Atomic Structure

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  • Created by: jodi
  • Created on: 07-01-19 16:54
Explain the trend in the first ionisation energies down group one.
Ionisation energy decreases down a group as more principle energy levels are added so the outer electron is increasingly getting further from it's nucleus and does not experience the full effect of the nuclear charge.
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Further explain the trend in the first ionisation energies down group one.
The outer electron is shielded more from inner electrons as the atomic radius increases therefroe less energy will be required to remove it.
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Explain the trends shown in the successive ionisation energies of magnesium.
The successive ioniation energies increase as an electron is removed each time due to a shorter distance between the outer electron and nucleus thus having an increased attraction, in addition to the lower shielding effect.
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Explain the general trend in the first ionisation energies across a period.
General increase. Due to increasing nuclear charge as each atom gains a proton. As a result, the outer electron experiences a stronger attraction to the nucleus thus more energy is required to remove it. Shielding stays constant thus takes no effect
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Why is the first ionisation energy of boron below that of beryllium?
Borons outer electron is being removed from a 2p orbital compard to a 2s in beryllium which is further from the nucleus therefore it has a smaller attraction and less energy is required to remove it.
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Why is the first ionisation energy of oxygen below that of nitrogen?
Oxygens outer electron is paired in a 2p orbital therefore it experiences repulsion and is easily removed to obtain a half filled 2p sub-shell.
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What are the factors which affect Ionisation energies?
Nuclear charge, Shielding, Distance
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Other cards in this set

Card 2

Front

Further explain the trend in the first ionisation energies down group one.

Back

The outer electron is shielded more from inner electrons as the atomic radius increases therefroe less energy will be required to remove it.

Card 3

Front

Explain the trends shown in the successive ionisation energies of magnesium.

Back

Preview of the front of card 3

Card 4

Front

Explain the general trend in the first ionisation energies across a period.

Back

Preview of the front of card 4

Card 5

Front

Why is the first ionisation energy of boron below that of beryllium?

Back

Preview of the front of card 5
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