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JordanThe boiling points of halogens generally increase as you move down the group from fluorine to iodine. This is due to the increase in the size and relative Atomic Mass of the atoms, which leads to stronger van der Waals forces between the molecules.
The boiling points of the members of last four groups of Periodic Table including Halogens increase from top to bottom with the rise of atomic size, it is due to the increase in molecular size which is responsible to increase the Vander waal's forces among the molecules.
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How can you account for the fact that all halogens easily become gases?
Halogens easily become gases because of their low boiling points and weak intermolecular forces. As you move down the halogen group in the periodic table, the atomic size increases, which leads to weaker intermolecular forces, making it easier for the halogens to transition from a solid or liquid state to a gas at relatively low temperatures.
Do the halogens have a higher boiling point going down the group and why is that?
Yes, halogens have a higher boiling point going down the group. This is because the atomic size increases with atomic number, leading to stronger London dispersion forces between molecules as the size increases. Consequently, more energy is required to overcome these forces, resulting in higher boiling points.
What is the trend in density as you go down the group of halogens?
The density increase down.
What is the density trend in halogens as you go sown the group?
As you move down the group of halogens in the periodic table, the density generally increases. This trend is due to the larger atomic and molecular masses of the heavier halogens, which outweigh the increase in volume. For example, fluorine and chlorine are gases at room temperature, while bromine is a liquid and iodine is a solid, reflecting their increasing densities. Thus, the trend shows that as you descend the group, the halogens become denser.
When was Boiling Points created?
Boiling Points was created on 2004-01-05.
