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Nomenclature

Nomenclature. Types of Chemical Substances. Inorganic elements molecular ionic Organic aliphatic cyclic substituted Common substances inorganic or organic. Naming. must be simple as possible must be unique. Elements. one kind of atom most are monoatomic (one atom)

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Nomenclature

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  1. Nomenclature

  2. Types of Chemical Substances • Inorganic • elements • molecular • ionic • Organic • aliphatic • cyclic • substituted • Common substances • inorganic or organic

  3. Naming • must be simple as possible • must be unique

  4. Elements • one kind of atom • most are monoatomic (one atom) • Cu, Fe, Al, He • 8 elements are diatomic (2 atoms) • H2 N2 O2 F2 Cl2 Br2 I2 (At2) • 2 are polyatomic • S8 • P4

  5. Common Substances • known by names other than their systematic names • be familiar with • formulas • systematic name • common name • know whether systematic or common name takes precedence

  6. Common Substances FormulaChemical NameCommon Name H2O hydrogen oxide water NaCl sodium chloride table salt HCl hydrogen chloride hydrochloric acid HNO3 hydrogen nitrate nitric acid H2SO4 hydrogen sulfate sulfuric acid H3PO4 hydrogen phosphate phosphoric acid CH3COOH acetic acid vinegar CaSO4calcium sulfate gypsum (dry wall) NH3 nitrogen trihydride ammonia

  7. Common Substances FormulaChemical NameCommon Name H2O2hydrogen peroxide hydrogen peroxide C2H5OH ethanol drinking alcohol CH3OH methanol wood alcohol CH4methane natural gas O3ozone ozone C12H22O11sucrose table sugar KCl potassium chloride potash NaOH sodium hydroxide lye, caustic soda CaO calcium oxide lime

  8. Molecular Compounds • made up of 2 non-metals bound together with covalent bonds:

  9. Molecular Compounds • can’t predict formula so naming is done on a numbering system. • prefixes in front of the element name tell you how many of that element are present in the compound: mono 1 hexa 6 di 2 hepta 7 tri 3 octa 8 tetra 4 nona 9 penta 5 deca 10

  10. Molecular Compounds • N2O5 dinitrogen pentaoxide (note ending) • CO2 carbon dioxide (no mono on first atom) • CO carbon monoxide • Cl2O7 dichlorine heptaoxide

  11. -ides C carbide Cl chloride N nitride As arsenide O oxide Se selenide F fluoride Br bromide Si silicide Te telluride P phosphide I iodide S sulfide

  12. Molecular Compounds • tetraphosphorus decaoxide P4O10 • tetrasulfur tetranitride S4N4 • bromine monofluoride BrF • diarsenic triselenide As2Se3

  13. Ionic Compounds • made up of cations and anions which come together as a result of ionic attraction:

  14. Ionic Compounds • there is no molecule, rather a crystal lattice. • chemical formula is ratio of cations to anions in crystal; formula unit • ionic substances are recognized because they contain a metal + non-metal

  15. Simple Ionic Compounds • cations from groups 1 & 2, Al, Zn, Ag, Cd, NH41+ (all have only one possible charge) • anions can be anything on the chart (including polyatomic ions) • only one formula unit possible, so name is a repetition of the ion names: • NaCl Na1+ Cl1- sodium chloride

  16. Simple Ionic Compounds • NH4NO3 NH41+ NO31- ammonium nitrate • Al2(CO3)3 Al3+ CO32- aluminum carbonate • Ag3P Ag1+ P3- silver phosphide

  17. Simple Ionic Compounds • cadmium chlorite Cd2+ ClO21- Cd(ClO2)2 • strontium nitride Sr2+ N3- Sr3N2

  18. Stock System • used when the cation can have more than one possible charge • used for all other metals on the Periodic Table. • the name of the compound includes the charge of the cation in roman numerals, in brackets after the cation name.

  19. Classical System • older system • much, much, older • largely replaced by Stock system, but is still around. • if see name be able to give formula. • never give classical name for any formula.

  20. Waters of Hydration • water molecules physically attached to ionic and molecular substances. • name and formula recognizes their presence.

  21. Waters of Hydration • gypsum typically attracts 4 water molecules per formula unit: CaSO4· 4 H2O • name the substance then use a numbering prefix followed by subscript hydrate: calcium sulfate tetrahydrate

  22. Using Ion Charge to Predict Formulas a) K1+, Br1- f) Hg2+ , O2- KBr HgO b) Ca2+, Cl1- g) K1+ , PO43- CaCl2 K3PO4 c) Li1+, H1- h) Pb4+, O2- LiH PbO2 d) Fe3+, OH1- i) NH41+ , SO42- Fe(OH)3 (NH4)2SO4 e) Ca2+, ClO41- j) Mg2+, BO33- Ca(ClO4)2 Mg3(BO3)2

  23. Using Formulas to Predict Ion Charge a) ZnSO4 f) KSCN Zn2+ SO42- K1+ SCN1- b) Mg(NO3)2 g) Na2SeO3 Mg2+ NO31- Na1+ SeO32- c) FeO h) Al2(Cr2O7)3 Fe2+ O2- Al3+ Cr2O72- d) LiHCO3 i) MgC2O4 Li1+ HCO31- Mg2+ C2O42- e) Hg2Cl2 j) SrH2 Hg22+ Cl1- Sr2+ H1-

  24. 1) NH3ammonia 2) Fe(NO3)2Fe2+ NO31-iron (II) nitrate 3) SO2sulfur dioxide 4) MgBr2Mg2+ Br1-magnesium bromide 5) GeCl4Ge4+ Cl1-germanium (IV) chloride 6) N2nitrogen 7) AlPO4Al3+ PO43-aluminum phosphate 8) C2H5OH ethanol 9) Li2CrO4Li1+ CrO42-lithium chromate 10) KH K1+ H1-potassium hydride 11) CuCr2O7Cu2+ Cr2O72-copper (II) dichromate 12) NH4NO3NH41+ NO31-ammonium nitrate

  25. 13) CO2carbon dioxide 14) P2O5  6 H2O diphosphorus pentaoxide hexahydrate 15) PbO Pb2+ O2-lead (II) oxide 16) BaS Ba2+ S2-barium sulfide 17) S8sulfur 18) Mo(NO3)7Mo7+ NO31-molybdenum (VII) nitrate 19) BaH2Ba2+ H1-barium hydride 20) CaSO4  4 H2O Ca2+ SO42-calcium sulfate tetrahydrate 21) O2oxygen 22) Al2O3Al3+ O2-aluminum oxide 23) PCl3phosphorus trichloride 24) CuSO3Cu2+ SO32-copper (II) sulfite

  26. 1) sodium fluoride Na1+ F1- NaF 2) potassium carbonate K1+ CO32- K2CO3 3) aluminum sulfide Al3+ S2- Al2S3 4) calcium bromide Ca2+ Br1- CaBr2 5) chlorine heptafluoride ClF7 6) silver oxide Ag1+ O2- Ag2O 7) ammonium sulfide NH41+ S2- (NH4)2S 8) barium hydroxide Ba2+ OH1- Ba(OH)2 9) phosphorus P4 10) mercurous chloride Hg22+ Cl1- Hg2Cl2 11) tin (II) nitrate Sn2+ NO31- Sn(NO3)2 12) potassium bisulfite K1+ HSO31- KHSO3

  27. 13) calcium carbonate Ca2+ CO32- CaCO3 14) ammonium sulfite NH41+ SO32- (NH4)2SO3 15) iron (II) hydroxide Fe2+ OH1- Fe(OH)2 16) uranium (VI) nitrate U6+ NO31- U(NO3)6 17) ozone O3 18) lithium dichromate Li1+ Cr2O72- Li2Cr2O7 19) hydrogen nitrate H1+ NO31- HNO3 20) barium bicarbonate Ba2+ HCO31- Ba(HCO3)2 21) nitrogen dioxide NO2 22) carbon monoxide CO 23) methanol CH3OH 24) ammonium oxalateNH41+ C2O42- (NH4)2C2O4

  28. Organic Nomenclature • 3 types of organic compounds important for this class: • aliphatic hydrocarbons - chains • cyclic hydrocarbons - rings • aromatic hydrocarbons - benzene rings

  29. Organic Nomenclature Naming hydrocarbons involves looking at 3 aspects: • Number of carbons linked in a continuous chain. • The presence of single, double or triple bonds in the carbon chain. • The presence of structures other than hydrogen attached to the main carbon chain (functional groups).

  30. 1. Length of Carbon Chain    • how many carbons are bonded in a chain gives the prefix of the name: 1 meth- 7 hept- 2 eth- 8 oct- 3 prop- 9 non- 4 but- 10 dec- 5 pent- 11 undec- 6 hex- 12 dodec-

  31. 1. Length of Carbon Chain    • other prefixes include: 13 tridec- 30 triacont- 14 tetradec- 40 tetracont- 15 pentadec- 50 pentacont- 20 eicos- 100 hect- 25 pentacos-

  32. 2. Family Background • carbon atoms make 4 chemical bonds. • carbon atoms can be linked to each other by one pair of electrons (single bond), two pair (double bond), or three pair (triple bond). • the presence of double or triple bonds on the carbon chain changes the chemical family.

  33. 2. Family Background • alkanes • all carbons are connected by single bonds • the suffix –ane is added to the name of the compound • the general formula is CnH2n+2 hexane

  34. alkenes • the carbon chain contains at least one double bond • the suffix –ene is added to the name of the compound • the general formula is CnH2n propene

  35. alkynes • the carbon chain contains at least one triple bond • the suffix –yne is added to the name of the compound • the general formula is CnH2n-2 propyne

  36. Isomers • is defined as the structure associated with a chemical formula. • for many organic compounds it is possible to have more than one isomer for a given formula. • the simplest isomers are alkenes and alkynes where the double or triple bond can have more than one location:

  37. C4H8 • 1-butene • 2-butene • number the carbons from the end closest to the multiple bond:

  38. Isomers • 1- hexene • the double bond is located closest to the left-hand side, so that is where numbering starts.

  39. Isomers • 2-hexene • the double bond is closer to the right-hand side, so numbering begins there.

  40. Isomers • 1-hexene • 1-hexene • these two are the same molecule.

  41. C4H6 • 1-butyne • 2-butyne

  42. Functional Groups • hydrocarbon chains • halogens • alcohols

  43. Functional Groups • Hydrocarbon chains are carbon chains attached to the main chain: this is called methylbutane

  44. Functional Groups • Prefixes are used to indicate the number of carbons in the chain: • 1 carbon - methyl- • 2 carbons - ethyl- • 3 carbons - propyl-

  45. Functional Groups • when it is possible to attach the hydrocarbon in more than 1 place numbering is used: • 2-methylpentane

  46. Functional Groups • 3-methylpentane • 4-methyl-2-pentene

  47. Functional Groups • 2,3-dimethylpentane

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