CHAPTER 4 NOTES AND VOCABULARY

Acid: a substance that provides H+ ions when dissolved in water
Acid-base neutralization reaction: a process in which an acid reacts with a base to yield water plus an ionic compound called a salt
Activity series: a lost of elements in order of their reducing ability in aqueous solution
Base: a substance that provides OH- ions when dissolved in water
Diprotic acid: an acid that has two dissociable protons
Dissociate: splitting apart to give ions when dissolved in water
Electrolyte: a substance that dissolves in water to produce ions
Half-reaction: the oxidation or reduction part of a redox reaction
Half-reaction method: a method for balancing redox equations
Hydronium ion, H3O+: the protonated water molecule, H3O+
Ionic equation: a chemical equation written so that ions are explicitly shown
Molecular equation: a chemical equation written using the complete formulas of reactants
Monoprotic acid: an acid that has a single dissociable proton
Net ionic equation: a chemical equation written so that spectator ions are removed
Nonelectrolyte: a substance that does not produce ions when dissolved in water
Oxidation: the loss of one or more electrons by a substance
Oxidation number: a value that measures whether an atom in a compound is neutral, electron rich, electron poor compared to an isolated atom
Oxidation-reduction (redox) reaction: a process n which one or more electrons are transferred between reaction partners
Oxidizing agent: a substance that causes an oxidation by accepting an electron
Oxoacid: an acid that contains oxygen in addition to hydrogen and another element
Precipitation reaction: a reaction in which an insoluble solid precipitate forms and drops out of solution
Redox reaction: an oxidation-reduction reaction
Reducing agent: a substance that causes a reduction by donating an electron
Reduction: the gain of one or more electrons by a substance
Salt: an ionic compound formed in a acid-base neutralization
Solubility: the amount of a substance that dissolves in a given volume of solvent at a given temperature
Spectator ion: an ion that appears on both sides of the reaction arrow
Strong acid: an acid that dissociates completely in water to give H+ ions and is a strong electrolyte
Strong base: a base that dissociates or reacts completely in water to give OH- ions and a strong electrolyte
Strong electrolyte: a compound that dissociates completely into ions when dissolved in water
Weak acid: an acid that dissociates incompletely in water an is a weak electrolyte Weak base: a base that dissociates or reacts incompletely in water and is a weak electrolyte
Weak electrolyte: a compound that dissociates incompletely when dissolved in water

4.1- SOME WAYS THAT CHEMICAL REACTIONS OCCUR * There are three categories of chemical reactions in aqueous solution. * Precipitation reactions, acid-base neutralization reactions and oxidation-reduction reaction. * Precipitation reactions * Most precipitation takes place when the anions an cations of two ionic compound change partners * Pb(NO3)2(aq) + 2KI(aq) 2KNO3(aq) + PbI2(s) * Acid-base neutralization reactions * Acids are compounds that produce H+ and bass produce OH- ions. So the neutralization reoves H+ and OH- ions from the solution * HCl(aq) + NaOH(aq) H2O(l)+ NaCl(aq) * Oxidation-reduction reactions * This is also known as redox reactions. The result of this is electrons transfer, the charges on atoms in t4he various reactants change. * Mg(s) + 2HCl(aq) MgCl2 + H2(aq)

* When metallic magnesium reacts with aqueous hydrochloric acid, a magnesium atom gives an electron to each of two H+ ions, forming Mg2+ ion and H2. The charge on the magnesium changes from 0 to +2 and the charge on each hydrogen changes from +1 to 0

4.2- ELECTROLYTES IN AQEOUS SOLUTION *