Chapter 3: Atomic Structure

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Chemistry Mind Map on Chapter 3: Atomic Structure, created by helensellers75 on 27/01/2014.
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Chapter 3: Atomic Structure
  1. How is it made?

    Annotations:

    • The only atom with no neutrons is the simplest isotope of Hydrog
    1. Most of mass is in the nucleus

      Annotations:

      • Proton: Charge +1 Mass 1 Electrons: Charge -1 Mass 1/1836 Neutron: Charge 0 Mass 1
      1. Numbers

        Annotations:

        • Atomic number= no of protons Mass number = number of protons + neutrons 35        Cl 17     
      2. Isotopes

        Annotations:

        • Isotopes are atoms with some atomic number but different mass numbers. They contain same number of protons but different numbers of neutrons
        1. Example:

          Annotations:

          • Isotope            Proton     Neutrons Hydrogen-1       1                0 Hydrogen-2        1                1 Hydrogen-3        1               2   
        2. The electrons

          Annotations:

          • Same as proton number Carbon- 6 electron Sodium- 11 electrons
          1. Shells

            Annotations:

            • Electrons exist around the nucleus in different energy levels called electron shells
            1. Organised

              Annotations:

              • 1st Shell = 2 2nd Shell= 8 3rd Shell = up to 18
          2. Relative Atomic Mass
            1. Chlorine

              Annotations:

              • Chlorine has 2 isotopes: Chlorine-35      Chlorine-37 Total mass of 100 atoms= (75 x 35)+ (25 x 37) = 3550 Average mass= 3550/100  = 35.5 Ar = 35.5
            2. Relative formular mass

              Annotations:

              • Hydrogen (H2) 1 x 2 = 2  H2O 1 x 2 + 16= 18
              1. Involving Crystallisation

                Annotations:

                • Hydrated Mg Sulphate  MgSO4. 7H2O - calculate Mr of MgSO4 = 24 + 32 + (4 x 16)= 120 Add 7 x Mr of H2O = 7 x 18= 126 Mr = 120 + 126 = 246
              2. The Mole
                1. Measure of an amount of substance

                  Annotations:

                  •  1 Mole is the amount that contains 6 x 10 (23)  particles of the substance
                  1. 6 x 10 (23) = Avagadro Number

                    Annotations:

                    • Sodium Chloride is an ionic compound and therfore doesn't contain molecules
                    1. Detail +

                      Annotations:

                      • 1 mol of Na contains AN atoms of Sodium 1 mol of H2 has AN molecules of hydrogen 1 mol of NaCl contains AN formulae of Sodium Chloride
                    2. Calculating mass of 1 mole
                      1. Ar in grams

                        Annotations:

                        •                   Ar                  Mass H               1                      1g O                16                   16g Na             23                    23g
                        1. Mr in grams:

                          Annotations:

                          •                      Mr                Mass H2                 1 x 2                2g H2O             2 x 1 + 16        18g
                        2. Molar Volume of Gas

                          Annotations:

                          • 1 mol has a volume of 24 dm (3) Volume = amount x 24 H     3 mol     3 x 24 = 72 CO2     0.25mol   0.25 x 24 = 6
                          1. Amount of Gas

                            Annotations:

                            • Amount of gas (moles) = volume/ 24 Methane     225.6 dm   225.6/24= 9.4 mol Oxygen    1200 cm (3) /1000        1.2/ 24 = 0.05 mol
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