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Nomenclature : Naming Chemicals

Nomenclature : Naming Chemicals. PO 4 3- phosphate ion. HC 2 H 3 O 2 Acetic Acid. SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!.

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Nomenclature : Naming Chemicals

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  1. Nomenclature: Naming Chemicals PO43- phosphate ion HC2H3O2 Acetic Acid SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")! C2H3O2- acetate ion

  2. Before naming…. • Some things you MUST know to be successful…. You really need to commit these things to memory

  3. Metals • Conductors • Lose electrons • Malleable and ductile

  4. Nonmetals • Brittle or gases • Gain electrons • Covalently bonds to each other

  5. Semi-metals or Metalloids • Characteristics of both metals and nonmetals • Metallic character increases as go down PT

  6. Alkali Metals

  7. Alkaline Earth Metals

  8. Transition metals

  9. Inner Transition Metals

  10. Halogens

  11. Noble Gases

  12. Ions • Atoms or groups of atoms with a charge. • Cations- positive ions - get by losing electron(s). • Anions- negative ions - get by gaining electron(s). • Ionic bonding- held together by the opposite charges. • Ionic solids are called salts.

  13. Common Ions of Elements +1 +3 +/-4 +2 -3 -2 -1 Variable, always +

  14. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd+2

  15. Polyatomic Ions • Groups of atoms that have a charge. • Ions that contain covalently bonded atoms * NO3- :nitrate ion * NO2- :nitrite ion • Yes, you have to memorize them. • List in your yellow folder: memorize this list!!!!

  16. Patterns for Polyatomic Ions • -ate ion • chlorate = ClO3- • -ate ion plus 1 O  same charge, per- prefix • perchlorate = ClO4- • -ate ion minus 1 O  same charge, -ite suffix • chlorite = ClO2- • -ate ion minus 2 O  same charge, hypo- prefix, -ite suffix • hypochlorite = ClO-

  17. Polyatomic Ions You can make additional polyatomic ions by adding a H+ to the ion! CO3-2 is carbonate HCO3– is hydrogen carbonate H2PO4– is dihydrogen phosphate HSO4– is hydrogen sulfate

  18. Forms of Chemical Bonds • There are 3 forms bonding atoms: • Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) • metal and non metal or polyatomics • The resulting cation and anion are attracted to each other by electrostatic forces. • Covalent—some valence electrons shared between atoms • we will just learn the rules for 2 non-metals. • Metallic – holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

  19. COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl- --> NaCl A neutral compound requires equal number of + and - charges.

  20. NH4+ Cl- IONIC COMPOUNDS ammonium chloride, NH4Cl

  21. Ionic compounds • If the cation is monatomic- Name the metal (cation) just write the name. • If the cation is polyatomic- name it. • If the anion is monatomic- name it but change the ending to –ide. • If the anion is poly atomic- just name it • Practice.

  22. Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calcium ion • 3. Monatomic anion = root + -ide • Cl- = chloride • CaCl2 = calcium chloride

  23. Naming Binary Ionic Compounds • Examples: NaCl ZnI2 Al2O3 sodium chloride zinc iodide aluminum oxide

  24. Learning Check Complete the names of the following binary compounds: Na3N KBr Al2O3 MgS sodium nitride potassium bromide aluminum oxide magnesium sulfide

  25. Monatomic Ions These are from the periodic table that you saw a few slides ago!

  26. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

  27. Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and themetalsin groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl3(Fe3+) iron (III) chloride CuCl (Cu+ ) copper (I) chloride SnF4 (Sn4+) tin (IV) fluoride PbCl2 (Pb2+) lead (II) chloride Fe2S3 (Fe3+) iron (III) sulfide

  28. Special names Cations Some Type II cations have a name using the “old” system as well as the “new system”. The old system, still widely used, adds to the root or stem of the Latin name of the metal the suffixes –ous and –ic. These represent the lower and higher charges respectively.

  29. Old Names for Type II ions

  30. Examples of Older Names of Cations formed from Transition Metals(you do not have to memorize these)

  31. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 CuCl SnO2 Fe2O3 Hg2S iron (II) bromide copper (I) chloride tin (IV) oxide iron (III) oxide mercury (I) sulfide

  32. Naming Ternary Compounds • Contains at least 3 elements • There MUST be at least one polyatomic ion (it helps to circle the ions) • Examples: NaNO3 Sodium nitrate K2SO4 Potassium sulfate Al(HCO3)3 Aluminum bicarbonate or Aluminum hydrogen carbonate

  33. Learning Check Match each set with the correct name: 1.Na2CO3 a) magnesium sulfite MgSO3 b) magnesium sulfate MgSO4 c) sodium carbonate 2 . Ca(HCO3)2 a) calcium carbonate CaCO3 b) calcium phosphate Ca3(PO4)2 c) calcium bicarbonate

  34. Match each set with the correct name: • 1.Na2CO3 a) sodium carbonate • MgSO3 b) magnesium sulfite • MgSO4 c) magnesium sulfate • 2 . Ca(HCO3)2 a) calcium bicarbonate • CaCO3 b) calcium carbonate • Ca3(PO4)2 c) calcium phosphate

  35. Name the following: Na2O CaCO3 PbS2 Sn3N2 Cu3PO4 HgF2 sodium oxide calcium carbonate lead (IV) sulfide tin (II) nitride copper (I) phosphate mercury (II) fluoride Mixed Practice!

  36. Covalent compounds • Two words, with prefixes. • Prefixes tell you how many. • First element whole name with the appropriate prefix, except mono. • Second element, -ide ending with appropriate prefix. • Practice

  37. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

  38. Molecular Nomenclature: Examples • CCl4 • N2O • SF6 • carbon tetrachloride • dinitrogen monoxide • sulfur hexafluoride

  39. More Molecular Examples • arsenic trichloride • dinitrogen pentoxide • tetraphosphorus decoxide • AsCl3 • N2O5 • P4O10

  40. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO CO2 PCl3 CCl4 N2O carbon monoxide carbon dioxide phosphorus trichloride carbon tetrachloride dinitrogen monoxide

  41. Learning Check 1. P2O5a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl2O7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl2 a) chlorine b) dichlorine c) dichloride

  42. Learning Check 1. P2O5a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl2O7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl2 a) chlorine b) dichlorine c) dichloride

  43. Mixed Review Name the following compounds: 1. CaO a) calcium oxide b) calcium(I) oxide c) calcium (II) oxide d) calcium monoxide 2. SnCl4 a) tin tetrachloride b) tin(II) chloride c) tin(IV) chloride 3. N2O3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

  44. Mixed Review Name the following compounds: 1. CaO a) calcium oxide b) calcium(I) oxide c) calcium (II) oxide d) calcium monoxide 2. SnCl4 a) tin tetrachloride b) tin(II) chloride c) tin(IV) chloride 3. N2O3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

  45. Overall strategy for naming chemical compounds.

  46. A flow chart for naming binary compounds.

  47. Common Names • A lot of chemicals have common names as well as the proper IUPAC name. • Chemicals that should always be named by common name and never named by the IUPAC method are: • H2O water, not dihydrogen monoxide • NH3 ammonia, not nitrogen trihydride

  48. Mixed Practice • BaI2 • P4S3 • Ca(OH)2 • FeCO3 • Na2Cr2O7 • I2O5 • Cu(ClO4)2 • CS2 • B2Cl4 • Barium iodide • Tetraphosphrus trisulfide • Calcium hydroxide • Iron (II) carbonate • Sodium dichromate • Diiodine pentoxide • Copper (II) perchlorate • Carbon disulfide • Diboron tetrachloride

  49. Acid Nomenclature • Acids • Compounds that form H+ in water. • Formulas usually begin with ‘H’. • In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) • Ternary acids are ALL aqueous • Two types of acids: • Oxyacids • Non-oxyacids

  50. Naming acids • If the acid doesn’t have oxygen • add the prefix hydro- • change the suffix -ide to -ic acid • HCl Hydrochloric acid • H2S Hydrosulfic acid • HCN Hydrocyanic acid

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