Describe and explain the trends in atomic radii, ionic radii, first ionization energies, electronegativities and melting points for the alkali metals (Li->Cs) and the halogens (F->I)
- The atomic radius increases down a group as the number of occupied electron shells (given by the period number) increases.
- The ionic radius increases down a group as the number of electron shells increases.
- Ionisation energies decrease down a group as the increased charge of the nucleus doesn't affect the outer electrons due to shielding and that the increased distance from the nucleus makes them easier to remove.
- Electronegativity decreases down a group as the bond electrons are furthest from the nucleus and so there is reduced attraction.
- Melting points decrease down the group for the alkali metals as metallic structures are held together by attractive forces between delocalized electrons and the positively charged ions. This attraction decreases with distance from the nucleus.
- Melting points increase down the group for halogens because the elements are held together by Van Der Waals forces and the increased number of electrons in the atom means the elements are held together more strongly.
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