TYPES OF REACTIONS：类型的反应.doc

Name: _ Period: _TYPES OF REACTIONS: SYNTHESIS REACTIONS (ALSO CALLED COMPOSITION REACTIONS)We will study three types of synthesis reactions. Only one compound will be produced in each of these reactions.1. Two elements react to form a binary compound.2. A metallic oxide and water react to form a metallic hydroxide. (base)3. A nonmetallic oxide and water react to form an acid.1. aluminum + oxygen aluminium oxide4 Al + 3 O22 Al2O32. lithium + sulfur 3. sodium + iodine 4. calcium + oxygen 5. calcium oxide + water calcium hydroxide (a base)6. sodium oxide + water sodium hydroxide (a base)7. sulfur + oxygen sulphur dioxide8. sulfur trioxide + water sulfuric acid9. carbon dioxide + water carbonic acid10. potassium + bromine DECOMPOSITION REACTIONS (ALSO CALLED ANALYSIS REACTIONS)One compound is usually heated or tortured to make it chemically decompose into two substances.1. Metallic carbonates decompose to metallic oxides and carbon dioxide gas.2. Metallic hydroxides decompose into metallic oxides and water.3. Metallic chlorates decompose into metallic chlorides and oxygen gas.4. Some binary compounds decompose into the elements they are made of.5. Some acids decompose into nonmetallic oxides and water.6. Metallic oxides decompose into metals and oxygen gas.1. calcium chlorate - calcium chloride + oxygen gas2. lithium oxide -3. barium carbonate - barium oxide + carbon dioxide gas4. sodium hydroxide sodium oxide + water 5. potassium bromide 6. sodium oxide 7. sodium chloride 8. carbonic acid carbon dioxide + water9. sulfuric acid sulfur trioxide + water10. copper(II) hydroxide copper(II) oxide and waterCOMBUSTION REACTIONSThe burning of hydrocarbons and other “fuels” in the presence of oxygen is called combustion. The products of complete combustion are water and carbon dioxide.1. pentane (C5H12) + oxygen water + carbon dioxide2. octane (C8H18) + oxygen 3. ethanol (C2H5OH) + oxygen 4. methane (CH4) + oxygen 5. ethene (C2H4) + oxygen Name: _ Period: _SINGLE REPLACEMENT REACTIONSUse the activity series to see if the reaction occurs. If the element is not active enough to replace the other element. Write “no reaction”. Metals1. Replacement of a metal in a compound by a more active metal, lithiumforming an element (metal) and a salt.potassiumcalcium2. Replacement of hydrogen in water by a more active metal,sodium forming a metallic hydroxide and hydrogen gas.magnesiumaluminum3. Replacement of hydrogen in acid by a more active metal,zinc forming a salt and hydrogen gas.chromiumiron4. Replacement of a halogen (Group 17) by a more active halogen,nickel forming an element (halogen) and a salt.tinleadHYDROGENNonmetals (Halogens)copperfluorinemercurychlorinesilverbromineplatinumiodinegold example: 1. potassium iodide + chlorine - potassium chloride + iodine2 KI + Cl2 2 KCl + I22. calcium + hydrochloric acid -3. sodium chloride + fluorine -4. aluminum + copper(II) nitrate -5. calcium + water - HOH6. silver + water -7. magnesium + hydrochloric acid -8. copper + sodium sulfate -9. potassium + water -10. potassium chloride + iodine -Name: _ Period: _DOUBLE REPLACEMENT REACTIONS (ALSO CALLED IONIC REACTIONS)Look at the solubility table to find a precipitate. If an acid and a base react, the reaction is a neutralization reaction, and a salt and water will be produced. SOLUBILITY RULESSoluble compounds:Insoluble compounds form precipitates:Acetates: ALL dissolve.Carbonate: ONLY Group 1 metals and NH4+1 Almost all form precipitatesHalides (chloride, bromide, iodide): Almost all dissolve. ONLY Ag+1,Pb+2,Hg2+2, and Cu+1Hydroxide: ONLY Group 1 metals, NH4+1, Sr+2, and Ba+2 Almost all form precipitates.Nitrates: ALL dissolve.Sulfide: ONLY Group 1 and Group 2 metals, and NH4+1Almost all form precipitates.Sulfate:Most dissolve. Only Ba+2, Sr+2, Pb+2, and Ca+2Sulfite: ONLY Group 1 metals and NH4+1 Almost all form precipitates.Phosphate ONLY Group 1 metals and NH4+1Almost all form precipitates.Group 1 metal compounds and ammonium salts: ALL dissolve.Write the word equation, then write the balanced chemical equation!1. silver nitrate + zinc chloride silver chloride + zinc nitrate2. lead(II) nitrate + sodium sulfate -3. sulfuric acid + sodium hydroxide -4. phosphoric acid + iron(II) hydroxide -5. iron(II) sulfate + ammonium sulfide -6. sodium hydroxide + acetic acid -7. lead(II) nitrate + potassium iodide -8. iron(III) chloride + silver nitrate -9. ammonium hydroxide + carbonic acid -10. copper(II) sulfate + barium chloride Name: _ Period: _Classify the reaction types and balance the following chemical equations:Reaction type:_ 1. _ Al + _ HCl - _ AlCl3 + _ H2_ 2. _ Ca + _ AgNO3 - _ Ca(NO3)2 + _ Ag_ 3. _ Fe(OH)3 + _ H2SO4 - _ Fe2(SO4)3 + _H2O_ 4. _ Cu + _ O2 - _ CuO_ 5. _ Na + NiCl2 - _NaCl + _ Ni_ 6. _CH3OH + _O2 - _ CO2 + _ H2O_ 7. _ H2CO3 - _ H2O + _ CO2_ 8. _ Al2O3 + H2O - _ Al(OH)3For each substance, write the balanced decomposition reaction (chemical reaction) and the dissociation reaction (br