Intermolecular Forces - Introduction (Edexcel IAL Chemistry)

Spec point — 7.1

Intermolecular Forces - Introduction

Intramolecular forces

• Intramolecular forces are forces within a molecule and are usually covalent bonds
• Covalent bonds are formed when the outer electrons of two atoms are shared
• Single, double, triple and co-ordinate bonds are all types of intramolecular forces

Intermolecular forces

• Molecules also contain weaker intermolecular forces which are forces between the molecules

• There are three types of intermolecular forces:

  • Induced dipole – dipole forces also called van der Waals or London dispersion forces

  • Permanent dipole – dipole forces are the attractive forces between two neighbouring molecules with a permanent dipole

  • Hydrogen Bonding are a special type of permanent dipole - permanent dipole forces

  • Intramolecular forces are stronger than intermolecular forces

    • For example, a hydrogen bond is about one tenth the strength of a covalent bond

  • The strengths of the types of bond or force are as follows:

The varying strengths of different types of bonds

Induced dipole-dipole forces:

• Induced dipole - dipole forces exist between all atoms or molecules

  • They are also known as London dispersion forces

• The electron charge cloud in non-polar molecules or atoms are constantly moving

• During this movement, the electron charge cloud can be more on one side of the atom or molecule than the other

• This causes a temporary dipole to arise

• This temporary dipole can induce a dipole on neighbouring molecules

• When this happens, the δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other

• Because the electron clouds are moving constantly, the dipoles are only temporary

Relative strength

• For small molecules with the same number of electrons, permanent dipoles are stronger than induced dipoles

  • Butane and propanone have the same number of electrons
  • Butane is a nonpolar molecule and will have induced dipole forces
  • Propanone is a polar molecule and will have permanent dipole forces
  • Therefore, more energy is required to break the intermolecular forces between propanone molecules than between butane molecules
  • So, propanone has a higher boiling point than butane

Pd-pd forces are stronger than id-id forces in smaller molecules with an equal number of electrons

Permanent dipole - dipole forces:

• Polar molecules have permanent dipoles
• The molecule will always have a negatively and positively charged end

• Forces between two molecules that have permanent dipoles are called permanent dipole - dipole forces
• The δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other

Hydrogen bonding

• Hydrogen bonding is the strongest form of intermolecular bonding

  • Intermolecular bonds are bonds between molecules
  • Hydrogen bonding is a type of permanent dipole – permanent dipole bonding

• For hydrogen bonding to take place the following is needed:

  • A species which has an O, N or F(very electronegative) atom bonded to a hydrogen

• When hydrogen is covalently bonded to an O, **N **or F, the bond becomes highly polarised

• The H becomes so δ⁺ charged that it can form a bond with the lone pair of an O, N or F atom in another molecule

• For example, in water

  • Water can form two hydrogen bonds, because the O has two lone pairs

Hydrogen bonding in water

Exam Hint Make sure to use a dashed, straight line when drawing your intermolecular forces! Hydrogen bonds should start at the lone pair and go right up to the delta positive atom - it must be really clear where your H bond starts and ends.