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Naming Compounds

Naming Compounds. Day 2. Working backwards: name to formula. It’s possible to determine a formula from a name E.g. What is the formula of sodium oxide? To get the answer, first write the valences: Na 1 O 2  Na 2 O What is the formula of copper(II) oxide? Cu 2 O 2  Cu 2 O 2  CuO

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Naming Compounds

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  1. Naming Compounds Day 2

  2. Working backwards: name to formula • It’spossibletodetermineaformulafromaname • E.g. What is the formula of sodium oxide? • To get the answer, first write the valences: Na1O2 Na2O • What is the formula of copper(II) oxide? Cu2O2 Cu2O2 CuO • For covalent compounds, simply use the prefixes to tell you the number of each element: • What is the formula for dinitrogen trioxide? N2O3 • Give formulae for: lithium sulfide, dinitrogen monoxide, lead(IV) sulfate

  3. Write and name the following covalent compounds (IUPAC) Li1S2 Li2S N2O Pb4(SO4)2 Pb2(SO4)4  Pb(SO4)2 lithium sulfide dinitrogen monoxide lead(IV) sulfate

  4. Assignment • 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

  5. Complete exercises on handout • Steps: • Determine if its ionic or covalent • If ionic, determine if its metal has one or more valence • Name according to appropriate rules

  6. 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

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

  8. 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) • Bases are named like other ionic compounds: • +veisnamedfirst,followedbythepolyatomicion - calcium hydroxide - copper(I) hydroxide - Al(OH)3 - NH4OH Ca(OH)2 CuOH aluminum hydroxide ammonium hydroxide

  9. Naming Acids: Binary acids • All acids start with H (e.g. HCl, H2SO4) • 2 acids types exist: binary acids and oxyacids Binary: H + non-metal. E.g. HCl Oxy: H + polyatomic ion. E.g. H2SO4 • Each have different naming rules. Binary acids: naming depends on state of acid • If it’s not aqueous: hydrogen + non-metal HCl(g) = hydrogen chloride • If it is aqueous: hydro + non-metal + ic acid HCl(aq) = hydrochloric acid (aqueous hydrogen chloride) HBr(s) HI(aq) H2S(aq) H2S(g) hydrogen bromide hydr(o)iodic acid hydrosulfuric acid hydrogen sulfide

  10. Naming Acids: Oxyacids • Naming does not depend on the state (aq) • 1) name the polyatomic ion 2) replace ate with ic, ite with ous 3) change non-metal root for pronunciation 4) add “acid” to the name E.g. H2SO3 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid HNO2 hypochlorous acid H3PO4(aq) carbonic acid

  11. Naming Acids: Oxyacids • Naming does not depend on the state (aq) • 1) name the polyatomic ion 2) replace ate with ic, ite with ous 3) change non-metal root for pronunciation 4) add “acid” to the name E.g. H2SO3 1) sulphite, 2) sulphous, 3) sulphurous, 4) sulphurous acid HNO2 hypochlorous acid H3PO4(aq) carbonic acid - nitrous acid - HClO - phosphoric acid - H2CO3

  12. Assignment: give formula or name a) HClO3 b) H2S(aq) c) HBr(aq) d) H3PO3 e) HIO3 f) hydrogen chloride g) hydrochloric acid h) sulfuric acid i) sulfuric acid j) chlorous acid k) hydrofluoric acid a) chloric acid b) hydrosulfuric acid c) hydrobromic acid d) phosphorous acid e) iodic acid f) HCl(g) g) HCl(aq) h) H2SO4(s) i) H2SO4(aq) j) HClO2 k) HF(aq)

  13. For more lessons, visit www.chalkbored.com 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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