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Nomenclature

Nomenclature. We can determine the formula of a compound by completing Lewis diagrams or via the criss cross method By knowing the valence of elements you can determine the formula of compounds E.g. what compound would form from Ca + S? Step 1 - write valences: Ca 2+ S 2-

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Nomenclature

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  1. Nomenclature

  2. We can determine the formula of a compound by completing Lewis diagrams or via the criss cross method • By knowing the valence of elements you can determine the formula of compounds • E.g. what compound would form from Ca + S? Step 1 - write valences: Ca2+S2- Step 2 - cross down valences: Ca2S2 Step 3 – reduce: CaS a) Al,Br b) K,S c) Zn,O d) Mg,N e) C,Cl f) Cu,O AlBr3 K2S ZnO Mg3N2 CCl4 CuO or Cu2O

  3. Ionic compounds Rules for naming • Names end in -ide. Example: sodium chloride • Metal (cation) comes 1st (not chlorine sodide) • Do not capitalize (unless it’s the start of a sentence) Give formulae & name: Ca + I, O + Mg, Na + S = Ca2I1 = CaI2 = calcium iodide = Mg2O2 = MgO = magnesium oxide = Na1S2 = Na2S = sodium sulfide

  4. Multiple valence: Latin naming • When the metal in an ionic compound is multivalent there are 2 methods: Latin (Common Name) or IUPAC (Stock Method) • As before, the name ends in -ide & metal is first • The metal is named with it’s Latin or English root and ends in -ic or –ous to denote valence. • E.g. Cu1 is cuprous, E.g. Cu2 is cupric • Lower = ous, Higher = ic • Give formulas and Latin names for: Cu2+ + Cl- = CuCl2 = cupric chloride = copper (II) chloride (IUPAC) Cu+ + Cl = CuCl = cuprous chloride = copper (I) chloride

  5. Multiple valence: IUPAC naming • Name ends in -ide, positive/metal comes first • The valence of the metal is indicated in brackets using roman numerals • E.g. Cu1 is copper(I), Cu2 is copper(II) • Numbers refer to valences not to #s of atoms • Try: • Cu2+Cl, Zn2 + Cl, Co2+Cl, Hg+S (do both) Cu2+Cl = Cu2Cl1 = CuCl2 = copper(II) chloride Zn2+Cl = Zn2Cl1 = ZnCl2 = zinc chloride Co2+Cl = Co2Cl1 = CoCl2 = cobalt(II) chloride Hg+S = Hg1S2 = Hg2S = mercury(I) sulfide Hg+S = Hg2S2 = HgS = mercury(II) sulfide

  6. So far we have given valences to single atoms • Li + O Compounds containing polyatomic ions Li1O2 Li2O • Groups of atoms can also have valences • “Polyatomic ions” are groups of atoms that interact as a single unit. • E.g. OH1, (SO4)2. Ba3(PO4)2 = barium phosphate • Naming compounds with polyatomic ions is similar to naming other ionic compounds • You should note that compounds with polyatomic ions have names ending in -ate or -ite not -ide • Note that most are negative, except ammonium • Name: Ca(OH)2, CuSO4, NH4NO3, Co2(CO3)3

  7. Compounds containing polyatomic ions Ca(OH)2 CuSO4 NH4NO3 Co2(CO3)3 - calcium hydroxide - copper(II) sulfate - ammonium nitrate - cobalt(III) carbonate

  8. Naming covalent compounds • prefixrefersto#ofatoms-notvalence • N2O4 = dinitrogen tetroxide • Exception:dropmonoforfirstelement • CO2 = carbon dioxide • The first vowel is often dropped to avoid the combination of “ao” or “oo”. • CO=carbonmonoxide(monooxide) • -ide ending, each element has “prefix” P4O10= tetraphosphorusdecoxide SO2= sulfur dioxide (dioxide) • Name: CCl4, P2O3,IF7

  9. Write and name the following covalent compounds (IUPAC) carbon tetrachloride diphosporus trioxide iodine heptafluoride CCl4 P2O3 IF7

  10. 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: 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

  11. 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

  12. 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 • Givethevalenceof • a)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) diphosphoruspentasulfide

  13. 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

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

  15. 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: • +ve is named first, followed by the polyatomic ion - calcium hydroxide - copper(I) hydroxide - Al(OH)3 - NH4OH Ca(OH)2 CuOH aluminum hydroxide ammonium hydroxide

  16. 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 hydroiodic acid hydrosulfuric acid hydrogen sulfide

  17. 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

  18. Naming Acids: Oxyacids HNO2 hypochlorous acid H3PO4(aq) carbonic acid - nitrous acid - HClO - phosphoric acid - H2CO3

  19. 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)

  20. Hydrates • Some compounds contain H2O in their structure. 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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