Ionic Radius: Increases down the group, decreases across a period
Ionisation Energy: Decreases down the group, increases across a period
The halogens show increasing boiling point down the group due to increasing van der Waals forces between molecules
Reactivity and Periodicity
- For the metals, the reactivity increases moving down the group
- This can be explained by ionisation energies. The group 1 metals will lose an electron to make an ion with a 1+ charge. The less energy needed to remove the electron, the more likely it is to happen and therefore the more reactive the metal
- Ionisation energy decreases down the group, so reactivity decreases
- For non-metals the situation reverses
- This is because the atoms gain an electron, so the more attraction there is between the outer electrons and the nucleus, the more reactive it is
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