What kind intermolecular force do you expect in the following substance?
1. Hydrogen iodide
2. Kryptone
1. strong, due to polarity of the electrostatic bond in HI
2. Weak, due to the complete electron shells of Kr. It does not easily acquire or lose electrons, and its interaction with other Kr atoms is very weak.
To determine the type of intermolecular force in a substance, we need to consider the types of molecules present and their properties.
1. Hydrogen iodide (HI):
In HI, hydrogen (H) has a partial positive charge and iodine (I) has a partial negative charge. This is because iodine is more electronegative than hydrogen, leading to a polar covalent bond. The intermolecular force in hydrogen iodide is a dipole-dipole force, which is a strong intermolecular force.
2. Krypton (Kr):
Krypton is an element from the noble gas group, which means its outer electron shell is already full. This results in Kr having a stable electronic configuration with no tendency to acquire or lose electrons. As a result, the intermolecular force in krypton is weak. The only intermolecular force present in krypton is London dispersion forces, which are caused by temporary fluctuations in electron distribution and induce temporary dipoles in adjacent atoms or molecules.
In summary, for hydrogen iodide (HI), the intermolecular force is a strong dipole-dipole interaction due to the polarity of the electrostatic bond. For krypton (Kr), the intermolecular force is weak and predominantly governed by London dispersion forces because of the complete electron shells and the resulting lack of strong intermolecular interactions.