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