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Unit 4

Unit 4. Inorganic Nomenclature. What We Hope to Learn This Unit. Identify the different types of ions and explain or describe each Identify the type of compound by its formula or name Identify and explain the major types of bonding (ionic and covalent)

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Unit 4

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  1. Unit 4 Inorganic Nomenclature

  2. What We Hope to Learn This Unit • Identify the different types of ions and explain or describe each • Identify the type of compound by its formula or name • Identify and explain the major types of bonding (ionic and covalent) • Write the names and formula for ionic and covalent compounds, given appropriate charts or data tables • Write the names and formula for hydrates and acid compounds, given appropriate charts or data tables

  3. Element Song • http://www.youtube.com/watch?v=pwPaqaQEuJw

  4. 4-1. The Chemical ElementsAn Introduction and Background Information How do I know if it is an Element? • Element’s are easy to ID • The first letter in the symbol is ALWAYS in upper case (capitals) • Second letters (if present) are ALWAYS in lower case • Identify as a compound/molecule or element: Fe HI ZnO NaCl Cr Al H CuF CO

  5. How are symbols and names chosen for elements? • Greek or Latin • named after the person who discovered the element • after other famous scientists to honor that person • Named after the location it was discovered in… Note that: • For many elements, the symbol is just the first letter (or first two letters) of the name of the element. • Note that the symbol for some elements is taken from the name in another language (Greek and Latin origins quite common) and is not the first two letters of the element's name in English.

  6. Some Examples: hydrogen, symbol H, is from the Greek words hudôr (water) and gennan (generate) oxygen, symbol, O, is from the Greek words oxus (acid) and gennan (generate) carbon, symbol C, is from the Latin carbo (coal) lead, symbol Pb, is for plumbum, which is "lead" in Latin gold, symbol Au, is for aurum, which is "gold" in Latin curium, symbol Cm, after Pierre and Marie Curie for their contributions to chemistry (Curium was discovered by G. T. Seaborg) lawrencium, symbol Lr, after Ernest Lawrence berkelium, symbol Bk, after Berkeley, California where much research was done on discovering new elements

  7. Definitions: • Anion = - charge • Cation = + charge • Monatomic = species with one atom • Diatomic = species with two atoms (same or diff) • Triatomic = species with three atoms (same or diff) • Polyatomic = general term to mean made up of many atoms (“poly” = more then one)

  8. Identifying the Different components of a Compound • The most important step in writing names and formulas is to ID the ions involved

  9. How do Metals and Nonmetals become ions?

  10. Metals ALWAYS LOSE electron to become stable Nonmetals ALWAYS GAIN electron to become stable

  11. What are Polyatomic Ions (PAI)? • A polyatomic ion is usually a charged species (ion) composed of two or more atoms covalently bonded

  12. How do PAI form? • collection of atoms has gained or lost an electron in a chemical reaction. • extra electrons are shared by all the atoms in the PAI (sort of smeared around the atoms in the ion).

  13. What does a formula mean? Cu(NO3)2 - Subscripts The subscripts say: there are 2- NO3 ions for every 1- Cu ion • The copper wants to get rid of 2 electrons and each NO3 ion can only accept 1 electron, so two are needed.

  14. Count up the # of each atom:Cu(NO3)2 Cu = 1 N = (2 x 1) = 2 O = (2x3) = 6 • The subscript outside of a bracket is multiplies by each subscript inside of the bracket • If there is no subscript, assume “1”

  15. Ionic Bonds • http://www.youtube.com/watch?v=xTx_DWboEVs&feature=related

  16. Ionic Compounds

  17. What happens when a metal has two electrons to get rid of the nonmetal can only accept one electron?

  18. Covalent Compounds

  19. 4.2. Naming Inorganic Compounds

  20. 1. Writing Names for Ionic Compounds(M (s)+ NM) The rules are : • Write the first name as it appears on the PT • Write the root of the second name as it appears on the PT BUT change the ending to “IDE” Li2S = Lithium sulphide AlI3 = Aluminum Iodide ZnO = Zinc Oxide

  21. Writing Formulas for Ionic Compounds(M (s)+ NM) The rules are: • Identify the charges for each ion from the PT • CRISS CROSS charges to make subscripts • Reduce if possible

  22. Magnesium chloride.

  23. Barium oxide.

  24. 2. Writing Names for (M (v)+ NM) The Rules are: • Write the first name as it appears on the PT BUT you must indicate the charge used by including a ROMAN NUMERAL immediately after the metals name • To find out what charge was used, you must uncross the charges. If the nonmetals charge is right, then the charges were not reduced, and the charge on the metal will be the roman numeral to use • Write the root of the second name as it appears on the PT BUT change the ending to “IDE”

  25. CuCl2 • uncross the charges = Cu+2 and Cl-1 • Cl is supposed to have a -1 charge • Name = copper(II) chloride CuO • uncross the charges = Cu+1 and O-1 • Oxygen is supposed to have a -2 charge, therefore the charges were reduced. • Multiply both charges by the same number to obtain the correct charge for the nonmetal. In this case multiply both by 2 • Now the charges are Cu+2 and O-2 • Name = copper(II) oxide

  26. Try these: • FeO • CrF • MnO2

  27. Try these: • FeO Iron(II) oxide • CrF3 Chromium(III) flouride • MnO2 Manganese(IV) oxide

  28. Writing Formulas for (M (v)+ NM) The rules: • Identify the charge for the metal from the roman numeral • Identify the charge on the nonmetal from the PT • Criss- cross charges to make subscripts • Reduce if possible

  29. copper(II) chloride Copper(I) oxide

  30. 3. Writing Names for (M (s)+ PAI) The rules: • Write the metals name as it appears on the PT (the first capital letter) • Identify the name of the polyatomic ion from your data booklet • Write the name of the poly as it appears Na2SO4 = sodium sulphate KOH = potassium hydroxide

  31. Writing Formulas for (M (s)+ PAI) The rules: • Identify the charges for each ion for the PT and the data booklet • Criss cross charges (never change the subscripts of the poly, do not use them as charges!) • Put brackets around the poly if there is a charge greater than 1 on the metal • The charge of the metal will stay on the OUTSIDE of the brackets • Reduce if possible

  32. silver cyanide • sodium phosphate

  33. 4. Writing Names for (M (v)+ PAI) The rules: • Write the first name as it appears on the PT BUT you must indicate the charge used by including a roman numeral immediately after the metals name • Identify the name of the polyatomic ion from your data booklet • Write the name of the poly as it appears Fe2(SO4)3 = iron(III) sulphate Pd (ClO)2 = lead(II) hypochlorite

  34. Writing Formulas for (M (v)+ PAI) The Rules: • Identify the charge for the metal from the roman numeral • Identify the charge on the poly from the Data booklet • Criss- cross charges to make subscripts • Use brackets if the charge on the metal is greater than 1 • Reduce if possible

  35. copper(II) chlorate

  36. 5. Writing Names for Covalent Compounds(NM + NM) The rules: • The subscript in front of each NM will be the GREEK PREFIX used Mono = 1 Penta = 5 Nona = 9 Di = 2 Hexa = 6 Deca = 10 Tri = 3 Hepta = 7 Tetra = 4 Octa = 8 • Look up the name of each NM from the PT, from the Greek prefix, place correct Greek prefix INFRONT of the NM’s name • Change the ending of the 2nd NM’s name to –ide • Do not use the word mono in front of the first NM’s name 

  37. SO3 = sulphur trioxide • P2S3 = diphosphorus trisulphide • BrF = bromine monoflouride

  38. Writing Formulas for Covalent Compounds(NM + NM) The rules: • The Greek prefix in front of the NM’s name will tell you the subscript to use in front of that NM’s symbol • Do not criss cross these prefixes!! Silicon tetraflouride = SiF4 Diphosphorus trisulphide = P2S3 Sulphur monoxide = SO

  39. 6. The Nomenclature of Hydrates • Hydrates are substances that include water into their formula. • The water is not actually part of the chemical substance and this is reflected in the way the formula is written. • Here is the example: CuSO4• 5 H2O • This formula means that for every one CuSO4 in the piece of this substance you are holding, there are also five water molecules. • No, the substance is not wet, it appears dry. There are some hydrates that have a wet appearance, but most appear perfectly dry to the eye and to the touch.

  40. The dot IS NOT a multiplication sign. • Here is the name: copper(II) sulfate• pentahydrate. • Notice penta meaning five and hydrate meaning water. Use this name both when writing the name or speaking it. • That means that when you hear "pentahydrate," you have to know to write the dot and then the 5 H2O.

  41. Practice Problems 1) Suppose you heard "trihydrate." What would you write? 2) Suppose you heard "octahydrate." What would you write? 3) Name this substance: MgSO4• 9 H2O 4) Write the formula for: barium chloride dihydrate

  42. Hydrate Problem Answers 1) trihydrate = • 3 H2O 2) octahydrate = • 8 H2O 3) Magnesium sulfate nonahydrate 4) BaCl2• 2 H2O

  43. 7. Acid Nomenclature • Acids • Compounds that form H+ in water. • Formulas usually begin with ‘H’. • Exceptions: H2O, CH3COOH

  44. Acid Nomenclature Flowchart

  45. Acid Nomenclature • HBr (aq) • H2CO3 • H2SO3 hydrobromic acid • 2 elements, -ide • 3 elements, -ate  carbonic acid  sulfurous acid • 3 elements, -ite

  46. Hydrofluoric acid • Starts with hydro-, binary • Ions = H + and F- • HF • Sulphuric acid • No hydro… means PAI present • -ic, was –ate, sulphate • Ions = H+ and SO4-2 • H2SO4 • Nitrous acid • -ous, was –ite, nitrite • Ions = H+ and NO2- • HNO2

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