Timeline for IAs 2017-18 -rev1

2017-18 Summary of Experiments Taken & Good Ideas Still Available:

Excellent, IB-appropriate library of procedures from the Royal Society of Chemistry (this one was shared on the summer assignment):

Vernier Chemistry Experiment Ideas (pre-programmed with instructions for probes):

Massey Chem is awesome! http://masseychem.weebly.com/ib-candidates.html
IA Overview from Massey Chem:
IA Report Guidelines from Massey Chem:
IA Scoring from IB Chem Guide:

IA Frequently Asked Questions (VERY HELPFUL!):

OLD but possibly useful IA Guide with checklist:

Sample IA's with Moderator Comments available, etc.

(Here you may browse through 10 official sample lab reports!):

Especially note the example Database IAs to see how their presentation & grading differs from that of the experimental IA's.

Ideas for IA Research Questions or Areas (most still need to be narrowed and focused):
From Massey Chem:
Assorted other ideas (some from Ms. Clewett- click tab at bottom for "Ideas if you are stuck"):
Some recent brainstorm favorites from Ms. Clewett for 2017-18:

How does the location of a double bond in a long, straight-chain alkyne (5-15 carbons) affect the boiling point of the alkene? (Use simulations to model the geometry of the alkene and databases such as PubChem, NIST, ChemSpider, etc. to obtain the boiling point information. (Note: Ms. Clewett had this idea when she was preparing slide 11 of the 8-8-17 PPT noticed the significant difference in boiling point between pent-1-yne and pent-2-yne; she wanted this to be an investigation of alkynes, but there don't seem to be as many of them in existence as there are of alkenes, so the RQ had to be modified from its original plan.)

How does the temperature/particle size/concentration of x affect the rate of reaction, for a reaction between (...)? MUST follow up stating that an increase is expected due to theory (for increasing temp or concentration OR for decreasing particle size) but whether the increase is linear, quadratic, exponential, etc. (or if it is necessarily a regular progression at all) is of interest to determine.
(Ways to determine rate of reaction must be considered and method be tested/verified during trial run. Things that change color, change pH, produce a precipitate, produce a gas, or change the total number of "free" ions present-conductivity of solution-are all workable here. Things that change temperature are okay here but may be better as calorimetry investigations.)

How is temperature change (and, by extension, enthalpy of reaction) affected by (...) in the reaction of (...)?
One option: q = m c {delta}T suggests a linear relationship, but can that relationship be confirmed for varying quantities of limiting reagent, up to and including stoichiometric equivalence (or even beyond that)?
Another option: for standard enthalpy of reaction, part of the standard conditions include one molar concentrations. How consistent are calculated values of enthalpy for {specify range of concentrations}?
Curious: when there is one, solid state limiting reagent and a solution of excess reagent, does the temperature change seem more proportional to the mass of the solution by itself or the total mass of all reactants? (IB markschemes have shown both methods of calculation to be acceptable)

How is percent yield affected by (temperature, molar ratios of reactants, volumes of solution, ...) in a reaction of (...)
It is expected that some loss will occur,

HL: effect of baking soda on pH of simulated blood buffer system (home remedy for colds, etc.)

HL: effect of temperature on solubility

How does pressure respond to temperature for a real gas (CO2, etc.)? Can R be calculated? How similar is the curve to ideal gas line? Are variations consistent w/ literature predictions?

Simulations - bond strength is said to increase with increasing polarity of the bond - is this a consistent, linear effect & can it be shown

Also: Reactivity in molecular crystals
Hydrogen bonds' role in molecular crystals and/or (density of solids) < (density of liquids) for other hydrogen bonded substances besides water and/or if hydrogen bonds are responsible for water being a liquid at room temperature, why are both pure ammonia and pure hydrofluoric acid gases at room temperature?

RSC Learn Chemistry website w/good start-off-your-preliminary-trial procedures (new links for Wooster students, for 2017-18):
Baby steps: http://www.rsc.org/learn-chemistry/wiki/Lab:List_of_introductory_level_Practical_Chemistry_experiments
Experiments for high school students: http://www.rsc.org/learn-chemistry/resource/listing?searchtext=&filter=all&fLevel=LEV00000005&fMediaType=MED00000006

IA Checklists - misc. sources
One source:

A second source:
Chemistry SL - IA - Checklist_2016_.pdf
Chemistry SL - IA - Checklist_2016_.pdf
Chemistry SL - IA - Checklist_2016_.doc
Chemistry SL - IA - Checklist_2016_.doc

"Lab writing hints"

Additional Resources:
Curious Curie: http://ibchemistryinvestigation.curiouscurie.com/
Haiku Learning: https://bsm.haikulearning.com/morourke/ibchemistry2016/cms_page/view/14765089
App (free download): smartib (for students, by students)

Biodiesel lab:
Biodiesel Lab.docx
Biodiesel Lab.docx