The intermolecular forces present in liquid chlorine are London dispersion forces. These are weak forces that occur between all molecules, including non-polar molecules like chlorine. They are caused by temporary imbalances in electron distribution within a molecule, leading to a temporary dipole moment.
The intermolecular forces in liquid chlorine are relatively weak, which allows the molecules to move past each other easily. This results in a low boiling point (-34.04°C) and low viscosity. Additionally, the weak forces do not allow for strong intermolecular interactions, resulting in low surface tension.
The intra molecular forces present in liquid chlorine are covalent bonds. Chlorine molecules are made up of two atoms bonded together by sharing electrons. These bonds are strong and hold the molecule together.
The strong covalent bonds within a molecule of liquid chlorine contribute to the stability of the substance. These bonds are difficult to break, meaning that the molecules will remain intact at normal temperatures and pressures.
Yes, the intermolecular forces in liquid chlorine can be manipulated. For example, by increasing the temperature, the molecules will gain more energy and will be able to overcome the weak intermolecular forces, resulting in the liquid becoming a gas. Additionally, adding solutes to the liquid can also affect the intermolecular forces, as the solutes may disrupt the interactions between chlorine molecules.