Download
types of chemical reactions n.
Skip this Video
Loading SlideShow in 5 Seconds..
Types of Chemical Reactions PowerPoint Presentation
Download Presentation
Types of Chemical Reactions

Types of Chemical Reactions

154 Vues Download Presentation
Télécharger la présentation

Types of Chemical Reactions

- - - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

  1. Types of Chemical Reactions Reactions can be classified by what happens.

  2. Learning Objectives • Distinguish between synthesis and decomposition reactions. • Identify replacement reaction as single or double replacement reactions. • Identify the characteristics common to all oxidation reactions. • Distinguish between decomposition and oxidation reactions. • Distinguish between oxidation, complete combustion and incomplete combustion. • Describe what happens in a neutralization reaction. *

  3. Synthesis Synthesis means “To make” AKA Chemical Marriage Characteristics 2 reactants (usually elements) 1 product General Equation A + B ---> AB Examples Na + Cl2 ---> NaCl + Energy Ca + S ---> CaS Fe + O2 ---> Fe2O3 Decomposition Decompose means “Tear up” AKA Chemical Divorce Characteristics 1 reactant 2 or more products General Equation AB ---> A + B Examples H2O +Energy ---> H2 + O2 NaCl + Energy ---> Na + Cl2 Na(ClO4) + Energy ---> Na + Cl2 + O2 * Synthesis and Decomposition

  4. Single Replacement AKA Chemical Dating One element replaces similar element in a compound Metals replace metals, etc Characteristics Reactants -1 element, 1 compound Products - 1 element, 1 compound Endo, neutral or exothermic General Reaction A + BC ---> AC + B Examples Na + HCl --> NaCl + H2 K + CuCl2 ---> CaCl2 + Cu Li + H(NO3) --- > Li(NO3) + H2 Double Replacement AKA Chemical Double Dating Metal elements in 2 compounds trade places Metals replace metals Characteristics 2 reactant compounds 2 product compounds Endo, neutral or exothermic General Reaction AB + CD ---> AD + CB Examples NaI + Cu(NO3)2 ---> Na(No3) + CuI2 NaS + FeCl3 ---> NaCl + Fe2S3 Single and Double Replacement

  5. Oxidation/Combustion Reactions • AKA Oxygen Assisted Divorce • In these reactions oxygen breaks up a compound combining with all elements in the reactant compound • Combustion is the oxidation of an organic compound • Characteristics: • Oxygen (O2) is a reactant • All products contain oxygen • Always exothermic • Combustion reactions always produce CO or CO2 and H2O • General Equations • Oxidation AB + O2 ---> AO + BO • Complete Combustion CxHx + O2 ---> CO2 + H2O • Incomplete Combustion CxHx + O2 ---> CO + H2O • Examples FeS + O2 ---> Fe2O3 + SO3 C6H12O6 + O2 ---> CO2 + H2O C3H8 + O2 ---> CO + H2O *

  6. Neutralization Reactions • AKA Having Kids • These 2 types of reactions destroy (Neutralize acids) • Characteristics • One of the reactants is an acid • The products are water, a salt and maybe CO2 • Always exothermic • General Reactions: Hydroxide Neutralization HX + M(OH) ---> H2O + MX Carbonate Neutralization HX + M(CO3) ---> H2O + MX + CO2 • Examples: HCl + NaOH ---> H2O + NaCl H(NO3) + Ca(OH)2 ---> H2O + Ca(NO3)2 H2(SO4) + K2(CO3) ---> H2O + K2(SO4) + CO2 *

  7. Identification Homework Identify each of the following chemical equations. 1. C2H8S + O2  H2O + CO2 + SO ____________ 2. N2 + H2  NH3 ____________ 3. Ca + HCl  CaCl2 + H2 ____________ 4. Fe2C + O2  FeO + CO2 ____________ 5. NaCl + BaO  BaCl2 + Na2O ____________ 6. H2SO4 + NaOH  Na2SO4 + H2O ____________ 7. C6H15 + O2  H2O + CO ____________ 8. C6H12O6  2C3H6O3 ____________ 9. H4C + MgCO3  H2CO3 + CO2 + Mg2C ____________ 10. Fe + O2  Fe2O3 ____________ 11. Li + H2O  Li2O + H2 ____________