Chem

Ionisation energy

The energy required to remove one electron from each atom in one mole of gaseous atoms to from one mole of gaseous 1+ ions

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Electron sheilding

The repulsion between electrons in different inner shells. Sheilding reduces the net attractive force from the positive nucleus on the outer shell electrons.

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Successive ionisation energies

A measure of the energy required to remove each electron in turn.

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Name the 3 factors affecting ionisation energy

1. Atomic radius 2. Nuclear charge 3. Electron sheilding or screening

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Explain the atomic radius, the greater the atomic radius...

The greater the atomic radius the smaller the nuclear attraction experienced by the outer electrons.

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Explain the nuclear charge, the greater the nuclear charge...

The greater the nuclear charge the greater the attractive force on the outer electrons

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Explain electron sheilding or screening (3 points)

Inner shells of electrons repel the outer-shell electrons, this repelling effect is called electron shielding, the more inner shells there are, the larger the sheilding effect and the small the nuclear attraction experienced by the outer electrons

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True or false: each successive ionisation energy is larger than the one before?

True

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each successive ionisation energy is larger than the one before? (3 points)

As each electron is removed, there is less repulsion between the electrons and each shell will be drawn slightly closer to the nucleus. As the distance of each electron from the nucleus decreases slightly the nuclear attraction increases.

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Sometimes you will see a large increase in successive ionisation energies. Why?

The large increase between the 1st and 2nd electron of Li shows that the second electron has been removed from a different shell, closer to the nucleus and with less sheilding from inner electrons.

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