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Chapter 5: Nomenclature

Chapter 5: Nomenclature. Nomenclature. Rules of writing chemical formulas and naming compounds. Binary Compounds. Composed of two elements (Ex) NaCl ; H 2 O 2) Names always ending with “ ide ” 3) Two kinds a) ionic: metal + nonmetal element (the building block called “formula unit”)

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Chapter 5: Nomenclature

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  1. Chapter 5: Nomenclature

  2. Nomenclature Rules of writing chemical formulas and naming compounds

  3. Binary Compounds • Composed of two elements (Ex) NaCl; H2O 2) Names always ending with “ide” 3) Two kinds a) ionic: metal + nonmetal element (the building block called “formula unit”) (1) Type I: metal from A-group (= representative groups) (Ex) BaF2 (2) Type II: metal from B-group (= transition metal) (Ex) AgCl b) covalent compounds: 2 nonmetal elements (the building block called “molecule”) (Ex) CO2

  4. Polyatomic Compounds • Composed of 3 or more elements (Ex) H2SO4, NaNO3 • Names of most polyatomic anions end with “ate” or “ite” ** Exception: OH‒ (hydroxide); CN‒ (cyanide) • Ionic component + covalent component • Ionic component: Type I and Type II • Type I = A-group • Type II = B-group (Ex) NaNO3 = Na+ + CO3― (Ex) Fe(NO3)2 = Fe2+ + 2 NO3‒ • Must memorize common polyatomic ions (Table 5.4). • Notice when the name ends with “ate” or “ite”

  5. Binary Ionic or Polyatomic Compounds • Metal + nonmetal • The total charge of cations and anions = 0 • Group 1 = 1+ • Group 2 = 2+ • Group 3 metals = 3+ • Group 15 nonmetals = 3- • Group 16 nonmetals = 2- • Group 17 nonmetals = 1- • Subscripts are used to get the total charge of 0 (Ex) Na+ + O2‒ ? • Coefficient tells how many molecules (Ex) CO2 = 1 molecule 2 CO2= 2 molecules

  6. Naming Compounds • Binary ionicwith A-group metal and with B-group metal • Binary covalent • Polyatomic with A-group metal and with B-group metal • Binary acids • Oxyacids

  7. Naming Binary Ionic Compounds A) A-group metal + nonmetal = Type I 1. Name the metal element 2. Name the nonmetal element with “ide” ending • oxygen  oxide • nitrogen  nitride • hydrogen  hydride • fluorine  fluoride • iodine  iodide • phosphorus  phosphide (Ex) Al2O3 = aluminum oxide

  8. B) B-group metal + nonmetal = Type II 1. Name the metal element. 2. Write the charge of a metal ion in Roman numeral (I, II, III, IV, V, VI, VII, VIII, IX, X) ** Determine the charge from the anions 3. Name the nonmetal with “ide” ending (Ex) NiF2 nickel (II) fluoride Cr2O7 chromium (VII) oxide **Exceptions: Zn is always +2 (no need to use a Roman numeral) Pb, Sn are not B-group elements but treat them like they are and need a Roman numeral. (Ex) ZnCl2 zinc chloride, not zinc(II) chloride PbO: lead (II) oxide, not lad oxide

  9. Naming Binary covalent compounds Read the subscript of the first element with a Greek prefix (di, tri, tetra penta, hexa, hepta, octa, nona, deca) ** Notice that mono is NOT included 2) Read the name of the first element 3) Read the subscript of the second element with a Greek prefix, including mono 4) Read the name of the second element with “ide” ending (Ex) CO = carbon monoxide CO2 = carbon dioxide PH4 = phosphorus tetrahydride

  10. Naming Polyatomic Compounds A) A-group metal • Name the metal ion (NH4+ the only nonmetallic cation= ammonium) • Name the polyatomic anion (Ex) Ba(NO3)2 = barium nitrate B) B-group metal • Name the metal ion • Write the charge of the metal ion with a Roman numeral *Figure out the charge from the anion 3) Name the polyatomic anion (Ex) Fe2(CO3)3 = iron (III) carbonate

  11. Acids Contains H element (Arrhenius Definition of Acid) Always aqueous solutions (Ex) HCl (g) vs. HCl (aq) Contain no oxygen (= binary acids) or contain oxygen (= oxyacids)

  12. Naming Binary Acids Start with “hydro” for hydrogen End with “ic acid” (Ex) HCl (aq): hydrochloric acid H2S (aq): hydrosulfuric acid

  13. Oxyacids • Contain two or more elements + oxygen • Naming oxyacids relies on the names of polyatomic anions • If the polyatomic anion’s name ends with “ate”, the acid’s name ends with “ic acid” • If the anion’s name ends with “ite”, then the acid’s name ends with “ous acid” (Ex) H2SO4 (aq): sulfuric acid (SO42‒= sulfate) H2SO3 (aq): sulfurous acid (SO32‒= sulfite)

  14. Practice: Write the formula • Sodium hydroxide • Potassium carbonate 3) Sulfuric acid 4) Dinitrogenpentoxide 5) Cobalt(III) nitrate

  15. Practice: Name the compounds • KNO3 • TiO2 • Sn(OH)4 • PBr5 • H2SO3 (aq)

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