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