Ionisation energy

• What factors impact ionisation energy?

  .

  • Atomic radius
  • Nuclear charge
  • Electron Shielding
• What is atomic radius?

  The distance between the outermost electron and the nucleus of the atom.
• How does atomic radius impact ionisation energy?

  As electrons move further away from the nucleus, the nucleus applies less forces of attraction due to the distance it must cover.
• How does nuclear charge affect ionisation energy?

  The greater the charge on the nucleus, the more attracted the electrons are to it (dependant on atomic number).
• How does electron shielding affect ionisation energy?

  Electrons on inner shells will repel those on outer shells.
• How many electrons can go into each shell?

  .

  1. 2 Electrons
  2. 8 Electrons
  3. 18 Electrons
  4. 32 Electrons
• How are the shells numbered?

  The principle quantum number (n)
• How many electrons can sub-shell s hold?

  2
• How many electrons can sub-shell p hold?

  6
• How many electrons can sub-shell d hold?

  10
• How many electrons can sub-shell f hold?

  14
• How can you represent orbitals and electrons in graphs?

  Using boxes for orbitals and arrows in opposite directions of pointing up and down for electrons.
• What shape is a s sub-shell?

  Sphere shape

  
• What shape is a p sub-shell?

  Dumbbell shape

  
• What shape is a d sub-shell?

  Cloverleaf shape

  
• Identify the sub-shells.

  .

  A) S orbital

  B) P orbital

  C) D orbital

  
• What is an orbital?

  The area around the nucleus that holds a maximum of 2 electrons and orbits in opposite directions.
• Describe a d sub-shell?

  .

  • Contains transition metals
  • Complex structure
  • In total can hold up to 10 electrons
• Describe a s sub-shell?

  .

  • Contains metals
  • Easiest structure
  • In total can hold up to 2 electrons
• Describe a p sub-shell?

  .

  • Contains non-metals
  • More complex structure than s-orbital
  • In total can hold up to 6 electrons
• Describe a f sub-shell?

  .

  • Contains lanthanides
  • Complex structure
  • In total can hold up to 14 electrons
• What is the sub-shell notation?

  1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 4d10 4f14
• What are the rules for filling sub-shells in a box diagram?

  .

  • Electrons must be added one at a time
  • Electrons must fill boxes from left to right
  • Electrons must be added to the lowest available shell first
  • Only two electrons to one orbital
  • Each orbital must be filled singularly before pairing
• Which sub-shells overlap?

  4s2 comes before 3d10
• Why must all orbitals be filled singularly before pairing?

  Half filled orbitals are more stable than having one full and one empty.
• What does isoelectric mean?

  Elements and ions with the same electronic configurations
• What are shells made up of?

  Sub-shells containing orbitals
• Describe the trend of ionisation energy across a period?

  .

  1. First Dip is due to the outermost electron going into the p sub-shell. This is a higher energy level than a s sub-shell and it is easier to remove an electron from
  2. Second Dip is due to the first pairing in the p sub-shell orbital. As these electrons repel each other the electron in the pair is easier to remove.

  A) Dip 1

  B) Dip 2

  
• What do the small peaks around the molecular ion represent?

  Isotopic molecules