Which type of attractive forces do you expect between HCl3,HF,HCL?
I am no chemist but those are all compounds between Hydrogen and halogens which desperately want to grab an electron to fill their outer shells so I would expect Hydrogen bonds where the Hydrogen partially gives up its sole electron.
The type of force is therefore electrostatic (Coulomb) force in the simple model of atoms.
To determine the type of attractive forces between molecules, we need to consider the intermolecular forces at play. The three molecules mentioned in the question are HCl3 (trichloromethane), HF (hydrogen fluoride), and HCl (hydrogen chloride).
Intermolecular forces arise due to interactions between molecules and can be classified into three main types:
1. London dispersion forces: These forces exist between all molecules, regardless of their polarity. They arise from temporary fluctuations in electron distribution within molecules, leading to instantaneous dipoles. London dispersion forces generally increase with increasing molecular size and surface area.
2. Dipole-dipole forces: These forces occur between polar molecules and arise from the attraction between the positive end of one molecule and the negative end of another. The strength of dipole-dipole interactions depends on the magnitude of the molecular dipole moment.
3. Hydrogen bonding: This type of intermolecular force is a strong form of dipole-dipole interaction. It occurs when a hydrogen atom is directly bonded to a highly electronegative atom (usually fluorine, oxygen, or nitrogen) and is attracted to a lone pair of electrons on another electronegative atom. Hydrogen bonding is responsible for many unique properties of water and certain other compounds.
Now, let's analyze the three molecules mentioned:
1. HCl3 (trichloromethane): This molecule is non-polar since the chlorine atoms are identical and cancel out any dipole moment. The only intermolecular force in trichloromethane is London dispersion forces.
2. HF (hydrogen fluoride): HF is a polar molecule due to the electronegativity difference between hydrogen and fluorine. Therefore, it exhibits dipole-dipole forces and hydrogen bonding due to the presence of the highly electronegative fluorine atom.
3. HCl (hydrogen chloride): Similar to HF, HCl is also a polar molecule because of the electronegativity difference between hydrogen and chlorine. Hence, it exhibits dipole-dipole forces but does not form hydrogen bonds as chlorine is less electronegative than fluorine.
In summary, the type of attractive forces expected between these molecules are:
- HCl3: London dispersion forces
- HF: Dipole-dipole forces and hydrogen bonding
- HCl: Dipole-dipole forces