Chemical Reactions

• Chemical Reaction


  refers to a process in which atoms of the same or different elements rearrange themselves to form one or more new substances
• several indicators that a chemical reaction has taken place

  • Color change
  • Temperature change
  • Emission of light
  • Evolution of gas
  • Precipitation
  • Change in voltage
• Chemical equation


  Consists of symbols and formulas of the reactants substance and their products
• reactants


  Reacting substances, can be shown on the left side of the arrow
• Products


  The substance produce from the reaction. This can be written on the right side of the arrow
• combination or synthesis


  Chemical reaction that involves two or more reactants that form a more complex substance
• decomposition or analysis


  The reaction in which compound is broken down into its components elements or into simpler compounds
• electrolysis


  Example of decomposition that can turn liquid water into hydrogen and oxygen
• Single replacement or substitution


  A reaction in which a more active free element represented by X replaces a less active one in a compound. These type of reaction produces a new compound and an element as products.
• activity series list


  Common metals in decreasing order of their ability to replace metal ions in a aqueous solution
• double replacement double, decomposition, or metathesis


  The reaction in which two compounds exchange, metallic and non-metallic ions to form new compounds
• two most common double replacement reaction

  • precipitation
  • neutralization
• precipitatesome reactions produce a solid compound
• precipitation reaction


  it usually results from mixing aqueous solutions of two compounds
• Neutralization reaction


  Acid and bases react to produce salt and water
• Strong bases


  are compounds that dissociate and form OH ions
• Hydrochloric acid


  is naturally produced in stomach to help in food digestion
• law of conversation of mass


  States that mass is neither created nor destroyed in any ordinary chemical reactions.
• Coefficients 


  Which are whole numbers placed before the symbols or formulas of reactants or products
• Deterioration


  Occurs when they are exposed to and react with certain substances in the environment
• Reduction-oxidation


  Reaction where there is a transfer of electrons between reactants
• oxidation


  Occurs when electrons are lost, indicated by an increase in the oxidation state of an element
• reduction


  Takes place where there is gain of electrons indicated by a decrease in the oxidation state of the element
• reducing agent


  The reactant that gives up electrons is said to be oxidized
• oxidizing agent


  The reactant that gains the electrons is reduced
• oxidation state or oxidation number


  Refers to the charge that the atom will have if all atoms represent as monatomic ions
• balancing this type of reaction requires tracking the oxidation states of the reactants in a technique known as oxidation state method
• voltaic cell


  Known as galvanic cell, use a spontaneous redox reaction to generate electrical energy via an external circuit
• electricity is generated by inducing reduction and oxidation reactions in the two separate surface called electrodes.
• electrode where oxidation takes place is called the anode and that where reduction occurs is the cathode
• Bioluminescence


  A light that can be produced by fireflies
• A rate of chemical reaction


  Refers to the speed that we should either decompose or combine to form new substances
• activation energy of a action


  is the minimum amount of energy that reactant particles must have to initiate the reaction
• types of reaction

  • Combination reaction
  • Decomposition reaction
  • Single replacement reaction
  • Double Replacement reaction