1. 1. Reactants = the substances youstart with 2. Products = the substances you end up with

2. - Page321ProductsReactants 3. The way atoms are joined is changedAtoms arent createdor destroyed. 4. the arrow () separates the reactantsfrom the products (arrowpoints to products)Read as: reacts toform or yields The plus sign = and 5. (s) after the formula = solid:Fe(s) (g) after the formula = gas:CO2(g) (l) after the formula = liquid:H2O(l) (aq) after the formula = dissolved in water, an aqueoussolution: NaCl(aq) is a salt water solution. 6. indicates a reversible reaction. shows that heat is supplied to the reaction., or is used to indicate a catalyst used supplied, in this case, platinum. , indicates a pressure other than STP. 7. used after a productindicates a gas has been produced: H2 used after a productindicates a solid has been produced: PbI2 8. Summary of Symbols 9. What is a Catalyst? A substance that speeds up areaction without being changedby the reaction. Enzymes are biological orprotein catalysts. 10. . Exothermic - reactions that releaseenergy to their surroundings (usually inthe form of heat) Endothermic - reactions that need toabsorb heat from their surroundings to proceed. 11. Spontaneous Reactions - Reactions that proceed immediately when two substances are mixed together. Not allreactions proceed spontaneously. Activation Energy the amount of energy that is required to start achemical reaction. Once activation energy is reached thereaction continues until you run out ofmaterial to react. 12. Uses formulas and symbols todescribe a reaction doesnt indicate how many. All chemical equations aresentences that describe reactions. 13. There are 8 elements thatnever want to be alone.They form diatomic molecules.H2 , N2 , O2 , F2 , Cl2 , Br2 , I2 ,and At2 The ogens and the ines 1 + 7 pattern on the periodictable 14. Solid iron reacts with oxygen gas to form solid iron oxide(rust). 15. A silver spoon tarnishes. The solid silverreacts with sulfur in the air to make solid silver sulfide, the black material we call tarnish. 16. Also called combinationreactions. 2 elements, or compoundscombine to make one compound.A + BABNa (s) + Cl2 (g)NaCl (s) Ca (s) +O2 (g)CaO (s) 17. SO3(s) + H2O(l) H2SO4 (s) We can predict theproducts if they are two elements.Mg (s) + N2 (g) Mg3N2 (s) 18. Additional Important Notes: a) Some nonmetal oxides reactwith water to produce an acid:SO2 + H2O H2SO3 (This is what happens to make acid rain)b) Some metallic oxides reactwith water to produce a base:CaO + H2O Ca(OH)2 19. decompose = fall apartone compound (reactant) falls apartinto two or more elements or compounds. Usually requires energy ABA + B electricityNaClNa + Cl2CaCO3 CaO + CO2 20. Can predict the products if it is a binary compound (made upof only two elements)Falls apart into its elementsH2O electricity H2 (g) + O2 (g)HgO Hg (s) + O2 (g) 21. If the compound has more than two elements you must be given one of the productsThe other product will befrom the missing piecesNiCO3 (aq) CO2(g)+ Ni(s)H2CO3(aq) H2 (g)+ CO2 (g) 22. Also referred to as single displacement One element replaces anotherReactantsmust be an elementand a compound.Productswill be a differentelement and a differentcompound. 23. Na + KClK + NaCl (Cations switched) F2 + LiCl LiF + Cl2(Anions switched) 24. A+BC AC+B2Na+ SrCl2Sr + 2NaClF2 + LiCl LiF + Cl2 25. We can tella reaction will happenSome are more active than otherMore active replaces less active 26. The Activity Series of MetalsHigherLithiumactivity Potassium 1) Metals can replace other Calcium Sodiummetals, provided they are Magnesiumabove the metal they are Aluminum Zinc trying to replace Chromium(for example, zinc will replace lead) Iron Nickel2) Metals above hydrogen can Lead Hydrogen replace hydrogen in acids. Bismuth Copper Mercury 3) Metals from sodium upward SilverLower Platinumcan replace hydrogen inactivity Gold water. 27. The Activity Series of HalogensHigher Activity Halogens can replace other Fluorinehalogens in compounds, Chlorine Bromine provided they are above the Iodinehalogen they are trying toLower Activity replace.2NaCl(s) + F2(g) ??? 2NaF(s) + Cl2(g) MgCl2(s) + Br2(g) ??? No Reaction! 28. Twothings replace eachother.Reactants must be two ionic compounds or acids.Usually in aqueous solution AB+CDAD+CB 29. ZnS + 2HClZnCl + H2SAgNO3 + NaClAgCl + NaNO3 30. NaOH + FeCl3 -The positive ions change place.NaOH + FeCl3Fe+3 OH- + Na+1 Cl-1= NaOH + FeCl3Fe(OH)3+ NaCl 31. Have certain driving forces, orreasons-Will only happen if one of the products:a) doesnt dissolve in water and forms a solid (a precipitate), orb) is a gas that bubbles out, orc) is a molecular compound (whichwill usually be water). 32. Combustion means add oxygenNormally, a compound composed of only C, H, (and maybe O) is reacted with oxygen usually called burning If the combustion is complete, the products will be CO2 and H2O.If the combustion is incomplete, the products will be CO (orpossibly just C) and H2O. 33. A reaction in which a compound (oftencarbon) reacts with oxygen CH4 + O2 CO2 + H2O C3H8 + O2 CO2 + H2O C6H12O6 + O2 CO2 + H2O 34. The charcoal usedin a grill is basically carbon.The carbon reactswith oxygen to yield carbon dioxide. Thechemical equation for this reaction is C + O2 CO2 35. An acid and a base react to form a salt and water.Always in aqueous solution Acid (H+) + Base (OH-) Salt + H2O NaOH + HCl NaCl + H2O NH4OH + H2SO4 (NH4)2SO4 + H2O 36. H2 + O2 SynthesisH2O Decomposition AgNO3 + NaCl Double replacement Zn + H2SO4 Single replacement HgODecomposition KBr +Cl2Single replacement Mg(OH)2 + H2SO3Double replacement 37. HNO3 + KOH Acid/Base CaPO4Decomposition AgBr + Cl2Single replacement Zn + O2Synthesis HgO + Pb Single replacement HBr + NH4OHAcid/Base Cu(OH)2 + KClO3Double replacement 38. An equation:Describes a reaction Must be balanced because to follow Law of Conservation of EnergyCan only be balanced by changing the coefficients.Has special symbols to indicate state, and if catalyst or energy is required. Can describe 5 different types of reactions.