Intermolecular Forces

ability of an atom in a particular molecule to attract bonding electrons to itself.

• ionisation energy

• electron affinity

• electronegativity

• atomic size

the product of the magnitude of the charge (δ) and the distance (d )

that separates the centre of positive and negative charge.

• ionisation energy

• electron affinity

• dipole moment

• atomic size

differences in electronegativity of the bonded atoms

• polar bonding

• non-polar bonding

• electron-electron repulsion

• effective nuclear charges

This molecule is

• Polar

• Non-Polar

This molecule is

• Polar

• Non-Polar

This molecule is

• Polar

• Non-Polar

This molecule is

• Polar

• Non-Polar

Two type of intermolecular forces ​ (a)   and ​ (b)  

• a)covalent bond
• a) hydrogen bond
• b)van der waals forces
• b) ionic bond

Polar covalent molecules are sometimes described as “dipoles” molecules as it has 2 poles.

• metallic bond

• Hydrogen bond
• dipole-dipole forces
• london dispersion forces

Results from instantaneous non-permanent dipoles created by random electron motion. The distribution of electrons at a given instant in time, may not be equal around an individual atom. This gives rise to a temporary dipole.

• metallic bond

• Hydrogen bond
• dipole-dipole forces
• london dispersion forces