<p>I went all the way back to 2007 for my FRQ’s because that is when I think (not sure) they started doing only three reactions for Q.5. I would highly stress practicing reactions, really easy way to boost your score considering they’re sooo easily memorized and worth 10% of your score. Could easily get you into that FIVE range if you’re consistent with MC.</p>
<p>We’ve been using three of those sites in the [Study</a> Guide Thread](<a href=“http://talk.collegeconfidential.com/sciences/1492199-official-ap-chemistry-exam-study-thread-2012-2013-a.html]Study”>http://talk.collegeconfidential.com/sciences/1492199-official-ap-chemistry-exam-study-thread-2012-2013-a.html).</p>
<p>@Niquii77 Oh okay! Thanks for referring me to that thread!</p>
<p>Are molecular orbitals generally on the test? On one practice test, I saw them on there as a MC. Is it worth to review them?</p>
<p>I would say YES! They are definitely worth it to review!</p>
<p>Especially hybridization; sometimes CB throws in a hybridization question on their FRQ 5 & 6; it’s to your advantage to maximize point totals.</p>
<p>What are you predictions for the FR for the coming Monday?</p>
<p>How does one practice those reactions, mentioned by Cindy11052 (Post #121)? Is there any guide for that? I think PR has something for that. I know Combustion fairly well, but is there any good explanatory guide for predicting those reactions? Also, are there any good guides for how to do well in FRQ in general? I feel that the MC is not so bad, but the FRQ is a bit scary. Guides for FRQ are also appreciated. I’m wondering if there is some resource, maybe khanacademy, that helps with those. Links, suggestions, and concepts appreciated.</p>
<p>Are you talkin about the Question 4 reactions?</p>
<p>A good way if predicting reactions is to know how to do reactions. I suggest leaning the types of reactions and being able to recognize the types. </p>
<p>Chemical Reaction links:
[Chemical</a> Reactions - Types of Chemical Reactions](<a href=“http://chemistry.about.com/od/chemicalreactions/a/reactiontypes.htm]Chemical”>Types of Chemical Reactions (With Examples))
[The</a> Common Types of Chemical Reactions - For Dummies](<a href=“http://m.dummies.com/how-to/content/the-common-types-of-chemical-reactions.html]The”>http://m.dummies.com/how-to/content/the-common-types-of-chemical-reactions.html)</p>
<p>Just posting so it’ll go to my phone. Good luck everyone.</p>
<p>Reviewing experiments?</p>
<p>Any major predictions for the labs… it is so much to review.</p>
<p>Oh and Cindy11052, THANK YOU SO MUCH FOR THOSE YOUTUBE VIDEOS! The third one was super helpful. Unfortunately, I actually learned some of the content for the first time from the video.</p>
<p>i took ap chem last yr and i made an amazing study guide that i cant find,but that made chem teh easiest exam to study for and i got a 5</p>
<p>Just reaction stuff; don’t have a virtual copy of it so I’m going to type it out~</p>
<p>Metal oxide + Water → Metallic Hydroxide
Example: CaO + H2O → Ca(OH)2</p>
<p>Nonmetal oxide + water → nonbinary acid
CO2 + H2O → H2CO3
SO2 + H2O → H2SO3</p>
<p>Decomp: Some of these will be the exact opposite as above!
So…no extra examples
Metallic hydroxide → metal oxide + water
Nonbinary acid → nonmetal oxide + water
nonbinary salt → metal oxide + nonmetal oxide
metallic chlorates → metallic chlorides + oxygen
example: KClO3 → KCl + O2</p>
<p>Whenever electricity is applied to a single reactant, think decomposition…</p>
<p>MEMORIZE the fact that Hydrogen peroxide decomposes into water and oxygen and that it is a common reducing agent.</p>
<p>H2O2 → H2O + O2</p>
<p>Metallic carbonates → metal oxides + carbon dioxide</p>
<p>CaCO3 → CaO + CO2</p>
<p>Ammonium carbonate (whenever ammonium is decomposed from an ionic solid, ammonia forms as a gas, Pungent odor can be observed —AP sometimes ask to describe what occurs)</p>
<p>(NH4)2CO3 —> 2NH3 + CO2 + H2O</p>
<p>Hydrolysis: compound reacting with water.
Watch for soluble salts like NaC2H3O2 (sodium acetate) whose anion is a conj base.
Watch for soluble salts whose cation would be a conjugate acid of a weak base and therefore undergoes hydrolysis.</p>
<p>For example, NaC2H3O2 + H2O…Only the C2H3O2- would react. Na+ is a spectator.
Therefore…C2H3O2- + H2O → OH- + HC2H3O2</p>
<p>Cations, if not spectators, always act as acids.
Anions, if not spectators always perform as bases</p>
<p>General tips: balance by mass and charge! know your oxidation numbers; thats a common after-question on the AP exam</p>
<p>Test the FRQ styles of the rxns using collegeboard examples! until you perfect them</p>
<p>—Continues later, I don’t want a wall of text, but coordinate compounds are next, with leqis base reactions and redox.</p>
<p>For those short on time but wanting to boost your score without the heavy memorization, try this link:</p>
<p><a href=“http://apchemistrynmsi.wikispaces.com/file/view/Very+Last+Minute+net+ionic+attack+strategies+new+format.pdf[/url]”>http://apchemistrynmsi.wikispaces.com/file/view/Very+Last+Minute+net+ionic+attack+strategies+new+format.pdf</a></p>
<p>OKayyyy… Coordinate complex ions.</p>
<p>Usually it involves a lewis base as the second portion of it. A lewis base or ligand are things such as NH3, H2O, OH-, CN-, Cl-. Anything that has an electron pair, WILL SHARE and will be a lewis base. It also involves the central ion, present usually in only one quantity and is the first portion of the equation. Examples of central ions involved are any transition metals and Al3+: like Ag+, Cu2+. Ni2+. Zn2+.</p>
<p>Basically you SMASH them together, and equal up the charges. You don’t have to memorize how many ligands are attached to each central ion, the AP exam will accept your equation as long as its within 1-6 of the attached ligand. Common consensus recommends that you add as much ligands so that it is twice the central ion’s charge.</p>
<p>Exampleee: </p>
<p>Aluminum chloride reacts with EXCESS hydroxide ions. </p>
<p>Therefore:
What is twice of aluminum’s charge? 3x2 = 6 …So attach 6 of the ligands, which is hydroxide. Remember.ligands have an electron pair to share!
Smash them together. 1 aluminum and six hydroxides. Like soooo.</p>
<p>Al(OH)6^3-.</p>
<p>Why is the charge 3-? Add it up Al3+ and 6 OH-… 3+ and 6(1-) → 3 + -6 = -3 is the overall charge.</p>
<p>If the ligand is neutral, like H2O, then the charge of the coordinate complex ion is the charge of the central ion. Example.</p>
<p>Al(H2O)6^3+</p>
<p>Usually the questions have words like “excess, or concentrated.” and</p>
<p>I didn’t quite address redox but an example is like.
The question may be worded as…Solid Manganese flakes are placed in a solution of copper (ii) sulfate. The copper sulfate implies that Cu is in solution, and thus acts as an ion.
Mn + Cu2+ —> Mn2+ + Cu</p>
<p>When these react, Mn is oxidized to Mn2+ and Cu2+ is reduced to Cu</p>
<p>Silly ways to remember flame tests-</p>
<p>Barium is green (Its chemical symbol is Ba. Think of the fact that green implies Beans and Artichoke, and those are green)
Sodium (Yellow…Think of what has a lot of sodium…cheese…which is yellow)
Copper is blue/green (Couldn’t think of one 
…)
Potassium is lilac or lavender (Think abouuutt how K is kind of like a sassy kind of way to text someone, and like how lilac/lavender are sassy colors)
Strontium’s flame test is red. Think Strontium…like STRONG, and red symbolizes dominance.
Calcium - orange…Orange juice is a big source of calcium.
Lithium (red): DO you even lift, yup another source of dominance.</p>
<p>This is how I’m remembering them, because remembering them by rote is just too boring and way too mainstream. Ha.</p>
<p>I’m going to use your color tricks. I love corny memory devices.</p>
<p>Are you memorizing common oxidation states for transition metals for the (potential) redox problem?</p>
<p>@nerdlyfe
I think I am 
I don’t know! I might cram like in the morning for those; there are kind of a lot ;(</p>
<p>Right now I’m trying to look through my notes for Equilibrium. Those are definitely the hardest chapter for me.</p>