Chapter 3§3.2 Ionic Bonds§3.2 Covalent Bonds§3.4 Compounds vs. Molecular Elements§3.5 Naming Compounds§3.5 Binary Ionic Compounds IMonoatomic Ion Names§3.5 Polyatomic IonsPowerPoint Presentation§3.5 Common Cations and Anions§3.5 Naming Binary Ionic CompoundsIron OxidesNaming Compounds§3.5 Binary Ionic CompoundsSlide 15§3.6 Binary Covalent Compounds§3.6 Prefixes for Covalent Compounds§3.6 Naming Covalent CompoundsIn Summary§3.6 Naming AcidsSlide 21Slide 23Naming OxidesNaming Ionic Compounds§3.7 Molar Mass§3.8 Mass Percent§3.8 Calculating Percent Composition§3.9 Formulas§3.9 Empirical vs. Molecular§3.9 Ionic Formulas§3.9 Determining Molecular Formula§3.9 Determining Molecular Formula I§3.9 Determining Molecular Formula II§3.9 Combustion AnalysisSlide 36Summary of Determining Molecular Formulas§3.10 Chemical Equations§3.10 Balancing Chemical EquationsSlide 40MOLECULES, COMPOUNDS AND CHEMICAL EQUATIONSChapter 3Skip section §3.11§3.2 Ionic BondsIonic bonds form due to electron transfer. The resulting ions are attracted by electrostatic forces.§3.2 Covalent BondsCovalent bonds form by sharing of electrons.§3.4 Compounds vs. Molecular ElementsAtomic elements (metals, noble gases) exist as single atoms.Molecular elements – the same element covalently bound to itselfoBr2, I2, N2, Cl2, H2, O2, F2 – diatomicoP4, S8, Se8Molecular compounds have ≥2 covalently bound nonmetals.Ionic compounds are composed of cations and anions.§3.5 Naming Compounds1. Binary Ionic Compounds (metal + nonmetal)The metal only forms 1 cation.2. Binary Ionic Compounds (metal + nonmetal)The metal forms ≥2 cations; requires a Roman numeral.3. Binary Covalent Compounds (nonmetal + nonmetal)§3.5 Binary Ionic Compounds I1. The cation is named first.2. The cation has the same name as its parent element.3. Name the anion as: (parent element root) + (–i de)Example: Ba3N2barium nitridenitrogen + ide = nitrideMonoatomic Ion Names§3.5 Polyatomic IonsLearn these.When naming, these metals don’t require a Roman numeral.§3.5 Common Cations and AnionsSc3+The metals shaded green only form one ion.§3.5 Naming Binary Ionic CompoundsMg3N2 SrCl2 LiH CaBr2 Aluminum bromide Magnesium sulfide Cesium oxide Magnesium nitrideStrontium chlorideLithium hydrideCalcium bromideAlBr3MgSCs2OIron OxidesFe2O3Fe3O4FeOA basic tenet of chemical nomenclature: every substance should have a unique name.Naming any of the following compounds “iron oxide” would be ambiguous:Naming Compounds§3.5 Binary Ionic CompoundsFor metals forming ≥2 cations (e.g., Fe2+, Fe3+) the charge must be stated with Roman numerals. Examples: SnF2SnO2Tin (II) fluorideTin (IV) oxide§3.5 Naming Binary Ionic CompoundsCuClHg2S MnPO4 CrO3 Mercury (II) sulfate Cobalt (II) bromide Lead (IV) nitrate Vanadium (V) hydroxide Copper (I) chlorideMercury (I) sulfideManganese (III) phosphateChromium (VI) oxideHgSO4CoBr2Pb(NO3)4V(OH)5§3.6 Binary Covalent CompoundsSame rules as before, but:1. Use prefixes to indicate the number of each atom.2. The prefix mono- is never used for naming the first element.Examples: B2O3CODiboron trioxideCarbon monoxide§3.6 Prefixes for Covalent Compounds§3.6 Naming Covalent CompoundsICl7CCl4BrCl XeF6 Boron tribromide Dichlorine monoxide Disulfur tetrafluoride Diphosphorus pentasulfide Iodine heptachlorideCarbon tetrachlorideBromine monochlorideXenon hexafluorideBBr3Cl2OS2F4P2S5In Summary§3.6 Naming AcidsAcids are substances that ionize in water to produce H+ ions (protons):HA (aq) → H+(aq) + A- (aq)Acids are named one of two different ways, depending on whether or not the anion (A-) contains oxygen.§3.6 Naming AcidsHBrphosphorous acidH3PO3hydrobromic acidphosphoric acidH3PO4§3.6 Naming AcidsH2CO3HC2H3O2 HF HCNH2C2O4Carbonic acidAcetic acidHydrofluoric acidHydrocyanic acidOxalic acidNaming OxidesP4O10 + 6H2O → 4H3PO4 S(s) + O2(g) → SO2(g) + H2O → H2SO3 Tetraphosphorus decaoxidePhosphoric acidsulfur dioxidesulfur trioxidesulfurous acid2S(s) + 3O2(g) → 2SO3(g) + 2H2O → 2H2SO4 sulfuric acidNaming Ionic Compounds2NaClO3(s) + H2SO4(l) → Na2SO4(s) + 2HClO3(l2KI + MnO2 + 3H2SO4 → I2 + MnSO4 + 2KHSO4 + 2H2O sodiumchloratesodiumsulfatesulfuricacidchloricacidmanganese (IV) oxidemanganese(II) sulfatepotassiumhydrogensulfateor bisulfate§3.7 Molar MassThe molar mass of a substance is the mass of one mole of the compound. Units are g/mol.A compound's molar mass is the sum of the atomic masses of its atoms. 2(1.00794) + 15.9994 = 18.0153 g/mol§3.8 Mass PercentWe can describe the composition of a compound in one of two ways: Molecular formula: the number of each atom it contains per molecule.Mass Percent: the percentage by mass (mass %) of it elements.mass % = mass of element in 1 mol cmpd (100%) molar mass of cmpd§3.8 Calculating Percent CompositionGold (III) chloride was once used to tint glass a deep red color. What is the percent composition of gold and chlorine in AuCl3? 1 gold atom: 1 x 197.0 g = 197.0 g3 chlorine atoms: 3 x 35.45 g = 106.35 g molar mass of AuCl3= 303.35 gMass % Au = 197.0 g Au (100%) = 64.94% Au 303.35 g AuCl3Mass % Cl = 106.35 g Cl (100%) = 35.06% Cl 303.35 g AuCl3§3.9 FormulasEmpirical Formula (EF) – the simplest formula with the correct ratio of atomsMolecular Formula (MF) – the formula with the actual number of atoms in the molecule. MFs are integer multiples of EFs:(E.F.)n = M.F. (n = 1, 2, 3...)§3.9 Empirical vs. Molecularstructure H-O-O-HCaF2namebenzenehydrogen peroxidesodium chloridemolecular formulaC6H6H2O2NaClempirical formulaCH HO NaClCCCCCCHHHHHH§3.9 Ionic FormulasNaF CaF2All ionic formulas are empirical formulas.To determine molecular formula from percent composition, the molar mass must be known.Two methods:1. Method I. The empirical formula is calculated followed by n where:n = (molar mass)/(molar mass of empirical formula)(E.F.)n = M.F. (n = 1, 2, 3...)2. Method II. Provides the molecular formula directly.§3.9 Determining Molecular FormulaC6.5H9O × 2 = C13H18O2§3.9 Determining Molecular Formula IThe pain reliever ibuprofen has the following mass percent composition: C