Chapter Fourteen Notes

Chapter Fourteen Notes - Precipitates are shown as solids...

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Chapter Fourteen Notes  Ionic and molecular compounds behave differently when dissolved in water Dissociation- Ions separate from one another when dissolved in water Dissociation is indicated by equations balanced by charge and atoms In 100% dissociation, a solution of 1 mol of NaOH dissociates to 1mol Na +  and 1 mol OH + Compounds of low solubility are considered insoluble Dissociation equations cannot be written for insoluble compounds In a double-replacement reaction, reactants are both soluble Usually one product is insoluble To see if a d-r reaction occurs, look at possible precipitates Determine if one precipitate is insoluble  If so, then the reaction will take place Reactions of ions are represented by net ionic equation Used instead of formula equations NIE includes compounds and ions that undergo a chemical change in aqueous solution Soluble ions compounds are shown as dissociated ions
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Unformatted text preview: Precipitates are shown as solids Spectator ions- ions that do not take part or change in the reaction These ions are eliminated in a net ionic equation Ionization- ions are formed from other solute molecules by action of solvent molecules Ionization is different from dissociation- ionic molecules dissolve and previously present ions separate In a covalent molecule, no ions were present in the undissolved compound Ions formed when a covalent molecule ionizes are hydrated Energy released when ions are hydrated provides energy to break covalent bonds H + doesn’t normally exist alone Transfers to a water molecule from covalent H 3 O + Called the hydronium ion Formation is highly exothermic Energy is used to ionize the molecular solute HF, HCl, HBr, HI strongly conduct a current HF is a weak conductor...
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This note was uploaded on 09/28/2010 for the course CHEM Chemistry taught by Professor Plants during the Spring '10 term at Clear Creek.

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