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CHEMICAL REACTIONS, K - Coggle Diagram

- - - - Example : 2Al(s) + 3CuCl(aq) --> 2AlCl(aq) + 3Cu(s)
        Cu + AlCl --> No reaction
      - To detemine the reactivity of each element we need to look at the Activity series
      - When displacing hydrogen in water or acid, there are only several elements can displace, they are highly reactive.
        
        For acid : the elements can displace hydrogen are elements above Hydrogen in the activity series table
        For water : The elements can displace hydrogen are above magnesium in the activity series table
- - - - Often described as reaction that creates a simpler compound
    - - Synthesis also happens in single, double displacement and combustion reactions
    - - When the reactants are solids, the reaction often occurs within solutions
    - - Synthesis experiments are conducted in high temperature
- - - - These reactions can be viewed as taking place in two steps, and can be written as net ionic equations.
        When a compound is in an aqueous solution (dissolved in water), then it exits as its separated ions.
      - How to write:
        1.Balance the molecular equations.
        2.Determine the states for each compounds.
        3.Get the ions for all aqueous compounds (complete ionic equations).
        4.Cross out spectator ions.
        5.Write down the remaining ions (net ionic equations)
      - Example: AgF + NaBr → AgBr + NaF (total ionic equation); Ag+ + Br- → AgBr(s) (net ionic equation
  - - - Some double displacement reactions can produce solids in their reactions. These solids will be found in one of the products and are called precipitates.
        Refers to the solubility table when balancing and predicting the products for this type of reaction.
      - Example: 2AgNO3 (aq) + CuCl2 (aq) → Cu(NO3)2 (aq) + 2AgCl(s)
    - - There is a special type of double displacement reaction that produces water as a product; called neutralization reactions. The product formed can be seen when the net ionic equation is written out.
      - General Formula: H+(aq) + OH-(aq) → H2O(aq)
    - - There are some reactions that can produce a gas in their product
        Two types of gases will be covered in CHE11: carbon dioxide (CO2) and ammonia (NH3).
        In both the cases of these gases, there are two reactions that happen right after one another (like a single process).
        
        Example: CH3COOH + NaHCO3 → NaCH3COO(aq) + H2O (l) + CO2 (g)
        
        Produces Ammonia (NH3): If the product of the double displacement reaction includes Ammonium Hydroxide (NH4OH), the product will have ammonia (NH3).
        
        Example: NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3 (g) + NaCl(aq)
        
        Produces Carbon Dioxide (CO2): If the product of the double displacement reaction includes carbonic acids (H2CO3), the product will have carbon dioxide (CO2) gas.
- - - - Binary Decomposition: Binary compounds (ionic and covalent) will tend to break down (decompose) into their substituent parts
      - Decomposition of Metal Nitrates: Metal nitrates (being non-binary compounds (will not break down into their individual elements. Instead, they will break down into a metal nitrite and oxygen gas. Other reactions can occur (i.e. production of nitrogen gas) depending on the conditions of the reaction.
      - Decomposition of Metal Carbonates: Metal carbonates (being non-binary compounds) will not break down into their individual elements. Instead, metal carbonates will predictably break down into a metal oxide and carbon dioxide.
      - Decomposition of Metal Hydroxides:Metal hydroxides (being non-binary compounds) will not break down into their individual elements. Instead, metal hydroxides will predictably break down into a metal oxide and water.