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Naming Compounds

Naming Compounds. Day 2. Lesson Review. Name each according to IUPAC rules: a) ZnS, b) FeCl 3 , c) CaCO 3 , d) P 2 O 5 , e) NaCN, f) N 2 F 2 , g) MgHPO 4 , h) Cu(BrO 3 ) 2 , i) K 2 O, j) BF 3 Give the valence of a) Fe in FeO, b) Mn in MnO 2

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Naming Compounds

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  1. Naming Compounds Day 2

  2. Lesson Review • Name each according to IUPAC rules: a) ZnS, b) FeCl3, c) CaCO3, d) P2O5, e) NaCN, f) N2F2, g) MgHPO4, h) Cu(BrO3)2, i) K2O, j) BF3 • Givethevalenceofa)FeinFeO,b)MninMnO2 • 3. Write formulas for: a) sodium oxide, b) potassium iodide, c) plumbic sulfide, d) mercury(I) oxide, e) ferrous oxide, f) iron(II) phosphate, g) copper(II) fluoride, h) dichlorine monoxide, i) silver sulfide, j)magnesiumnitride, k)aluminumhypochlorite, l) iodine pentafluoride, m) calcium chromate, n) diphosphorus pentasulfide

  3. Answers – 1, 2 • zinc sulfide • iron(III) chloride • calcium carbonate • diphosporus pentoxide • sodium cyanide • dinitrogen difluoride • magnesium hydrogen phosphate • copper(II) bromate • potassium oxide • boron trifluoride 2 a) 2 b) 4

  4. Answers – 3 • Cl2O • Ag2S • Mg3N2 • Al(ClO)3 • IF5 • CaCrO4 • P2S5 • Na2O • KI • PbS2 • Hg2O • FeO • Fe3(PO4)2 • CuF2

  5. Properties of Acids • All acids start with H (e.g. HCl, H2SO4) • 2 acid types exist: binary acids and oxyacids • Each have different naming rules.

  6. Naming Acids Binary Acids: • Contain “H” and one other element • Depends on the state of the acid To Name non-aqueous (solid or gas): Hydrogen “nonmetal” – change the ending to -ide To Name aqueous: (prefix) hydro- “nonmetal name” (suffix) –icacid HCl (g)hydrogen chloride H2S (g)hydrogen sulfide HCl (aq)hydrochloric acid H2S (aq)hydrosulfuric acid

  7. HBr(s) HI(aq) H2S(aq) H2S(g) hydrogen bromide hydr(o)iodic acid hydrosulfuric acid hydrogen sulfide

  8. Naming Oxyacids • Contain “H”, “O” and one more element • Naming does not depend on the state (aq) Steps 1) name the polyatomic ion 2) replace -ate with ic, -ite with ous 3) change non-metal root for easier pronunciation 4) add “acid” to the name E.g. H2SO3 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid

  9. nitricacid nitrousacid phosphoricacid phosphorousacid HNO3 HNO2 H3PO4 H3PO3 H2SO4 H2SO3 sulfuricacid sulfurousacid HClO4 HClO3 HClO2 HClO perchloricacid chloricacid chlorousacid hypochlorousacid

  10. Naming Bases • Bases contain an OH group • C6H12O6 does not have an OH group • If an OH group is present it will be clearly indicated: e.g. NaOH, Ca(OH)2 • Also notice that bases have a metal (or positive ion such as NH4+ at their beginning) To name: “metal” + “hydroxide” Ex: NaOH = Sodium Hydroxide KOH = Potassium Hydroxide

  11. Ca(OH)2 CuOH aluminum hydroxide ammonium hydroxide - calcium hydroxide - copper(I) hydroxide - Al(OH)3 - NH4OH

  12. Practicing Naming Acids & Bases

  13. Practicing Naming Acids & Bases

  14. Hydrates • Some compounds contain H2O in their struc-ture. These compounds are called hydrates. • This is different from (aq) because the H2O is part of the molecule (not just surrounding it). • The H2O can usually be removed if heated. • A dot separates water: e.g. CuSO4•5H2O is copper(II) sulfate pentahydrate. • A greek prefix indicates the # of H2O groups. sodium sulfate decahydrate nickel(II) sulfate hexahydrate Na2CO3•H2O BaCl2•2H2O Na2SO4•10H2O NiSO4•6H2O sodium carbonate monohydrate barium chloride dihydrate

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