1 / 54

Chemistry SM-1131 Week 9 Lesson 1

Chemistry SM-1131 Week 9 Lesson 1. Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008. Class Today. Tests-returned Chemical Reactions Types of Chemical Reactions Balancing Chemical Reactions

vida
Télécharger la présentation

Chemistry SM-1131 Week 9 Lesson 1

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry SM-1131Week 9 Lesson 1 Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008

  2. Class Today • Tests-returned • Chemical Reactions • Types of Chemical Reactions • Balancing Chemical Reactions • New Material: Double Displacement, acid base, spectator ions, solubility rules, precipitation reactions • Take Home Quiz (described only if there is time) due Monday!

  3. Test • 1-Mg(NO3)2, magnesium nitrate, Mg1N2O6 • 2-Fe(III)2(SO3)3, Iron (III) sulfite, Fe2S3O9 • 3-dinitrogen pentaoxide, diphosphorustetraoxide, CCl4, H2O, SF6 • 4-NH4MnO4, ammonium permanganate, N1H4Mn1O4 • 5- H3PO4, phosphoric acid, H3P1O4 • 6- 48amu, 164amu, 400amu, 18amu, 78amu

  4. test • .31 mol O3, .159mol Na3PO4, .22mol Fe(III)2(SO4)3, 1.11e5 mol H2O, 5.76e-5 mol CaF2 • 720gO3, 4.26e3g Na3PO4, 3.52e4 g Fe(III)2(SO4)3, 3.6e7g H2O, 0.35g CaF2 • Moles  atoms in a sec • 27% carbon

  5. Test Q9 15 moles O3 x 6.02e23 molecules O3x 3 atoms = 2.709e25 1 mole O3 1 molecule O3 unit is atoms

  6. Test 11 • Percent Composition for C6H6 and C2H2 • %C= 92.3% • %H= 7.7% • 7.7H  7.7g • 7.7g H x 1 g H/ mol = 7.7 mol H • 92.3%  92.3g C • 92.3 g C x 1mol C/ 12g C = 7.7 mol C • 7.7/7.7 =1… C1H1 for both

  7. N=6 • Molecular formula/empirical formula = N • N=6 means that the molecule is 6 times bigger than the empirical formula you just got. • The empirical formula you just got was C1H1, so the molecular formula is C6H6.

  8. Chemical Reactions • A chemical reaction is a rearrangement of atoms. • Reactants  Products

  9. Evidence of a Chemical Reaction • Heat and Light • Formation of solids • Gas emitting • Changing colors • Change in temperature

  10. Some quick vocab • (g) means the substance is a gas • (l) means the substance is a liquid • (s) means the substance is a solid • (aq) means the substance is aqueous • Aqueous means dissolved in water.

  11. Rules about Chemical Equations • Remember that law of conservation of mass? • Matter can neither be created nor destroyed. • We’ll start with skeleton equations • We’ll alter it to make a balanced equation.

  12. Counting molecules and atoms • 2H2O • 4Mg(NO3)2 • The 2 and the 4 are called coefficients, just like 5X in math where the 5 is the coefficient.

  13. Types of Chemical Reactions • There are 5 main types of reactions • Combination aka synthesis • Decomposition • Combustion • Single displacement • Double displacement • (Acid Base, gas evolution, precipitation, oxidation and reduction aka redox)

  14. Combination Reactions • 2 things come together to make 1 thing. • Carbon and Hydrogen react to form the compound methane. • C + H2 CH4 is the skeleton equation • C + 2H2 CH4 is the balanced equation

  15. Combination Reaction 2 • Mg and oxygen react at high temperature what is formed? • Mg + O2 MgO • O2 is diatomic when written into reactions (HINClBrOF) • (How’d I know MgO, well 4 steps: symbols, charges, switcheroo, reduce) • To balance it…

  16. Balancing Chemical Reactions • ___ Mg + ___ O2 ___MgO • 1- for all ionic compounds correctly establish their formula • 2-List all elements in the rxn under the arrow • 3-Count the number of atoms of each type on both sides of the equation • 4-Starting with metals change the coefficients until both sides are balanced. DO NOT CHANGE CHEMICAL FORMULAS.

  17. Balancing Chemical Reactions • ___ Mg + ___ O2 ___MgO ___Mg___ ___O___ • ___ Mg + ___ O2 ___MgO 1 Mg 1 2 O 1 NOT BALANCED • ___ Mg + ___ O2 _2_MgO 1 Mg 2 2 O 2 NOT BALANCED • _2_ Mg + ___ O2 _2_MgO 2 Mg 2 2 O 2 BALANCED

  18. More examples • N2 + 3H2 2NH3 • 2Al + 3F2  2AlF3 • P4 + 5O2  P4O10 • SO3 + H2O  H2SO4

  19. Decomposition • When things decompose they break down. This reaction is where 1 molecule breaks down into several molecules. • Iron(III) chloride decomposes at high temperature into it’s elements. • FeCl3 Fe + Cl2 • Not balanced, again HINClBrOF

  20. Electrolysis of water • Electrolysis is when you put a current through water. Water turns into it’s elements. Write and balance the reaction. • ___H2O  ___H2 + ___O2 _2H 2 _1O_2 • _2_H2O  ___H2 + ___O2 _4H_2 _2O_2 • _2_H2O  _2_H2 + ___O2 _4H_4 _2O_2

  21. More examples of Decomposition • CaCO3 CaO + CO2 • 2 HgO  2 Hg + O2 • 2 KClO3  2KCl + 3O2

  22. Combustion Reactions • Combustion means burning and fire. What two things does fire require? O2 and something to burn. We normally burn hydrocarbons (Hydro=H, Carbon = C therefore stuff made up of H and C). • The products are always CO2 and H2O. • Methane and Oxygen burn write the equation. • ___CH4+ ___O2 ___ CO2 + ___H2O

  23. Balance a combustion • ___CH4+ ___O2 ___ CO2 + ___H2O __C __ __H __ __O __ (it comes from 2 places) Balance this reaction now

  24. Balanced Reaction • _1_CH4+ _2_O2 _1_ CO2 + _2_H2O 1_C 1_ 4_H 4_ 4_O 4_ (it comes from 2 places)

  25. Harder example • C2H6 + O2 CO2 + H2O 2 C 1_ 6 H 2_ 2 O 3_ • C2H6 + 3.5 O2 2 CO2 + 3 H2O 2 C 2_ 6 H 6_ 7 O 7_(no such thing as 0.5O2)

  26. Double all the coefficients • 2C2H6 + 7 O2 4 CO2 + 6 H2O 4 C 4_ 12 H 12_ 14 O 14_ All combustion reactions will be just like one of those two reaction.

  27. Displacements • These are the 2 hardest to tell apart when starting. • Single displacements typically have 1 lone element on both sides of the reaction • Double displacements look like the biggest reactions out there, and you’ll see that the two metals switch places

  28. Single Displacement • Magnesium metal starts making hydrogen gas when it’s dropped in aqueous hydrochloric acid. What’s the full reaction? ___Mg + ___HCl ___ H2+ __ ?

  29. Single Displacement • ___Mg + ___HCl ___ H2+ __ MgCl? • NO! 4 steps when writing ionic salts ALWAYS! So, it’s MgCl2 • ___Mg + ___HCl ___ H2+ __ MgCl2 1 Mg 1_ 1 H 2_ 1 Cl 2_ ___Mg + _2_HCl  ___ H2+ __ MgCl2

  30. Single Displacement • ___Mg + _2_HCl  ___ H2+ __ MgCl2 • Notice: Mg is elemental on the left side, and Hydrogen is elemental on the right side. • The single lone element was displaced by a different lone element.

  31. More Examples • 3AgCl + Al  AlCl3 +3 Ag • 2Na + H2O  H2 + 2NaOH • Zn3N2 + 3Mg  Mg3N2 + 3Zn

  32. Double Displacementel double • Silver nitrate and sodium chloride react to form silver chloride and sodium nitrate. Write and balance the reaction. • KEY POINT: FIGURE OUT THE FORMULA FOR EACH INORGANIC PIECE AND DON’T MESS WITH THE FORMULA FOR THE REST OF THE TIME!

  33. El Double • AgNO3 + NaCl AgCl + NaNO3 • It’s already balanced. • The Ag and Na switched places. • That’s why it’s a double displacement.

  34. El Double 2 • Barium nitrate and potassium sulfate reaction to form barium sulfate and potassium nitrate. Write and balance the equation. Ba(NO3)2 + K2SO4 Ba(SO4) + KNO3 Ba _ K _ (NO3) _ (SO4) _

  35. Acid Base • These are like double displacement reactions, except one of the compounds is going to be an acid and the other will be an ionorganic salt • Salt just means combination of a cation and anion in a solid form • Hydrochloric acid and sodium hydroxide react together. Write the reaction.

  36. ACID BASE • HCl + NaOH ____ + ____ • The “metals” swithc places. So H and Na will switch. Na will be with Cl, and H will be with OH • HCl + NaOH NaCl + H2O

  37. Acid Base • Phosphoric acid and sodium hydroxide are stirred in a beaker together what products are made?

  38. Acid Base • H3PO4 + NaOH Na3PO4 + H2O = skeleton • Balance this

  39. Solubility • Often times we perform a double displacement reaction to actually collect one of the products. We can make certain compounds crash out of (precipitate) an aqueous solution because of how soluble some compounds are. • We’ll take two soluble compounds, they will react, and they will typically make one soluble product and one insoluble product.

  40. Na2SO4 and BaCl2 • Na2SO4 + BaCl2 NaCl + Ba(SO4) skeleton • Balance this (if you make a compound Na2Cl2 you are wrong and bad! We don’t mess with formulas after they are set. We just change coefficients).

  41. Solubility Rules • You did that reaction in lab! The BaSO4 was a powder that crashed out of solution and you filtered it off! Why did it crash out? Because of solubility rules.

  42. Solubility Rules • Any compound with Li, Na, K, or NH4 will always be soluble • Any compound with NO3 or C2H3O2 will always be soluble • Compounds with Cl, Br, I will be soluble except with Ag, Hg or Pb • Compounds with SO4 will be soluble except with Sr, Ba, Pb, or Ca • Compounds with CO3 and PO4 are insoluble unless with Li, Na, K or NH4

  43. Barium • Ok, so let’s take our barium and sulfate reaction and try to figure out which are soluble pieces and which are not.

  44. Solubility Rules with Sulfate lab • Na2SO4(?) + BaCl2(?) NaCl(?)+ Ba(SO4)(?) • Compounds with Na are ? • Compounds with Cl are? • Compounds with Na are? • Compounds with Sulfate are? Except with?

  45. Solubility • Na2SO4(aq)+ BaCl2(aq) NaCl(aq)+ Ba(SO4)(s)

  46. Dissolving • So, what happens when an inorganic compounds dissolves (this is totally different than a molecular compound dissolving)? • Water molecules act as crowbars that split molecules into pieces. The two pieces formed are the cations and the anions. • When you see table salt it’s the compound NaCl. When you dissolve it in water it’s actually Na+ and Cl-.

  47. Try some more • Ag(NO3) Ag+ and NO3- • Na2(SO4) 2Na+ and SO4-2 • H3PO4 3H+ and PO43- • Na(OH)  Na + and OH- • Li3(PO4)  3Li+ and PO43-

  48. Molecular Compounds • Molecular compounds don’t do that. • C6H6O6(s)  C6H6O6(aq) no change occurs.

  49. Spectator • Spectator ions- reactions have components that aren’t that important to the overall effect. We can tell they aren’t that important because they appear on both sides of the chemical equation. They aren’t really participating, they are just hanging out. We call them spectator ions.

  50. Net Ionic Equations • Net just means overall, so we’re trying to figure out what’s the overall reaction. • Aluminum chloride and sodium phosphate undergo a double displacement reaction. What precipitates and what’s the net ionic equation? • AlCl3 + Na3PO4 AlPO4 + NaCl = skeleton • AlCl3 + Na3PO4 AlPO4 + 3NaCl = balanced • AlCl3(aq)+ Na3PO4(aq) AlPO4(s)+ 3NaCl(aq) total eq

More Related