The main tasks of Chap 8 Sect 1 - Writing reactions from word problems – challenging Sect 2 - Balance Equations—easiest Sect 3 - Classify Equations, Complete Equations—challenging Sect 4 – Write Net Ionic equations Classifying Reactions You will learn to recognize the different types of reactions AND How to complete products (predict). Combustion Reactions “Burning” • Oxygen is a reactant. • Energy is produced Combustion of carbon compounds yield carbon dioxide(CO2) and water (H2O ). • Mg + O2 MgO • CH4 + O2 CO2 + H2O Synthesis Reactions Two or more elements or compounds combine to form ONE PRODUCT. • Mg + O2 MgO • H2 + O2 H2O • SO 3 ( g ) H 2 O ( l ) H 2 SO 4 ( aq ) Decomposition Reactions ONE REACTANT (compound) breaks into elements or smaller compounds. • H2O H2 + O2 • MgO Mg + O2 Displacement Reactions • Also called Replacement reactions • Single Displacement/Replacement – Use the Activity series • Double Displacement/Replacement – Precipitation Reactions • Use the Solubility Rules – Acid Base Reactions Single Displacement Part of an ionic compound is removed and replaced by a new element. • ELEMENT + COMPOUND COMPOUND + ELEMENT There are 2 subtypes of single replacement reactions. - Cationic replacement - Anionic replacement Single Displacement subtype CATIONIC REPLACEMENT: • If the Element is a Metal, it replaces the metal in the compound. • Cu + AgNO3 Cu(NO3)2 + Ag Single Displacement subtype: ANIONIC REPLACEMENT: • If the Element is a Non-metal, it replaces the non-metal in the compound. • Cl2 + NaBr NaCl + Br2 Single Replacement Rxns • To determine if a Single Replacement Reaction really happens, use the ACTIVITY SERIES reference sheet. • If an element is higher on the chart, it will become a compound. • If the higher element is already in a compound, then NO reaction occurs Double Replacement Rxns • Two Ionic Compounds that exchange partners. • XY + AB AY + XB • Only Positive with Negative • Positive Ion listed first Double Replacement Rxns • To determine if the reaction occurs, use the SOLUBILITY RULES. • A reaction occurs if a solid or water forms when two aqueous solutions of ionic compounds are mixed. • If the products are both aqueous ionic compounds, then no reaction occurs. Solubility Rules info. • Soluble = dissolves in water = (aq) = clear • Insoluble= doesn’t dissolve in water = SOLID = (s) = cloudy = precipitate = ppt Section 4: Net Ionic Equations • Three ways to write the same equation (usually with double replacement rxns): • 1. Complete Molecular Equation • 2. Complete Ionic Equation • 3. Net Ionic Equation Dissolving (aq) separates the ions • • • • NaCl (s) in water NaCl (aq) NaCl (aq) means Na+(aq) + Cl- (aq) The Ions move separately in solution. In some equations we separate the ions and write the charges. Complete Molecular Eqn • This is what we have been doing. Write the compounds with the ions together. • Example: NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3(aq) Complete Ionic Eqns • Write the aqueous compounds as separate ions. Be sure to put the CHARGES ON THE IONS! • Keep the solid(insoluble) or water molecules together. • Example: + Na (aq) + Cl (aq) + Ag+(aq) + NO3 (aq) AgCl (s) + Na+(aq)+ NO3-(aq) Net Ionic Equations • Take the Complete ionic equation and remove any ion that is aqueous on both sides. These ions are called Spectator Ions. OR • Find the Solid product or water, keep that part AND keep the reactant ions that made the solid or water. • Ex: Ag+ (aq) + Cl- (aq) AgCl(s) Net Ionic Eqns with Acids and Bases( H+ and OH-) When acids (HA) and Bases (ZOH) mix, the H+ and OH- combine to become H2O(l). This is called a neutralization reaction. The water H2O(l) stays together like insoluble solids. So you keep it in the Net Ionic equation. Ex. H+ + OH- H2O Example: Complete and Net Ionic Equations page 1 Cu(NO3 )2 (aq) + NaOH(aq) ???? 1) Write Complete Molecular Equation: Cu(NO3 )2 (aq) + NaOH(aq) Cu(OH)2 (s) + NaNO3 (aq) 2) Write Complete Ionic Equation: [separate all (aq), put charges on ions; keep solids together.] Cu+2(aq) +2NO3 -1(aq) + 2Na+1 (aq) + OH-1 (aq) Cu(OH)2 (s) + 2Na+1 (aq) + And then… 2NO3 -1 (aq) Example: Complete and Net Equations page 2 Ionic 3) Write Net Ionic Equation: [eliminate spectator ions, keep ions that make solid, keep solids.] Cu+2(aq) + OH-1 (aq) Cu(OH)2 (s)