Objectives

Define and recognize Bronsted-lowery acids and bases.

Define a Lewis acid and a Lewis base.

Name compounds that are acids under the Lewis definition but are not acids under the Bronsted-Lowery definition.

  1. Section 15.2 Acid-Base Theories
    1. Bronsted-lowery Acids and Bases
      1. Bronsted-lowery acid is defined as a molecule or ion that is a proton donor
        1. When H+ is donated
        2. By definition can be a Bronsted-lowery acid and not an Arrhenius.
      2. Bronsted-lowery base is a molecule or ion that is a proton acceptor
        1. Ammonia is a proton acceptor
        2. NaOH is an Arrhenius base but not an Bronsted-lowery base.
      3. Bronsted-Lowery acid-base reaction- protons are transferred from one reactant (the acid) to another (the base).

       

       

       

       

    2. Monoprotic and Polyprotic acids
      1. monoprotic- an acid that can donate only one proton per molecule
      2. polyprotic- an acid that can donate more then one proton per molecule.
        1. Diprotic- two protons
        2. Triprotic- donate three protons
    3. Lewis Acids and Bases
      1. Lewis acid is an atom, ion, or molecule that accepts an electron pair to form a covalent bond.
      2. Lewis base is an atom, ion, or molecule that donates an electrom pair to form a colvalent bond.
      3. Lewis acid-base reaction- is the formation of one or more covalent bonds between an electron-pair and an electron-pair acceptor.
    4. Comparison of all definitions of acids and bases

    Table 15-5

    Type

    Acid

    Base

    Arrhenius

    		    

    Bronsetd-Lowery

    		    

    Lewis

    		    

     

     

    Objectives

    Describe a conjugate acid, a conjugate base, and an amphoteric compound.

    Explain the process of neutralization.

    Explain how the acid rain damages marble structures.

     

  2. Section 15-3 Acid-Base reactions
    1. Conjugate Acids and Bases
      1. Conjugate base is the species that remains after a Bronsted-lowery acid has given up a proton.
      2. Conjugate acid- the species that is formed when a Bronsted-lower base gains a proton.
      3. Practice
      4. Strength of Conjugate Acids and Bases.
        1. The stronger an acid the weaker its conjugate base; the stronger a base is the weaker it conjugate acid.
        2. Refer to table 15-6 to determine if strong acid or base.
    2. Amphoteric Compounds
      1. Compounds that can act as either an acid or base
      2. Water
    3. Neutralization Reactions
      1. Strong Acid-Strong Base Neutralization
      2. Neutralization is the reaction of hydronium ions and hydroxide ions to from water molecules.
    4. Acid Rain
      1. Many industrial process produce gases such as NO, NO2,CO2,SO2
      2. These dissolve in atmospheric water to produce an acid.
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