AP+'Must-knows'

Here's a list of things that we MUST know both in the short term (chapter/unit tests) and for the long term (AP exam).

At best, this is a work in progress--I'll add to it as it occurs to me, but ideally YOU should be making such a list for yourself and adding to it as you see fit.

From our Ch. 5: a molecule ||= Write this as ions ||
 * **__Solubility Rules__**--You must have them memorized. Start with the "always-always-always" soluble ions, then work on the "usually soluble" ions (know the exceptions), and finally the more quirky ones. Hint: If you know the "always soluble" anions and cations, that'll carry you through many/most of the problems. If you want to get through //**all**// the problems, learn better!
 * __**IDs of strong acids and strong bases**__--Again, to be memorized. There are 6 strong acids you want to know: three binary SA's (HCl/hydrochloric, HBr/hydrobromic, HI/hydroiodic), and three ternary SA's (HNO 3 /nitric, H 2 SO 4 /sulfuric, HClO 4 /perchloric). By correctly ID-ing an acid as strong, we can correctly treat it in net ionic equations. The strong bases include all hydroxides of 1A metals (MOH), and Ca(OH) 2, Sr(OH) 2 , and Ba(OH) 2 . I suppose that all metal hydroxides are strong, but only these are soluble--Again, this tells us how to treat them in a net ionic equation.
 * You should know how to __**predict products/write equations for the reactions of metal oxides in water, as well as of nonmetal oxides in water**__. Strive to know these generically, so that you learn to approach the reactions of CaO, Na 2 O, and BaO with water almost as if they're all the same.
 * __**Acid-Base reactions**__--For now, we're not getting too detailed, but what are the products (generically speaking) of an acid-base reaction?
 * __**Gas-forming reactions**__--We've got 5 in our text. Learn these (getting the theme here?) generically, so that you can apply this understanding to many possible reactions that fit. One example: A metal sulfite reacts with a strong acid to give SO2 gas, water, and a salt. Knowing this, you should be able to write formulas for all products for the reaction of __**any**__ metal sulfite with __**any**__ strong acid. Gases given off include SO 2, H 2 S, CO 2 , and NH 3.
 * Net ionic equation rules: Here you get to apply your expertise about salt solubility, IDs of strong/weak acids, strong/weak bases to show what form chemical species exist in during a reaction, as well as which species undergo change. You've got to know how to treat these species as they exist--put an "x" in the correct column for each type of species (did I miss any type of species that should be included?)
 * =  ||= Write this as
 * Strong Acid ||  ||= X ||
 * Weak Acid ||= X ||  ||
 * Strong Base ||  ||= X ||
 * Weak Base ||= X ||  ||
 * Soluble Ionic Compound ||  ||= X ||
 * Insoluble Ionic Compound ||= X ||  ||
 * Molecular Gas in Water ||= X ||  ||
 * Soluble Molecule in Water ||= X ||  ||
 * Molecular Liquid in Water ||= X ||  ||

= C o l o r s : I file this under "Chemistrivia" because it seems sort of random and doesn't have a set place in our curriculum where we learn it.= First: Many many transition metal ions make colored compounds. Compounds with Permanganate (MnO 4 -1 ) are PURPLE : KMnO 4, NaMnO 4 Compounds with Chromate (CrO 4 -2 ) are YELLOW : K 2 CrO 4 Compounds with Dichromate (Cr 2 O 7 -2 ) are ORANGE : (NH 4 ) 2 Cr 2 O 7 Na 2 Cr 2 O 7 Compounds with copper ions (Cu +2 or Cu +1 ) are generally BLUE CuCl 2 Cu(NO 3 ) 2 CuSO 4. 5H 2 O Compounds with Nickel ions (generally Ni +2 ) are GREEN : NiCl 2

2nd: Some elements are colored: Chlorine is a greenish gas Iodine is a dark solid that when heated sublimes to become a violet vapor Bromine is a orangey liquid at room temperature.

You //must// know at least half of all of the references made in class, and //must// have complete knowledge of the //__Back to the Future__ Trilogy.//