Chapter 11-11.3 Reactions in Acqueous Solution
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| 11.3 What does a net ionic equation show? | An equation that shows dissolved ionic compounds as dissocated free ions
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| 11.3 What are dissociatetd free ions? | A general process in which ionic compounds (complexes, or salts) separate or split into smaller particles, ions, or radicals, usually in a reversible manner.
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| 11.3 How can you predict the formation of a precipitate in a double-replacement reaction? | By using general rules for solubility.
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| 11.3 What the soluble ionic compounds? | 1. Salts of alkali metals and ammonia (MgS04)2. Nitrate salts and Chlorate salts (CaCl2)3. Sulfate salts (FeS)4. Chloride salts (CaCl2)
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| 11.3 What types of sulfate salts are not soluble? | Pb2+, Ag+, Hg22+, Ba2+, Sr2+, and Ca2+
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| 11.3 What types of chloride salts are not soluble? | Ag+, Pb2+, Hg22+
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| 11.3 What ionic compounds are mostly insoluble? | Carbonates, phosphates, chromates, sulfides and hydroxides
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| 11.3 What is a spectator ion? | an ion that appears on both sides of an equation and not directly involved in the reaction. Pb(s) + AgNo3(aq)-----Ag(s) + Pb(No3)2 (aq). Pb is the spectator ion
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| 11.3 Complete ionic equation | an equation that shows dissolved ionic compounds as dissociated free ions
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| 11.3 Net ionic equation | Equation for the reaction of a solution that shows only those particles that are directly involved in the chemical change. Ag+(aq) + Cl (aq)---------AgCl(s)
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| 11.3 How do you write a balanced net ionic equation? | 1. write the complete ionic equation for the reaction.2. shwo any soluble ionic compounds as individual ions3. Eliminate aqueous ions that appear as both reactants and products4. Balance the net ionic equation.
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| 11.3 What happens to compounds in water? | 1. some dissolve and others do not2. Soluble compounds dissolve in water3. Insoluble compounds do not dissolve in water
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| 11.3 When does an aqueous solution occur? | has to be a homogenous mixture and when a compound or element dissolve in water.
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| 11.3 Do aqueous solutions contain a mixture of ions that could react with each other? | Yes
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| 11.3 Do many reactions occur between aqueous solutions containing ions? | Yes
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| 11.3 What do an ionic equation show? | The ions and non-ionic compounds that are present in a reaction
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| 11.3 What are the four rules about net ionic equations? | 1. Aqueous solutions occur when a compound or element dissolves in water.2. Many aqueous solutions contain a mixture of ions that could react with each other.3. Many reactions occur between aqueous solutions containing ions.4. ionic equation.
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| 11.3 What are the two types of ionic equations? | Complete and Net ionic
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| 11.3 What is a complete ionic equation? | an equation for a reaction that shows dissolved ionic compounds as dissocated free ions.
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| 11.3 What are the solubility rules for ionic compounds? | 1. salts of alkali metals and ammonia re soluble.2. Nitrate salt & chlorate salts are soluble;3. Sulfate salts (exceptions-Pb,Ag,Hg,Ba,Sr,CA) soluble;4. Cl salts execpt (ag, Pb, Hg)soluble;5. Carbonates, phosphates, chromates, S2 & OH insolubl
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| 11.3 What is a precipitate? | insoluble ionic compound (ie insoluble salts)
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