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Nomenclature

Nomenclature. Unit: Nomenclature. Topic: Type I and type II Binary Compounds. Objectives: Day 1 of 3 I will understand the difference between a Type 1 and type 2 ionic compound I will understand how we name type one and two Ionic Compounds. Quickwrite.

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Nomenclature

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  1. Nomenclature

  2. Unit: Nomenclature Topic: Type I and type II Binary Compounds Objectives: Day 1 of 3 • I will understand the difference between a Type 1 and type 2 ionic compound • I will understand how we name type one and two Ionic 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. Ionic Compounds with a Metal & 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 an Ionic Compound • An Ionic Compound contains a cation (positive ion) and anion (negative ion)

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

  7. Rules for naming 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

  8. What is a 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

  9. Ionic Compounds: Type 1 & 2 • 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 a Na1+ charge • Type 2 ionic compounds contain a metal cation that can have different charges • For example, Iron can have more than one charge: Fe2+ & Fe3+ Na+ Fe2+ Fe3+

  10. Ionic Compounds: Type 1 & 2 • 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+

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

  12. Type 1 Ionic Compounds Iodide Potassium I- K+ Potassium Iodide

  13. Type 1 Ionic Compounds Oxide Magnesium always has a 2+ charge O2- Mg2+ Mg2+ Potassium Iodide Magnesium Oxide

  14. Ionic Compounds: Type 2 • 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 referred to PbCl2 or PbCl4 • Therefore, we need a way to specifying which cation is present • Is it Pb2+ & Pb4+ ? Pb2+ Pb4+

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

  16. Type 2 Ionic CompoundsTransition 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+

  17. Type 2 Ionic CompoundsTransition 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+

  18. Type 1 & Type 2 Ionic CompoundsWhat’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

  19. What’s are the 2 types of 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+ changes Answer Bank Anion Different Two Cation Changes metals different

  20. Ionic Compounds: Type 2 • 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-

  21. Ionic Compounds: Type 2 • 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!

  22. Practice: Write the formula for the following type 1 and 2 ionic compounds: Type 1: 3. Copper (I) chloride 4. Copper (II) chloride 5. Lead (IV) Sulfide 1. Potassium Oxide 2. Calcium Chloride -K2O -CaCl2 Type 2: - CuCl -CuCl2 -PbS2

  23. What are the names of the following type 1 and 2 ionic compounds? 1. CaCl2 2. MgI2 - Calcium Chloride - Magnesium Iodide Type 1: Type 2: - Copper (I) Chloride - Iron (II) Oxide -Lead (IV) Chloride 3. CuCl 4. FeO 5. PbCl4

  24. Summarize: • When naming Ionic compounds, the cation is named _____ and the ______ second • When naming Ionic compounds, the anion ends in ____. • What do the Roman Numerals indicate in an ionic compound??? • Write the name for MgF2 • Write the name for PbO2

  25. Unit: Nomenclature Topic: Covalent Compounds Objectives: Day 2 of 3 • To learn the naming rules for Covalent compounds • To learn that covalent compounds form between 2 nonmetals • To understand what polyatomic ions are and how they form compounds

  26. 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??? Carbon is not a metal!!!! • Why do you think we use prefixes such as tri- on words like triceratops, tricycle or tripod????

  27. 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

  28. Carbon Monoxide Made of 2 nonmetals: carbon & oxygen Covalent Compounds Nonmetals • CovalentCompounds contain only nonmetals

  29. Rules for Naming Covalent 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

  30. Prefixes PrefixExample

  31. Covalent 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!

  32. Naming Covalent Compounds • Let’s look at – SO3: • 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

  33. Covalent 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 pentaoxide

  34. What are covalent compounds and how do we name them? • 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

  35. Practice: #1-3 on your whiteboards and write the NAMES for the following covalent compounds: • PCl5 =_____________________ • P4O6 =_________________________ • N2O3 =_____________________ Phosphorous Pentachloride Tetraphosphorous Hexaoxide Dinitrogen Trioxide

  36. Practice: #1-3 on your whiteboards and write the formulas for the following covalent compounds: NO2 • Nitrogen dioxide = ____________ • Diphosphorus Pentachloride = _________ • Dinitrogen Pentoxide= ____________ P2Cl5 N2O5

  37. 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! [ ]+

  38. Common Polyatomic Ions • You must memorize!

  39. [ ]+ 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

  40. Ionic 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

  41. Ionic 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

  42. 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 ioniccompounds, the charges need to be neutral • Ag+ needs be balanced by the negatively charged polyatomic ion NO3- • Therefore we write: Silver (I) Nitrate

  43. 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!!!!

  44. What are Ionic Compounds with Polyatomic Ions? polyatomic • Compounds that contain a _________ ion • Ex: NaOH & CaCO3 Answer Bank polyatomic More Two N2O5 Penta- Nonmetals charge

  45. Practice: #1-3 on your whiteboards and write the formulas for the following compounds: K3PO4 • Potassium Phosphate = ___________ • Copper (II) sulfate = __________ • Calcium Carbonate =__________ CuSO4 CaCO3

  46. Practice: #1-3 on your whiteboards and write the NAMES for the following compounds: • NaOH =____________________ • MgCO3 =_________________________ • Fe(NO3)3 = ____________________ Sodium Hydroxide Magnesium Carbonate Iron (III) Nitrate

  47. Summarize: • Covalent compounds form between 2 ______ • In covalent compounds, _______ are used to show the number of atoms • Polyatomic ion is a group of two or ____ atoms that have a particular _____to them. • Review: Ionic compounds form between a metal and a __________ • Write the polyatomic compound that forms between the silver Ag+ cation and needs be negatively charged polyatomic ion NO3-

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

  49. 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????

  50. 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 andwere 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

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