Bond energy

• The?bond energy?is the energy required to?break?one mole of a particular covalent bond in the gaseous states
  • Bond energy has units of kJ mol-1
• The?larger?the bond energy, the?stronger?the covalent bond is

Bond length

• The?bond length?is?internuclear distance of two covalently bonded atoms
  • It is the distance from the nucleus of one atom to another atom which forms the covalent bond
• The?greater?the forces of attraction between electrons and nuclei, the more the atoms are pulled closer to each other
• This?decreases?the?bond?length?of a molecule and?increases?the?strength?of the covalent bond
• Triple bonds?are the?shortest?and?strongest?covalent bonds due to the large electron density between the nuclei of the two atoms
• This increase the forces of attraction between the electrons and nuclei of the atoms
• As a result of this, the atoms are pulled closer together causing a shorter bond length
• The increased forces of attraction also means that the covalent bond is?stronger

Triple bonds are the shortest covalent bonds and therefore the strongest ones

Reactivity of covalent molecules

• The?reactivity?of a covalent bond is greatly influenced by:
  • The bond?polarity
  • The bond?strength
  • The bond?type?(σ/π)

Worked example: Bond lengths & bond energies

Answer

Answer 1:?Going down the halogen group, the atoms are bigger; the attractive force between the bonding electrons and the nucleus get smaller so less energy is needed to break the atom

Answer 2:?Going down the group the increase in bond length is approximately 0.14-0.20 nm

Fluorine is smaller than HCl, so a value between 0.09 and 0.11 nm is acceptable for the bond length

Answer 3:?The hydrogen halide with the longest bond length and therefore smallest bond energy is the most reactive as it takes the least energy to break apart the hydrogen and halide atoms apart

Therefore, HI is the most reactive hydrogen halide