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WOU ES 105 - Types of Reactions

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Chemistry ReviewTwo Types of ReactionsAcid-Base ReactionsHydronium IonDissolving HCl makes acidDissolving NH3 makes baseMeasuring Acid StrengthAcid Base ReactionsOxidation-Reduction ReactionsBatteriesElectric CircuitElectrolysisAluminum from electrolysisCorrosionRust reduces strengthCorrosionZinc sacrifice metalCombustion ReactionsMethane CombustionPeriodic TableGroups or FamiliesIons of Element GroupsCovalent BondsPolar Covalent BondsPolar Covalent BondsCompoundsChemical EquationsFormula Mass/Molar MassMolar mass of propane C3H8Grams calculated from MolesMass to moles relationshipProportionsProblemProblemProblem: 192 g O2→ ? g SO2ProblemChemistry ReviewChapter 18 Review QuestionsWill be EXTRA CREDITTwo Types of Reactions• Acid-Base reactions• Oxidation-Reduction reactionsAcid-Base Reactions• Transfer of hydrogen ions—protons• Makes water into H3O+and OH¯• Hydronium and HydroxideHydronium IonDissolving HCl makes acidDissolving NH3 makes baseMeasuring Acid Strength• Measure of acidity is pH– Concentration of H3O+in powers of 10– Negative of that power is the pH– pH of pure water is 7– Acids 0 to 7, bases 7 to 14• Use electric current to determine pHAcid Base Reactions• Neutralize one another• Acid + Base → Water + Salt• Generic term salt is the ionic product of an acid-base reactionCaCO3+ 2HCl →CO2+ H2O + CaCl2Oxidation-Reduction Reactions• Transfer of electrons• Often bonding with oxygen• Identifying the components of reaction—look for the transfer of electrons– Loss of Electrons—Oxidation (LEO)– Gain of Electrons—Reduction (GER)– (LEO the lion goes GER) =)Batteries• Batteries function because of an oxidation-reduction reaction– Anode—source of electrons– Cathode—destination of electrons• Need to have a way for electrons to get back to their source– Complete the circuit– Salt bridge or other deviceElectric CircuitElectrolysis• Electroplating is a useful Oxidation-Reduction Reaction– Ancient weak-acid electric circuits probably were utilized for this• Electrolysis breaks covalent bonds– Aluminum oxide ore– Water can be source of hydrogen and oxygen, • For use in a fuel cell• Combining the two becomes source of electricityAluminum from electrolysisCorrosion• An oxidation-reduction reaction• Metals combine with oxygen– the oxide product has different properties• Weaker• Greater volumeRust reduces strengthCorrosion• An oxidation-reduction reaction• Metals combine with oxygen– Some metals coated or connected by electric circuit with others as a ‘sacrifice’ metal to protect strength of another• Zinc oxidizes more readily than iron• Attached to steel ship keels and rudders• Zinc galvanized nailsZinc sacrifice metalCombustion Reactions• Combustion is an oxidation-reduction reactionCH4+ 2 O2→ CO2+ 2 H2O– Methane: C and H are oxidized– Oxygen is reducedMethane CombustionPeriodic TableGroups or Families• Alkali Metals• Alkaline Earth Metals• Transition Metals• Oxygen Group (chalcogens)• Halogens• Noble GasesIons of Element Groups• Alkali Metals + 1• Alkaline Earth Metals + 2• Transition Metals +, number variable• Oxygen Group - 2• Halogens - 1• Noble Gases no ions formed (usually)Ionic bonds form ionic compoundsNeed even ratio of charges in the compoundsCovalent Bonds• When the two atoms are the same, electrons within covalent bond shared evenly.• Nonpolar• They may be shared unevenly, however, when the bonded atoms are different.• Forms a dipole—has uneven chargePolar Covalent Bonds• Greater electronegativity means greater “pulling power” on the electrons• Greater difference of electronegativity: stronger dipole formed in bondHighLowPolar Covalent BondsCompounds• More than one type of atom in the molecule• Has a Chemical Formula• Sodium Chloride NaCl• Ammonia NH3• Subscript tells how many of each• (Subscript 1 is omitted)Chemical Equations•C+O2 ÆCO2•C(s) +O2 (g) ÆCO2 (g)• Reactants on left, products on right• Each are balanced because same number of atoms of reactants as products• Letter subscript refers to the phase of the substanceFormula Mass/Molar Mass• Mole: A super-large number, 6.02 × 1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number.The formula mass of a substance expressed in grams contains one mole.Substance Formula MassCarbon, C 12Oxygen, O232Carbon dioxide, CO244Sucrose, C12H22O11342Molar mass of propane C3H8• assume molar mass of C = 12 g/mole– 3 C x 12 g/mole = 36 g/mole• assume molar mass of H = 1 g/mole– 8 H x 1 g/mole = 8 g/mole• 8 g/mole + 36 g/mole = 44 g/mole C3H8Grams calculated from Moles• Can find the mass of substance from knowing molar mass and molesNa=23 g/mole ¼ mole• Multiply molar mass times moles• 23 g/mole x 0.250 moles = 5.75 gMass to moles relationshipProportions• Mathematical device to compare ratios• Be sure you keep same:samein columns and rowsExampleorb of molesa of molesb of a of =ggb of molesb of a of molesa of gg=Problem• 60 grams NO• How many grams NO2produced?22NOONO →+Balance Equation2222 NOONO →+Problem• 60 grams NO• How many grams NO2produced?• Molar mass of each component NO=30 g/mol, O2=32 g/mol NO2=46 g/molHow many moles of NO is 60 g?Molar ratios?How many moles of NO2 is producedHow many grams is that? 2:1:2292 g2 moles2222 NOONO →+Problem: 192 g O2→ ? g SO2• Balance first• Then determine molar ratios•3 O2to 2 SO2•3:2OHSOOSH2222+→+OHSOOSH22222232+→+Problem• Find molar mass of O2so you can determine moles of O2 O2: (2 O=32) = 32 g/mol O2 SO2: (S=32)+(2 O=32) = 64 g/mol SO2 H2O: (2 H=2) + (O=16) = 18 g/mol H2O H2S: (2 H=2) + (S=32) = 34 g/mol H2S


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WOU ES 105 - Types of Reactions

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