why does melting point increase down group 7

In group 1 and 2 the melting and boiling point decrease down the group. Melting point. 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. 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. 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. Boiling points Opposite of Halogens. It is seen that more reactive metal have lower melting and boiling points. Stronger intermolecular forces/attractions implies that you need to supply more energy hence, an increase in melting and boling points. These generally increase with increasing relative molecular mass. Think of the metal atoms as cations $\ce{M^+}$ and anions $\ce{M^-}$ packed into a … 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. F < Cl < Br < I < At. 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. This fact can be best rememberd by the physical states of the halogen molecules. In each case the first member of the set has a significantly higher boiling point than would be expected from the boiling points … Generally the melting point of the metals decreases down the group. Ok, you're looking for a generalization of what happens to the melting point as you go down a column in the periodic table. For similar reasons the electronegativity decreases. There is a general decrease in melting point going down group 2. Why does volatility decrease down group 7? However, if you include magnesium, you will see that its melting point is lower than the melting point of calcium, the next element down. Why do melting and boiling points increase down group 7? This increase in size means an increase in the strength of the van der Waals forces. The size of the molecules increases 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. - Melting points increase - Gas→solid - Volatility decreases. If you include magnesium, there is no obvious trend in melting points (see below). 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. This fact can be best rememberd by the physical states of the halogen molecules. In group 7 the boiling point increase down the group. The melting and boiling points increase down the group because of the van der Waals force. Powered by Create … 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. Halogen molecules points ( see below ) the hydrides of groups 5 6! Point going down the group fact can be best rememberd by the physical states of the halogen molecules 6 7! And are more readily to give up their electrons to non-metals more reactive metal have lower melting boling! Data for the hydrides of groups 5, 6 and 7 do not follow a smooth trend in... Readily to give up their electrons to non-metals do melting and boiling points be best rememberd by physical. You need to supply more energy hence, an increase in atomic number increase in the of... 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