Chemical Reactions 1. H2 + I2 HI S 2. Na + H2O NaOH + H2 SR 3. CO + O2 CO2 S 4. KClO3 KCl + O2 D 5. KNO3 KNO2 + O2 D 6. NaOH + H2SO4 Na2SO4 + H2O DR 7. N2 + H2 NH3 S 8. Zn + AgCl ZnCl2 + Ag SR 9. P4O10 + H2O H3PO4 S

Chemical Reactions 10. H2O2 H2O + O2 D 11. Zn + CuSO4 ZnSO4 + Cu SR 12. KOH + H3PO4 K3PO4 + H2O DR 13. S8 + O2 SO2 S 14. C6H12O6 C2H5OH + CO2 D 15. KCN + HCl KCl + HCN DR 16. Al + O2 Al2O3 S 17. Cu + HCl CuCl2 + H2 SR 18. Cl2 + KBr KCl + Br2 SR

Chemical Reactions 19. Si + Cl2 SiCl4 S 20. HgO Hg + O2 D 21. H2 + Cl2 HCl S 22. K + FeI3 Fe + KI SR 23. C + O2 CO2 S 24. HNO3 + Ba(OH)2 Ba(NO3)2 + H2O DR

Reaction Types -empirical formulas S = Synthesis = A + X AX D = element or simple compound element or simple compound compound D = Decomposition = AX A + X compound element or simple compound element or simple compound SR = Single Replacement = AX + B BX + A compound element compound element AX + Y AY + X DR = Double Replacement = AX + BY BX + AY compound compound compound compound

-balancing an equation -the Law of Conservation of Matter states that 25. C3H8 + O2 CO2 + H2O compound element compound compound AX + Y AY + XY = Combustion Chemical Reactions -balancing an equation -the Law of Conservation of Matter states that matter is neither created or destroyed by ordinary chemical means, only changed in form C3H8 + 5 O2 3 CO2 + 4 H2O 3 Carbon atoms 3 1 Carbon atom 8 Hydrogen atoms 8 2 Hydrogen atoms 10 2 Oxygen atoms 10 7 3 Oxygen atoms

26. H3PO4 + Ca(OH)2 Ca3(PO4)2 + H2O 2 H3PO4 + 3 Ca(OH)2 Ca3(PO4)2 + 6 Hydrogen phosphate Calcium hydroxide Calcium phosphate Hydrogen hydroxide 2 H3PO4 + 3 Ca(OH)2 Ca3(PO4)2 + 6 H2O 3 1 Calcium atoms 3 Calcium atoms 12 9 5 Hydrogen atoms 12 2 Hydrogen atoms 2 1 Phosphorus atoms 2 Phosphorus atoms 14 10 6 Oxygen atoms 14 9 Oxygen atoms 27. C4H10 + O2 CO2 + H2O butane Oxygen Carbon dioxide water 2 C4H10 + 13 O2 8 CO2 + 10 H2O 8 4 Carbon atoms 8 1 Carbon atoms 20 10 Hydrogen atoms 20 2 Hydrogen atoms 26 2 Oxygen atoms 26 12 3 Oxygen atoms

Reaction Types I. Synthesis -chemical reactions in which ____ or _____ simpler substances react to form ____ ________ two more one product -Example #1: 2 Mg + O2 2 MgO 2 S + O2 2 SO2 -Example #2: 2 Na + Cl2 2 NaCl 2 H2 + O2 2 H2O -each of the four examples of chemical reactions are also ____________, as _____ energy is _________ in the formation of ____ ______ than is required to break the bonds in the initial __________ exothermic more released new bonds reactants

Reaction Types II. Combustion -chemical reactions in which _______ combines with a substance to form ____ or _____ _______ and releases ______ in the forms of ____ and _____ oxygen one more oxides energy heat light -Example #1: 1 CH4 + 2 O2 1 CO2 + 2 H2O -Example #2: 2 CH3OH + 3 O2 2 CO2 + 4 H2O -Example #3: 2 C2H5OH + 7 O2 4 CO2 + 6 H2O -each of the four examples of chemical reactions are also ____________, as _____ energy is _________ in the formation of ____ ______ than is required to break the bonds in the initial __________, and the ________ are _____ stable than the __________ exothermic more released new bonds reactants products more reactants

Predicting and Balancing Equations Aluminum sulfate + Lithium Lithium sulfate + Aluminum compound element compound element AX + B SR BX + A 1 Al2(SO4)3 + 6 2 Li 3 Li2SO4 + 2 Al 1. Identify the type of substances in the reactants or products 2. Identify the reaction type, using empirical formulas 3. Using empirical formulas, predict the names of the products 4. Write correct chemical formulas for reactants and products 5. Use coefficients to balance equation

-chemical reactions in which ____ __________ Reaction Types III. Decomposition -chemical reactions in which ____ __________ breaks down into ____ or _____ _________ or _________ ___________ one compound two more elements simpler compounds -Example #1: 2 H2O2 1 O2 + 2 H2O KI -Example #2: 2 H2O 1 O2 + 2 H2 electricity -Example #3: C3H5N3O9 N2 + CO2 + H2O + O2 Nitroglycerine IV. Single Replacement -chemical reactions in which the atoms of a more __________ ________ replace the atoms of another ________ in a _________ reactive element element compound -Example #1: 1 Zn + 2 CuNO3 1 Zn(NO3)2 + 2 Cu -Example #2: 1 Mg + 2 H2O 1 Mg(OH)2 + 1 H2 1 Ca + 2 H2O 1 Ca(OH)2 + 1 H2 2 Na + 2 H2O 2 NaOH + 1 H2 Na > Ca > Mg

Reaction Types IV. Single Replacement -reactivity series - + + + - - - Mg(NO3)2 Cu(NO3)2 Fe(NO3)3 Zn(NO3)2 - + + + Mg - - - - Cu - - - Fe + - + + - Zn 1. Write a complete balanced equation for each reaction that took place: a. b. c. d. e. f. 2. List the four metals, in order, from most reactive to least reactive:

-chemical reaction in which both the Reaction Types V. Double Replacement -chemical reaction in which both the _________ _____ and the _________ _____ exchange between ____ __________ positive ions negative ions two compounds -Example #1: 2 NaOH + 1 CuCl2 2 NaCl + 1 Cu(OH)2 -Example #2: 1 NaOH + 1 HCl 1 NaCl + 1 HOH -Example #3: 1 NaHCO3 + 1 HCl 1 NaCl + 1 H2CO3 VI. Reactions in Aqueous Solutions -some ___________ compounds such as ________ or ________ dissolve in water, because they are ______, like water molecular sucrose ethanol polar -some ___________ compounds such as ________________ dissolve in water, but because they are extremely ______, they ________ in water molecular Hydrogen chloride polar HCl H+ + Cl- (aq) (aq) ionize Hydrogen chloride Hydrochloric acid

VI. Reactions in Aqueous Solutions -when ______ compounds Reaction Types VI. Reactions in Aqueous Solutions -when ______ compounds dissolve in water, (being already made up of _____), they ___________, or _______ from each other ionic ions NaOH Na+ + OH- dissociate separate (aq) (aq) Sodium hydroxide -______ ___________ reactions often take place in ________ __________ double replacement aqueous solutions Writing an Ionic Equation – in a reaction that forms a precipitate Balanced Chemical Equation 2 NaOH + 1 CuCl2 2 NaCl + 1 Cu(OH)2 Complete Ionic Equation 2 Na+ + 2 OH- + 1 Cu2+ + 2 Cl- (aq) (aq) (aq) (aq) 2 Na+ + 2 Cl- + 1 Cu(OH)2 (aq) (aq) (s) Net Ionic Equation 2 OH- + 1 Cu2+ 1 Cu(OH)2 (aq) (aq) (s)

Writing an Ionic Equation – in a reaction that forms water Balanced Chemical Equation 1 NaOH + 1 HCl 1 NaCl + 1 HOH Complete Ionic Equation 1 Na+ + 1 OH- + 1 H+ + 1 Cl- (aq) (aq) (aq) (aq) 1 Na+ + 1 Cl- + 1 HOH (aq) (aq) (l) Net Ionic Equation 1 OH- + 1 H+ 1 HOH (aq) (aq) (l) Writing an Ionic Equation – in a reaction that forms a gas Balanced Chemical Equation 1 NaHCO3 + 1 HCl 1 NaCl + 1 H2O + 1 CO2 Complete Ionic Equation 1 Na+ + 1 HCO3- + 1 H+ + 1 Cl- (aq) (aq) (aq) (aq) 1 Na+ + 1 Cl- + 1 HOH + 1 CO2 (aq) (aq) (l) (g) Net Ionic Equation 1 HCO3- + 1 H+ 1 HOH + 1 CO2 (aq) (aq) (l) (g)