1. Nomenclature

2. Topic: Type I and type II Binary Compounds
Unit: Nomenclature
Topic: Type I and type II Binary Compounds
Objectives: Day 1 of 3
I will know what a binary compound is
I will understand the difference between a Type 1 and type 2 binary compound
I will understand how we name type one and two binary compounds

3. Quickwrite Answer one of the questions below 1-2 sentences:
Nomenclature is the method by which we name and organize compounds and molecules; given this, why do you think it is important to have a “naming” system for chemicals?
Consider the compound NaCl, what comes first, the cation or the anion???

4. Nomenclature In chemistry, we have system of naming chemical compounds
The name implies something about he composition of the compound
After learning the system, you should be able to name a compound when you are given it’s formula

5. Binary Compounds
First, we will begin by discussing the system for naming binary compounds
Binary compounds are composed of two elements-NaCl
Binary compounds are divided into 2 types:
Compounds that contain a metal and nonmetal
Compounds that contain 2 nonmetals
Carbon Monoxide

6. What are Binary Compounds?
A Compound composed of _____elements
2 types:
Compounds that contain a metal and nonmetal
Ex, NaCl & MgO
Compounds that contain 2 non_____
Ex. SO2 & CO
two
Answer Bank
Anion
Different
Two
Cation
Changes
metals

7. Compounds with a Metal and Nonmetal
When a metal (such as sodium) combines with a nonmetal such as (chlorine), the resulting compound (NaCl) is Ionic in Nature
If you remember, the metal (sodium) loses one electron and the Nonmetal (chlorine) gains an electron
The result is a Binary Ionic Compound
A Binary Ionic is a compound that contains a cation(positive ion) and anion (negative ion)

8. Balancing Ionic Compounds
Chlorine (Cl) is
A 1- Anion
Sodium (Na) is
a 1+ Cation
Cl-
Na+
(Charge 1+) (Charge 1-) Net Charge: 0

9. What is a Binary Ionic Compound?
A compound that contains a _____(positive ion) and an_____(negative ion)
They form between a _____ and a non-metal Ex: KBr & Fe2O3
cation
Answer Bank
Anion
Different
Two
Cation
Changes
metals
anion
metal

10. 2 Types of Binary Ionic Compounds
There are two types of binary Ionic compounds
Type 1 and type 2
In Type 1 ionic compounds, the metal cation charge never changes
For example, sodium always has 1+ charge
Type 2 (II) ionic compounds contain a metal cation that can have different charges
For example, Iron can have more than one charge: Fe2+ & Fe3+

11. Type 1 Binary Compounds
Type 1 binary compounds contain a metal with only one charge
That is, the metal present forms only one type of cation
For example, the sodium metal cation (Na+) is always has a plus one charge, it doesn’t change
The magnesium ion (Mg 2+) always has plus two charge
Na+
Mg 2+

12. Rules for naming Type 1 Ionic Compounds
The cation is always named
first and the anion second
2.The cation takes it name from
the name of the element
For example, Na+ is called sodium
And Mg 2+ is called magnesium
3.The anion takes it’s name by
Taking the first part of the
Element name and adding
-ide to the end
For Example: The Cl- ion
is called Chloride & the
O2- ion is called oxide

13. Type One Ionic Compounds
Chloride
Sodium
always has 1+ charge
Cl-
Na+
Sodium Chloride

14. Type One Ionic Compounds
Iodide
Potassium I- K+
Potassium Iodide

15. Type One Ionic Compounds
Oxide
Magnesium
always has a 2+ charge
O2-
Mg2+
Mg2+
Potassium Iodide
Magnesium Oxide

16. Type 2 Binary Ionic Compounds
Type 1 ionic compounds are always the have the same charge such as Na+ or Mg 2+
Type 2 Ionic Compounds contain Cations that have various charges of Fe2+ & Fe3+ or Pb2+ & Pb4+
Mg2+
Na+
Fe2+
Pb2+
Fe3+
Pb4+

17. Type 2 Binary Ionic Compounds
Other metals, such as Lead Pb2+ & Pb4+ also can have more than one charge
This means that if we saw the name lead chloride, we wouldn’t know whether it reffered to PbCl2 or PbCl4
Therefore, we need a way to specifying which cation is present
Is it Pb2+ & Pb4+ ?
Pb2+
Pb4+

18. Type 2 Binary Ionic Compounds Transition Metals
Transition metals can take on many different charges (+, 2+, 3+, or 4+), therefore they form type 2 Ionic Compounds

19. Type 2 Binary Ionic Compounds Transition Metals
Copper (Cu) is transition metal, it likes to be either Cu+ or Cu2+, therefore it forms a type 2 binary ionic compound
Cu2+
Cu+

20. Type 2 Binary Ionic Compounds Transition Metals
Iron (Fe) is transition metal, it likes to be either Fe2+ or Fe3+, therefore it forms a type 2 binary ionic compound
Fe3+
Fe2+

21. Type 1 & Type 2 Compounds What’s the difference?
Type 2 ionic compounds form between
Transition metals (Fe3+ , Cu+, Pb4+)
These cations can have various charges
Type 1 ionic compounds form between
group 1 and 2 cations (Na+, Mg+, Ca+)
These cations never vary in charge

22. Type 1 = Cation charge never______ Ex. Na1+ & Mg +2
What’s the difference between type 1 and type 2 binary ionic compounds?
Type 1 = Cation charge never______
Ex. Na1+ & Mg +2
Type 2 = Cation can have ________charges therefore we use roman numerals to indicate charge Ex. (Fe2+, Fe3+) & (Cu+ , Cu+2)
changes
Answer Bank
Anion
Different
Two
Cation
Changes
metals
different

23. = 0 Type 2 binary compounds ?
To deal with the complexity of multiple charge, chemists use roman numerals to specify the charge on the cation
Consider the binary ionic compound FeCl2
Is it Fe2+ or Fe3+?
We know chlorine has a (1-) charge
To balance the charge of 2(-1) chlorine atoms we need a charge Positive two (2+) ?
Fe2+
= 0
Cl-
Cl-

24. Type 2 Binary Ionic Compounds
So how would we write FeCl2?
WE call this iron (II) chloride
Lets take another look at rust: Fe2O3
Who knows the charge on the iron cation?
Let’s do the math!
(?) + 3(2-) = 0
2(?) + 3(2-) = 0
2(3+) + -6 = 0
So the charge, is Fe3+, written as Iron (III) oxide!

25. Potassium Oxide Calcium Chloride -K2O -CaCl2 Copper (I) chloride
Practice: Write the formula for the following type 1 and 2 ionic compounds:
Type 1:
Potassium Oxide
Calcium Chloride
-K2O
-CaCl2
Type 2:
Copper (I) chloride
Copper (II) chloride
Iron (III) Oxide
Lead (IV) Sulfide
- CuCl
-CuCl2
-Fe2O3
-PbS2

26. What are the names of the following type 1 ionic compounds?
- Calcium Chloride
- Magnesium Iodide
Type 1:
CaCl2
MgI2
Type 2:
- Copper (I) Chloride
- Iron (II) Oxide
-Lead (IV) Chloride
CuCl
FeO
PbCl4

27. Nomenclature
Flow Chart

28. Summarize: Try to list two examples of type 1 ionic compounds:
Explain the difference between type one and type two compounds:
Write the name for MgF2
Write the name for PbO2

29. Topic: Type 3 and type 4 Compounds
Unit: Nomenclature
Topic: Type 3 and type 4 Compounds
Objectives: Day 2 of 3
To learn the naming rules for type 3 compounds
To learn that type 3 compounds form between 2 nonmetals
To understand what polyatomic ions are and they form compounds

30. Quickwrite Answer one of the questions below 1-2 sentences:
Consider the Compound CO2, how is this compound different from NaCl???
Once again consider the compound CO2, how do you think we should go about naming this compound???
Why do you think we use prefixes such as tri- on words like triceratops, tricycle or tripod????

31. Compounds that Contain only Nonmetals
If you remember, Binary compounds are divided into 2 types:
Compounds that contain a metal and nonmetal (ionic)
Compounds that contain 2 nonmetals (covalent)
The compound below, carbon monoxide is made of carbon and oxygen—2 nonmetals
Carbon Monoxide

32. Carbon Monoxide Nonmetals
Made of 2 nonmetals: carbon & oxygen
Compounds that Contain only Nonmetals
Type 3 (III) Binary Compounds contain only nonmetals
Type 3 (III) binary compounds have similar naming rules to binary ionic compounds previously discussed
Nonmetals

33. Rules for Naming Type 3 (III) Binary Compounds
2. The 2nd element is named
as though it were an anion
For example- the oxygen in CO is oxide
3. Prefixes are used to denote
the numbers of atoms-
mono- 1, di- 2, & tri- 3
The first element in the formula is named
first, and the full element name is used
For example: we just say carbon
for carbon monoxide
4. The prefix mono- is never used for
naming the first element
For Example: CO is called carbon monoxide
Not monocarbon monoxide
Carbon Monoxide

34. Prefixes mono- (one) CO - carbon monoxide di- (two)
            Prefix                             Example                           
mono- (one)
CO     -  carbon monoxide
di- (two)
CO2    -  carbon dioxide
tri- (three)
N2O3    -  dinitrogen trioxide
tetra- (four)
CCl4    -  carbon tetrachloride
penta- (five)
N2O5    -  dinitrogen pentoxide
hexa- (six)
UF6    -  uranium hexafluoride

35. Naming type 3 (III) Binary Compounds
Using the rules, let’s look at CO2:
Name the first element using the full element name: Carbon
Name the second element as though it were an anion: -oxide
Use prefixes to denote the number of atoms: one carbon, do use mono- for the first element carbon, 2 oxygen atoms: use the prefix di-
Carbon Dioxide!

36. Naming type 3 (III) Binary Compounds
Let’s look at – SO3 and N2O5:
Name the first element: Sulfur
Name the second element as anion: Oxide
Use Prefix: Tri-
Do not use mono- for the first element!
Sulfur Trioxide

37. Naming type 3 (III) Binary Compounds
Let’s look at one more –N2O5:
Name the first element: Nitrogen
Name the second element as anion: Oxide
Use Prefixes: Di- (for nitrogen) & Penta- (for oxygen)
Remember: there are 2 nitrogen atoms!
So the last rule does not apply and we get: dinitrogen pentoxide

38. What are type 3 covalent compounds?
Neutral compounds that form between 2 ________
Prefixes are used below:
1-mono-, 2-di-, 3-tri-, 4-tetra-, 5-_____, 6-hexa-
Ex: CO2 ,SO3, _____
Nonmetals
Answer Bank
polyatomic
More
Two
N2O5
Penta-
Nonmetals
charge
Penta-
N2O5

39. Practice: Write names of the following Type 3 (III) binary compounds?
PCl5 =_____________
P4O6 =_____________
N2O3 =_____________
Phosphorous pentachloride
Tetraphosphorous hexaoxide
Dinitrogen trioxide

40. Practice: Write the formula for the following Type 3 Molecular compounds:
NO2
Nitrogen dioxide = ____________
Diphosphorus Pentachloride = _________
Dinitrogen pentoxide = ____________
Carbon dioxide = __________
P2Cl5
N2O5
CO2

41. Polyatomic Ions
Polyatomic Ions are a group of two or more atoms that have a particular charge to them
An example would include the ammonium ion NH4+
It is composed of 1 nitrogen atom and 4 hydrogen atoms which give it a 1+ charge
These ions are assigned special names that you must memorize!
[ ]+

42. Common Polyatomic Ions
You must memorize!

43. What are Polyatomic Ions?
more
A group of two or ____ atoms that have a particular _____to them
Ex: CO32-, NH4+ & OH-
Answer Bank
polyatomic
More
Two
N2O5
Penta-
Nonmetals
charge
charge
[ ]+

44. Type 4 (IV): Compounds with Polyatomic Ions
Let us look at the compound ammonium nitrate NH4NO3 (a very explosive chemical)
Ammonium Nitrate is made up of 2 polyatomic ions NH4+ & NO3-
When two polyatomic ions come together, a compound (NH4NO3) forms between them

45. Type 4 (IV): Compounds with Polyatomic Ions
Naming ionic compounds that contain polyatomic ions is very similar to naming ionic compounds
For example, the compound NaOH is called sodium hydroxide
The cation, Sodium (Na) comes first and the anion (OH-) comes second

46. Naming Compounds with Polyatomic Ions
Let’s look at one more example: AgNO3
The Ag+ cation comes first, and the negative polyatomic (NO3-) anion comes second
Just like in ionic compounds, the charges need to be neutral
Ag+ needs be balanced by the negatively charged polyatomic ion NO3-
Therefore we write: Silver (I) Nitrate

47. Naming Compounds with Polyatomic Ions
There are no rules for polyatomic ions, you must memorize them!
That means you need to memorize the charge, and the composition for them
You will be quizzed on them!!!!

48. What are type 4 compounds?
Polyatomic
Compounds that contain a ________ ion
Ex: NaOH & CaCO4
Answer Bank
polyatomic
More
Two
N2O5
Penta-
Nonmetals
charge

49. What are the formulas for the following compounds?
K3PO4
Potassium Phosphate = ___________
Copper (II) sulfate = __________
Calcium Carbonate =__________
CuSO4
CaCO3

50. What are the names of the following polyatomic ions?
Ammonium nitrate
NH4NO3 =________________
NaOH =__________________
CaCO3 =__________________
Fe(NO3 )3 = __________________
Sodium Hydroxide
Calcium Carbonate
Iron (III) Nitrate

51. Summarize: Type 3 binary compounds form between 2 ______
List two examples of a type 3 compound:
A polyatomic ion is a group of two or ____ atoms that have a particular _____to them.
An example of a polyatomic ion is_____.
List two examples of a type 4 compound:

52. Unit: Nomenclature Topic: Naming Acids Objectives: Day 3 of 3
I will know how to define an acid
I will know how we name acids

53. Quickwrite Answer one of the questions below 1-2 sentences:
What do you know about acids???
Why do you think lemons are so sour???
What do you think acids react so easily with other substances????

54. Acids
Certain compounds when dissolved in water produce and donate hydrogen ions (H+) to other chemicals
Hydrogen Ions are very reactive and readily bond with other substances
These compounds are called acids and were first recognized by their sour taste of their solution
For example, citric acid is responsible for the sour taste of lemons and limes
Acids have a pH less than 7

55. What are Acids?
Compounds when dissolved in water produce and donate ________ ions (H+)
Acids taste sour and have a pH less than ___
Answer Bank
contains 7
-ate
Hydrogen
-ic
Oxygen
hydrogen 7

56. Naming Acids
Certain compounds when dissolved in water produce hydrogen ions (H+)
These compounds are called acids and were first recognized by their sour taste of their solution
For example, citric acid is responsible for the sour taste of lemons and limes
We’ll learn more about acids later
Today we are going to discuss the rules for naming acids

57. 1. If the anion does not contain oxygen,
Rules for Naming Acids
1. If the anion does not contain oxygen,
the acid is named with prefix hydro-
and the suffix –ic. For example,
consider HCl. Does it have oxygen?
No, so we say hydrochloric acid
2. When an anion contains oxygen, the acid
name is formed from the root name of the
central element of the anion or the anion
name, with a suffix of -ic or -ous.
When the anion name ends in -ite,
the suffix -ous is used. For example:
When the anion name ends in -ate,
the suffix -ate is used. For example:
Acid
Anions ending with -ite
Name: change -ite to -ous
H2SO3
SO sulfite
sulfurous acid
H3PO3
PO phosphite
phosphorous acid
HNO2
NO nitrite
nitrous acid
Acid
Anions ending with -ate
Name: change -ate to -ic
H2SO4
SO sulfate
sulfuric acid
H3PO4
PO phosphate
phosphoric acid
HC2H3O2
C2H3O2- acetate
acetic acid

58. How do we name acids? Example:
If the anion does not contain _______add the prefix hydro- and suffix -____
Ex: HCl becomes hydrochloric acid
HF becomes hydroflouric acid
If the anion ________ oxygen, change the ____ to -ic and
-ite to -ous
Example:
oxygen
Answer Bank
contains 7
-ate
Hydrogen
-ic
Oxygen
-ic
contains
-ate
H2SO4
SO sulfate
sulfuric acid
H2SO3
SO sulphite
sulfurous acid

59. Practice: Write the name of the following acids:
H2SO3 =_______________
H2SO4 =_______________
HCl =_______________
HBr =_______________
Sulfurous Acid
Sulfuric Acid
Hydrochlric Acid
Hydrobromic Acid

60. Practice: HF H2CO3 HBr H3PO3
Write the chemical formula for the following acids:
Hydrofluoric Acid =_____________
Carbonic Acid =_____________
Hydrobromic Acid =_____________
Phosphorous Acid =_____________ HF
H2CO3
HBr
H3PO3

61. Summarize:
If the anion does not contain ______ then we add the prefix _____ and suffix _____.
If the anion contains_____, change ____ to___ and ____ to ____.
Review: Complete the table
Formula:
Name:
Type 1,2,3,4?
Fe2O3
Dinitrogen Pentaoxide
Sodium Hydroxide