It is seen that more reactive metal have lower melting and boiling points. The size of the molecules increases down the group. Notice how the data for the hydrides of groups 5, 6 and 7 do not follow a smooth trend. 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. There is a general decrease in melting point going down group 2. However, if you include magnesium, you will see that its melting point is lower than the melting point of calcium, the next element down. Powered by Create … For similar reasons the electronegativity decreases. 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). Generally the melting point of the metals decreases down the group. Melting point. This fact can be best rememberd by the physical states of the halogen molecules. Group 17 elements exist as simple diatomic molecules. 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. - Size of atoms increases - More electrons - Larger size of molecules - Stronger van der waals forces between molecules - Molecules held together more strongly. Why does volatility decrease down group 7? Why does the melting point get lower going down the Alkali Metal Group with increase in atomic number? F < Cl < Br < I < At. These generally increase with increasing relative molecular mass. 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. 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 … 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. - Melting points increase - Gas→solid - Volatility decreases. 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. Think of the metal atoms as cations $\ce{M^+}$ and anions $\ce{M^-}$ packed into a … Stronger intermolecular forces/attractions implies that you need to supply more energy hence, an increase in melting and boling points. Boiling points 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. 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