1. Chemical Nomenclature

2. Ionic Bonds vs Covalent Bonds
Metal + Non-Metal
Metal (CATION) always first followed by Non-metal (ANION)
Electrons are Transferred
Covalent Bonds (Sometimes called Molecular)
Non-metal + Non-metal
Electrons are Shared
We will talk more about how these bonds form, their properties, etc next semester

3. Two Types of Compounds Ionic Molecular Smallest piece Formula Unit
Molecule
Types of elements
Metal and Nonmetal
Nonmetals
Solid, liquid or gas
State
solid
Melting Point
High >300ºC
Low <300ºC

5. Ionic Compounds with Transition Metals
IONIC NOMENCLATURE
Ionic Nomenclature
Binary Compounds
Ternary Compounds
Ionic Compounds with Transition Metals

6. Binary Ionic Compounds
Binary = 2 elements total in the cmpd
Naming Binary Compounds
Take the cation (metal) and name it just like the element on the periodic table
Take the anion (non-metal) and change the ending of the element to –ide
Ex: Al2O3 = Aluminum Oxide

7. Most commonly missed –ide changes
Oxygen = Oxide
Sulfur = Sulfide
Hydrogen = Hydride
Phosphorus = Phosphide
Nitrogen = Nitride
Silicon = Silicide
Selenium = Selenide
Carbon = Carbide

8. Practice These:
NaCl
Mg3N2
K2S
LiH
SrBr2
AlP

9. Writing Formulas for Binary Ionic Compounds
Step 1
Write elements with their charges (M first, then NM)
Step 2
Cross charges and make subscripts from them (remove + or - ) Write elements together as compound
Step 3
If necessary, simplify subscripts to lowest terms
Al+3 O2-
Al2O3
Step 3 not necessary

10. When Step 3 is needed Step 1 Step 2 Step 3 Al+3 N3- Al3O3 AlO
Write elements with their charges (M first, then NM)
Step 2
Cross charges and make subscripts from them (remove + or - ) Write elements together as compound
Step 3
If necessary, simplify subscripts to lowest terms
Al+3 N3-
Al3O3
AlO
(3 & 3 both divisible by 3 to give 1)

11. When Step 3 is needed Step 1 Step 2 Step 3 Mn+4 O2- Mn2O4 MnO2
Write elements with their charges (M first, then NM)
Step 2
Cross charges and make subscripts from them (remove + or - ) Write elements together as compound
Step 3
If necessary, simplify subscripts to lowest terms
Mn+4 O2-
Mn2O4
MnO2
(2 & 4 both divisible by 4 to give 1 & 2)

12. Ternary Ionic Compounds
Ternary = 3 or more elements in compound
Naming Ternary Ionic Compounds
Name like Binary (element name + --ide)EXCEPT when POLYATOMIC IONS are used as metals or non-metals
You will need to memorize the most common polyatomic Ions

13. Polyatomic Ions to Memorize (Name, Formula & Charge)

14. Practice (it may help to put parentheses around polyatomic when you ID them)
NH4Cl
Mg(OH)2
NaNO3
AlPO4
K2SO4
H2O2

15. Formulas for Ternary Compounds (involve polyatomic ions)
Still… cation FIRST, anion SECOND
Na+ OH-
Criss-cross the superscript charge to get the subscripts.
Na1 OH1
Reduce the subscript to the least whole number ratio if needed.
NaOH

16. Ternary Compounds (Cont.)
If polyatomic ion has a subscript in the formula greater than 1, you must put parentheses around the polyatomic ion and place the subscript outside the parenthesis.
Al(OH)3

17. Practice Example: Barium nitrate
1. Write the symbols/formulas for the cation and anion, including CHARGES!
2. Cross Charges.
3. Simplify subscripts. Use parentheses if you need more than one of a polyatomic ion.

18. Practice Example: Ammonium sulfate
1. Write the formulas for the cation and anion, including CHARGES!
2. Cross Charges.
3. Simpifly subscripts. Use parentheses if you need more than one of a polyatomic ion.

19. Try these on your own… Magnesium carbonate Strontium hydroxide
Aluminum phosphate

20. Ionic Compounds with Transition Metals
Remember Transition Metals are called transition because they can have varying oxidation states!!!

21. Metals that form more than One Cation
The name of metals with two or more positive ions
(cations) use a Roman numeral to identify ionic charge.
Lead Pb lead(II)
Pb lead(IV)
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

22. Naming Ionic Compounds with Transition Metals
Step 1:
The easiest way to do this is to uncross the subscripts back to charges.
ALWAYS MOVE THE ANION’S CHARGE BACK FIRST! CHECK & MAKE SURE THE ANION CHARGE IS WHAT IT SHOULD BE!
Ex. Fe3N2 uncrossed: Fe2+ N3-
What we expect on N
Ex. MnO2 uncrossed: Mn+2 O-1
NOT WHAT WE EXPECT ON O! WE KNOW O should be a -2 which meant the subscripts simplified. So….
REAL ANSWER: MnO2 uncrossed: Mn+4 O2-

23. Naming Ionic Compounds with Transition Metals
Step 2-4
Once you know the charges, now name the transition metal with Roman Numerals:
I II III IV V VI
Ex: Fe+3 O2-
Iron (III) Oxide
Ex: Mn+4 O2-
Manganese (IV) Oxide

24. Writing Formulas for Ionic Compounds with Transition Metals
Just like Binary & Ternary Rules
Now the metal charge is given to you, you don’t need to remember it or look it up!
Don’t forget ONLY transition metals use roman numerals
Don’t forget about your polyatomics

25. Practice!!! Mn2O7 NbCl5 TiP Pd(SO4)2 PtF2 Os2O3 Ir(NO3)4 Co(ClO)2
Fe2S3
AuI3
Manganese (VII) Oxide
Niobium (V) Chloride
Titanium (III) Phosphide
Palladium (IV) Sulfate
Platinum (II) Fluoride
Osmium (III) Oxide
Iridium (IV) Nitrate
Cobalt (II) Hypochloride
Iron (III) Sulfide
Gold (III) Iodide

26. Sometimes….
You will see Transition metals named by their classical/traditional names.
I want you to be aware of the following, but you won’t be tested over them in this class

27. Traditional (Classical)
Systematic (STOCK)
Name
Traditional (Classical)
Fe3+
Iron (III)
Ferric
Fe2+
Iron (II)
Ferrous
Cu2+
Copper (II)
Cupric
Cu1+
Copper (I)
Cuprous
Sn4+
Tin (IV)
Stannic
Sn2+
Tin (II)
Stannous
Pb4+
Lead (IV)
Plumbic
Pb2+
Lead (II)
Plumbous

28. Traditional System Name the metal first; use Latin names of metals.
In binary compounds the nonmetal takes the suffix –ide. (Like before)
The ion with the lower charge takes the suffix
–ous
The ion with the higher charge takes the suffix –ic.

29. Naming Covalent Compounds
Covalent Nomenclature
Diatomic Molecules
Binary Molecules
Remember, covalent bonds form between a non-metal and a non-metal and the electrons are shared!

30. Br2I2N2Cl2H2O2F2 Diatomic Molecules
When some elements are by themselves, with no other element, they pair up with other elements that are like them.
They are called diatomic molecules!
We name them just by the element name on the periodic table
Br2I2N2Cl2H2O2F2

31. Practice Br2 H2 Oxygen Chlorine Bromine Hydrogen O2 Cl2
If these 7 elements are paired with other elements, they will NOT be named like this! They will be named like we talk about later!

32. Binary Covalent Compounds
Covalent Compounds use Prefixes to name compounds
ALWAYS use prefixes except:
Only use mono on the second element
If you have a diatomic molecule
1st: (prefixelementname) 2nd:(prefixelementendinide)
PREFIXES 1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hepta 8-octa 9-nona 10-deca

33. Examples
P2O5 diphosphorous pentoxide OF2 oxygen difluoride PBr3 phosphorous tribromide

34. Practice! CO2 CO P2O5 N2O SiO2 CBr4 SO2 PBr5 ICl3 NI3 N2O3 B2H6 NBr3
SCl6
P4O10
S7O2
Carbon dioxide
Carbon monoxide
Diphosphorous pentaoxide
Dinitrogen monoxide
Silicon dioxide
Carbon tetrabromide
Sulfur dioxide
Phosphorous pentabromide
Iodine trichloride
Nitrogen triiodide
Dinitrogen trioxide
Diboron hexahydride
Nitrogen tribromide
Sulfur hexachloride
Tetraphosphorous decaoxide
Heptasulfur dioxide

35. To Get Covalent Formulas, just go backwards….

36. In reverse to get Formulas!
1. Silicon tetrafluoride 2. Dinitrogen trisulfide 3. Sulfur trioxide 4. Dinitrogen tetroxide 5. Nitrogen monoxide 6. Nitrogen dioxide 7. Tetraphosphorous octaoxide 8. Tetraphosphorous nonasulfide 9. Diarsenic pentoxide 10. Phosphorous trichloride 11. Carbon tetrachloride 12. Dihydrogen monoxide 13. Selenium hexafluoride 14. Iodine heptafluoride 15. Tetraarsenic decoxide 16. Carbon disulfide 17. Oxygen difluoride
SiF4
N2S3
SO3
N2O4 NO
NO2
P4O8
P4S9
As2O5
PCl3
CCl4
H2O
SeFl6
IF7
As4O10
CS2
OF2

37. Naming Acids Acid formulas usually begin with H
We name them according to how the ANION name ends!
Common Acids we use:
HCl: Hydrochloric Acid
HNO3: Nitric Acid
H2SO4: Sulfuric Acid

38. HCl: Hydrochloric Acid
Anion Ending
Acid Name
Example
Binary Acids (no oxygen in formula)
-ide
Hydro-(stem) –ic Acid
HCl: Hydrochloric Acid
(from chloride)
Ternary Acids (oxygen in the formula)
-ate
(stem)-ic acid
HNO3:
Nitric Acid
(from nitrate)
-ite
(stem)-ous Acid
H2SO3
Sulfurous Acid
(from sulfite)
(per)-ic
per-stem-ic Acid
HClO4
Perchloric
Acid
Hypo-ite
per-stem-ous Acid
HClO
Hypochlorous Acid

39. Acid Nomenclature Flowchart

40. Acid Nomenclature HBr (aq) H2CO3 H2SO3  hydrobromic acid
No oxygen, -ide
 hydrobromic acid
Has oxygen, -ate
 carbonic acid
Has oxygen, -ite
 sulfurous acid

41. Acid Nomenclature hydrofluoric acid sulfuric acid nitrous acid  H+ F-
2 elements
 H+ F-
 HF (aq)
3 elements, -ic
 H+ SO42-
 H2SO4
3 elements, -ous
 H+ NO2-
 HNO2

42. Name ‘Em!
HI (aq)
HCl
H2SO3
HNO3
HIO4

43. Write the Formula! Hydrobromic acid Nitrous acid Carbonic acid
Phosphoric acid
Hydrotelluric acid

44. Hydrates Some compounds contain H2O in their structure.
These compounds are called hydrates.
This is different from (aq) because the H2O is part of the molecule (not just surrounding it).
The H2O can usually be removed if heated.
A dot separates water: e.g. CuSO4•5H2O is copper(II) sulfate pentahydrate.
Name the ionic part (the salt) just the way you would as before; a greek prefix indicates the # of H2O groups.

45. Hydrates (examples) Na2SO4•10H2O sodium sulfate decahydrate NiSO4•6H2O
sodium carbonate monohydrate
barium chloride dihydrate
sodium sulfate decahydrate
nickel(II) sulfate hexahydrate
Na2CO3•H2O
BaCl2•2H2O

46. Nomenclature Summary Flowchart