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Unit 7 pwrpoint
Uploaded: A week ago
Contributor: 1032637
Category: Biology
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Tags: Unit7, PowerPoint,
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Filename:   Copy of Unit 07.pdf (1.56 MB)
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Unit 7 powerpoint
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1/8/19 Vocabulary •For each vocabulary word, compete the FrayerModel Definition Picture Unit 07 NOT from Google! Representing Change WORD Examples Non-Examples Graphical Verbal Vocabulary •Balanced Equations •Chemical Energy •Reactants Unit 07 •Products Representing Change Diagrammatical Mathematical 1 1/8/19 Initial Mass of iron nails Initial Observations Nail Lab Nail Lab Post-RxnObservations What is the ratio of Copper Produced to Iron •Procedure (Day 2) Consumed in a replacement reaction? Mass of Filter Paper • Record observations Post-Drying Observations •Procedure (Day 1) • Obtain and mass a piece of filter paper • Obtain 25 mL of Copper(II) Chloride solution • Scrape the solid copper into the filter paper • Mass of Filter Paper + Cu Record the mass of 2 small iron pieces • Place nails into a small beaker for the drying oven • Record observations of both reactants Final Mass of iron nails • Pour liquid into filter paper • Place nails into the copper solution • Rise precipitate 2x with water, 1x with 1M HCl, 1x with water • Place filter paper and copper into a small beaker for the drying oven Nail Lab Nail Lab •Procedure (Day 3) •Questions • Record the mass of the iron nails and of the filter paper + copper • Why did the reaction stop? • Which reactant was used up? How do you know? • Describe what happened to the atoms of iron during the reaction? What •Calculations happened to the copper atoms? • Determine the mass of copper produced. • If you had placed 5 nails in the beaker, would anything about the reaction • Convert to moles have changed? (observations, reaction speed, amount of copper, ratio, …) • Determine the mass of iron consumed. • Looking at the accepted copper to iron ratio, what accounts for the difference • Convert to moles compared your ratio? • Calculate the ratio: moles of copper to moles of iron • Express as integers (1.33 à4/3 or 0.67 à2/3) 2 1/8/19 Conductivity of Substances Rearranging Atoms Question (from start of lab) •Create a CER document with your What is the ratio of Copper Produced to Iron •Describe what you already know about: lab partners Consumed in a replacement reaction? • Our Current Model of the Atom Claim (answer to question) • Conservation of Mass (give an example) Evidence (Data/Calculations/Graphs) • Chemical Formulas (give an example) • Subscripts in Formulas (give an example) Reasoning (explanation of the Data) • Coefficients (give an example) Rearranging Atoms Rearranging Atoms •Use Legos to create the REACTANTS •___H2+ ___O2à___H2O •For each reaction, how does the TOTAL number of Reactant Atoms •Rearrange the legosto create the •___H2+ ___Cl2à___HCl compare with the TOTAL number of Product Atoms? PRODUCTS •___Na + ___O2à___Na2O •How does this explain the Conservation of Mass? •If you have random leftovers, you th • ___N2+ ___H2à___NH3 •Looking at ammonia (the product in the 4 equation) must START OVER • What does the coefficient tell us about this substance? • ADD extra reactant molecules so that you •___CH4+ ___O2à___CO2+ ___H2O • What do the subscripts on the nitrogen and hydrogen tell us about this substance? will NOT have any leftovers •___NO + ___O2à___NO2 •Draw a particle diagram and write a • ___Fe + ___Cl2à___FeCl3 balanced chemical equation 3 1/8/19 Rearranging Atoms Good Morning •Atoms are REARRANGEDin a Chemical Reaction •Please balance the following equations • Equations show EVERY atom •___NO + ___O2à___NO2 •Balancing Equations • Particle Diagram and Inventory • Add COMPOUNDS until equal • MINOH • ___Fe + ___Cl2à___FeCl3 • Multiple Places = Last Rearranging Atoms Rearranging Atoms •___NaCl+ ___ F2à___NaF+ ___Cl2 •___Na + ___I2à___NaI •___N2O à___N2+ ___O2 •___KClO3à___KCl+ ___O2 •___KI + ___Cl2à___KCl+ ___I2 •___HCl+ ___Ca(OH)2à___CaCl2+ ___H2O •___Pb(NO3)2+ ___KI à___PbI2+ ___KNO3 •___NaCl+ ___O2à___NaClO3 •___CH4O + ___O2à___CO2+ ___H2O 4 1/8/19 Rearranging Atoms Good Morning •___K3PO4+ ___HClà___KCl+ ___H3PO4 •Get out Homework •___S + ___O2à___SO3 •Please balance the following equations •___AlCl3+ ___F2à___AlF3+ ___Cl2 •___Li2O + ___H2O à___LiOH •___AgNO3+ ___MgCl2à___AgCl + ___Mg(NO3)2 •___N2+ ___O2à___N2O5 •___K + ___MgBr2à___KBr+ ___Mg Homework Rearranging Atoms • K3PO4+ 3HCl à3KCl + H3PO4 •___AlBr3+ ___K2SO4à___KBr+ ___Al2(SO4)3 • 2S + 3O2à2SO3 •___C3H8+ ___O2à___CO2+ ___H2O • 2AlCl3+ 3F2à2AlF3+ 3Cl2 •___FeCl3+ ___NaOHà___Fe(OH)3+ ___NaCl •2AgNO3+ MgCl2à2AgCl + Mg(NO3)2 •___P4+ ___O2à___P2O5 •2N2+ 5O2à2N2O5 •___Li2O + ___H2O à___LiOH •___K + ___MgBr2à___KBr+ ___Mg •___C6H12O6+ ___O2à___CO2+ ___H2O 5 1/8/19 Types of Chemical Reactions Types of Chemical Reactions •5 Basic Types of Chemical Reactions •Synthesis • 2 Reactants form 1 Product A + B àAB ___Mg + ___O2à___MgO Types of Chemical Reactions Types of Chemical Reactions •Decomposition •Single Replacement • 1 Reactant forms 2 Products • 1 Element replaces Another AB àA + B A + BC àAC + B ___H2O2à___O2+ ___H2O ___Mg + ___HC2H3O2à___Mg(C2H3O2)2+ ___H2 6 1/8/19 Types of Chemical Reactions Types of Chemical Reactions •Double Replacement •Combustion • 2 Elements switch Partners • Hydrocarbon combines with Oxygen gas AB + CD àAD + CB • Produces CO2and H2O CxHyOz+ O2àCO2+ H2O ___Pb(NO3)2+ ___KI à___ PbI2+ ___KNO3 ___C3H8+ ___O2à___CO2+ ___H2O Types of Chemical Reactions Homework •Classify the following •Balance the equations AND identify the reaction type • 2H2+ O2à2H2O •___K3PO4+ ___HClà___KCl+ ___H3PO4 • Br2+ MgI2àMgBr2+ I2 • 2HgO à2Hg + O2 •___S + ___O2à___SO3 • AgNO3+ NaClàAgCl + NaNO3 •___AlCl3+ ___F2à___AlF3+ ___Cl2 • C2H6O + 3O2à2CO2+ 3H2O •___AgNO3+ ___MgCl2à___AgCl + ___Mg(NO3)2 •Go back in your notes and classify each of the equations we have •___N2+ ___O2à___N2O5 already balanced. 7 1/8/19 Products of Chemical Reactions Products of Chemical Reactions •Determining the Type of Reaction based on Reactants ONLY •Tests for Gases •Hydrogen Gas (H2) • Burning Splint à“POP” Sound • Single Oxygen Gas (O2) Double • Glowing Splint àStarts Burning Decomposition Combustion Replacement Replacement •Carbon Dioxide Gas (CO2) YES YES YES YES • Burning Splint àGoes Out • Bubbled into lime water àcloudy Single Element NO CxHyOz NO NO NO CO2Ca(OH)2àCaCO3(s)+ H2O Only 1 + 2 Ionic Compounds + Reactant Ionic Compound or Acids O2 or Acid Synthesis Products of Chemical Reactions Products of Chemical Reactions •Classify the following •Classify the following reactions. • ___H2+ ___Cl2à • ___AlBr3+ ___K2SO4à • ___Li + ___MgI2à • ___C3H8+ ___O2à • ___NaHCO3à • ___FeCl3+ ___NaOHà • ___NaOH+ ___HClà • ___P2O5à • ___C2H6+ ___O2à • ___Li2O + ___H2O à • ___K + ___MgBr2à • ___C6H12O6+ ___O2à 8 1/8/19 Homework Products of Chemical Reactions •Classify the following reactions. •Predicting Products • ___AlBr3+ ___K2SO4àDR • Identify the Type of Reaction • ___C3H8+ ___O2àComb • Use the Reference Table • ___FeCl3+ ___NaOHàDR • ___P2O5àDecomp • • ___Li2O + ___H2O àSyn Tips: • ___K + ___MgBr2àSR • Acid: Starts with H (HCl, H2SO4), “Smash Crap Together” - • ___C6H12O6+ ___O2àComb • Base: Hydroxide (OH) • Metals: Ionic Compounds àAdd up charges • USE THE GENERAL FORM!!! Products of Chemical Reactions Products of Chemical Reactions •BaCO3à •CO + H2O à •Na + H2O à •Li + FeCl2à •Li2O + H2O à •Sr(OH)2à •CH4+ O2à •HF + LiOHà •NaCl+ Ag2SO4à •C3H8+ O2à 9 1/8/19 Products of Chemical Reactions Products of a Chemical Reaction •Ca(NO3)2+ (NH4)2CO3à •C3H6O + O2à •Al + F2à •HNO3+ Ba(OH)2à •C2H6+ O2à •Mg + HBr à •H2SO3à •BeO+ H2O à •F2+ KClà •RbClO3à Replacement Reactions Replacement Reactions •Not all Replacement Reactions will occur •Single Replacement • Single Replacement = Activity Series • Single Element must be ABOVE • Double Replacement = Solubility Rules •K + ZnCl2à •Br2+ ZnCl2à •Ca + H2O à •Bi + HClà 10 1/8/19 Replacement Reactions Replacement Reactions •Sb + H2O à •Double Replacement • Reactions MUST form a solid (precipitate) or water • ALL Aqueous (soluble) = NO RXN •HBr + Zn à •F2+ KClà •BaS+ Na à Replacement Reactions Replacement Reactions •Double Replacement •CoCl2(aq)+ Al(NO3)3(aq)à • Solubility: Soluble = Aqueous Insoluble = Solid •Fe(C2H3O2)3(aq)+ KF(aq)à NaF Co(NO3)2 Al(OH)3 •HI(aq)+ LiOH(aq)à BaSO4 Mg3(PO4)2 (NH4)2S •(NH4)2S(aq)+ SnBr2(aq)à 11 1/8/19 Replacement Reactions Ionic Equations •H3PO4(aq)+ RbCl(aq)à •When dissolved in water, IONS can move around àConduct Electricity •Ag2S(aq)+ CuCl2(aq)à • This can be represented using Ionic Equations •NaOH(aq)+ H2SO4(aq)à •Molecular Equation: Pb(NO3)2(aq)+ KI(aq)à •FeCl2(aq)+ H2S(aq)à •Complete Ionic Equation: • Separate (aq) into ions •Net Ionic Equations • Remove Spectator Ions Ionic Equations Ionic Equations •Molecular: CaCl2(aq)+ Na2CO3(aq)àCaCO3(s)+ 2NaCl(aq) •Molecular: Na2S(aq)+ 2HCl(aq)à2NaCl(aq)+ H2S(g) •CIE: •CIE: •NIE: •NIE: 12 1/8/19 Ionic Equations Ionic Equations •Molecular: 2Fe(s)+ 3CuCl2(aq)à3Cu(s)+ 2FeCl3(aq) •Molecular: 3Li(s)+ FeCl3(aq)àFe(s)+ 3LiCl(aq) •CIE: •CIE: •NIE: •NIE: Ionic Equations Ionic Equations •Molecular: H2SO4(aq)+ Ba(OH)2(aq)à •Molecular: NaF(aq)+ FeCl3(aq)à •CIE: •CIE: •NIE: •NIE: 13
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