Monday: Today we started the equilibrium unit with my oscillating rxn demo that didn’t work probably b/c I did not use distilled water! Ugh! Then we did the reversible reactions simulation from PhEt and then did the penny moving lab to derive the equilibrium constant and learn the difference between the constant and the equilibrium position as well as factors that affect both of those.  In the last 15 minutes I went through some of the notes I’ve given you including the graphs and how to write equilibrium constants from reactions + the meaning of the equilibrium constant.

Tuesday: 

Monday: Dye fading lab! Note to self: blue needs full strength bleach and takes only about 5 min. Red works the best with the weaker bleach. Yellow does not work. Also, we need more colorimeters!

Tuesday: Do Dye Fading Lab Analysis

Wedneseday: We started with the ozone article and questions after you guys got your labs turned in.  This was good b/c it let you practice reaction mechanism stuff. We briefly reviewed a couple of concepts like intermediate v catalyst  v. activated complex/transition state and which step in a mechanism is the slowest (highest activated complex).  Then I started my lecture on the Arrhenius equation but we didn’t get very far before class was over.  Basically gave you the equations but didn’t do any problems…

Thursday: Today we finished up the  activation energy concepts and went over some half life stuff that can also be tricky (know %’s).  Then I handed out the review guides and the dye fading labs so you can spend tomorrow reviewing for your test on Monday.  Here’s the notes and what not from yesterday and today.  List of topics for test:

• Check detailed list on unit outline.
• Boltzmann distribution
• Effusion/Diffusion
• Collision theory & 4 factors that affect rxn rates. Incorporate Boltzmann in to discussion for Temp and Catalysts
• Potential energy diagrams that show affect of catalyst. Identify number of steps, contrast activated complex w/ intermediate.
• Rate laws
  • Differential: using does rate double when concentration doubles?
  • Integrated: plot graphs of concentration v. time and determine which is most linear.
    •  Use linear equation to solve for conc at certain times,
    • half lives,
      • find half life from graph of concentration of reactant v. time and deterimine if first or 2nd order.
  • Reaction mechanisms – use mechanism to determine rate law, molecularity, identify mechanisms that don’t fit rate laws.
• Activation energy (arrhenius equation)
• Apply above to ozone layer depletion and catalytic convertor.

Friday: no class. I am at a conference. study for your kinetics test on Monday (here’s the answer key to the review guide that says IB HL at the top)

Monday: Today we did chemactivity 36 to learn how to calculate reaction rates.  I tried to do the iodine clock demo, but it did not work for some reason…next we tried the iodine clock lab but had major difficulties with it. Some of you got no results and some of you had the middle concentrations change color the fastest.  Weird. Will have to make new stuff.

Homework: continue with readings on catalytic convertor/air pollution and effusion/diffusion.

Tuesday: Today we learned how to determine the rate law and read reaction rate graphs.  Homework is to finish pages 13 to 15 in packet.

Wednesday: Grading day, no school.

Thursday: Today we started with a review of determining rate law.  So many of you professed having major difficulty with the homework that I gave some time to explain some of the harder problems. Boo!  I also went over our first integrated rate law (just first order). Here’s the notes.  

Homework is to watch the reaction mechanisms video being careful to watch for these items.  Also continue to work on packets and textbook problems listed on unit outline (rubric).

Monday: Design lab time! Last day to collect all your data.  Grades as follows: Due next Monday, Nov 9th.

So for Methods/Error Analysis make sure you:

• Calculations
  • Show work/ justify with words as you go along like you did on mixtures lab
  • Justify number of sig figs in final molar mass.
  • Calculate percent error.
    • Sample 1 was Na
    • Sample 2 and 3 were K
•  Procedures
  •    Say what you are doing (steps),
  •    why you are doing it that way (rationale for choices – use KMT principles),
  •    how you will get an answer (calculation), including plan for certain sig figs
• Error Analysis/Conclusion
  •  Did you get good R values? Was one gas better than the other? Are they similar? Why should they be similar?
  • Limitations of method/equipment/conclusions,
  • discussion of variability (precision…number of decimal places since you don’t have multiple trials) and accuracy (percent error) of the data that is justified
    • State the error
    • Determine whether it was random or systematic and justify this
    • What effect did the error have on the results – in detail. Do math if necessary. Do not just say it would throw off the result. Give an example.

Tuesday: No school, teacher professional day (also voting day)

Wednesday: Test

Thursday: Simulation on Rxn Rates.  HW: Work on lab

Friday: Boltzmann notes and worksheet + catalyst demos, potential energy diagrams and explanations of Temp and Ea using Boltzmann. HW: effusion/diffusion reading and questions and catalytic converter article.

Monday: Gas Laws Simulation Lab

Tuesday: Today we went over the Dumas method of determining molar mass.  We did #13 in the packet (and connected to empirical formula).  Then I gave you a copy of this set of procedures and data to see how you could do this experimentally.  Real value was ethanol.  The last bit of class we worked on multiple choice problems and I pointed out how with gases at the same T and P, volume ratios could be considered the same as mole ratios.

Wednesday: Today we started out finishing the multiple choice questions in your packet as well as predicting reactions, recalling net ionic and drawing pics.  The biggest takeaway is that metals are always solid and do not have charges and do not dissolve when mixed with water (they react, but are not soluble in their elemental, non-ionized, form).  Also when drawing gases, make sure to draw them outside the beaker.  Next we went over Dalton’s law of partial pressure and did the more advanced calculations involving mole fraction, collecting a gas over water and what pressure and volume to use in PV=nRT when you have a mixture of gases.  For the last 20 minutes you planned the next design lab.  The goal is to design a lab to measure R for two different gases and to see that the R’s are the same for different gases and to compare to accepted value.  Today’s notes (including answers for MC) are here.

Thursday, Friday:   Design lab

Monday: Finish lab/ Review

Wednesday: Test

Monday: Your goal is to figure out which alkali metal it is.  As a group you will write procedures that will both explain the procedures and the calculations behind the procedures.  You will do the lab on Monday and hopefully have enough time to do the calculations. Homework will be to write a conclusion.  Grades will be: Data Collection, Experimental methods (grade based on procedures and evaluation of procedures), and Math.  Notes and lab instructions.

So for Methods/Error Analysis make sure you:

• Calculations
  • Show work/ justify with words as you go along like you did on mixtures lab
  • Justify number of sig figs in final molar mass.
  • Calculate percent error.
    • Sample 1 was Na
    • Sample 2 and 3 were K
•  Procedures
  •    Say what you are doing (steps),
  •    why you are doing it that way (rationale for choices),
  •    how you will get an answer (calculation), including plan for certain sig figs
• Error Analysis/Conclusion
  • Limitations of method/equipment/conclusions,
  • discussion of variability (precision…number of decimal places since you don’t have multiple trials) and accuracy (percent error) of the data that is justified
    • State the error
    • Determine whether it was random or systematic and justify this
    • What effect did the error have on the results – in detail. Do math if necessary. Do not just say it would throw off the result. Give an example.

Lab due MONDAY October 26th.

Tuesday: Review for test

Wednesday: Test.  Homework is to work on conclusion (nevermind about videos)

Thursday: Gas laws notes and practice.

Homework:  Make sure you do #5.119 before class tomorrow!

• Gas laws; 5.39-5.49 (odd only)
• 57, 59, 73, 117,119 (ideal)
• 5.63, 67, 69, 71 (molar mass and density)

Friday: Today we are going to start with learning other reactions that produce a gas then do the baggy challenge. Next we will get into kinetic molecular theory including real vs. ideal gases. Here’s the notes.

Homework: finish conclusion and other textbook problems (5.27,28, 33, 142, 21, 22, 23)

Monday: No school – Columbus Day

Tuesday: Today we went over gravimetric analysis (see videos on unit 2 page if you missed them or need help).  I showed you how vacuum filtration works and we did the lab based problem on page 22 of the packet.  This is actually the answer, but we just covered up the answer and went through the problem on a separate sheet of paper. The rest of class you worked on other gravimetric analysis problems 4.83, 4.85, 4.87.

Wednesday: No class cuz you were all taking the PSATs

Thursday: Today we started by going over the terms saturated, unsaturated, soluble, insoluble and partially soluble – and drew pictures for them. The key to showing the difference between saturated and unsaturated is to know the solubility limit of the compound.  If there’s a lower molarity than the solubility limit = unsaturated, if = molarity to solubility limit = saturated.  Saturated solutions are easy to detect if enough has been mixed that a precipitate has formed.   Then we worked on practice problems in the packet – pages 15 and 16.  3 answers on page 16 are wrong on the key (key is on page 23).  The net ionic reaction for #9, 10 and 11 should have the solids in them since solids are included in net ionic reactions.  When I wrote the answer key I wrote the net ionic rxns as if they solids were aqueous. So here’s the answer for number 12) Fe(HCO₃)₃ + 3H⁺(aq) –> 3H₂O(l) + 3CO₂(g) + Fe³⁺(aq)

Homework: Neutralization problems: 4.31, 89, 91, 93 and rest of gravimetric analysis problems: 4.115, 4.117, 4.119

Friday: Today we are going to start with page 19 in your packet…multiple reactions and mole ratios! It turns out that you can string mole ratios from one reaction to another reaction, you can multiply reactions times a coefficient and you can add reactions together.Then your goal is to write procedures for a lab…here’s the premise: I am going to give you a sample of an alkali metal carbonate – basically a white powder that you know has a carbonate ion and an alkali metal ion, but you don’t know which alkali metal it is.  Your goal is to figure out which alkali metal it is.  As a group you will write procedures that will both explain the procedures and the calculations behind the procedures.  You will do the lab on Monday and hopefully have enough time to do the calculations. Homework will be to write a conclusion.  Grades will be: Data Collection, Experimental methods (grade based on procedures and evaluation of procedures), and Math.  Notes and lab instructions.

Monday: Review for the stoichiometry test tomorrow.  We started with homework problems and it became apparent that most of you had not done much limiting reactant work so we started going over the first problem on the limiting reactant section.  This was helpful because some of you were thinking of this in terms of atoms rather than molecules…you must use mole ratio, can’t just total up all the atoms of each type and then figure out the limiting reactant since reactions won’t always occur like that.  I also showed 3 different ways for figuring out excess and then asked you guys to write down your preferred method.  The rest of class we worked more LR problems.  In the last few minutes we did a combustion analysis problem just to refresh your memory.

Tuesday: Test on stoichiometry.

Homework: Dilution and molarity videos. The first two listed are the ones I think you need to watch even though you’ve seen 2.b.1.5.   The next 3 are only if you truly don’t remember molarity at all or have difficulty calculating the number of ions from the moles of an ionic compound (like how many moles of nitrate ions in 54.0 g of Cu(NO3)2?)

• 2.b.1.4 Molarity of ions
• 2.b.1.5 Dilutions (from first year chem)

Watch these three only if you need them!

• 2.b.1.1 Intro to Solutions (From first year chem – if you want to review vocab like solute and solvent.  Molarity is introduced near the end.)
• 2.b.1.2 Molarity (from first year chem, just shows the math for various problems, but doesn’t explain what molarity is)
• 2.b.1.3 Moles of ions (This is not about molarity, but is about using subscripts to determine moles of ions something you will need to do molarity of ions)

Wednesday: 

Today we reviewed the process of dissolving for both ionic and covalent compounds and I gave the definition of electrolyte.  We worked on 4.20 in the textbook which unlike last year was not confusing at all…no one had any questions really.  So the rest of class we worked on various molarity and dilution problems including  showing how to solve various problems.  Notes from last year (which have a bit more detail as I had to review a number of concepts that we didn’t have to review this year) are here.  Notes from this year are here.

• basic molarity (but see chem 1 videos for more if you need it)
• molarity w/ multiple solutions
• dilutions
• molarity mixing two solutions
• dealing w/ mass percent.

Homework: textbook problems and packet (page 1 on molarity of ions, page 2 on molarity w/ multiple solutions and dilutions)

Thursday: We started by learning to prepare solutions using volumetric flasks and then you prepared calcium chloride and sodium oxalate solutions in preparation for lab tomorrow.  The rest of class you spent reviewing naming acids rules and practicing.

Friday: Today we started by predicting double displacement reactions including two special types: neutralization and acids with carbonates. We went over complete ionic, net ionic, spectator ions and  and drawing pictures. Here’s the notes. Second half of class you completed the chemical formulas lab (will need to be logged in to APS google to open).

Homework: write-up

Monday: You took your 1b test on moles and formulas and then we did some review of percent yield.

Homework: watch video 2.a.3.1.  If that one doesn’t work, watch 2.a.3.2, 2.a.3.3, 2.a.3.4 all found on unit 2 page.  Try problem 3.93 from the end of chapter 3 in your textbook.

Tuesday: Limiting reactant demo and LR practice in the packet.

Wednesday: Micromole rockets lab

Thursday: Green chem pre-lab

Friday: Green chem lab – first part of class you got into mixed groups and presented the 3 different ways of doing the calculations. Then you went and did the lab and many had time to do the calculations. Write up is to do calculations only.  No conclusion. Percent purity was 84.58% (actual value).   Remember to show your logic as you are doing the calculations!

Monday: Avogadro lab.  Hopefully there will be enough time to talk through the conclusion so you won’t have so much to do tonight!

Tuesday: The plan is to go over the grading system so you guys are clear on what you need to do to get an A, B, etc. and so that you can understand how to interpret your grade in activegrade.com. Then we’re going to do some empirical and molecular formula problems and explain them at the molecular level. But we didn’t do this… instead we worked on the calculations for the Avogadro lab since many of you weren’t sure about them.

Homework: Hydrate video

Wednesday: I realized that an important key in explaining/justifying calculations is starting with the definitions/properties of atoms and molecules. So we started with a brainstorm of these.  Here’s the notes which went over empirical and molecular formulas as well as hydrates and most importantly, their justification at the molecular/atomic level!

HW: Textbook problems / finish lab

Thursday: No class b/c it was short and A block was cancelled.

Friday: We did some challenge problems for A block, making sure to learn to do them in 2 ways and be able to explain all the different methods.  During B block we went over determining empirical formula using combustion analysis. Video here:

• 1.b.3.4 Empirical Formula from Combustion Analysis (for AP! but there is a typo! The compound is not made of C, O and N, but C, H and N. On Youtube)

Homework: Study for moles and formulas test on Monday