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Definition of the first ionisation energy
The energy needed to remove one electron from
each atom in one mole of gaseous atoms.
This can be written by using the formula;
X(g) X(g) + e
It is important to
note the gaseous
state of the atom
and ion…read more

Slide 3

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What effects the first ionisation
energies?
· Shielding from electrons
· Atomic radius
· Charge of the nucleus…read more

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Shielding
· This is when electrons in lower sub-shells
block the nucleus from the valence electrons
(electrons in the outer shell).
· This lessens the attractive force between the
nucleus and the valence electron, making the
valence electron easier to remove.
· Evidence for this is the trend down group 2
Valence electron
Shielding electrons…read more

Slide 5

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Atomic Radius
· This is just a fancy name for the distance
between the nucleus and the valence (outer)
electron
· The bigger the atomic radius, the weaker the
force of attraction is between the nucleus and
the valence electron, so there is a lower
ionisation energy
Smaller atomic radius, so Larger atomic radius, so
greater force of attraction smaller force of attraction
between the nucleus and the between the nucleus and the
valence electron valence electron…read more

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Charge of the nucleus
· The higher the mass number, the higher the
charge of the nucleus
· The higher the charge of the nucleus, the
more attracted the electrons are to the
nucleus, making them harder to remove
· Evidence for this is the trend in ionisation
energies across period 3…read more

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