acid
Chlorous Acid