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~ combustion analysis CxHyOz + O2 → CO2 + H2O

~ PF3 + BCl3 → F3PBCl3~ metal + nonmetal → ionic salt

2Mg + O2 → 2MgO~ metal + H2O → H2 + OH- + metal ion

2Na + 2H2O → H2 + 2OH- + 2Na+

~ metal oxide + H2O → OH- + metal ion CaO + H2O → 2OH- + Ca2+

~ metal hydride + H2O → H2 + OH- + metal ion~ metal carbonate → CO2 + metal oxide

CuCO3 → CO2 + CuO~ metal sulfite → SO2 + metal oxide~ (NH4)2CO3 → 2NH3 + CO2 + H2O~ 2NaHCO3 → Na2CO3 + CO2 + H2O~ 2H2O2 → 2H2O + O2

~ 2KClO3 → 2KCl + 3O2

~ acid + base → water + ionic salt~ formation rxn

standard state elements → 1 mol compound~ net ionic equation

solubility rules; always soluble: alkali metal ions, CH3COO-, NH4

+, NO3-

usually soluble: Cl-, Br-, I- (except with Ag+, Pb2+, Hg2

2+) usually soluble: SO4

2- (except with Ba2+, Ca2+, Pb2+, Sr2+) usually insoluble: OH-, S2- (except with Ba2+, Ca2+, Sr2+)

strong acids: HCl, HBr, HI, HClO4, HNO3, H2SO4

~ redox rxns▪ Fe + Cu2+ → Fe2+ + Cu

oxidation: loss of e-

reduction: gaining of e-

reducing agent: reactant that oxidizes oxidizing agent: reactant that reduces

▪ more positive standard reduction potential = better▪ how to tell if rxn is redox:

neutral metals present in acidic:

↔ H2O2 → H2O↔ MnO4

- → Mn2+

↔ Cr2O72- → Cr3+

↔ MnO2- → Mn2+

↔ NO3- → NO

dis/comproportionation↔ Cl2 → Cl- + OCl- (basic)↔ Br- + BrO3

- → Br2 (acidic)

↔ I- + IO3- → I2 (acidic)

~ 2I- + 2H2O → I2 + H2 + 2OH-

~ brønsted acid-base rxns (Na+, K+, Cl- spectator)~ nonmetal oxide + water → oxoacid (HmXOn); oxidation number

doesn’t change~ nonmetal oxide (XOn) + hydroxide → HXOn+1

-

~ complex ions Mn+ + L → M(L)2n

(charge)

Mn+ = TRANSITION METAL ion L: ligand = NH3 (charge = original charge), CN-, SCN-, OH-, Cl-