Density & Electronegativity & Solubility
Density of Halogen
Generally, the densities of all of the elements increase as you go down the group. The reason may be that as you go down a group, the atomic structure increases. So as you go down the group 7A and element in the halogen family would have the same volume, the atomic mass increases. Density is mass divided by volume, so this causes the density to.
Generally, the densities of all of the elements increase as you go down the group. The reason may be that as you go down a group, the atomic structure increases. So as you go down the group 7A and element in the halogen family would have the same volume, the atomic mass increases. Density is mass divided by volume, so this causes the density to.
Electronegativity of Halogen
The number of valence electrons increases due to the increase in energy levels as the elements progress down the group. The electrons are not as near to the nucleus anymore. Therefore, the nucleus and the electrons are not as attracted to each other as much. An increase in shielding is observed. Electronegativity will therefore decrease down the group.
The number of valence electrons increases due to the increase in energy levels as the elements progress down the group. The electrons are not as near to the nucleus anymore. Therefore, the nucleus and the electrons are not as attracted to each other as much. An increase in shielding is observed. Electronegativity will therefore decrease down the group.
Solubility of Halogen
Halogens, being group VII elements, are non-polar substances requiring an electron to complete their octet thus forming covalent bonds in molecules. The forces between these molecules are called Van der Waals forces. However, in water the hydrogen molecules are the most prominent. Being a polar substance, its intra-molecular forces are higher in strength when compared to the Van der Waals forces in halogens. This hydrogen molecule bonding opposes the formation of bond between the halogen and water molecules.
As the water molecules have stronger intra-molecular forces and halogens have only the Van der Waals forces, they can form only weak intra-molecular bonds with water molecules.
The strongest type of intermolecular attraction is the presence of dipole-dipole forces. When halogen is mixed with water, the new intermolecular forces being formed are also the dipole-dipole forces, which however are weak, and thus the energy released in forming these weak bonds is negligible and is insufficient to overcome the intermolecular bonds that are existing in each of the samples. Thus, the formation of solution using halogen as solute and water as solvent is not possible.
A solution with halogen and water is not likely to form as halogen is insoluble in water. Due to absence of energy in the intra-molecular bonds between water and halogens, the strong bonds between each of water and halogen molecules cannot be broken thus making the halogen insoluble in water.
As the water molecules have stronger intra-molecular forces and halogens have only the Van der Waals forces, they can form only weak intra-molecular bonds with water molecules.
The strongest type of intermolecular attraction is the presence of dipole-dipole forces. When halogen is mixed with water, the new intermolecular forces being formed are also the dipole-dipole forces, which however are weak, and thus the energy released in forming these weak bonds is negligible and is insufficient to overcome the intermolecular bonds that are existing in each of the samples. Thus, the formation of solution using halogen as solute and water as solvent is not possible.
A solution with halogen and water is not likely to form as halogen is insoluble in water. Due to absence of energy in the intra-molecular bonds between water and halogens, the strong bonds between each of water and halogen molecules cannot be broken thus making the halogen insoluble in water.