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Chemical Nomenclature

Chemical Nomenclature . Written by Y. Deng, J. Bazzi and D. Bandyopadhyay Produced by the Science Learning Center (SLC) University of Michigan -Dearborn 2013. What is Chemical Nomenclature?. A set of rules to generate systematic names for chemical substances Language of c hemistry

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Chemical Nomenclature

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  1. Chemical Nomenclature Written by Y. Deng, J. Bazzi and D. Bandyopadhyay Produced by the Science Learning Center (SLC) University of Michigan -Dearborn 2013

  2. What is Chemical Nomenclature? Aset of rules to generate systematic names for chemical substances Language of chemistry Used by scientists, particularly chemists, to communicate and discuss the issues related to chemistry ?

  3. Purpose To introduce the systems of chemical nomenclature used to name inorganic compounds and to write chemical formulas of inorganic compounds.

  4. Inorganic vs. Organic Compounds Inorganic compounds are referred traditionally to those extracted from non-living things (e.g., rocks) and viewed as being synthesized by geological systems. Examples: calcium carbonate (a major compound found in rocks): CaCO3 Sodium chloride (a major compound found in table salt): NaCl Organic compounds, on the other hand, are referred traditionallyto those found in living things (e.g., plants and animals) and mainly contain carbon-hydrogen chain and ring structures. Examples: Ethanol (one of the fermentation products of grapes): CH3CH2OH Caffeine (one of the components found in coffee beans):

  5. Specific Objectives: • 2. Name inorganic compounds. Write correct chemical formulas for inorganic compounds. • 3. Determine the electric charges of ions involved in ionic compounds.

  6. Part I The Periodic table of elements and symbols of the elements

  7. The Periodic Table of the Elements is a tabular arrangement of the chemical elements, organized on the basis of their atomic numbers (i.e., the number of protons in their nuclei) and recurring chemical properties. • There are 118 elements currently listed on the periodic table. About 90 elements are found in nature. The remaining ones have been produced artificially using high energy particle accelerators.

  8. Eachelementhasitsnameandsymbol. The symbol can be up to three letters. The first letter must be capitalized and the second and third, if any, are ina lower case. Examples: Name Symbol Nitrogen N Chlorine Cl Unun­pentiumUup

  9. Thesymbolsoftheelementsarederivedfrom: • Englishnames • hydrogen – H • calcium– Ca • phosphorus – P • Latinnames • Ferrum (iron) – Fe • Aurum (gold) – Au

  10. Chemical SymbolsDerivedfromTheirEnglishNames

  11. Chemical SymbolsDerivedfromTheirLatinNames

  12. The main group elements that must be memorized, indicated ingreencolorfortheirsymbols and names

  13. The transition metal elements that must be memorized, indicated inredcoloroftheirsymbols and names

  14. Exercise 1 Write names or symbols of the following elements. • Ca 8 . tin • K 9. silicon • Co 10. gold • Mn 11. copper • Cr 12. carbon • Fe 13. neon • P 14. bromine

  15. Part II Naming Binary Ionic Compounds (Containing Two Different Elements)

  16. Naming Binary Ionic Compounds An ionic compoundis a chemical compound in which ions are held together bytheelectrostaticforcesbetweenoppositelychargedbodies. Usually, the positively charged portion consists of metal cations(e.g.,Na+)and the negatively charged portion consists of anions(e.g.,Cl-).

  17. Formation of An Ionic Compound e - Cl Na Cl- Na+ A sodium atom loses an electron to form a positive ion (cation): Na+. A chlorine atom gains an electron to form a negative ion (anion): Cl-. The cation and the anion are held together bytheelectrostaticforces (ionic bond) to form an ionic compound.

  18. RulesforNaming Binary Ionic Compounds For example: Chlorine (Cl) isthe name of the element. When a chlorine atom gains an electron, it becomes an anion, chloride(Cl-). NaCl Whennaming cations,the name of the element is used. When naming anions that are derived from an atom of the element,the name of the element is modified with the suffix –ide added. 3.Write thesymbolofthecation first,and thenthesymbolofthe anion.

  19. Formation of Magnesium Chloride Mg Cl e- e- Cl Write the formula with the positive & negative charges balanced. Cl- Cl- Mg2+ Mg 2+ +2Cl-MgCl2 A subscript “2” is used to indicate number of chloride ion present in a magnesium chloride compound.

  20. RulesforNaming Binary Ionic Compounds (Continued) 4. Compounds are electrically neutral, thus the total number of cations and anions must be such that positive and negative charges balance to zero. 5. The number of each ion present in the compound is designated by a subscript following its chemical symbols. For example, an aluminum oxide compound consists of 2 aluminum cation (Al3+) and 3 oxide anions (O2-). MgCl2 Al2O3

  21. A modified periodic table useful for writing formulas for binary ioniccompounds.The numbers in blue indicate the common charges of cations and anions after these atoms gain or lose electrons. Non-metals Metals

  22. Examples of Binary Ionic Compounds

  23. Some metals can form cations with different charges. These cations can be named using two systems: (a) Stock System: The charges of cations can be described by using Roman numerals. Ex.Ironcanformtwocations:Fe2+&Fe3+ FeCl2:iron(II)chloride FeCl3:iron(III)chloride (pronounce: iron-two chloride; iron-three chloride) • (b) Classical system: • Assignthe ending “ous” to the cationswith fewer positive charges and the ending “ic” to the cations with more positive charges • Ex.Ironcanformtwocations:Fe2+&Fe3+ • FeCl2:ferrouschloride • FeCl3:ferricchloride

  24. Naming of Cations Using the Classical and Stock Systems:

  25. Additional Examples ofBinaryIonic Compounds

  26. Exercise 2 Give the names or formulas of the following binary ionic compounds. If a compound can be named by both the Stock and the Classical systems, provide both names. 1. CaO2 8. aluminum chloride 2. NaH 9. calcium phosphide 3. Mg3N2 10. stannous oxide 4. FeI3 11. ferric bromide 5. CuCl12. ferrous bromide 6. CuCl2 13. barium nitride 7. Ba3P2 14. nickel(III) chloride

  27. Part III Naming Ionic Compounds Containing Polyatomic Ions

  28. Names of Some Oxo-Anions • An oxo-anion usually contains two elements in which one of them must be oxygen. Theoxo-anionsof some elements (in blue) can have eithera suffix -ate or -ite added to the root names of the elements. For example, SO42-andSO32- areoxo-anions of sulfur element. Their names are sulfate and sulfite, respectively.

  29. Names of Common Polyatomic Ions

  30. Names of Common Polyatomic Ions (cont.)

  31. Examples of Ionic Compounds with Polyatomic Ions

  32. Exercise 3 Give the names or formulas of the following ionic compounds with polyatomic ions. If a compound can be named by both the Stock and the Classical systems, provide both names. • 1. CaSO3 8. calcium phosphate • 2. NaHCO3 9. cuprous sulfite • 3.Hg2(NO3)210. ammonium nitrite • 4. Hg(NO2)211. ferrous dihydrogen phosphate • 5. Cu(CH3COO)212. barium cyanide • 6. Ba(SCN)213. potassium permanganate • 7. Na2Cr2O714. plumbous carbonate

  33. Part IV Naming Acids and Bases

  34. An acid is a substance that ionizes in water to produce hydrogen ions (H+). A base is a substance that ionizes in water to produce hydroxide ions (OH-). A. Acids without oxygen atoms The following compounds are named depending on whether they are present as pure substances or are dissolved in water to form aqueous solutions .

  35. B. Common oxo-anions and their corresponding oxo-acids.

  36. C. Common organic acids

  37. D. Bases

  38. Exercise 4 Give the names or formulas of the following acids and bases. If an acid or a base can be named by both the Stock and the Classical systems, provide both names. • 1. HF (aqueous solution)8. nitric acid • 2. H2SO39. aluminum hydroxide • 3. H2CO310. ferric hydroxide • 4. H2S (pure substance)11. cuprous hydroxide • 5. Hg2(OH)212. hydrocyanic acid • 6. Fe(OH)2 13. nitrous acid • 7. H3PO4 14. sulfuric acid

  39. Part V Naming Hydrates

  40. Hydrates–compounds that have a specific number of water molecules attached to them. Examples: • BaCl2·2H2O • CuSO4·5H2O • MgSO4·7 H2O

  41. The First Ten Greek Prefixes

  42. Examples of Hydrates and Their Names The Greek prefixes are used to indicate the number of water molecules in hydrates. • BaCl2·2H2O Name: barium chloride dihydrate (2) CuSO4·5H2O Name : copper(II) sulfate pentahydrate(Stock System) Orcupric sulfate pentahydrate(Classical System) (3)MgSO4·7 H2O Name: magnesium sulfate heptahydrate

  43. Exercise 5 Give the names or formulas for the following hydrates. If a hydrate can be named by both the Stock and the Classical systems, provide both names. • LiCl·H2O (6) barium chloride dihydrate • MgSO4·7H2O (7) sodium carbonate decahydrate • CoCl2·6H2O (8) ferrous sulfate hexahydrate • CuSO4·5H2O (9) strontium nitrate tetrahydrate • Na2SO4∙10H2O (10) manganese(II) nitrate tetrahydrate

  44. Part VI Naming Binary Molecular Compounds(containing Two elements, but don’t contain cations and anions)

  45. Rules for Naming Binary Molecular Compounds Examples of binary molecular compounds: CO2, CCl4 Whennaming the first element, the name of the element is used. Then name the second element by taking the first part of the element name and adding the suffix “ide”. Use Greek prefixes to denote the number of atoms of each element present. The prefix “mono” can be omitted for the first element. For oxides, the ending “a” in the prefix is sometimes omitted.

  46. Examples CO: carbon monoxide (not monocarbon monoxide) CO2: carbon dioxide SO3: sulfur trioxide N2O4: dinitrogen tetroxide (not tetraoxide) PCl5: phosphorus pentachloride S2F10: disulfurdecaflouride

  47. An exception to the use of Greek prefixes involves molecular compounds containing hydrogen Traditionally, many of these compounds are called either by their common names or by names that do not specifically indicate the number of H atoms present. Examples: CH4 - methane; NH3 – ammonia; PH3 – phosphine H2O- water; H2S – hydrogen sulfide; SiH4 -silane

  48. Exercise 6 Give the names or formulas for the following binary molecular compounds. NO 8. dinitrogen monoxide SO2 9. boron trichloride Cl2O7 10. diarsenicpentoxide PBr3 11. sulfur hexachloride SF6 12. nitrogen triiodide P2O5 13. carbon tetra bromide 7. CCl4 14. diphosphoruspentoxide

  49. Acknowledgements The authors would like to thank Ali Bazzi, Ogie Stewart and Ruixiao Zuo for their valuable comments and suggestions that were of great help in preparing and improving this module. The authors would like to thank Annette Sieg, Assistant Director of SLC, as well as the SLC staff for their help and technical support.

  50. Exercise 1 – Key Write names or symbols of the following elements • Ca calcium 8 . tin Sn • K potassium 9. silicon Si • Co cobalt 10. gold Au • Mnmanganese 11. copper Cu • Cr chromium 12. carbon C • Feiron 13. neon Ne • P phosphorus 14. bromine Br

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