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Single Replacement Reactions: A +BC  AC + B

Single Replacement Reactions: A +BC  AC + B. An element takes the place of another element in a compound. It could be a metal taking the place of another metal or hydrogen or a halogen taking the place of another halogen. MgSO 4 (aq) + Fe(s). Mg(s) + FeSO 4 (aq) 

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Single Replacement Reactions: A +BC  AC + B

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  1. Single ReplacementReactions: A +BC  AC + B An element takes the place of another element in a compound. It could be a metal taking the place of another metal or hydrogen or a halogen taking the place of another halogen. MgSO4 (aq) + Fe(s) Mg(s) + FeSO4(aq)  Cl2(g) + KBr(aq)  Fe(s) + MgSO4 (aq)  Br2 (aq) + KCl(aq)  Magnesium is more active than Iron and KCl(aq) + Br2 (aq) Chlorine is more active than Bromine! N.R. N.R.

  2. Lithium For metals: Li Cs Rb K Ba Sr Ca Na La Mg Be Al Mn Zn Cr Fe Cd Co Ni Sn Pb H Cesium Activity Series: Rubidium Potassium Barium For halogens: Strontium Activity Decreases Calcium Sodium Activity Decreases F Cl Br I Fluorine Lanthanum Magnesium Chlorine Beryllium Bromine Aluminum Iodine Manganese Zinc H Cu Hg Ag Pt Au Chromium Hydrogen Iron Copper Cadmium Mercury Cobalt Nickel Silver Tin Platinum Lead Gold Hydrogen

  3. Double Replacement Reactions : AB +CD  AD + CB It is a reaction between two ionic compounds in which the ions switch positions: The positive of the first combines with the negative of the second and the positive of the second with the negative of the first. MgCO3(s) + FeSO4(aq)  BaCl2(aq) + KBr(aq)  Fe(NO3)3(aq)+Ca3(PO4)2(s) CuBr2 (aq) + KCl(aq)  MgSO4 (aq) + FeCO3 (s) 2 BaBr2(aq) + KCl(aq) 2 Ca(NO3)2(aq)+ FePO3(s) 2 2 3 CuCl2 (aq) + KBr(aq) 2 2

  4. One of the types of double-replacement reactions is when a precipitate is formed. When a precipitate is formed, the compound will be either insoluble or slightly soluble. An example of this type of reaction is: Pb(NO3)2(aq) + 2KI (aq) --> Double-replacement reactions PbI2(s) + 2KNO3(aq) When one of the products is a gas, double-replacement reactions also occur. For example: FeS(s) + 2HCl(aq) --> H2S(g) + FeCl2(aq) An example of a double-replacement reaction where water is one of the products is: HCl(aq)+ NaOH(aq) --> NaCl (aq) + H2O(l) This is a neutralization reaction: Acid + Base = Salt + Water http://www.cameron.k12.wi.us/high/chemistry/drreac.html

  5. Combustion of a hydrocarbon: Hydrocarbon+O2(g)C O2(g)+H2O(g) When a substance combines with oxygen releasing a large amount of energy in the form of light and heat, it is a combustion reaction. An example of a combustion reaction is: C3H8 + 5O2 --> 3CO2 + 4H2O + +  http://www.cameron.k12.wi.us/high/chemistry/comreac.html http://newtraditions.chem.wisc.edu/FPTS/fbeqns/eqncombf.htm

  6. Decomposition Reactions:ABC… A +B +C … Decomposition: the breaking down of a compound into one or more substances. (usually energy is required) EXAMPLES:CO2 (g) ----- C(s) + O2(g) 2Fe2O3 (s)- 4Fe(s) + 3O2 (g) • Generalizations: • A binary compound decomposes into two elements. • A hydroxide of the metal decomposes into an oxide of the metal and water. • A ternary salt decomposes into an oxide of the metal and an oxide of the non metal. • A ternary or oxoacid decomposes into the oxide of a non metal and water .

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