Electron arrangements in ionisation energy
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What is the definition for ionisation energy?
the energy required to remove a mole of electrons from a mole of atoms in the gaseous state.
What is the ionisation energy measured in?
KJ mol-1
What is the abbreviation for ionisation energy?
IE
The first electron is the easiest electron to remove. Why is this?
Because it is being removed from a neutral atom.
The second electron is slightly harder to remove than the first. Why is this?
The second electron needs more energy to remove because it is being removed from a +1 ion.
The third electron needs even more energy to be removed. Why is this?
This is because the third electron is being removed from a +2 ion.
Draw a diagram for the 3 successive ionisation energies of sodium
Na(g) –> Na+(g) + e- (first IE) Na+(g) –> Na2+(g) + e- (second IE) Na2+(g) –> Na3+(g) + e- (third IE)
Which electron is the easiest to remove?
The first one that is furthest way from the positive nucleus
Which electrons are the hardest to remove?
The two nearest to the positive charge of the nucleus in the first energy level
Why does the ionisation energy increase across a period?
because the nuclear charge is increasing and this makes it more difficult to remove an electron
The ionisation energy increases across the…
periods in the periodic table
Why is it easier to remove paired electrons?
Because the repulsion between the two negative forces makes them easier to remove
The ionisation levels decrease as they go down a..
group in the periodic table
Why do the ionisation levels decrease as they go down a group in the periodic table?
The outer electron gets further from the nucleus as you go down the groups so the electrons do not have the same pull of attraction from the positive nucleus.
What do the inner electrons do to the nuclear charge?
They shield it from the outer electrons