1. Naming Chemical Compounds

2. Binary Ionic Compounds
Binary = 2 types of elements
Ionic = made of ions
Compound = atoms bonded together

3. Ionic Compounds Positive ions attracted to Negative ions
Form a FORMULA UNIT
Cation first
Anion second

4. Type I The cation has a only one charge (oxidation #)
Alkali Metals (group 1A) +1
Alkaline Earth Metals (group IIA) +2
Group IIIA +3
Silver Ag+
Zinc Zn2+

5. Elemental anions When an element becomes an anion, Name ends in –ide
Fluoride
Chloride
Bromide
Oxide
Sulfide
Nitride
Phosphide

6. Type II
The cation (metal) has a more than one charge (oxidation #)
All Transition metals except for Ag and Zn (for our purposes)
Roman numeral is written after the CHARGE on the metal
Fe2+
Fe3+
Cu+
Cu2+
Iron(II)
Iron(III)
Copper(I)
Copper(II)
Ferrous
Ferric
Cuprous
Cupric

7. Naming ionic compouds (Type I and II)
First name cation
Type I
Just name metal element
Then name anion
Drop the last syllable
Elemental anions – Add the suffix “–ide”
Polyatomic Ions – Use the name of the PAI
Type II
Name metal element
Place roman numeral in parenthesis after name showing charge
To write most formulas
“swap ‘n’ drop”
Reduce atom ratios to smallest whole number ratios

8. Name the following: Na3N MgCl2 Al2O3 CuCl CuCl2 PbBr4 Sodium nitride
Magnesium chloride
Aluminum oxide
Copper(I) chloride
Copper(II) chloride
Lead(IV) bromide

9. Determine the formula of the following
Aluminum chloride
AlCl3

10. Polyatomic Ions Many anions are not just ions of one element.
When used in a compound
Use the name of the polyatomic ion as the anion
Polyatomic Ions
Many atoms with overall charge
Example: Chlorate ClO3-
Mostly nonmetals bonded to
Oxygen

11. Polyatomic Ion Naming Name the main element in the polyatomic ion
Drop last syllable add ending “–ate”
Example: Chlorate ClO3-
One fewer oxygen
Ends in “-ite”
Example: Chlorite ClO2-
One fewer than (-ite) oxygen
Hypo = under
Example: Hypochlorite ClO-
More oxygen than main ion
Hyper = over
Shortened to “per”
Example: Perchlorate ClO4-

12. Common Polyatomic Ions
NO3-
Nitrate
NO2-
Nitrite
SO42-
Sulfate
SO32-
Sulfite
PO43-
Phosphate
PO33-
Phosphite

13. Common Polyatomic Ions
Hydrogen can attach to polyatomic ions as H+
This adds H and reduces the overall charge by +1
Add the word Hydrogen before the PAI name.
Use prefix to denote how many hydrogen are present
PO43-
Phosphate
HPO42-
Hydrogen Phosphate
H2PO41-
Dihydrogen Phosphate
CO32-
Carbonate
HCO31-
Hydrogen carbonate

14. Molecular Compounds (Type III)
Lets start today by learning about a new way to view elements on the periodic table Lewis Dot/ Electron Dot Diagrams
Drawings represent just the outside (Valence) electrons
These are the only electrons that interact when elements react
Molecular compounds or Molecules
Made of two non-metals
SHARE electrons to get stable - 8 electrons in outside
Not bonded by positive and negative ions

15. How to tell if it’s Type III
Check FIRST element – is it a non-metal?
If YES, it’s a Type III
Write the name of the first element
Then name the second element
Drop the last syllable
Elemental anions – Add the suffix “–ide”
Use prefixes to denote number of each element

16. Prefixes Naming Molecular Compounds (Type III)
Use PREFIXES to show number of each element
Prefixes 1 2 3 4 5 6 7 8 9 10 11 12
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
Undec
Dodec

17. Using prefixes If there is only one of the first element
you omit the “mono”
DO NOT omit any other prefixes
The more electronegative element goes last
Electronegativity is an elements electron pulling power
Scale from
4.0 – F
.87 -Fr
Highest values are around F (O, N, Cl)

18. Name the following PCl3 CO2 NO N2O4 N2F5 OF2 Phosphorus trichloride
Carbon dioxide
Nitrogen monoxide
Dinitrogen tetroxide
Dinitrogen pentafluoride
Oxygen difluoride

19. Acids: 2 types 1. Those that are just H and one other element:
Consider Hydrochloric Acid
HCl
2. Those that contain a PAI (usually with oxygen)
Consider Sulfuric Acid
H2SO4
All acids have the H+ ion in them as the cation.
All acids have “acid” in their name

20. Naming Acids that do not contain oxygen
If the acid is just H+ and one other element and DOES NOT CONTAIN OXYGEN:
Give the Root name of anion element
Add the Suffix –ic on anion
Add the Prefix hydro-
Add the word acid to the end
Examples HF
H2S
Hydrofluoric Acid
Hydrosulfuric Acid

21. Naming Acids that contain oxygen
If the acid CONTAINS OXYGEN
Basically H+ and a polyatomic ion
Write the Root name of the PAI
If anion ends in -ate,
acid ends in –ic
If anion ends in –ite
acid ends in –ous

22. Naming Acids Examples #’s 40 and 48 H2SO4 H2SO3 HNO3 HNO2 HC2H3O2
Phosphoric Acid
Carbonic Acid
Assignment: Page
Sulfuric Acid
Sulfurous Acid
Nitric Acid
Nitrous Acid
Acetic Acid
H3PO4
H2CO3
#’s 40 and 48

23. Organic Molecules (Alkanes, Alkenes, Alkynes)
Carbon based
Naming is based on
Number of carbons in a chain
If carbon chain is straight or branched
If there are single, double or triple bonds
Where functional groups are attached
Functional groups
Groups of atoms attached to the carbon chain that always have the same properties no matter what molecule with which they are attached.

24. Alkanes The simplest Organic Molecules Only contain C & H CnH2n+2
Carbons single bonded to each other
Called carbon chain
Hydrogen bonded to Carbon
All alkanes end in –ane
C6H14
Hexane

25. Prefixes Prefixes pertain to all types of carbon molecules
Denote the length of the C chain.
Meth - 1C
Eth C
Prop - 3C
But C
Pent - 5C
Hex - 6C
Hept - 7C
Oct - 8C
Non - 9C
Dec - 10C
Undec - 11C
Dodec - 12C

26. What would you call a hydrocarbon that has:
9 carbons:_________
10 carbons:________
11 carbons: ________
12 carbons: ________

27. Alkenes and Alkynes Alkenes CnH2n Alkynes CnH2n-2
Carbons have a double bond between them
Alkynes CnH2n-2
Carbons have a triple bond between them
C6H12
Hexene
C6H10
Hexyne

28. Isomer Molecule with SAME formula but DIFFERENT structure
Naming Isomers of Alkenes and Alkynes
Find # of carbons in longest chain containing double or triple bonds
This gives the chemical its root name
Add suffix -ene, -yne to end of root
Carbon #1 is the end of chain closest to
The double or triple bond
Identify location of the 1st C to touch the double or triple bond
Write number to left of chemical name

29. Branched Hydrocarbons
Find # of carbons in longest chain containing s. d. or t. bonds
This gives the chemical its root name
Add suffix –ane, -ene, -yne
Carbon #1 is the end of chain closest to
Branch or (R group) for single bonds
The double/ triple bond
Identify the branch or (R group) - alkyl
Named by the number of carbons it has.
Specify location of Branch or (R group)
Use Carbon # that the group is attached to in longest chain.
If more than one alkyl group is the same
use prefix di, tri, etc. to alkyl name
Branch should be listed in alphabetical order
disregarding prefix (di, tri, tetra,….)

30. Branched Hydrocarbon Substituent Alkyl groups (R)- end in -yl
Methyl - 1C
Ethyl C
Propyl - 3C
Butyl C
Pentyl - 5C
Hexyl - 6C
Heptyl - 7C
Octyl - 8C
Nonyl - 9C
Decyl - 10C
Undecyl - 11C
Dodecyl - 12C

31. What is the name of the compound?
Hints
Number the Carbon chain from side closest to first alkyl group
Single carbon branch called methyl
Double carbon group called ethyl
More than one branch, use prefixes di-, tri-, etc.
4 ethyl,4 methyloctane
2,4 dimethylhexane

32. Tricky ones!!! See if you can name these.
Each END of a molecule is a Carbon atom.
No Hydrogens are indicated, they are assumed.
See if you can name these.

33. What are the names of the structural Isomers of Octane?
Hint: There are more than 8 of them.

34. Six functional groups (R groups)
Most important to the chemistry of life:
Hydroxyl = (-OH)
Carbonyl = (-C=O)
Carboxyl = (HO-C=O), (COOH)
Amino = (-NH2)
Sulfhydryl = (-SH)
Phosphate = (O=PO3-2), (PO4-2)

35. Alcohols Name the length of the carbon chain
Have an –OH group attached
Name the length of the carbon chain
Use prefix as root word
Identify by the carbon # that has –OH attached
Place this number to the left of the chain length.
Place the suffix –ol on the end of the word
Draw the following
2-propanol
1-Butanol
3-Octanol

36. What are the formulas for these alcohols?

37. Alcohols
Some alcohols have common names like glycerol

38. Halo hydrocarbons Functional group is a halogen (X = F, Cl, Br, I)
General Formula
R – X
Naming (fluoro, chloro, bromo, iodo) prefix
Select longest chain containing halogen
Number so that C with halogen gets lowest number:
2-fluoropropane
H |
F | H- C - -H
| H
F |
H | H C -
| H

39. Ethers Functional group General Formula Naming - O – R – O – R’
Name the R group as an alkyl
Name the R’ group as an alkyl
End in ether
CH3–CH2–O–CH3
ethyl methyl ether

40. methanal (formaldehyde)
Aldehydes
Functional group
- C – H
General Formula
R – C – H
Naming
Name the R group
Change the ending to -al || O
methanal (formaldehyde) || O
ethanal

41. Another way to name Alkenes
Name length of chain first using prefix
Put Carbon # of double bond next
Place –ene on the end