Ionisation Energy- The energy required to remove an electron from each atom in a mole of gaseous atoms.
Na(g) ----> Na+(g) + e- (Example of equation for first ionisation energy)
Na+(g) ----> Na2+(g) + e- (Example of equation for second ionisation energy)
Factors affecting ionisation energy-
- If the atomic radius is larger, the nuclear attraction felt by electrons on the outer shells is reduced, this decreases the first ionisation energy.
- The greater the charge on the nucleus, the greater the attractive force on the outer electrons, this increases the first ionisation energy as it makes the electrons harder to lose.
- The more electron shells there are, the greater the effect of electron shielding, this decreases the nucluear attraction on outer electrons, and actively repels them due to the other electrons sharing the same charge, thus decreasing the first ionisation energy.
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