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Ionisation Energies
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- 1What is an ionisation energyAmount of energy required to remove 1 mol of electrons from one mol of gaseous atoms of an element, it is an endothermic reaction
- 2Effect of nuclear chargeMore protons meaning a stronger nuclear attraction, so electrons need more enrgy to be removed
- 3Effect of atomic radiusAttraction falls off rapidly with distance, meaning attraction falls
This means higher shielding meaning that outer shell electrons have less attraction - 4Ionisation energy down a groupAss you go down a group they decrease
This is because atomic radius increases meaning more shielding so attraction of outer shell electrons falls - 5Ionisation energies across periodsThey increase because proton number increases so electrons are pulled in with a larger positive, decreasing atomic radius. Also they stay in the same shell
- 6Why is there a drop between group 2-3Because outer electron is in a p-orbital, this has a higher energy so the electron is found further away
They are shielded by s-orbitals meaning it overides the increased nuclear charge - 7Drop between group 5-6In group 5 on electron is removed from a lone orbital, however group 6 has two repelling electrons meaning they repel eachother so are easier to remove
- 8Successive ionisation energiesThey increase because when electrons are removed there's less repulsion, what the atom becomes more positive resulting in electrons being held stronger
There are big jumps when a new shell is broken in to
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- A-Level (3.1 ) Chemistry Fichas sobre Ionisation Energies , creado por Reuben Veysey-Smith el 22/02/2016.
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- Reuben Veysey-Smith
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