In group 1 and 2 the melting and boiling point decrease down the group. - Size of atoms increases - More electrons - Larger size of molecules - Stronger van der waals forces between molecules - Molecules held together more strongly. This fact can be best rememberd by the physical states of the halogen molecules. Generally the melting point of the metals decreases down the group. It is seen that more reactive metal have lower melting and boiling points. Why does the melting point get lower going down the Alkali Metal Group with increase in atomic number? Boiling points Group 17 elements exist as simple diatomic molecules. This increase in size means an increase in the strength of the van der Waals forces. F < Cl < Br < I < At. Why do melting and boiling points increase down group 7? These generally increase with increasing relative molecular mass. The boiling points of group 13 and 14 elements decrease down the group, which is opposite to the trend suggested by van der Waals interactions. In each case the first member of the set has a significantly higher boiling point than would be expected from the boiling points … Opposite of Halogens. If you include magnesium, there is no obvious trend in melting points (see below). IN group 1 and 2 the metal become more reactive down the group and are more readily to give up their electrons to non-metals. Melting point. I suspect that the increase in melting point results from the change in crystal structure and the increasing metallic character of the elements as you go down the group. Stronger intermolecular forces/attractions implies that you need to supply more energy hence, an increase in melting and boling points. The size of the molecules increases down the group. However, if you include magnesium, you will see that its melting point is lower than the melting point of calcium, the next element down. This is because as the metal ions get larger the distance between the bonding electrons and the positive nucleus gets larger and reduces the overall attraction between the two. This fact can be best rememberd by the physical states of the halogen molecules. The force of attraction which keep these simple molecules together is temporary dipole-dipole attraction, also termed Van Der Waal’s (VDW) forces of attraction. For similar reasons the electronegativity decreases. Why does volatility decrease down group 7? Ok, you're looking for a generalization of what happens to the melting point as you go down a column in the periodic table. - Melting points increase - Gas→solid - Volatility decreases. There is a general decrease in melting point going down group 2. In group 7 the boiling point increase down the group. 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