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 are attracted to Negative ions
FORMULA UNIT
Cation always comes first, then anion

4. Elemental anions
When an element becomes an anion, it starts to end in –ide
Fluoride
Chloride
Bromide
Oxide
Sulfide
Nitride
Phosphide

5. Type I The cation has a predictable charge Alkali Metals +1
Alkaline Earth Metals +2
Group 3A +3
Silver Ag+
Zinc Zn2+

6. Type II Fe2+ Fe3+ Cu+ Cu2+ The cation has a variable charge
All Transition metals except for Ag and Zn (for our purposes)
The name will have a roman numeral to denote the CHARGE on the cation
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
Just the name of element if Type I
Name of element and roman numeral with charge on cation if Type II
Then name anion
Elemental anions end in “–ide”
When determining the formula, remember “swap ‘n’ drop”

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
Magnesium Oxide
Sodium nitride
Calcium chloride
Copper(I) sulfide
Lead (II) bromide
Iron(III) oxide
AlCl3
MgO
Na3N
CaCl2
Cu2S
PbBr2
Fe2O3

10. Polyatomic Ions Many anions are not just ions of elements.
Polyatomic Ions = many atomed particle with an overall charge
Mostly nonmetals bonded to Oxygens

11. Polyatomic Ion Naming Main polyatomic ion One fewer oxygens
Ends in “–ate”
Example: Chlorate ClO3-
One fewer oxygens
Ends in “-ite”
Example: Chlorite ClO2-
Even fewer oxygens
Hypo = under
Example: Hypochlorite ClO-
More oxygens than main ion
Hyper = over, shortened to “per”
Example: Perchlorate ClO4-

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

13. Common Polyatomic Ions
Hydrogen can attach to the polyatomic ions as H+
This adds an H and reduces the overall charge by 1
PO43-
Phosphate
HPO42-
Hydrogen Phosphate
H2PO41-
Dihydrogen Phosphate
CO32-
Carbonate
HCO31-
Hydrogen carbonate
(bicarbonate)

14. Name these compounds with PAIs
AlPO4
Cu(NO3)2
Na2SO4
NaHCO3
Mg3(PO4)2
Aluminum phosphate
Copper(II) nitrate
Sodium sulfate
Sodium bicarbonate
Magnesium Phosphate

15. Molecular Compounds
Molecular compounds are not bonded by positive and negative ions
They SHARE electrons
Made of two non-metals
Cannot predict or explain charges (no charges, because not LOSING or GAINING electrons – SHARING)

16. Naming Molecular Compounds (Type III)
Because there is no way to neutralize the compounds (like for ions) we must determine how many there are another way:
Use PREFIXES

17. How to tell if it’s Type III
Check the FIRST element – is it a non-metal?
If YES, it’s a Type III
Name the first element as the element
Name the second element ending in “-ide”

18. Prefixes 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 910
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

19. Using prefixes
If there is only one of the first element, you may omit the “mono”
You may not omit any other prefixes
The more electronegative element goes last (upper right hand corner)
F, O, N, Cl,

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

21. Naming Practice! For each of the following compounds, determine whether it is type I, II, or III.
FeCl3
NaCl
Cu(OH)2
N2O
BaSO4
PO5
(NH4)CO3
SnBr2

22. Naming Practice! For each of the following compounds, determine the CHARGE on the cation (+1, +2, +3, or +4) 3 2 4
FeCl3
Cu(OH)2
Cr2S3
NiS
Pb(NO3)2
SnCl4

23. Acids All acids have the H+ ion in them as the cation.
All acids have “acid” in their name
Consider Hydrochloric Acid
HCl

24. Naming Acids If the anion DOES NOT CONTAIN OXYGEN: Examples
Prefix hydro-
Root name of anion element
Suffix –ic
Examples HF
H2S
Hydrofluoric Acid
Hydrosulfuric Acid
Hydrooxygenic acid

25. Naming Acids If the anion CONTAINS OXYGEN (ie: is a polyatomic ion)
Root name of the PAI
If anion ends in -ate,
acid ends in –ic
If anion ends in –ite,
acid ends in –ous

26. Naming Acids Examples H2SO4 H2SO3 HNO3 HNO2 HC2H3O2 Phosphoric Acid
Carbonic Acid
Sulfuric Acid
Sulfurous Acid
Nitric Acid
Nitrous Acid
Acetic Acid
H3PO4
H2CO3

27. Organic Molecules Carbon based Naming is based on number of carbons
Functional groups
Sets of molecules attached to the carbons
Naming is also based on what functional groups are where

28. Alkanes The simplest organic molecules are Alkanes.
Carbons are all single bonded to each other
When not bonded to another carbon, bonded to a Hydrogen
All alkanes end in -ane

30. Prefixes
Note that the prefixes pertain to all types of carbon based molecules with any types of functional groups or chains
Meth
Eth
Prop
But
Pent
Hex
Hept
Oct

31. Alkenes and Alkynes
A functional group can be a set of atoms, or the way they are bonded.
Alkenes
Carbons have double bonds between them
Alkynes
Carbons have triple bonds between them

32. Alkenes and Alkynes To Name All alkenes end with –ene.
All alkynes end with –yne
Number the carbons in the longest chain.
Carbon 1 is at the end of the chain closest to the first functional group
Put the number that the bond is on, then the chain length
(some name by putting the number BEFORE the functional group ending)

33. Isomer = molecule with SAME formula but DIFFERENT structure

34. Alcohols Have an –OH group attached
Name the carbon chain (prefix and bond)
End in –ol
Indicate which carbon the –OH is on
2-propanol
1-Butanol
3-Octenol

35. What are the formulas for these alcohols?

36. Alcohols
Some alcohols have common names like glycerol

37. Branched Hydrocarbons
The longest continuous chain of carbon atoms gives the root name/prefix.
Substituent is named by the number of carbons.
Specify location of substituent by numbering carbon atoms in longest chain.
Substituent often referred to as R or R’ (for second substituent)

38. Substituent often referred to as R or R’ (for second substituent)
If more than one alkyl group, use prefix di, tri, etc. to alkyl name
Substituents listed in alphabetical order (disregarding prefix)

39. Branched Hydrocarbon Substituent Alkyl groups

40. What is the name of the compound?
Hints
Number Carbon chain from on side closest to first alkyl group
Single carbon branch called methyl, triple carbon group called propyl
More than one branch, use prefixes di-, tri-, etc.
4 ethyl,5 methyl heptane
2,4 dimethyl hexane

41. Tricky ones!!!
Each END of a line is a Carbon atom. No H’s are indicated, but they are assumed
See if you can name these.

42. Halohydrocarbons Functional group is a halogen (X = F, Cl, Br, I)
General Formula
R – X
Naming
Select longest chain containing halogen
Number so that C with halogen gets lowest number

43. 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

44. Aldehydes Functional group General Formula Naming - C – H R – C – H
Name the R group
Change the ending to -al || O || O