The type of forces which exist in liquid hydrogen fluoride A. Only inter molecular forces B. Only intra molecular forces C. Both A&B D. HF does not exist as a liquid.
Answers
Explanation:
inter molecular Force option beta is right
Answer:
The forces that hold atoms together within a molecule are known as intramolecular forces. The forces that exist as the interactions between the molecules are known as the intermolecular forces.
Explanation:
Hydrogen bonding is the major intermolecular force in hydrogen fluoride (HF) (as hydrogen is bonded to fluorine). Dipole-dipole forces (also known as Van der Waals' forces) and London dispersion forces both occur because the molecule is polar.
The electron charge cloud, or the electrons around an atom's nucleus, is always moving in a non-polar molecule. This movement causes the electron cloud to flow toward one side of the molecule as opposed to the other.
This causes this portion of the molecule to briefly become somewhat negative. The other portion then starts to turn marginally positive. This is referred to as a temporary dipole. The London dispersion force of attraction is responsible for this.
The electrostatic force between (permanent) polar molecules is known as the dipole-dipole force. The molecular positive and negative ends are drawn together in this interaction.
The fluorine atom, which possesses three lone pairs of electrons, is bound to the hydrogen atom in an HF molecule.
Hence, the type of forces that exist in liquid hydrogen fluoride is only the intermolecular forces.
The correct option is A. Only intermolecular forces.
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