University:
Winston-Salem Forsyth County Schools
Course:
AP Chemistry
Academic year:

2009
Views:

111

Pages:

1
Author:

gynhennaubtb

STUFF I SHOULD KNOW FOR THE AP TEST BUT DO NOT KNOW YET IONS LIST acetate aluminum ammonium barium bicarbonate bisulfate bisulfide bisulfite bromate bromide bromite calcium carbonate chlorate chloride chlorite chromate chromium cupric cuprous cyanide dichromate C2H3O2– Al3+ NH4+ Ba2+ HCO3– HSO4– HS– HSO3– BrO3– Br– BrO2– Ca2+ CO32– ClO3– Cl– ClO2– CrO42– (yellow) Cr3+ Cu2+ (blue) Cu+ (green) CN– Cr2O72– (orange) ferric ferrous fluoride hydrogen hydronium hydroxide hypobromite hypochlorite hypoiodite iodate iodide iodite lead lithium magnesium manganese mercuric mercurous nickel nitrate nitride nitrite Fe3+ (yellow) Fe2+ (green) F– H+ H3O+ OH– BrO– ClO– IO– IO3– I– IO2– Pb2+ Li+ Mg2+ Mn2+ Hg2+ Hg22+ Ni2+ (green) NO3– N3– NO2– oxalate oxide perbromate perchlorate periodate permanganate peroxide phosphate phosphide phosphite potassium silver sodium stannic stannous strontium sulfate sulfide sulfite thiocyanate thiosulfate zinc C2O42– O2– BrO4– ClO4– IO4– MnO4– (purple) O22– PO43– P3– PO33– K+ Ag+ Na+ Sn4+ Sn2+ Sr2+ SO42– S2– SO32– SCN– S2O32– Zn2+ SOLUBILITY RULES STRONG OXIDIZERS (Oxidizing Agents) Always soluble: alkali metal ions (Li+, Na+, K+, Rb+, Cs+), NH4+, NO3–, ClO3–, ClO4–, C2H3O2– MnO4– in acid solution MnO2 in acid solution MnO4– in neutral or basic sol’n Cr2O72– in acid solution Cr2O72– with a base CrO42– in basic solution HNO3, concentrated HNO3, dilute (e.g. 6 M) H2SO4, hot, concentrated Free halogens (e.g. Cl2) H2O2 in acid solution Note: H2O2 decomposes Na2O2 HClO4 Generally soluble: (mnemonics) Cl–, Br–, I– Soluble except Ag+, Pb2+, Hg22+ (AP/H) F– Soluble except Ca2+, Sr2+, Ba2+, Pb2+ , Mg2+ (CBS-PM) SO42– Soluble except Ca2+, Sr2+, Ba2+, Pb2+ (CBS/PBS) Generally insoluble: O2–, OH– Insoluble except alkali metal ions and NH4+ Ca2+, Sr2+, Ba2+ (CBS) somewhat soluble CO32–, PO43–, S2–, SO32–, C2O42–, CrO42– Insoluble except alkali metals and NH4+ GASES THAT FORM  H2CO3  CO2 + H2O  NH4OH  NH3 + H2O  H2SO3  SO2 + H2O  H 2S  HNO2  NO + NO2 + H2O  HCN WEAK ELECTROLYTES Weak Acids (esp. HC2H3O2 and HF) (Memorize the 8 strong acids… all others are weak) HCl hydrochloric acid HNO3 nitric acid HBr hydrobromic acid HIO4 periodic acid HI hydroiodic acid H2SO4 sulfuric acid HClO4 perchloric acid HClO3 chloric acid Ammonium Hydroxide (NH4OH  NH3(aq)) Water (H2O) DRIVING FORCES –– Double Replacement    Insoluble Solid (Precipitate) Weak Electrolyte (H2O or Weak Acid) Gas Formation  Mn2+ + H2O  Mn2+ + H2O  MnO2  Cr3+ + H2O  CrO42– + H2O  CrO2– + H2O  NO2 + H2O  NO + H2O  SO2 + H2O  halide ions (Cl–)  H2O  H2O + O2  NaOH  Cl– + H2O Other Oxidizers Metal-“ic” ions (e.g. Sn4+, Fe3+)  “-ous” ions (Sn2+, Fe2+) H2 O  H2 + OH– STRONG REDUCERS (Reducing Agents) Halide ions (e.g. Cl–)  Free halogen (Cl2) Free metals  metal ions “ites” SO32– or SO2, NO2–  “ates” SO42–, NO3– Free halogens, dil. basic sol’n  hypohalite ions (ClO–) Free halogens, conc. basic sol’n  halate ions (ClO3–) S2O32–  S4O62– Other Reducers Metal-“ous” ions (e.g. Sn2+) H2 O  “-ic” ions (Sn4+)  O2 + H +