This increase in size means an increase in the strength of the van der Waals forces. In group 1 and 2 the melting and boiling point decrease down the group. It is seen that more reactive metal have lower melting and boiling points. If you include magnesium, there is no obvious trend in melting points (see below). Melting point. 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. F < Cl < Br < I < At. This fact can be best rememberd by the physical states of the halogen molecules. These generally increase with increasing relative molecular mass. There is a general decrease in melting point going down group 2. Why does volatility decrease down group 7? 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. Think of the metal atoms as cations $\ce{M^+}$ and anions $\ce{M^-}$ packed into a … However, if you include magnesium, you will see that its melting point is lower than the melting point of calcium, the next element down. as u go down a group , with increase in the atomic mass vanderwaal's force of attraction increases, thus increasing the melting and boiling point.Intermolecular forces. Generally the melting point of the metals decreases down the group. Why does the melting point get lower going down the Alkali Metal Group with increase in atomic number? Notice how the data for the hydrides of groups 5, 6 and 7 do not follow a smooth trend. Boiling points Stronger intermolecular forces/attractions implies that you need to supply more energy hence, an increase in melting and boling points. Stronger intermolecular forces/attractions implies that you need to supply more energy hence, an increase in melting and boling points. - Size of atoms increases - More electrons - Larger size of molecules - Stronger van der waals forces between molecules - Molecules held together more strongly. Group 17 elements exist as simple diatomic molecules. Opposite of Halogens. Ok, you're looking for a generalization of what happens to the melting point as you go down a column in the periodic table. Why do melting and boiling points increase down group 7? For similar reasons the electronegativity decreases. 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. Powered by Create … In each case the first member of the set has a significantly higher boiling point than would be expected from the boiling points … In group 7 the boiling point increase down the group. 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