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Net ionic equations are equations that show only the soluble, strong electrolytes reacting (these are represented as ions) and omit the spectator ions, which go through the reaction unchanged. When you encounter net ionic equations on the SAT II Chemistry test, you’ll need to remember the following solubility rules, so memorize them! Also keep in mind that net ionic equations, which are the bare bones of the chemical reaction, usually take place in aqueous environments. Here are those solubility rules: Most alkali metal compounds and compounds are soluble.
Cl-, Br-, I- compounds are soluble, except when they contain Ag+, , or Pb2+. F- compounds are soluble, except when they contain group 2A metals. , , , and CH3COO- compounds are soluble.
compounds are soluble, except when they include Ca2+, Sr2+, Ba2+, Ag+, Pb2+, or . , , , , S2-, OH-, and O2- compounds are insoluble.
Group 2A metal oxides are classified as strong bases even though they are not very soluble.
chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise indicated. Represent substances in solution as ions if the substance is extensively ionized. Omit formulas for any ions or molecules that are unchanged by the reaction. In ALL cases a reaction occurs. You need not balance. Note: the reactions are not broken down by type on the actual AP exam. Score one point for correct reactants and 2 points for correct products. I. DOUBLE REPLACEMENT
Solubility rules that apply to water solution:
(1) All alkali metal (lithium, sodium, potassium, rubidium, and cesium) compounds are soluble. (2) All acetate, ammonium, chlorate, and nitrate compounds are soluble. (3) Chlorides,...
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