nomenclature topic: type i and type ii binary compounds objectives: day 1 of 3 i will know what a...
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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