10/23/09 Naming Compounds Day 2

Working backwards: name to formula 10/23/09 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

Write and name the following covalent compounds (IUPAC)‏ 10/23/09 Write and name the following covalent compounds (IUPAC)‏ lithium sulfide dinitrogen monoxide lead(IV) sulfate Li1S2  Li2S N2O Pb4(SO4)2  Pb2(SO4)4  Pb(SO4)2

Assignment 10/23/09 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 Give the valence of a) Fe in FeO, b) Mn in MnO2 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) magnesium nitride, k) aluminum hypochlorite, l) iodine pentafluoride, m) calcium chromate, n) diphosphorus pentasulfide

Complete exercises on handout 10/23/09 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

Answers – 1, 2 zinc sulfide iron(III) chloride calcium carbonate 10/23/09 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

Answers – 3 Na2O KI PbS2 Hg2O FeO Fe3(PO4)2 CuF2 Cl2O Ag2S Mg3N2 10/23/09 Na2O KI PbS2 Hg2O FeO Fe3(PO4)2 CuF2 Cl2O Ag2S Mg3N2 Al(ClO)3 IF5 CaCrO4 P2S5

Naming Bases Bases contain an OH group 10/23/09 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

Naming Acids: Binary acids 10/23/09 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

Naming Acids: Oxyacids 10/23/09 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

Naming Acids: Oxyacids 10/23/09 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

Assignment: give formula or name 10/23/09 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)‏ 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

For more lessons, visit www.chalkbored.com Hydrates 10/23/09 For more lessons, visit www.chalkbored.com 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