Ionisation Energy
- 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
- Atomic radius increases and more shielding
- 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
- Therefore paired electrons would repel as like charges repel making it easier to take electrons away
- Bonded pair of electrons in an orbital and 2 unpaired electrons
- 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
- Easier to remove electron and has larger distance from nucleus poisitve attraction
- 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
- Net charge on the nucleus, after allowing for the electrons in orbit around the nucleus shielding its full charge
Comments
No comments have yet been made