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.

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

Unit: Nomenclature

QuickwriteAnswer 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???

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

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

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

Answer BankAnion

DifferentTwo

CationChangesmetals

two

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)

Chlorine (Cl) isA 1- Anion

Sodium (Na) is a 1+ Cation

Balancing Ionic Compounds

Na+Cl-

(Charge 1+) (Charge 1-) Net Charge: 0

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

Answer BankAnion

DifferentTwo

CationChangesmetals

cationanion

metal

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+

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+

Rules for naming Type 1 Ionic Compounds

1.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 byTaking 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

ChlorideSodiumalways has 1+ charge

Type One Ionic Compounds

Na+Cl-

Sodium Chloride

IodidePotassium

Type One Ionic Compounds

K+I-

Potassium Iodide

OxideMagnesiumalways has a 2+ charge

Type One Ionic Compounds

Mg2+

Potassium Iodide

Mg2+

O2-

Magnesium Oxide

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+

Fe2+

Fe3+

Pb2+

Pb4+

Na+

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+

Type 2 Binary Ionic CompoundsTransition Metals

• Transition metals can take on many different charges (+, 2+, 3+, or 4+), therefore they form type 2 Ionic Compounds

Type 2 Binary Ionic CompoundsTransition Metals

• Copper (Cu) is transition metal, it likes to be either Cu+ or Cu2+, therefore it forms a type 2 binary ionic compoundCu+

Type 2 Binary Ionic CompoundsTransition Metals

• Iron (Fe) is transition metal, it likes to be either Fe2+ or Fe3+, therefore it forms a type 2 binary ionic compoundFe2+

Type 1 & Type 2 CompoundsWhat’s the difference?

Type 1 ionic compounds form between group 1 and 2 cations (Na+, Mg+, Ca+)

These cations never vary in charge

Type 2 ionic compounds form between Transition metals (Fe3+ , Cu+, Pb4+)

These cations can have various charges

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)

Answer BankAnion

DifferentTwo

CationChangesmetals

changes

different

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+)

= 0? Fe2+

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!

Copper (I) chloride

Copper (II) chloride

Iron (III) Oxide

Lead (IV) Sulfide

Practice: Write the formula for the following type 1 and 2 ionic compounds:

- CuCl

-CuCl2-Fe2O3

-PbS2

-K2O

-CaCl2

Potassium Oxide

Calcium Chloride

Type 1:

Type 2:

What are the names of the following type 1 ionic compounds?

CaCl2MgI2

- Calcium Chloride- Magnesium Iodide

Type 1:

Type 2:

CuCl

FeO

PbCl4

- Copper (I) Chloride- Iron (II) Oxide-Lead (IV) Chloride

Nomenclature Flow Chart

Summarize:• Try to list two examples of type 1 ionic

compounds:

• Try to list two examples of type 2 ionic compounds:

• Explain the difference between type one and type two compounds:

• Write the name for MgF2

• Write the name for PbO2

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

Unit: Nomenclature

QuickwriteAnswer 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????

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

• Type 3 (III) Binary Compounds contain only nonmetals

• Type 3 (III) binary compounds have similar naming rules to binary ionic compounds previously discussed

Compounds that Contain only Nonmetals

Nonmetals

Carbon MonoxideMade of 2 nonmetals: carbon & oxygen

Rules for Naming Type 3 (III) Binary Compounds

1.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

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

4. The prefix mono- is never used for naming the first element

For Example: CO is called carbon monoxideNot monocarbon monoxide

Carbon Monoxide

Prefixes            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

• 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!

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

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

Naming type 3 (III) Binary Compounds

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, _____

NonmetalsAnswer Bank

polyatomicMoreTwo

N2O5

Penta-Nonmetals

charge

Penta-N2O5

Practice: Write names of the following Type 3 (III) binary compounds?

• PCl5 =_____________

• P4O6 =_____________

• N2O3 =_____________

Phosphorous pentachloride

Tetraphosphorous hexaoxide

Dinitrogen trioxide

• Nitrogen dioxide = ____________

• Diphosphorus Pentachloride = _________

• Dinitrogen pentoxide = ____________

• Carbon dioxide = __________

Practice: Write the formula for the following Type 3 Molecular compounds:

NO2

P2Cl5N2O5

CO2

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!

[ ]+

Common Polyatomic Ions• You must memorize!

What are Polyatomic Ions?

• A group of two or ____ atoms that have a particular _____to them

• Ex: CO32-, NH4

+ & OH-

[ ]+

Answer Bankpolyatomic

MoreTwo

N2O5

Penta-Nonmetals

charge

more

charge

• 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

Type 4 (IV): Compounds with Polyatomic Ions

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

• 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

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!!!!

Naming Compounds with Polyatomic Ions

What are type 4 compounds?

• Compounds that contain a ________ ion

• Ex: NaOH & CaCO4 Answer Bankpolyatomic

MoreTwo

N2O5

Penta-Nonmetals

charge

Polyatomic

What are the formulas for the following compounds?

• Potassium Phosphate = ___________

• Copper (II) sulfate = __________

• Calcium Carbonate =__________

K3PO4

CuSO4

CaCO3

What are the names of the following polyatomic ions?

• NH4NO3 =________________

• NaOH =__________________

• CaCO3 =__________________

• Fe(NO3 )3 = __________________

Ammonium nitrate

Sodium Hydroxide

Calcium CarbonateIron (III) Nitrate

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:

Topic: Naming Acids

Objectives: Day 3 of 3

• I will know how to define an acid

• I will know how we name acids

Unit: Nomenclature

QuickwriteAnswer 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????

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

What are Acids?

• Compounds when dissolved in water produce and donate ________ ions (H+)

• Acids taste sour and have a pH less than ___

Answer Bankcontains

7-ate

Hydrogen-ic

Oxygen

hydrogen

7

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

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.

Acid Anions ending with -ate Name: change -ate to -ic

H2SO4 SO42- sulfate sulfuric acid

H3PO4 PO43- phosphate phosphoric acid

HC2H3O2 C2H3O2- acetate acetic acid

When the anion name ends in -ate, the suffix -ate is used. For example:When the anion name ends in -ite,

the suffix -ous is used. For example:

Acid Anions ending with -ite Name: change -ite to -ous

H2SO3 SO32- sulfite sulfurous acid

H3PO3 PO33- phosphite phosphorous acid

HNO2 NO2- nitrite nitrous acid

How do we name acids?

1. If the anion does not contain _______add the prefix hydro- and suffix -____

Ex: HCl becomes hydrochloric acid

HF becomes hydroflouric acid

2. If the anion ________ oxygen, change the ____ to -ic and

-ite to -ous

Example:H2SO4 SO4

2- sulfate sulfuric acid

H2SO3 SO32- sulphite sulfurous acid

oxygen

-ic

contains-ate

Answer Bankcontains

7-ate

Hydrogen-ic

Oxygen

Practice:Write the name of the following acids:

1. H2SO3 =_______________

2. H2SO4 =_______________

3. HCl =_______________

4. HBr =_______________

Sulfurous AcidSulfuric Acid

Hydrochlric Acid

Hydrobromic Acid

Practice:Write the chemical formula for the following

acids:

1. Hydrofluoric Acid =_____________

2. Carbonic Acid =_____________

3. Hydrobromic Acid =_____________

4. Phosphorous Acid =_____________

HFH2CO3

HBrH3PO3

Summarize:1) If the anion does not contain ______ then we

add the prefix _____ and suffix _____.

2) If the anion contains_____, change ____ to___ and ____ to ____.

Review: Complete the table

Formula: Name: Type 1,2,3,4?

Fe2O3

Dinitrogen Pentaoxide

Sodium Hydroxide