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Chapter 4

Chapter 4. Nomenclature. Naming Compounds. Section 4.1 – Binary Ionic Compounds Objective: To master the steps of naming binary compounds of a metal and a nonmetal. Terms:. Binary Ionic compound – contain a positive cation (written 1 st ) and a negative anion.

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Chapter 4

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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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