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CHEMICAL REACTIONS

CHEMICAL REACTIONS. How can we determine if a reaction will occur? What are the different types of reactions? How can we predict the products of a reaction? What are solubility rules?. Will a reaction occur?. If a solid is formed (a precipitate) If water is formed If a gas is formed

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CHEMICAL REACTIONS

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  1. CHEMICAL REACTIONS How can we determine if a reaction will occur? What are the different types of reactions? How can we predict the products of a reaction? What are solubility rules?

  2. Will a reaction occur? • If a solid is formed (a precipitate) • If water is formed • If a gas is formed • If electrons are transferred Then it is likely that a chemical reaction took place. • Also, if a new odor is produced, a new color is produced, or a change in energy (temperature, light, sound) occurs it is likely that a reaction occurred.

  3. Types of Chemical Reactions • Double Displacement (Precipitation) • Combustion • Single Replacement • Synthesis • Decomposition

  4. Predicting Products of Double Replacement Reactions • If a solid forms from the combining of two aqueous solutions, a reaction has occurred. • For our purposes, we will assume that all double replacement reactions occur. • However, please know that if both products are soluble in water, there will be no reaction. You will not be asked to predict this.

  5. Double Displacement Practice • Magnesium chloride solution is mixed with sodium carbonate solution (carbonate is CO3-2) • Potassium chloride solution is mixed with a silver nitrate solution (nitrate is NO3-1) • Sodium hydroxide (hydroxide is OH-1)is mixed with an aluminum sulfate solution (sulfate is SO4-2)

  6. Predicting Products of Combustion • Always water and carbon dioxide • Is a type of redox

  7. Single Replacement ( a type of Redox) • Use a metal activity series to determine if a reaction will occur. • If it will, cations trade places on the product side of the equation. • Ex. Mg + FeCl2 MgCl2 + Fe • Magnesium is more reactive than iron, so it replaces it and forms magnesium chloride

  8. Synthesis ( a type of Redox) • Balance the charges of the reactants to form the product • Example: Mg + Cl2 MgCl2

  9. Decomposition ( a type of Redox) • One reactant breaks into 2 or more products • Sometimes the component elements, but not always. • Examples: • 2H2O  2H2 + O2 • CuCO3  CuO + CO2

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