logging in or signing up types of chemical reactions aSGuest3277 Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 17160 Category: Education License: All Rights Reserved Like it (13) Dislike it (4) Added: November 15, 2008 This Presentation is Public Favorites: 3 Presentation Description No description available. Comments Posting comment... By: malla.avinash (8 month(s) ago) please allow me to download this ppt Saving..... Post Reply Close Saving..... Edit Comment Close By: manavgoyal10 (19 month(s) ago) how to download this Saving..... Post Reply Close Saving..... Edit Comment Close By: vishal_23 (20 month(s) ago) how to download this..? Saving..... Post Reply Close Saving..... Edit Comment Close By: DENTISTRY (27 month(s) ago) THANKS for ppt Saving..... Post Reply Close Saving..... Edit Comment Close By: DENTISTRY (27 month(s) ago) plz allow to download this ppt Saving..... Post Reply Close Saving..... Edit Comment Close loading.... See all Premium member Presentation Transcript Types of Chemical Reactions : Types of Chemical Reactions Writing Chemical Reactions Types of Reactions : Types of Reactions Many chemical reactions have defining characteristics which allow them to be classified as to type. Types of Chemical Reactions : Types of Chemical Reactions The five types of chemical reactions in this unit are: Combination Decomposition Single Replacement Double Replacement Combustion Combination Reactions : Combination Reactions Two or more substances combine to form one substance. The general form is A + X AX Example: Magnesium + oxygen magnesium oxide 2Mg + O2 2MgO Magnesium + Oxygen : Magnesium + Oxygen Combination Reactions : Combination Reactions Combination reactions may also be called composition or synthesis reactions. Some types of combination reactions: Combination of elements K + Cl2 One product will be formed Combination Reactions : Combination Reactions K + Cl2 Write the ions: K+ Cl- Balance the charges: KCl Balance the equation: 2K + Cl2 2KCl Combination Reactions : Combination Reactions Some types of combination reactions: Oxide + water Nonmetal oxide + water acid SO2 + H2O H2SO3 Metal oxide + water base BaO + H2O Ba(OH)2 Combination Reactions : Combination Reactions Some types of combination reactions: Metal oxides + nonmetal oxides Na2O + CO2 Na2CO3 CaO + SO2 CaSO3 Decomposition Reactions : Decomposition Reactions One substance reacts to form two or more substances. The general form is AX A + X Example: Water can be decomposed by electrolysis. 2H2O 2H2 + O2 Electrolysis of Water : Electrolysis of Water Decomposition Reactions : Decomposition Reactions Types of Decomposition Reactions: Decomposition of carbonates When heated, some carbonates break down to form an oxide and carbon dioxide. CaCO3 CaO + CO2 H2CO3 H2O + CO2 Decomposition Reactions : Decomposition Reactions Types of decomposition reactions: Some metal hydroxides decompose into oxides and water when heated. Ca(OH)2 CaO + H2O Note that this is the reverse of a similar combination reaction. Decomposition Reactions : Decomposition Reactions Types of decomposition reactions: Metal chlorates decompose into chlorides and oxygen when heated. 2KClO3 2KCl + 3O2 Zn(ClO3)2 ZnCl2 + 3O2 Some of these reactions are used in explosives. Decomposition Reactions : Decomposition Reactions Some substances can easily decompose: Ammonium hydroxide is actually ammonia gas dissolved in water. NH4OH NH3 + H2O Some acids decompose into water and an oxide. H2SO3 H2O + SO2 Decomposition Reactions : Decomposition Reactions Some decomposition reactions are difficult to predict. The decomposition of nitrogen triiodide, NI3, is an example of an interesting decomposition reaction. Nitrogen triiodide : Nitrogen triiodide Single Replacement Reactions : Single Replacement Reactions A metal will replace a metal ion in a compound. The general form is A + BX AX + B A nonmetal will replace a nonmetal ion in a compound. The general form is Y + BX BY + X Single Replacement Reactions : Single Replacement Reactions Examples: Ni + AgNO3 Nickel replaces the metallic ion Ag+. The silver becomes free silver and the nickel becomes the nickel(II) ion. Ni + AgNO3 Ag + Ni(NO3)2 Balance the equation: Ni + 2AgNO3 2Ag + Ni(NO3) Metal Tree : Metal Tree Single Replacement Reactions : Single Replacement Reactions Not all single replacement reactions that can be written actually happen. The metal must be more active than the metal ion. Aluminum is more active than iron in Al + Fe2O3 in the following reaction: Thermite Reaction : Thermite Reaction Thermite Reaction : Thermite Reaction Al + Fe2O3 Aluminum will replace iron(III) as was seen in the video. Iron(III) becomes Fe and aluminum metal becomes Al3+. 2Al + Fe2O3 2Fe + Al2O3 Single Replacement Reactions : Single Replacement Reactions An active nonmetal can replace a less active nonmetal. The halogen (F2, Cl2, Br2, I2) reactions are good examples. F2 is the most active and I2 is the least. Cl2 +2 NaI 2 NaCl + I2 Double Replacement Reactions : Double Replacement Reactions Ions of two compounds exchange places with each other. The general form is AX + BY AY + BX Metathesis is an alternate name for double replacement reactions. NaOH + CuSO4 : NaOH + CuSO4 Double Replacement : Double Replacement NaOH + CuSO4 The Na+ and Cu2+ switch places. Na+ combines with SO42- to form Na2SO4. Cu2+ combines with OH- to form Cu(OH)2 NaOH + CuSO4 Na2SO4 + Cu(OH)2 2NaOH + CuSO4 Na2SO4 + Cu(OH)2 CuSO4 + Na2CO3 : CuSO4 + Na2CO3 Double Replacement : Double Replacement CuSO4 + Na2CO3 Cu2+ combines with CO32- to form CuCO3. Na+ combines with SO42- to form Na2SO4. CuSO4 + Na2CO3 CuCO3 + Na2SO4 Na2CO3 + HCl : Na2CO3 + HCl Double Replacement : Double Replacement Na2CO3 + HCl Notice that gas bubbles were produced rather than a precipitate. What was the gas? Write the double replacement reaction first. Double Replacement : Double Replacement Na2CO3 + HCl Na+ combines with Cl- to form NaCl. H+ combines with CO32- to form H2CO3. Na2CO3 + 2HCl 2NaCl + H2CO3 H2CO3 breaks up into H2O and CO2. Double Replacement : Double Replacement The gas formed was carbon dioxide. The final balanced reaction is: Na2CO3 + HCl NaCl + H2O + CO2. Balance the equation. Na2CO3 + 2HCl 2NaCl + H2O + CO2 Combustion Reaction : Combustion Reaction When a substance combines with oxygen, a combustion reaction results. The combustion reaction may also be an example of an earlier type such as 2Mg + O2 2MgO. The combustion reaction may be burning of a fuel. Combustion Reaction : Combustion Reaction Methane, CH4, is natural gas. When hydrocarbon compounds are burned in oxygen, the products are water and carbon dioxide. CH4 + O2 CO2 + H2O CH4 + 2O2 CO2 + 2H2O Combustion Reactions : Combustion Reactions Combustion reactions involve light and heat energy released. Natural gas, propane, gasoline, etc. are burned to produce heat energy. Most of these organic reactions produce water and carbon dioxide. Practice : Practice Classify each of the following as to type: H2 + Cl2 2HCl Combination Ca + 2H2O Ca(OH)2 + H2 Single replacement Practice : Practice 2CO + O2 2CO2 Combination and combustion 2KClO3 2KCl + 3O2 Decomposition Practice : Practice FeS + 2HCl FeCl2 + H2S Double replacement Zn + HCl ? Single replacement Zn + 2HCl ZnCl2 + H2 Types of Chemical Reactions : Types of Chemical Reactions Read Chapter 8-2 Review nomenclature Do all of the practice exercises given in class. You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
types of chemical reactions aSGuest3277 Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 17160 Category: Education License: All Rights Reserved Like it (13) Dislike it (4) Added: November 15, 2008 This Presentation is Public Favorites: 3 Presentation Description No description available. Comments Posting comment... By: malla.avinash (8 month(s) ago) please allow me to download this ppt Saving..... Post Reply Close Saving..... Edit Comment Close By: manavgoyal10 (19 month(s) ago) how to download this Saving..... Post Reply Close Saving..... Edit Comment Close By: vishal_23 (20 month(s) ago) how to download this..? Saving..... Post Reply Close Saving..... Edit Comment Close By: DENTISTRY (27 month(s) ago) THANKS for ppt Saving..... Post Reply Close Saving..... Edit Comment Close By: DENTISTRY (27 month(s) ago) plz allow to download this ppt Saving..... Post Reply Close Saving..... Edit Comment Close loading.... See all Premium member Presentation Transcript Types of Chemical Reactions : Types of Chemical Reactions Writing Chemical Reactions Types of Reactions : Types of Reactions Many chemical reactions have defining characteristics which allow them to be classified as to type. Types of Chemical Reactions : Types of Chemical Reactions The five types of chemical reactions in this unit are: Combination Decomposition Single Replacement Double Replacement Combustion Combination Reactions : Combination Reactions Two or more substances combine to form one substance. The general form is A + X AX Example: Magnesium + oxygen magnesium oxide 2Mg + O2 2MgO Magnesium + Oxygen : Magnesium + Oxygen Combination Reactions : Combination Reactions Combination reactions may also be called composition or synthesis reactions. Some types of combination reactions: Combination of elements K + Cl2 One product will be formed Combination Reactions : Combination Reactions K + Cl2 Write the ions: K+ Cl- Balance the charges: KCl Balance the equation: 2K + Cl2 2KCl Combination Reactions : Combination Reactions Some types of combination reactions: Oxide + water Nonmetal oxide + water acid SO2 + H2O H2SO3 Metal oxide + water base BaO + H2O Ba(OH)2 Combination Reactions : Combination Reactions Some types of combination reactions: Metal oxides + nonmetal oxides Na2O + CO2 Na2CO3 CaO + SO2 CaSO3 Decomposition Reactions : Decomposition Reactions One substance reacts to form two or more substances. The general form is AX A + X Example: Water can be decomposed by electrolysis. 2H2O 2H2 + O2 Electrolysis of Water : Electrolysis of Water Decomposition Reactions : Decomposition Reactions Types of Decomposition Reactions: Decomposition of carbonates When heated, some carbonates break down to form an oxide and carbon dioxide. CaCO3 CaO + CO2 H2CO3 H2O + CO2 Decomposition Reactions : Decomposition Reactions Types of decomposition reactions: Some metal hydroxides decompose into oxides and water when heated. Ca(OH)2 CaO + H2O Note that this is the reverse of a similar combination reaction. Decomposition Reactions : Decomposition Reactions Types of decomposition reactions: Metal chlorates decompose into chlorides and oxygen when heated. 2KClO3 2KCl + 3O2 Zn(ClO3)2 ZnCl2 + 3O2 Some of these reactions are used in explosives. Decomposition Reactions : Decomposition Reactions Some substances can easily decompose: Ammonium hydroxide is actually ammonia gas dissolved in water. NH4OH NH3 + H2O Some acids decompose into water and an oxide. H2SO3 H2O + SO2 Decomposition Reactions : Decomposition Reactions Some decomposition reactions are difficult to predict. The decomposition of nitrogen triiodide, NI3, is an example of an interesting decomposition reaction. Nitrogen triiodide : Nitrogen triiodide Single Replacement Reactions : Single Replacement Reactions A metal will replace a metal ion in a compound. The general form is A + BX AX + B A nonmetal will replace a nonmetal ion in a compound. The general form is Y + BX BY + X Single Replacement Reactions : Single Replacement Reactions Examples: Ni + AgNO3 Nickel replaces the metallic ion Ag+. The silver becomes free silver and the nickel becomes the nickel(II) ion. Ni + AgNO3 Ag + Ni(NO3)2 Balance the equation: Ni + 2AgNO3 2Ag + Ni(NO3) Metal Tree : Metal Tree Single Replacement Reactions : Single Replacement Reactions Not all single replacement reactions that can be written actually happen. The metal must be more active than the metal ion. Aluminum is more active than iron in Al + Fe2O3 in the following reaction: Thermite Reaction : Thermite Reaction Thermite Reaction : Thermite Reaction Al + Fe2O3 Aluminum will replace iron(III) as was seen in the video. Iron(III) becomes Fe and aluminum metal becomes Al3+. 2Al + Fe2O3 2Fe + Al2O3 Single Replacement Reactions : Single Replacement Reactions An active nonmetal can replace a less active nonmetal. The halogen (F2, Cl2, Br2, I2) reactions are good examples. F2 is the most active and I2 is the least. Cl2 +2 NaI 2 NaCl + I2 Double Replacement Reactions : Double Replacement Reactions Ions of two compounds exchange places with each other. The general form is AX + BY AY + BX Metathesis is an alternate name for double replacement reactions. NaOH + CuSO4 : NaOH + CuSO4 Double Replacement : Double Replacement NaOH + CuSO4 The Na+ and Cu2+ switch places. Na+ combines with SO42- to form Na2SO4. Cu2+ combines with OH- to form Cu(OH)2 NaOH + CuSO4 Na2SO4 + Cu(OH)2 2NaOH + CuSO4 Na2SO4 + Cu(OH)2 CuSO4 + Na2CO3 : CuSO4 + Na2CO3 Double Replacement : Double Replacement CuSO4 + Na2CO3 Cu2+ combines with CO32- to form CuCO3. Na+ combines with SO42- to form Na2SO4. CuSO4 + Na2CO3 CuCO3 + Na2SO4 Na2CO3 + HCl : Na2CO3 + HCl Double Replacement : Double Replacement Na2CO3 + HCl Notice that gas bubbles were produced rather than a precipitate. What was the gas? Write the double replacement reaction first. Double Replacement : Double Replacement Na2CO3 + HCl Na+ combines with Cl- to form NaCl. H+ combines with CO32- to form H2CO3. Na2CO3 + 2HCl 2NaCl + H2CO3 H2CO3 breaks up into H2O and CO2. Double Replacement : Double Replacement The gas formed was carbon dioxide. The final balanced reaction is: Na2CO3 + HCl NaCl + H2O + CO2. Balance the equation. Na2CO3 + 2HCl 2NaCl + H2O + CO2 Combustion Reaction : Combustion Reaction When a substance combines with oxygen, a combustion reaction results. The combustion reaction may also be an example of an earlier type such as 2Mg + O2 2MgO. The combustion reaction may be burning of a fuel. Combustion Reaction : Combustion Reaction Methane, CH4, is natural gas. When hydrocarbon compounds are burned in oxygen, the products are water and carbon dioxide. CH4 + O2 CO2 + H2O CH4 + 2O2 CO2 + 2H2O Combustion Reactions : Combustion Reactions Combustion reactions involve light and heat energy released. Natural gas, propane, gasoline, etc. are burned to produce heat energy. Most of these organic reactions produce water and carbon dioxide. Practice : Practice Classify each of the following as to type: H2 + Cl2 2HCl Combination Ca + 2H2O Ca(OH)2 + H2 Single replacement Practice : Practice 2CO + O2 2CO2 Combination and combustion 2KClO3 2KCl + 3O2 Decomposition Practice : Practice FeS + 2HCl FeCl2 + H2S Double replacement Zn + HCl ? Single replacement Zn + 2HCl ZnCl2 + H2 Types of Chemical Reactions : Types of Chemical Reactions Read Chapter 8-2 Review nomenclature Do all of the practice exercises given in class.