1 / 49

Inorganic chemical nomenclature (textbook: 12 - 25)

Inorganic chemical nomenclature (textbook: 12 - 25). Noble gases. Alkaline earth metals. Chalcogens. Alkali metals. Halogens. NONMETALS. SEMIMETALS. METALS. Electronegativity Oxidation state (oxidation number) Valence Ionic charge - "real electric charge"

ewa
Download Presentation

Inorganic chemical nomenclature (textbook: 12 - 25)

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Inorganic chemical nomenclature(textbook: 12 - 25)

  2. Noble gases Alkaline earth metals Chalcogens Alkali metals Halogens NONMETALS SEMIMETALS METALS

  3. Electronegativity Oxidation state (oxidation number) Valence Ionic charge - "real electric charge" cations: Na+ Ca2+ Al3+ anions: Cl- SO42-

  4. Chemical formulas We have several types of formulas: (according to the information they contain) 1) Empirical formula 2) Molecular formula 3) "Condensed formula" 4) Structural formula 5) Structural formula showing unshared electrons

  5. 1) EMPIRICAL - relative number of each type of atom (ratio of the elements) - e.g. H2SO4 Al2O3 CH2O 2) MOLECULAR - real number of atoms in the molecule - e.g. H2SO4 Al2O3 C6H12O6 3) "CONDENSED" (functional groups) - characteristic groups of atoms (=functional groups) - e.g. Mg(OH)2 (NH4)2SO4 K4[Fe(CN)6]

  6. 4) STRUCTURAL - types and arrangement of bonds between atoms 5) STRUCTURAL with unshared electrons - shows also unshared (non-bonding) electron pairs

  7. Latin nomenclature (INN) INN = International Nonproprietary Names - intended to be used worldwide for the identification of a given pharmaceutical substance - free of any protection of rights of ownership - recommendations come from World Health Organization (WHO)

  8. "Drug names" TRADE NAME - registered to pharmaceutical company - protection of rights of ownership CHEMICAL NAME - long, difficult GENERIC NAME (INN) – "free" e.g. simvastatinum - trade names in the Czech republic: Zocor, Simgal, Simvor, Vasilip, Simvastatin AL, APO-Simva, ... ... - statinum  drug for lowering cholesterol

  9. Symbols of chemical elements - derived from LATIN name K Kalium N Nitrogenium Na Natrium B Borum Br Bromum Ag Argentum Ar Argonum As Arsenum English name - - - > symbol ? Le Pb L lead Plumbum

  10. Trip to linguistics (morphology) PREFIX STEM of the word SUFFIX (ending) hypo - chlor - ate 1. nominative Natrium 2. genitive Natrii 3. dative Natrio 4. accusative Natrium 5. vocative Natrium 6. ablative Natrio Latin is a highly inflected language. nouns - six cases - many declensions

  11. Genitive forms element names - usual ending: - UM Lithium, Ferrum, Cuprum, Calcium genitive form - I Lithii, Ferri, Cupri, Calcii Plumbum - - > Plumbi Natrium - - > Natrii

  12. Elements with different namesin English and in Latin !!! Sb antimony Stibium Cu copper Cuprum Au gold Aurum Fe iron Ferrum Pb lead Plumbum Hg mercury Hydrargyrum Ni nickel Niccolum K potassium Kalium Si silicon Silicium Ag silver Argentum Na sodium Natrium Sn tin Stannum W tungsten Wolframium

  13. Numerical prefixes 1mono 11 undeca 2 di 12 dodeca 3 tri 13 trideca 4 tetra 5 penta 20 eicosa 6 hexa 100 hecta 7 hepta 8 octa 1/2 hemi 9 nona 3/2 sesqui 10 deca

  14. Names of oxides 1) Oxides of NONMETALS - numerical prefixes CO carbon monoxide CO2 carbon dioxide SO2 sulfur dioxide SO3 sulfur trioxide As2O3diarsenic trioxide As2O5diarsenic pentoxide

  15. Names of oxides 1) Oxides of METALS Only one oxid. state:CaO calcium oxide Al2O3 aluminum oxide More oxid. states: FeO iron (II) oxide Fe2O3 iron (III) oxide

  16. Names of oxides (INN) Genitive form of the name for the element + OXIDUM (numerical prefixes are employed) K2O Dikalii oxidum CaO Calcii oxidum Al2O3Dialuminii trioxidum SnO2 Stanni dioxidum Sb2O5Distibii pentaoxidum SO3 Sulfuris trioxidum ! ( sulfur, -is ) 3rd decl.

  17. Names of peroxides element + PEROXIDE H2O2 hydrogen peroxide Na2O2 sodium peroxide BaO2 barium peroxide

  18. Names of peroxides (INN) Genitive form of the name for the element + PEROXIDUM H2O2 Hydrogenii peroxidum Na2O2 Natrii peroxidum BaO2 Barii peroxidum

  19. Names of hydroxides element + HYDROXIDE ( if element forms more hydroxides – specify it ! ) NaOH sodium hydroxide Ca(OH)2 calcium hydroxide Mg(OH)2 magnesium hydroxide Fe(OH)2iron (II) hydroxide Fe(OH)3iron (III) hydroxide

  20. Names of hydroxides (INN) Genitive form of the name for element + HYDROXIDUM ( numerical prefix: if element forms more hydroxides ) NaOH Natrii hydroxidum Ca(OH)2 Calcii hydroxidum Mg(OH)2 Magnesii hydroxidum Fe(OH)2Ferri dihydroxidum Fe(OH)3Ferri trihydroxidum

  21. Names of acids 1. Acids not containing oxygen ("binary acids") HYDRO.... -IC ACID or HYDROGEN .... -IDE HF hydrofluoricacid HCl hydrochloricacid HBr hydrobromicacid HI hydroiodic acid H2S hydrogensulfide HCN hydrogencyanide

  22. 2. Oxyacids How many oxyacids can the element form ? a) only one.... -IC ACID H2CO3 carbonicacid H3BO3boricacid H2SiO3 silicicacid H2MoO4 molybdicacid !!!

  23. a) two Lower oxidation n. .... -OUS ACID Higher oxidation n. .... -IC ACID H2SO3 sulfurousacid H2SO4 sulfuricacid HNO2 nitrousacid HNO3 nitricacid H3PO3 phosphorousacid H3PO4 phosphoricacid

  24. a) more than two the halogens Cl, Br, I HClO hypochlorousacid HClO2 chlorousacid HClO3 chloricacid HClO4perchloricacid The same way: "traditional" H2MnO4 manganicacid HMnO4permanganicacid

  25. Names of acids (INN) 1. Acids not containing oxygen ("binary acids") ACIDUM HYDRO …… -ICUM HF Acidum hydrofluoricum HCl Acidum hydrochloricum HBr Acidum hydrobromicum HI Acidum hydroiodicum H2S Acidum hydrosulfuricum HCN Acidum hydrocyanicum

  26. 2. Oxyacids How many oxyacids can the element form ? a) only oneACIDUM ……-ICUM H2CO3 Acidum carbonicum H3BO3Acidumboricum H2SiO3 Acidum silicicum H2MoO4 Acidum molybdaenicum

  27. a) two Lower oxidation n.ACIDUM ……-OSUM Higher oxidation n.ACIDUM ……-ICUM H2SO3 Acidum sulfurosum H2SO4 Acidum sulfuricum HNO2 Acidum nitrosum HNO3 Acidum nitricum H3PO3 Acidum phosphorosum H3PO4 Acidum phosphoricum

  28. a) more than two the halogens Cl, Br, I HClO Acidum hypochlorosum HClO2 Acidum chlorosum HClO3 Acidum chloricum HClO4 Acidum hyperchloricum ( perchloricum ) The same way: "traditional" H2MnO4 Acidum manganicum HMnO4 Acidum hypermanganicum

  29. Names of salts 1. Salts of binary acids (acids not containing oxygen) cation + ……- IDE more oxidation states of cation: specify it ! e.g. iron (II) NaCl sodium chloride AgI silver iodide KCN potassium cyanide ZnS zinc sulfide

  30. Common elements with two oxidation states in cations FeIIiron (II)ferrousFeIIIiron (III)ferric CuIcopper (I)cuprousCuIIcopper (II) cupric HgImercury (I) mercurousHgIImercury (II) mercuric AuIgold (I)AuIIIgold (III) SnIItin (II)stannousSnIVtin (IV) stannic TlI thallium (I)TlIIIthallium (III) PbII lead (II)plumbousPbIVlead (IV) plumbic

  31. Salts of elements with more oxidation states FeCl2 iron (II) chloride FeCl3 iron (III) chloride CuI copper (I) iodide CuI2 copper (II) iodide Hg2Cl2 mercury (I) chloride HgCl2 mercury (II) chloride

  32. 2. Salts of oxyacids cation + … -ATE ( if acid -ic ) … - ITE ( if acid -ous ) according to acid also: HYPO- PER- Na2CO3 sodium carbonate K2SO3 potassium sulfite NaClO sodium hypochlorite FeSO4 iron (II) sulfate NH4BrO2 Ammonium bromite

  33. Names of salts (INN) 1. Salts of binary acids (acids not containing oxygen) genitive form of the cation + ……- IDUM more oxidation states of cation: lower: -osi higher -i NaCl Natrii chloridum AgI Argenti iodidum KCN Kalii cyanidum ZnS Zinci sulfuridum!!!

  34. Common elements with two oxidation states in cations FeIIFerrosi FeIII Ferri CuI Cuprosi CuII Cupri HgI Hydrargyrosi HgII Hydrargyri AuI Aurosi AuIII Auri SnIIStannosi SnIVStanni TlI Thallosi TlIII Thallii

  35. Salts of elements with more oxidation states FeCl2 Ferrosi chloridum FeCl3 Ferri chloridum CuI Cuprosi iodidum CuI2 Cupri iodidum Hg2Cl2 Hydrargyrosi chloridum HgCl2 Hydrargyri chloridum

  36. 2. Salts of oxyacids cation in genitive + … -AS ( if acid -icum ) ( -osi, -i ) … - IS ( if acid -osum ) according to acid also: HYPO- HYPER- Na2CO3 Natrii carbonas K2SO3 Kalii sulfis NaClO Natrii hypochloris FeSO4 Ferrosi sulfas NH4BrO2 Ammonii bromis

  37. Names of hydrogensalts HYDROGEN (numerical prefix if needed) NaHS sodium hydrogensulfide NaHCO3 sodium hydrogencarbonate KHSO3 potassium hydrogensulfite Na3PO4 sodium phosphate Na2HPO4 sodium hydrogenphosphate NaH2PO4 sodium dihydrogenphosphate

  38. Names of hydrogensalts (INN) prefix: HYDROGENO- (numerical prefix if needed) NaHS Natrii hydrogenosulfuridum NaHCO3 Natrii hydrogenocarbonas KHSO3 Kalii hydrogenosulfis Na3PO4 Natrii phosphas Na2HPO4 Natrii hydrogenophosphas NaH2PO4 Natrii dihydrogenophosphas

  39. Names of basic salts Mg(OH)Cl Magnesium chloride hydroxide Cd(OH)I Cadmium iodide hydroxide Al(OH)CO3 Aluminum carbonate hydroxide

  40. Names of basic salts (INN) prefix: SUB- Mg(OH)Cl Magnesii subchloridum Cd(OH)I Cadmii subiodidum Al(OH)CO3 Aluminii subcarbonas

  41. Names of hydrates ….. HYDRATE numerical prefix CuSO4 . 5 H2O copper (II) sulfate pentahydrate MgCl2 . 6 H2O magnesium chloride hexahydrate CaSO4 . 1/2 H2O calcium sulfate hemihydrate anhydrous: (Only if you want to point out this.) Na2CO3 sodium carbonate anhydrous

  42. Names of hydrates (INN) ….. HYDRICUS ( -UM) numerical prefix CuSO4 . 5 H2O Cupri sulfas pentahydricus MgCl2 . 6 H2O Magnesii chloridum hexahydricum CaSO4 . 1/2 H2O Calcii sulfas hemihydricus anhydrous: (Only if you want to point out this.) Na2CO3 Natrii carbonas anhydricus

  43. Names of polyacids and their salts (Number of central atoms is expressed by numerical prefix) H2B4O7tetraboric acid Na2B4O7 sodium tetraborate H2Cr2O7dichromic acid K2Cr2O7 potassium dichromate

  44. Names of polyacids and their salts (INN) (Number of central atoms is expressed by numerical prefix) H2B4O7 Acidum tetraboricum Na2B4O7 Natrii tetraboras H2Cr2O7 Acidum dichromicum K2Cr2O7 Kalii dichromas

  45. "Functional replacement" derivatives of oxyacids Peroxyacids -O-H group replaced by -O-O-H (HOO)NO2peroxynitric acid (HOO)2CO diperoxycarbonic acid Thioacids oxygen is replaced by sulfur ( -O-H replaced by -S-H ) =O replaced by =S H2S2O3thiosulfuric acid H2CS3trithiocarbonic acid

  46. "Functional replacement" derivatives of oxyacids (INN) Peroxyacids -O-H group replaced by -O-O-H (HOO)NO2 Acidum peroxonitricum (HOO)2CO Acidum diperoxocarbonicum Thioacids oxygen is replaced by sulfur ( -O-H replaced by -S-H ) =O replaced by =S H2S2O3 Acidum thiosulfuricum H2CS3 Acidum trithiocarbonicum

  47. Double salts (salts containing more than one cation or anion) AlK(SO4)2Aluminum potassium sulfate CaMg(CO3)2Calcium magnesium carbonate ZnBrF Zinc bromide fluoride Cu3(CO3)2F2Copper (II) carbonate fluoride

  48. Double salts (INN) (salts containing more than one cation or anion) AlK(SO4)2Aluminii kalii sulfas CaMg(CO3)2Calcii magnesii carbonas ZnBrF Zinci bromidum fluoridum Cu3(CO3)2F2Cupri carbonas fluoridum

More Related