Ionisation Energy

HideShow resource information
  • Created by: Jasmin
  • Created on: 02-11-13 14:38
View mindmap
  • Ionisation Energy
    • Energy required to remove 1 electron from each atom in 1 mole of gaseous atom
    • Factors affecting I.E
      • Distance from nucleus: I.E decreases as go down group, distance increases
      • Nuclear charge: I.E increases if charge increases, higher no. of protons, higher the charge
      • Shielding (repulsion) by electrons in inner shell's between nucleus and outer electron
    • Go down group
      • Atomic radius increases and more shielding
        • Less/weaker attractions from nucleus to electrons in outer shell
    • Go across period
      • Nuclear charge increases as more protons
      • Atomic radius decreases therefore stronger attraction from nucleus to electron in outer shell
    • Electron repulsion
      • Bonded pair of electrons in an orbital and 2 unpaired electrons
        • Therefore paired electrons would repel as like charges repel making it easier to take electrons away
          • No change in electron shielding
    • Increased shielding, longer distance from nucleus
      • Easier to remove electron and has larger distance from nucleus poisitve attraction
        • Because more orbitals in way of nucleus
    • Effective Nuclear Charge
      • Net charge on the nucleus, after allowing for the electrons in orbit around the nucleus shielding its full charge
        • Increases as go up gorup
        • Positive ions get smaller as take away electrons
        • Negative ions get larger as forces of attraction stay the same
        • Atomic radii decreases as go down group. Greater nuclear charge increases force of attraction on the electrons, drawing them closer to the nucleus


No comments have yet been made

Similar Chemistry resources:

See all Chemistry resources »See all Energetics resources »