Predicting Products of Reactions Synthesis: Reactants combine to form a single product – make sure the product has an acceptable formula (ions are correct charges, etc.) Decomposition: Reactant breaks down into simpler products Binary compounds decompose into elements Carbonates produce CO2 and oxide Na2CO3  Na2O + CO2 Explosives produce gases

Predicting Products of Reactions Single Replacement – Element replaces another element (generally, metal or hydrogen replace one another, nonmetal replaces nonmetal) Double Replacement – Positive ions “switch” partners Combustion – reaction with O2 produces oxides (often H2O and CO2)

Examples – Predict products and write balanced equations Decomposition of calcium carbonate Decomposition of aluminum oxide Al + Cl2  Zn + HCl  Combustion of butane (C4H10) Ca(NO3)2 + K2CO3  Ca + H2O 

Energy and Chemical Reactions Endothermic – A process that absorbs heat energy from its surroundings. * Causes the temperature of surrounding substances to decrease. EXAMPLES? Exothermic – A process that gives off heat to its surroundings. * Causes the temperature of surrounding substances to increase.

Acids and Bases Acid – a compound that yields H+ ions in aqueous solution. Formula contains H as first element. Base – a compound that yields OH- ions in aqueous solution. Formula contains hydroxide (OH-) ions.

Acid-Base Reactions Double Replacement Example HNO3 + NaOH  Products of acid-base reactions: Water (HOH = H2O) Ionic Compound (salt – general term)

Examples Complete and balance the following acid base reactions: HCl + KOH  H3PO4 + Mg(OH)2  H2SO4 + NaOH 