Nomenclature

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

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???

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 two Answer Bank Anion Different Two Cation Changes metals

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)

Balancing Ionic Compounds Chlorine (Cl) is A 1- Anion Sodium (Na) is a 1+ Cation Cl- Na+ (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 cation Answer Bank Anion Different Two Cation Changes metals anion 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 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

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

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

Type One Ionic Compounds Oxide Magnesium always has a 2+ charge O2- Mg2+ Mg2+ Potassium Iodide 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+ Mg2+ Na+ Fe2+ Pb2+ Fe3+ Pb4+

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

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+

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+

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

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

= 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-

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!

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

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

Nomenclature Flow Chart

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

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

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????

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

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

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

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

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!

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

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

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

Practice: Write the formula for the following Type 3 Molecular compounds: NO2 Nitrogen dioxide = ____________ Diphosphorus Pentachloride = _________ Dinitrogen pentoxide = ____________ Carbon dioxide = __________ P2Cl5 N2O5 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? 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 [ ]+

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

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

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

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!!!!

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

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

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

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

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????

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 Bank contains 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

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 SO32- sulfite sulfurous acid H3PO3 PO33- phosphite phosphorous acid HNO2 NO2- nitrite nitrous acid 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

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 SO42- sulfate sulfuric acid H2SO3 SO32- sulphite sulfurous acid

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

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

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