Electron arrangement

• Energy Levels


  • 1
  • 2
  • 3
  • 4
• Sublevel


  s, p, d, f
• Bohr Model


  De Broglie - wave particle duality
• De Broglie


  Heisenberg - It is impossible to measure at the same time both the velocity and the position of the electron
• Orbital


  Region of space around the nucleus where there is a high probability of finding an electron
• Energy Level


  The fixed amount of energy which an electron can have in an atom
• Sublevel


  A subdivision of an energy level consisting of one or more orbitals of the same energy
• Anion


  Negatively charged atom that has gained electrons
• Cation


  Positively charged atom that has lost electrons
• Chromium has a 3d5 4s1 electron configuration, filling the d sublevel first
• Copper has a filled d sublevel
• Aufbau principle 


  When electrons are filling energy levels/ sublevels, they always occupy the lowest energy level available to them.
• Hunds rule of maximum multiplicity 


  States that when 2 or more orbitals of equal energy are available to an electron they fill them singly before filling them in pairs.
• Pauli's exclusion principle


  States that when 2 or more electrons occupy an orbital, they have opposite magnetic spin.
• Wave-partical duality: electrons have some properties of particles and some properties of waves.
• Orbit: the fixed path one body takes around another.