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CHEMICAL REACTIONS

This guide explores the fundamentals of chemical reactions, including how to determine if a reaction will occur and the different types of reactions. Key indicators of a reaction taking place include the formation of a solid (precipitate), water, a gas, or the transfer of electrons. We also outline solubility rules and discuss predicting products of double replacement, combustion, synthesis, and decomposition reactions. Practical examples illustrate reaction predictions and highlight the importance of the activity series in single replacement reactions.

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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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