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Nomenclature of compounds

Unit 1-6 (chapter 2.7). Nomenclature of compounds. Nomenclature:. Inorganic binary compounds Ionic & covalent bonds Compounds composed of two elements. Nomenclature:. Binary ionic compounds (type 1) Cation written first Monatomic cation named from element Anion second

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Nomenclature of compounds

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  1. Unit 1-6 (chapter 2.7) Nomenclature of compounds

  2. Nomenclature: • Inorganic binary compounds • Ionic & covalent bonds • Compounds composed of two elements

  3. Nomenclature: • Binary ionic compounds (type 1) • Cation written first • Monatomic cation named from element • Anion second • Monatomic anion named from the root of the element and changing the ending to -ide

  4. Nomenclature: • Binary ionic compounds (type 2) • When cations form more than one type of positively charged ion, the charge on the ion is indicated by Roman numerals • Example – iron (III) & iron (II) • ALSO – for metals with only two ions – the ion with the higher charge ends in –ic and the ion with the lower charge ends in –ous • Example – ferric & ferrous (aka: iron)

  5. Nomenclature:

  6. Nomenclature: • Binary covalent compounds • First element in the formula is named first using the full element name • Second element is named like anions (root of element & -ide) • Prefixes are used to denote numbers of atoms present in the compound • Exception: mono- is not used with the first element

  7. Nomenclature: • Prefixes: • Mono- = 1 • Di- = 2 • Tri- = 3 • Tetra- = 4 • Penta- = 5 • Hexa- = 6 • Hepta- = 7 • Octa- = 8 • Nona- = 9 • Deca- = 10

  8. Nomenclature: • Another exception: • Some binary covalents are referred to by their common names NOT their systemic names • Examples: water, ammonia

  9. Nomenclature:

  10. Nomenclature: • Ionic compounds with polyatomic ions • Polyatomic names aren’t changed when naming compounds • Oxyanions can vary in the number of oxygen atoms composing the polyatomic ion • With variation - name changes BUT CHARGE DOES NOT CHANGE

  11. Nomenclature: • When there are two possible oxyanions, most oxygen atoms ends in –ate & fewest oxygen atoms ends in –ite • When there are more than two possible oxyanions: • Most oxygen atoms also ends in –ate AND it is given the prefix per- • Fewest oxygen atoms also ends in –ite AND it is given the prefix hypo-

  12. Nomenclature: • Examples: • Sulfate (SO42-) & sulfite (SO32-) • Perchlorate (ClO4-), chlorate (ClO3-), chlorite (ClO2-), & hypochlorite (ClO-)

  13. Nomenclature of acid: • Acids • Acids w/oxyanions • Acid name formed from the root of the anion name and the ending is –ic or –ous depending on whether the oxyanion is an –ate or an –ite • ate becomes –ic & -ite becomes -ous • Acids w/o oxyanions • The prefix hydro- is used and the ending of the anion is -ic

  14. Naming Oxyacids & Oxyanions • Oxyacid: polyatomic acid that contains a nonmetal bonded to one or more oxygen atoms H3BO3 H2CO3 HNO3 X X XH3PO4 H2SO4 HClO3 H3AsO4 H2SeO4 HBrO3 X HIO3 Also: H2CrO4 = chromic acid

  15. Oxyanions: polyatomic anions that contain a nonmetal bonded to one or more oxygen atoms.

  16. Other Oxyacids Patterns H3PO4 phosphoric acid H2PO41-dihydrogen phosphate HPO42-hydrogen (or monohydrogen) phosphate PO43-phosphate H2CO3carbonic acid HCO31- hydrogen carbonate or bicarbonate CO32- carbonate

  17. Nomenclature:

  18. Mixed Practice • Dinitrogen monoxide • Potassium sulfide • Copper (II) nitrate • Dichlorine heptoxide • Chromium (III) sulfate • Ferric sulfite • Calcium oxide • Barium carbonate • Iodine monochloride • N2O • K2S • Cu(NO3)2 • Cl2O7 • Cr2(SO4)3 • Fe2(SO3)3 • CaO • BaCO3 • ICl

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

  20. Naming Hydrates • Name the compound, then the Greek prefix, and then add -hydrate. Ex: CuSO4۰5 H2O copper (II) sulfate pentahydrate

  21. Nomenclature: • A HYDRATE is an salt that has water molecules trapped within its crystals. • Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes. • Mono- for one; di- for two; tri- for three; etc.

  22. Hydrate Examples: • WRITING FORMULAS: copper(II) fluoride tetrahydrate CuF2·4 H2O calcium nitrate trihydrate Ca(NO3)2 ·3 H2O • WRITING NAMES: MgSO4· 7 H2O magnesium sulfate heptahydrate FeCl2 · H2O iron (II) chloride monohydrate

  23. Naming Compounds Flow Chart Does the formula start with H? NO YES Does it begin with a metal that has more than one oxidation number? (e.g. Fe, Ni, Cu, Sn, Hg) NO YES It is an acid (must be aqueous). Does the acid contain a polyatomic ion? NO YES Name the first element followed by its oxidation number (Roman Numeral) or “old school” –ic or –ous endings. Does the acid end with a polyatomic ion? –ite –ate Does the formula contain a polyatomic ion? NO YES Name the polyatomic ion, replacing the –ate ending with –ic. Add the word acid. Are both elements nonmetals? NO YES Name the first element, then the polyatomic ion. If two elements are present, name both, then the polyatomic ion (e.g. NaHCO3 is sodium hydrogen carbonate). Name the first element, Then the second element with an –ide ending. Name the polyatomic ion, replacing the –ite ending with –ous. Add the word acid. Name the first element using the proper prefix (never mono–). Name the second element with the proper prefix (including mono–) and –ide ending. 1 = mono– 4 = tetra– 7 = hepta– 10 = deca– 2 = di– 5 = penta– 8 = octa– 3 = tri– 6 = hexa– 9 = nona–(notnano–) Write the prefix hydro–, then the name of the second element with –ic ending. Add the word acid.

  24. Complex ions and coordination compound Complex:species in which a central metal ion (usually a transition metal) is bonded to a group of surrounding molecules or ions Coordination compound: compound that contains a complex ion or ions.

  25. A coordination compound, or complex, consists of: • Metal ion: • Ligand or complexing agent: molecule or ion with a lone pair of e- that bonds to a metal ion

  26. A coordination compound, or complex, consists of: • Metal ion • mostly transitional metal, except for Al3+ • Acts as an e- pair acceptor • Electrophile: species that is “e- poor” and seeks e- (gets attacked by nucleophile) • Ligand or complexing agent: molecule or ion with a lone pair of e- that bonds to a metal ion • Acts as an e- pair donor • Coordinate covalent bond: metal-ligand bond • Nucleophile:species that is “e- rich” and seeks an e- poor area of a molecule (seeks an electrophile)

  27. Lewis Structures of common ligands NH3 CN- S2O32- SCN- H2O (not always included in formula, however)

  28. Complexation reactions • Ligand usually added “in excess” • Usually result in color changes (colors generally originate from e- transitions in a partially filled d shell) • Change properties of metal ion • Thermodynamic (DH, DS, DG) • Electrochemical (Eº)

  29. The golden-orange compound is Co*6NH3Cl3 while the purple compound only has 5 ammonia molecules in the coordinated compound. As shown in the ball-and-stick model, the chlorides serve as counter ions to the cobalt/ammonia coordiation complex in the orange compound, while one of the ammonia molecules is replaced by Cl in the purple compound. In both cases, the coordination geometry is octahedral around Co.

  30. Notation • Write complexes in square brackets, with charge on outside Ex: Cu2+ (aq) + 4 NH3 (aq) → [Cu(NH3)4]2+ (aq) :NH3 2+ :NH3 H |Cu2+ (aq) + 4 :N ─ H (aq) → Cu | H H3N: :NH3

  31. Nomenclature • Name cation before anion; one or both may be a complex. (Follow standard nomenclature for non-complexes.) • Within each complex (neutral or ion), name all ligands before the metal. • Name ligands in alphabetical order • If more than one of the same ligand is present, use a numerical prefix: di, tri, tetra, penta, hexa, … • Ignore numerical prefixes when alphabetizing.

  32. Nomenclature (continued) • Anionic ligand: • an –o ending is used in place of any anions. • Br-bromo- CN-cyano- Cl-chloro- OH-hydroxo- • For anions ending in –ate, the –o is substituted for the –e . • For neutral ligands, the name of the molecules is used, with the exception of

  33. If the complex is an anion, use –ate suffix after metal Record the oxidation number of the metal in parentheses (if appropriate). Ex: [Co(NH3)5Cl]Cl2 pentamminechlorocobalt (III) chloride

  34. Nomenclature practice potassium hexacyanoferrate (II) tetrammineaquacyanochromium (III) chloride sodium tetrahydroxoaluminate 1. K4[Fe(CN)6] 2. [Cr(NH3)4(H2O)CN]Cl2 3. Na[Al(OH)4]

  35. Writing Formulas of Coordination Complexes • Given Name → Write Formula • The formula of a coordination complex is written in a different order than its name. The chemical symbol of the metal center is written first. The ligands are written next, with anion ligands coming before neutral ligands. If there is more than one anion or neutral ligand, they are written in alphabetical order according to the first letter in their chemical formula. •  Practice: • sodium tetrahydroxoaluminate • Na[Al(OH)4]

  36. handout HOmework

  37. Introduction to Organic compounds

  38. First Ten Alkanes (nonpolar, oil like) Alkane = CnH2n+2

  39. Structural Shorthand Explicit hydrogens (those required to complete carbon’s valence) are usually left off of drawings of hydrocarbons C1 C2 C3 C4 C1 C3 C4 C2 Line intersections represent carbon atoms

  40. Structural Isomers Isomers are molecules with the same chemical formula, but different organization of atoms (different bonding) n-Pentane, C5H12 Isopentane, C5H12 Neopentane, C5H12

  41. Rules for Naming Alkanes The positions of substituent groups are specified by numbering the longest chain of carbon atoms sequentially, starting at the end closest to the branching. 1 2 3 4 Methyl

  42. RULES FOR NAMING ALKANES The location and name of each substituent are followed by the root alkane name. The substituents are listed in alphabetical order (irrespective of any prefix), and the prefixes di-, tri-, etc. are used to indicate multiple identical substituents. 1 2 3 4 Name: 2-methylbutane Methyl

  43. Alkenes Contain Carbon-CarbonDouble bonds Ethene

  44. Alkynes Contain Carbon-Carbon Triple Bonds Ethyne

  45. Reactions of Alkenes and Alkynes Hydrogenation Propene Propane Halogenation 1-Pentene 1-2-dibromopentene Polymerization Small molecules are joined together to form a large molecule Polyethylene

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