Atomic Structure

Mindmap for F321 1.1.1 Atomic Structure. Outlines the subatomic particles, isotopes and nuclides.

HideShow resource information
View mindmap
  • F321 1.1.1 Atomic Structure
    • The Sub-Atomic Particles
      • An atom must have the same number of electrons as protons. This makes all atoms neutral
    • Nuclides
      • The term used to describe any atom of which the atomic number and the mass number are specified
      • Written as-
        • Mass Number
          • (nucleon number)
            • The number of protons and neutrons present in the nucleus of the atom
        • X
        • Atomic Number
          • (proton number)
            • the number of protons present in the nucleus of the atom
              • in atoms the proton number is always equal to the number of electrons
      • Calculations
        • Number of Electrons
          • Positive ion (cation)
            • Subtract charge from atomic number
          • Negative ion (anion)
            • Add charge to atomic number
        • Number of Neutrons
          • Subtract atomic number from mass number
    • Isotopes
      • Definitions
        • Isotope
        • Relative atomic mass (Ar)
          • Average mass of the naturally occurring isotopes of the element relative to the mass of an atom of Carbon-12 which has a mass of 12
        • Relative isotopic mass
          • Average mass of a naturally occurring isotope of the element relative to the mass of an atom of Carbon-12 which has a mass of 12
      • Calculating relative atomic mass from isotopic abundance
        • Multiply abundance (%) by isotopic masses
  • Found in NUCLEUS
    • Neutrons
      • 0 Charge (neutral)
      • Relative Mass= 1
      • The Sub-Atomic Particles
        • An atom must have the same number of electrons as protons. This makes all atoms neutral
    • Protons
      • +1 Charge
      • Relative mass= 1
      • Every atom of the same element has the same proton number
    • Nucleus is tiny and extremely dense compared to the volume of an atom
  • Occupy a space somewhere OUTSIDE Nucleus
    • Electrons
      • -1 Charge
      • Relative Mass= 1/2000
      • Held in place my an electrostatic force from the nucleus
  • Add them together
    • Multiply abundance (%) by isotopic masses
  • Divide by 100
    • Add them together

    Comments

    Shannon Tennant-Smith - Team GR

    Amazing resource! Will definitely be coming back to this!

    Similar Chemistry resources:

    See all Chemistry resources »See all The Periodic Table resources »