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Mastering the Nomenclature of Binary and Polyatomic Compounds

This chapter focuses on mastering the steps for naming binary compounds involving metals and nonmetals, as well as polyatomic ions. It explains the differences between Type I and Type II binary ionic compounds and provides detailed rules for naming them, including the use of Roman numerals for cations. The section on Type III compounds introduces the use of prefixes when naming binary compounds containing only nonmetals. Additionally, the chapter covers naming polyatomic ions and acids based on anion composition, aiding in the proper naming of various chemical compounds.

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Mastering the Nomenclature of Binary and Polyatomic Compounds

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  1. Chapter 4 Nomenclature

  2. Naming Compounds • Section 4.1 – Binary Ionic Compounds • Objective: • To master the steps of naming binary compounds of a metal and a nonmetal.

  3. Terms: • Binary Ionic compound – contain a positive cation (written 1st) and a negative anion. • To name these compounds simply name the ions. Type I compounds – forms only one type of cation Type II compounds – can form two or more cations that have different charges.

  4. Table 4.1

  5. Rules for Type I • Cation is always 1st, anion 2nd. • Cation takes its name from the element. • Anion takes the root of the element name and adds “ide” to the end • Ex.: NaCl is Sodium Chloride

  6. Practice • Name the following: • CsF • AlCl3 • MgI2 • MgO • KI • CaS

  7. Practice • Name the following: • CsF – Cesium fluoride • AlCl3 –Aluminum chloride • MgI2 – Magnesium iodide • MgO – Magnesium oxide • KI – Potassium iodide • CaS – Calcium sulfide

  8. Type II Compounds • Many metals can form more than one type of ion. • Pb can be 2+ or 4+ in compounds. • Type II are almost always transition metals. • Chemists use Roman numerals to specify the charge of the ion. • FeCl2 – what is the charge of Fe?

  9. FeCl2 • Fe can be 2+ or 3+ • The charge of the compound must =0. • Find the charge of Cl (-1). Two Cl ions are present for a charge of 2-. • For the compound to =0, Fe must be 2+. • Compound is Iron (II) chloride.

  10. Table 4.2

  11. Practice • Name the following: • CuCl • Fe2O3 • CoCl3 • CuI • HgCl2 • PbS

  12. Practice • Name the following: • CuCl – Copper(I) chloride • Fe2O3 –Iron (III) oxide • CoCl3 – Cobalt(III) chloride • CuI – Copper(I) iodide • HgCl2 – Mercury(II) chloride • PbS – Lead(II) sulfide

  13. Figure 4.1: A flow chart for naming binary compounds.

  14. Type III Compounds • Section 4.2 • Objective: • To master naming binary compounds containing only nonmetals.

  15. Prefixes • Mono – 1 • Di- 2 • Tri -3 • Tetra – 4 • Penta – 5 • Hexa – 6 • Hepta – 7 • Octa - 8

  16. Rules for Naming • The 1st element uses its full name. • The 2nd element is named as if it is an anion. • Prefixes are used to denote the number of atoms present. • Mono is never used to name the 1st element.

  17. Practice • BF3 • NO • N2O5 • CO2 • NO2 • CCl4

  18. Practice • BF3 – Boron trifluoride • NO – Nitrogen monoxide • N2O5 –Dinitrogen pentoxide • CO2 - Carbon dioxide • NO2 – Nitrogen dioxide • CCl4 – Carbon tetrachloride

  19. Naming Compounds containing Polyatomic Ions • Section 4.4 • Objective: To master naming of common polyatomic ions and how to use them in naming compounds.

  20. Figure 4.2: Overall strategy for naming chemical compounds.

  21. Terms: • Polyatomic ions – several atoms bound together with an overall charge. • Treated as a single entity.

  22. Table 4.4

  23. -ite, –ate, hypo- and per- in oxyanions • When there are 2 members in a series the one with the smaller number of atoms ends in –ite, and the one with the larger number of atoms ends in –ate. • SO32- (sulfite) and SO42- (sulfate) • Hypo- (less than), per- (more than) • Hypochlorite (ClO-) and perchlorate (ClO4-)

  24. Naming Polyatomic ions • Naming is similar to binary compounds • Must identify the ions –memorize the common ones! • Roman numerals are also used if a metal with more than one type of charge is present.

  25. Practice • Na2SO4 • KH2PO4 • Fe(NO3)3 • Mn(OH)2 • Na2SO3

  26. Practice • Na2SO4 – Sodium sulfate • KH2PO4 – Potassium dihydrogen phosphate • Fe(NO3)3 –Iron(III) nitrate • Mn(OH)2 – Manganese(II) hydroxide • Na2SO3 – Sodium sulfite

  27. Naming Acids • Section 4.5 • Objectives: • To identify how anion composition determines the acid’s name. • To identify common acids.

  28. Terms: • Acids – when dissolved in water produce H+ ions, have a sour taste. • Is a molecule with one or more H+ ions attached to an anion. • Naming depends on whether the anion contains oxygen.

  29. Rules for Naming Acids • If the anion doesn’t contain Oxygen use the prefix hydro-and suffix –ic on the root name. • HCl – hydrochloric acid

  30. With Oxygen • If the anion ends in –ate, the suffix –ic is used. • H2SO4 – sulfuric acid • IF the anion ends in –ite, the suffix –ous is used. • H2SO3 – sulfurous acid

  31. Practice • HF • H3PO3 • HNO3

  32. Practice • HF – Hydrofluoric acid • H3PO3 – Phosphorous acid • HNO3 – Nitric acid

  33. Writing Formulas from Names • Section 4.6 • Objective: • To master writing the formula for a compound from its name.

  34. Writing Formulas from Names

  35. Writing Formulas from Names

  36. Quiz Yourself • Click here to take a practice test for naming.

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