Solubility Rules, Reaction Prediction, & All the Stuff I Should Know Reference Sheet for AP ChemistrySolubility For the AP Chemistry exam you need to have memorized the following: Six Strong Acids = SA o The 6 SA are soluble, meaning the weak acids = WA may not be 100% soluble. Strong Bases = SB o The SB are soluble while the weak bases = WB may not be 100% soluble. Soluble Substances (dissolve in aqueous solution) Insoluble Substances (will not dissolve in aqueous solutions or will form precipitates) The weird substances that do not follow regular rules, but are soluble. Strong Acids or the BIG 6: Acronym P.I.N. C.B.S. 1. P = perchloric acid = HClO4 2. I = hydroiodic acid = HI 3. N = nitric acid = HNO3 4. C = hydrochloric acid = HCl 5. B = hydrobromic acid = HBr 6. S = sulfuric acid = H2SO4 Strong Bases: Note these are Group 1 (Li to Cs) & Group 2 (Ca to Ba) metals. All other bases are WEAK. 1. 2. 3. 4. 5. LiOH NaOH KOH RbOH CsOH 6. Ca(OH)2 7. Sr(OH)2 8. Ba(OH)2 Always Soluble: 1. 2. 3. 4. All metals in Group 1 (unless with O2-) NH4+ (no exceptions) NO3- (no exceptions) C2H3O2- (sometimes written as CH3COO-) Insoluble or Not Aqueous: Halogens/Halides are soluble with all elements/polyatomics unless they get “SLaMmed” into a precipitate. 1. S = silver = Ag. Example AgCl = solid/insoluble/ppt. 2. L = lead = Pb. Example PbCl2 = solid/insoluble/ppt. 3. M = mercury = Hg. Example HgCl2 = solid/insoluble/ppt. Sulfates are soluble unless they get “CaBaSr SLaMmed” into a precipitate. 1. Ca = CaSO4 = solid/insoluble/ppt. 2. Ba = BaSO4 = solid/insoluble/ppt. 3. Sr = SrSO4 = solid/insoluble/ppt. Phosphate (PO43-) & Carbonates (CO32-) are INSOLUBLE except with group 1 & NH4+. Sulfides (S2-) are INSOLUBLE except with group 1, 2, & NH4+ Weirdo’s: These substances do not follow regular rules, but they are soluble and break down accordingly. 1. NH4OH NH3 + H2O 2. H2CO3 CO2 + H2O 3. H2SO3 SO2 + H2O Solubility & Equation Ref Sheet for AP chem 5-2010 1 public. 8. Sodium Acetate is dissolved in water. See Na+ & Cl.+ H+ H2O (Net Ionic equation: spectator ions are crossed out.htm 9.(complete ionic equation) 3. just like something that is soluble.+ H2O HC2H3O2 + OH. When writing equations do not leave them together as a compound. 5.(NET IONIC EQUATION) Types of Equations to Know 1. i. Another Example of Net Ionic Equations: i. SA Example: HCl(aq) is really H+ + Cl2.General Information for Writing Equations 1. Na+ + Cl. a.in step 2 of the example above. Na+ + OH. instead separate them into ions. Example of a net ionic equation: i. SA & SB completely dissociate. Weak Acid Example: H2SO3(aq) H2SO3 3. Na+ + C2H3O2.+ H2O HC2H3O2 + Na+ + OH. Complete the equation in net ionic form. sodium hydroxide and hydrochloric acid are mixed 1.+ H2O (equation with soluble ions & insoluble items) 3. Redox Solubility & Equation Ref Sheet for AP chem 5-2010 2 . 4. NaC2H3O2 + H2O HC2H3O2 + NaOH (starter equation) 2. Interesting website: http://www.asu. they are like fans on the sidelines. They do not participate in the reaction. Weak Base: Cu(OH)2 Cu(OH)2 d.edu/~jpbirk/CHM-115_BLB/Chpt24/sld018. These ions are equal & on opposite sides of the arrow and therefore can be crossed out.+ H++ Cl. 1. so they are cancelled out. 3. only substances involved in reaction are remaining. 1. Strong Acids & Strong Bases i. 6. Note that acetic acid is a WA so it does not break up into ions. 2. Decomposition: AB A + B Synthesis (combination): A + B AB Combustion: Hydrocarbon + O2 CO or CO2 + H2O Single Replacement: A + BC AC + B Double Replacement – precipitate (also called metathesis): AB + CD AD + CB Double Replacement – neutralization (acid + base salt + water) Double Replacement – hydrolysis (water + a salt ) Coordination Compound/Ligand type reaction a. Spectator Ions = the ions that do not participate in the reaction. NaOH + HCl NaCl + H2O (full equation) 2. C2H3O2. 7. iii. SB Example: LiOH Li+ + OH4. ii. c. OH. b. Net Ionic Equations –be able to write all equations as net ionic equations. Ammonium hydroxide NH3 + H2O i. (NH4)2CO3 NH3 + CO2 + H2O d. H2O2 H2O + O2 j. H2CO3 CO2 + H2O f. Synthesis Reactions a. which means you do not necessarily need to know the chart. A single element that is more reactive will replace an element in a compound. This is both a single replacement and a redox reaction since electrons were transferred. Complete: hydrocarbon + O2 CO2 + H2O b. H2SO3 SO2 + H2O e. Ca(OH)2 CaO + H2O h. Decomposition Reactions a. Binary compounds two elements i. Although. b.Equations in Depth 1. Example: NaCl + AgNO3 NaNO3 + AgCl i. Ag + Cl2 AgCl b. Nonmetal oxide + H2O an acid i. Metal oxides + H2O a base i. Solubility & Equation Ref Sheet for AP chem 5-2010 3 . This is where you need to know the solubility rules and how to write net ionic equations. KClO3 KCl + O2 c. Base metal oxide + H2O i. Combustion a. Sulfurous acid acid SO2 + H2O i. 5. SO2 + H2O H2SO3 3. Ammonium carbonates NH3 + CO2 + H2O i. Net ionic form: Cl-(aq) + Ag+(aq) AgCl(s) 1. H2SO4 SO3 + H2O g. b. NH4OH NH3 + O2 2. Hydrogen Peroxide H2O + O2 i. CuO + H2O Cu(OH)2 c. In net ionic form: Li + Ca2+ Li+ + Ca 2. Carbonates CO2 + metal oxide i. Li + CaCl2 LiCl + Ca 1. Double Replacement Precipitate a. Note this is also a redox reaction. H2O H2 + O2 i. Carbonic acid CO2 + H2O i. i. Metal + Nonmetal a salt i. Chlorates metallic chloride + O2 i. Single Replacement a. Na2CO3 CO2 + Na2O b. Acids in general nonmetal oxide + water i. the reactions they put on the exam generally take place. Incomplete: hydrocarbon + O2 CO + H2O 4. A reactivity sheet is not supplied on the AP exam. in a compound. Example: Cu2+(aq) + NH3(aq) [Cu(NH3)4]2+(aq) a. Double Replacement Neutralization a.6. This occurs when a salt reacts with water. H2O b. Strong Acid + Strong Base create a neutral product d. Know these Ligands (electron pair donors) i. Fe. OHc. Cu. CN-. basic. i. complex ions or coordination compounds are formed. Ag(NH3)2+ 2. How do you figure out the number of ligands & the final charge? i. HCl + NaOH NaCl + H2O 1. e. Cd(CN)323. What the Ligands might bond with: i. Fe(CN)63+ d. Ammonia: 1. whichever is greater dictates the pH. Multiple this oxidation number by 2 and this gives you the number of ligands to add to the cation. or neutral product depending upon the Ka & Kb. Find Overall Charge: 1Cu2+ + 4NH30 = 2+ 2. b. CN iii. Zn(OH)423. NH3 (ammonia or amine) ii. Ag(CN)22. 1. Cu(NH3)42+ 3. Hence. Cyanide: 1. This electron pair bonds to a central atom. Zn. Example: Sodium Acetate is dissolved in water: NaC2H3O2 + H2O HC2H3O2 + NaOH 1. Find # ligands: (2+)x2 = 4 b. You will lose points on the AP exam if the charge does not correctly add up. Hydroxide: 1. Another Example: NH3(aq in excess) + Cu(OH)2(s) [Cu(NH3)4]2+(aq) + OH-(aq) a. Ni.+ H2O HC2H3O2 + OH8. The IMPORTANT part is the FINAL CHARGE on the complex ion. Cr(OH)63iii. Some salts just dissolve and some salts react with the water. which means they are Lewis Bases. Common Lewis Bases (act as ligands or the electron pair donor): i. Net Ionic Equation: C2H3O2. Al(OH)42. Acid + Base Salt + Water i. Strong Acid + Weak Base create an acidic product e. SCNSolubility & Equation Ref Sheet for AP chem 5-2010 4 . Ag. Ni(NH3)62+ ii. These complex ions tend to be rich in color. 7. Find the oxidation number of the cation. Double Replacement Hydrolysis a. NH3. Coordination/Ligand Type Reactions a. Co. Key Word – in excess. Common Lewis Acids (act as the ligand acceptor or electron pair acceptor): i. Net Ionic Form: H+ + OH. usually the cation of a transition metal. What is a ligand? Ligands are electron pair donors. Weak Acid + Strong Base create a basic product c. Weak Acid + Weak Base can create an acidic. Cr. OH-. Al f. ii. Halide ions ii. HClO4 xii. N. Cl. Cr2O7 in acidic solution v. MnO2 in acidic solution iii. H2O2 Products Formed Mn2+ Mn2+ MnO2 Cr3+ NO2 NO SO2 Metallous ion (lower oxidation #) Halide ion NaOH ClCO2 O2 or H2O b. Metallous ions (lower oxidation #) Products Formed Free halogens/halides = diatomic Metal ions sulfate ions (SO42-) nitrate ions (NO3-) hypohalite ions (Br2 BrO-) halite ion (Cl2 ClO2-) metallic ions (higher oxidation #) Polyatomic Ions To Know These are not the only polyatomics to know. but at least it’s a start! 1C2H3O2BrO3ClOClO2ClO3ClO4CNHCO3HCOOpermanganate MnO4nitrite NO2nitrate NO3hydroxide OHbisulfite HSO3thiocyanate SCNiodate IO3acetate bromate hypochlorite chlorite chlorate perchlorate cyanide bicarbonate formate carbonate dichromate chromate manganate oxalate silicate selenate sulfite sulfate 2CO32Cr2O72CrO42MnO42C2O42SiO32SeO42SO32SO42- borate phosphate phosphate 3BO33PO33PO43- ammonium hydronium 1+ NH4+ H3O+ Diatomic elements to Memorize H. MnO4. O. Diatomic halides in conc basic soln vii. C2O42xiii.in neutral or basic solution iv. Common Reducing Agents (loss electrons) i.9. Metallic ions (higher oxidation #) ix. HNO3 concentrated vi. HNO3 dilute vii. Oxidation & Reduction a. Free Halogens x. BrINClHOF = ClOBr H. Diatomic halides in dilute basic soln vi.in acidic solution ii. Common Oxidizing Agents (gain electrons) i. FIN (clobber Huck Fin) Solubility & Equation Ref Sheet for AP chem 5-2010 5 . Nitrite ions (NO2-) v. F. Na2O2 xi. MnO4. H2SO4 hot concentrated viii. and I = HNOFClBrI = Dr. Br. Sulfite ions or SO2 iv. Free metals iii. 1. 2. Alcohol: R – OH 6.3 and.4 = para Functional Groups 5. Ketone: 8. Aldehydes: 7.Other Things to Add to Your Study Note Cards Free Energy G = – # = Spontaneous G = + # = NOT spontaneous G = 0 = Equilibrium You can remember the following with this: Go Home To Supper: Ho So Go Ho Go Ho So So – + – + – + + + Spont. Substituted Benzene: ortho = 1. Amide: Solubility & Equation Ref Sheet for AP chem 5-2010 6 . 4. Amine: R – NH2 12. Alkanes: CnH2n + 2 Alkenes: CnH2n Alkynes: C2H2n-2 Aromatics (benzene) C6H6 a. meta = 1. Carboxylic Acid: 10. Ether: R – O – R 9.2. 3. Ester: 11. only @ high Temps – – Spont only @ low Temps Organic Chemistry General Organic Chemistry 1. Examples: CH4. C(graphite). Hybridization. 3 = f Steric Number.O. Examples: H2S. WC. etc. & Shape Steric Number Hybridization Basic Shape 1 s ------------------ 2 sp linear 3 sp2 trigonal planar 4 sp3 tetrahedral 5 sp3d trigonal bipyramidal 6 sp3d2 octahedral Bond Orders Bond B. CaCO3. SiC. Strontium = red 6. Barium = Green Sodium = yellow Copper = blue (w/ green) Potassium = lavender 5. 2. C(diamond). Note: graphite = London dispersion too. Pb. Lithium = red 7. SO2 H-F.Flame Test Colors 1. H-O-. -1/2 0 = s. H-N-. Ag. 1 = p. H2O Jmetals. 2 = d.3… 0…. 4. 3. 2. = bond order Type of bonds involved single 1 sigma = σ double 2 sigma + pi or σ + π triple 3 sigma+ pi+pi = σ+π+ π Intermolecular Forces (IMF’s) London dispersion dipole-dipole Hydrogen bonding metallic ionic covalent network Solubility & Equation Ref Sheet for AP chem 5-2010 Nonpolar molecules.(n-1) -l to +l (small letter L) +1/2. Note: “ates” contain covalent bonds. SiO2. He polar molecules. NaCl. 7 .. Calcium = orange Quantum Numbers n l ml ms l 1. NH3. salts. Si. Zn + 2HCl H2 + ZnCl2 Oxidizing Acid.+ H2 Non-oxidizing Acid. Ag.enter 8 . Time slope = -k 1st Order ln[R] vs Time slope = -k 2nd Order 1/[R] vs. Pt.Activity of Metals (Four Groups) Metals Groups I & II All others React with… H2O. Time slope = k Nuclear Chemistry Alpha 4 2 Beta/Electron 0 1 He e Neutron 1 0 n Positron 0 1 e Electrochemical Cells Anode oxidation -side lower Eo e. Hg Au.leave Solubility & Equation Ref Sheet for AP chem 5-2010 Cathode reduction +side higher Eo e. Ir Orders of Reactions & Graphs that give STRAIGHT LINES (kinetics) 0-Order [R] vs. Ex: HCl.) Cu + HNO3 NO2 + H2O + Cu2+ Aqua Regia (HNO3 + HCl) Cu. Ex: Li + H2O Li+ +OH. HNO3 or H2SO4 (conc.