WPHS Chemistry



WPHS ChemistryUnit 4Chemical ReactionsBergmann-SamsChemistry: Unit 4 Outline: Chemical ReactionsAssignmentOnly in ClassCheckPodcast 4.1: Converting Word Equations into Formulaic EquationsWorksheet 4.1: Converting Word Equations into Formulaic EquationsPodcast 4.2: Balancing Chemical EquationsWorksheet 4.2: Balancing Chemical EquationsPodcast 4.3: Reaction Types OverviewWorksheet 4.3: Reaction Types OverviewLab: Types of Reactions LabXPodcast 4.4: Predicting Single Replacement ReactionsWorksheet 4.4: Predicting Single Replacement ReactionsLab: Activity Series of a MetalXPodcast 4.5: Predicting Double Replacement ReactionsWorksheet 4.5: Predicting Double Replacement ReactionsLab: Small Scale Double ReplacementXPodcast 4.6: Complete Ion and Net Ionic EquationsWorksheet 4.6: Complete Ion and Net Ionic EquationsPodcast 4.7: Mixed Types of ReactionsWorksheet 4.7: Mixed Types of ReactionsDemo: Light your teacher on FIRE!!!XUnit 4 Review (Review)Unit 4 VocabularyUnit 4 ExamXUnit 4 Vocabularyword equation chemical equationskeleton equationCatalystCombination ReactionsDecomposition ReactionSingle Replacement ReactionDouble Replacement ReactionprecipitateCombustion ReactionIonIonic and Net Ionic EquationsCut out the following 2 tables and put them in the back of your composition book. These are reference tables that you will use throughout the year.Activity of Metals SeriesMetalIon FormedLithium: LiLi+Potassium: KK+Barium: BaBa2+Calcium: CaCa2+Sodium: NaNa+Magnesium: MgMg2+Aluminum: AlAl3+Manganese: MnMn2+Zinc: ZnZn2+Chromium: CrCr3+Iron: FeFe3+Cadmium: CdCd2+Cobalt: CoCo2+Nickel: NiNi2+Tin: SnSn2+Lead: PbPb2+Hydrogen: H2H+Copper: CuCu2+Silver: AgAg+Mercury: HgHg2+Platinum: PtPt2+Gold: AuAu3+Solubility TableKey: (s) = solid, (aq)= aqueous: soluble in water, H2O = water formed (NE)= does not exist, AcetateBromideCarbonateChlorateChlorideChromateHydroxideIodideNitrateOxidePhophateSulfateSulfideAluminum(aq)(aq)NE(aq)(aq)NE(s)(aq)(aq)(s)(s)(aq)(s)Ammonium(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)NE(aq)(aq)(aq)Barium(aq)(aq)(s)(aq)(aq)(s)(s)(aq)(aq)(aq)(s)(s)(s)Calcium(aq)(aq)(s)(aq)(aq)(aq)(s)(aq)(aq)(s)(s)(s)(s)Copper II(aq)(aq)(s)(aq)(aq)NE(s)(aq)(aq)(s)(s)(aq)(s)Hydrogen(aq)(aq)Gas(aq)(aq)NEH2O(aq)(aq)NE(s)(aq)(s)Iron II(aq)(aq)(s)(aq)(aq)NE(s)(aq)(aq)(s)(s)(aq)(s)Iron III(aq)(aq)NE(aq)(aq)(s)(s)(aq)(aq)(s)(s)(aq)(s)Lead II(aq)(s)(s)(aq)(s)(s)(s)(s)(aq)(s)(s)(s)(s)Magnesium(aq)(aq)(s)(aq)(aq)(aq)(s)(aq)(aq)(s)(s)(aq)(s)Manganese II(aq)(aq)(s)(aq)(aq)NE(s)(aq)(aq)(s)(s)(aq)(s)Mercury II(aq)(aq)NE(aq)(aq)(s)(s)(aq)(aq)(s)(s)(aq)(s)Potassium(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)Silver I(aq)(s)(s)(aq)(s)(s)(s)(s)(aq)(s)(s)(aq)(s)Sodium(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)(aq)Strontium(aq)(aq)(s)(aq)(aq)(s)(aq)(aq)(aq)(aq)(s)(aq)(aq)Tin II(aq)(aq)NE(aq)(aq)(s)(s)(aq)(aq)(s)(s)(aq)(s)Tin IV(aq)(aq)NENE(aq)(aq)(s)(aq)(aq)(s)NE(aq)(s)Zinc II(aq)(aq)(s)(aq)(aq)(s)(s)(aq)(aq)(s)(s)(aq)(s) Types of Reactions LabPurpose: To observe the different types of reactions: single replacement, synthesis, decomposition, combustion, double replacement.Single Replacement (Zinc + Hydrochloric Acid)Synthesis (Hydrogen + Oxygen)Decomposition (Hydrogen Peroxide (H2O2))Combustion (Cellulose (C6H12O6) + Oxygen)Double Replacement (Calcium Chloride + Sodium Carbonate)Part A: Single Replacement and SynthesisPlace one square of Zinc into a medium test tube.Add 10mL of 1.0M HClCover the test tube with your thumbRecord observationsWrite the chemical reaction for this single replacement reactionHave your partner light a wood splintRelease your thumb and immediately have your partner place the wood splint near the mouth of the test tube.Record your observationsWrite the chemical reaction for this synthesis reaction (water is a product).OBSERVATIONS and REACTIONSPart B: Decomposition and CombustionPlace 10ml of hydrogen peroxide into a medium test tubeAdd 0.2g of MnO2 (MnO2 is a catalyst and is not part of the reaction)Record your observationsWrite the chemical reaction for this decomposition reaction (products are water and oxygen gas)While the decomposition reaction is still occurring light a wood splint, let it burn for a few seconds and blow it out.While the wood splint is still glowing (but not burning), place it into the mouth of the test tube.Record your observationsWrite the chemical reaction for this combustion reaction between cellulous and oxygen.OBSERVATIONS and REACTIONSPart C: Double ReplacementObtain 1mL of 1.0M Calcium Chloride and 1mL of 1.0M Sodium CarbonateMix the two solutions in a medium test tubeRecord your observationsWrite the chemical reaction for this double replacement reactionOBSERVATIONS and REACTIONSActivity Series of Metals LabPurpose: To observe an activity series of different metals.Procedure: Using the well plates, select a row of wells for each solution listed in the data table. Make sure that you write down which letter and number your wells are for each solution. There should be three wells for each solution (one of the three for each of the metals).Put five drops of each solution in the wells chosen for that solution. Put one piece of magnesium in one of the wells for each solution. For example, you should have a well of copper sulfate with magnesium in it, a well of magnesium sulfate with magnesium in it, and a well of sodium chloride with magnesium in it, a well of zinc sulfate with magnesium in it and a well of silver nitrate with magnesium in it. Repeat step 3 with copper instead of magnesium.Repeat step 3 with zinc instead of magnesium.After l minute has passed, make observations of both the metal strips and the solutions. Put these observations in a data table in your comp book that looks like the one below. Label this data table as 1 minute.After 5 total minutes have passed, take another set of observations. Make another data table like the one below and label it 5 minutes.After 15 total minutes have passed, take another set of observations. Again, make another data table and label it 15 minutes.Data Table:CuSO4MgSO4NaClZnCl2AgNO3Cu metalMg metalZn metalAnalysis Questions: (as always with labs, these questions should be written in complete sentences)Why doesn’t the metal react with the same metal solution?In which wells did the appearance of the metal change? Be sure to tell your teacher what both of the reactants of the well were.Write a balanced equation for each visible reaction between a metal and it’s solution. Be sure to identify what types of reactions these are.Based on the results of your experiment construct your own activity series for the five metals. Put the most active metal first and the least active metal last. Be sure to include your reasoning for your rankings.In a short summary paragraph, describe and explain the patterns that you see in your reaction table. Double Replacement LabUse Beral Pipets to add each solution on the grid. For those that have a reaction occur, describe the reaction. For those that do not, record NVR (No visible reaction) When done you need to:Write out each complete reaction that occurs (you must balance it)Write out the ionic equation for each reaction that occurs.Write out the net-ionic equation for each reaction that occurs.Put “flimsy” over the top of this page and mix all of the chemicals. Do not mix the same chemical with the same.ChemicalNaClAgNO3Pb(NO3)2Na2SO4BaCl2NaOHNa3PO4NaClXXXXXXAgNO3XXXXXXPb(NO3)2XXXXXXNa2SO4XXXXXBaCl2XXXXXXNaOHXXXXXXNa3PO4XXXXXXData Table: Write in your observations here.ChemicalNaClAgNO3Pb(NO3)2Na2SO4BaCl2NaOHNa3PO4NaClAgNO3Pb(NO3)2Na2SO4BaCl2NaOHNa3PO4 Worksheet 4.1: Converting Word Equations to Formulaic EquationsWrite each of the following equations using chemical symbols and all other appropriate symbols. Remember to put state of matter in parenthesis and subscripted.Iron is heated in the presence of solid sulfur to from solid iron III sulfideGaseous methane CH4 is reacted with oxygen gas to form carbon dioxide gas and water vaporAqueous copper II chloride is added to aqueous lead II nitrate to from solid lead II chloride and aqueous copper II nitrateChlorine gas is bubbled into aqueous sodium bromide to form aqueous sodium chloride and liquid bromineSolid silver is added to aqueous gold III chloride to form solid gold and silver I chloride.Gaseous ammonia(NH3) is bubble into water to form aqueous ammonium hydroxideWorksheet 4.2: Balancing Chemical EquationsBalance the following equations__HgO __Hg+__O2__HCl+__Mg__H2+MgCl2 __CH4+__O2__CO2+__H2O __C6H12O6+ __O2__CO2+ __H2O__H2+__O2__H2O__H2+__N2__NH3__NO+__O2__NO2__Al2O3__Al+__O2__CaO+__H2O__Ca(OH)2Hydrogen gas reacts with iodine to produce hydroiodic acid.Sulfur reacts with oxygen to produce sulfur dioxide.Calcium acetate reacts with sodium carbonate to produce calcium carbonate and sodium acetate.Iron combines with oxygen and water to form iron (III) hydroxideSulfur trioxide is bubbled through water to produce sulfuric acidCopper-bottomed cooking pans turn black because copper combines with oxygen to form copper (II) oxide.Magnesium hydroxide neutralizes stomach acid, HCl, to produce magnesium chloride and water.Worksheet 4.3Now go back to Worksheets 4.1 and 4.2 and write down the type of each reactionWorksheet 4.4: Predicting Single Replacement Reactions Predict the products and balance the following single replacement reactions. If no reaction occurs write N.R. For transition metals use the following charges:Fe (s)+ CuCl2(aq) Hg(l)+Sn(SO4)2 (aq) Ba (s)+Ni3(PO4)2 (aq)Pb(s)+Au(NO3)3 (aq)Li(s)+HOH(l)K(s)+AgCl(s) Ca(s)+NaOH(aq) Cu(s)+Fe(OH)3(aq) Fe(s)+Cu(OH)2(s)Lead II Chloride + MagnesiumBarium Nitrate + ZincPotassium + Tin IV NitrateCopper + Silver NitrateSodium Phosphate + PotassiumGold + Hydrochloric acidMagnesium + Aluminum HydroxideIron + Copper II SulfateIron + Nickel II IodideSodium Permanganate + Calciumhydrochloric acid + ZincAluminum + Iron II dichromate Worksheet 4.5: Predicting Double Replacement ReactionsComplete and Balance the following reactions. If no reaction occurs then write N.R. Na2SO4 (aq) + Ba(NO3)2(aq) ---->NaNO3(aq) + NH4Cl(aq) ----->Pb(NO3)2 (aq) + Na2CrO4(aq)ZnCl2(aq) + K2CO3(aq) ---->Ammonium Chloride + Silver Nitrate ------>Barium Acetate + Copper II ChromateSolutions of Silver Nitrate and ammonium chloride are mixedSolutions of Lead II nitrate and Sodium Chloride are mixedSolutions of zinc sulfate and magnesium chloride are mixedSolutions of Ammonium phosphate and Zinc Chlorate are mixedSolutions of Aluminum bromide and Iron II Iodide are mixedSolutions of sodium sulfide and Iron II Chlorate are mixedSolutions of copper II bromide and potassium phosphate are mixedSolutions of barium acetate and zinc sulfate are mixed Worksheet 4.6: Complete Ion and Net Ionic EquationsFor the following reactions write the:Complete Equation (Indicate states): BalanceIonic EquationNet Ionic EquationZnCl2 (aq) + Na2S (aq) ZnS(s) + NaCl(aq)(NH4)3PO4 + AgNO3 Magnesium Nitrate + Potassium phosphate Magnesium Phosphate (s) + Potassium Nitrate.Lead II Acetate + Potassium IodideWorksheet 4.7: Mixed Types of ReactionsDirections: For each of the following reactions:Identify the type of reaction (Single Replacement, combination, double replacement, decomposition, or combustion)Complete the reaction (Put NR if no reaction takes place)Balance itIndicate states of matter for each substance (solid, liquid, gas, aqueous)NaCl(aq) + AgNO3(aq) Fe(s) + CuSO4(aq) C4H10(g) + O2(g) Ba(NO3)2(aq) + Na2SO4 (aq) AgNO3(aq) + Li(s)LiBr(aq) + Cu(s) MgS(s) + NaOH Hg(l) + LiClLi(s) + HgCl2(aq)C3H8(g)+ O2(g) Ammonium Nitrate is added to sodium chlorideLithium Chloride is added to Zinc PhosphateZinc is added to lithium chlorideIron is added to a solution of silver nitrateA solution of copper II sulfate is added to an iron nailOctane (C8H18) is burned in air A solution of Tin IV sulfate is added to a solution of ammonium hydroxideSodium hydroxide is added to hydrochloric acidCalcium hydroxide is added to sulfuric acidNickel is added to hydrochloric acidStrontium is added to waterHydrochloric acid is added to copper metalSolid bismuth is added to a solution of barium hydroxide.Methanol (CH3OH) is burned in airSolid gold is added to hydrochloric acidUnit 4 Review SheetPart A: Balance the following reactions and indicate whether they are synthesis or decomposition reactions.1.SO3+H2O--->H2SO4Type:_____________2.H2O--->H2+O2Type:_____________3.HgO--->Hg+O2Type:_____________4.Al2O3(s)--->Al(s)+O2(g)Type:_____________5.P+O2--->P2O5Type:_____________Part B: Predict the products and indicate type (include states):1. KBr --->Type: _________2. Li + Cl2 --->Type: _________3. Rb2CO3 --->Type: _________4. NiO --->Type: _________5. CO2 + H2O--->Type: _________Part C: Predict the products, balance, include states, and indicate type. Molten sodium is reacted with chlorine gasType: _________Calcium is added to water(think of water as HOH)Type: _________Aluminum chloride decomposes into its elementsType: _________Potassium and Bromine are reactedType: _________Iodine reacts with hydrogenType: _________Part D:Write the molecular equation, the complete ionic equation, and the net ionic equation for each reaction. Aqueous lithium phosphate reacts with aqueous calcium chlorideAqueous potassium chloride reacts with aqueous lead II chlorateAqueous manganese II nitrate reacts with aqueous sodium sulfide. ................
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