44. Combustion Reaction of a carbon-based compound with oxygen 2 C 4 H 10 + 13 O 2 8 CO 2 + 10 H 2 O butane

45. Combustion Alcohol lamp C 2 H 5 OH + 3 O 2 2 CO 2 + 3 H 2 O

46. Synthesis Forming a single compound from two or more reactants H 2 + O 2 H 2 O

47. Synthesis Forming a single compound from two or more reactants 2 Na + Cl 2 2 NaCl

48. Decomposition Breakdown of a single compound (Opposite of synthesis) 2 NaN 3 2 Na + 3N 2

49. Decomposition Breakdown of a single compound (Opposite of synthesis) NH 4 NO 3 N 2 O + 2 H 2 O

50. Single Displacement A single element reacts with a Compound and displaces another element from that compound Zn + 2 HCl ZnCl 2 + H 2

51. Single Displacement A single element reacts with a Compound and displaces another element from that compound 2 K + 2 H 2 O 2 KOH + H 2

52. Activity Series Element Reactivity K Ca Na React with cold water and acids to replace hydrogen; react with oxygen to form oxides Mg Al Zn Fe React with steam (not cold water) and acids to replace hydrogen; react with oxygen to form oxides Ni Pb Do not react with water; react with acids to replace hydrogen; react with oxygen to form oxides H 2 Cu React with oxygen to form oxides Ag Au Unreactive; form oxides only indirectly

55. Double Displacement Two compounds exchange ions and Form new compounds Pb(NO 3 ) 2 + KI PbI 2(s) + 2 KNO 3

56. Net Ionic Equations When aqueous solutions are mixed, new ionic combinations are made. Mass and Charge must be conserved. Na 2 SO 4(aq) + Sr(NO 3 ) 2(aq) SrSO 4(s) + 2 NaNO 3(aq) precipitate

57. Net Ionic Equations Precipitate = insoluble solid that Separates from solution Na 2 SO 4(aq) + Sr(NO 3 ) 2(aq) SrSO 4(s) + 2 NaNO 3(aq) precipitate

58. Net Ionic Equations Na 2 SO 4 - > 2 Na + + SO 4 2- Sr(NO 3 ) 2 - > Sr 2+ + 2 NO 3 - NaNO 3 - > Na + + NO 3 - Na 2 SO 4(aq) + Sr(NO 3 ) 2(aq) SrSO 4(s) + 2 NaNO 3(aq) precipitate

59. Net Ionic Equations Na 2 SO 4 - > 2 Na + + SO 4 2- Sr(NO 3 ) 2 - > Sr 2+ + 2 NO 3 - NaNO 3 - > Na + + NO 3 - 2 Na + + SO 4 2- + Sr 2+ + 2 NO 3 - SrSO 4(s) + 2 Na + + 2 NO 3 - spectator ions precipitate

60. Solubility Rules All alkali metal and NH 4 + salts are soluble; All nitrates (NO 3 ) are soluble; All Halides (F, Cl, Br, I) are soluble except Ag + and Pb 2+ Sulfates(SO 4 ), except for Ca 2+ , Ba 2+ , Sr 2+ , Pb 2+ are soluble Carbonates (CO 3 ) are insoluble except for alkali metal and NH 4 .

61. Net Ionic Equations Li 2 CO 3 + BaBr 2 BaCO 3 + 2 LiBr

62. Net Ionic Equations Li 2 CO 3 -> 2 Li + + CO 3 2- BaBr 2 -> Ba 2+ + 2 Br - Li 2 CO 3 + BaBr 2 BaCO 3 + 2 LiBr precipitate

63. Unit 5 Review Molar Mass g <-> atoms/molecules <-> moles Percent Composition Empirical and Molecular Formula Chemical equations: Word Equations, Balancing