Electrons

Electrons

1. Orbitals

   • s orbital - max 2 electrons
   • p orbital: max 6 electrons
   • d orbital: max 10 electrons
   • f orbitals

2. Energy Diagrams: allows us to track an electrons transition between orbitals based on the absorption or emission of photons

   • Each energy level has a quantum number; the higher the number, the higher the energy
   • NOT ORBITS! -- represents ENERGY ONLY; NOT distance from the nucleus
   • Absorption
   • Emission

3. Have wave/particle duality -- just like light!

   • Double slit experiment (electrons shot through slits into aluminum foil) shows wave interference

4. Quantum Numbers

   • Principle Quantum Number (n): determines the energy of the orbital and identifies its shell; the larger the number, the higher the energy and the larger the orbital
   • Angular Momentum (l): identifies the type of orbital (s,p,d,f...) and subshell
   • Magnetic (m *sub l): specifies a particular orbital with a subshell (i.e. the orientation of the orbital)
   • Spin (m *sub s): describes the spin of the electron in the orbital

5. Core vs. Valence

   • low energy, close to nucleus, closed shell (full orbital) -- # of core electrons in an element is based on the noble gas before element of interest (plus any additional full d orbitals)
     • Effective Nuclear Charge = nuclear charge ( # of protons) - # of shielding (core) electrons; Zeff = Z - S
   • high in energy, shell is not closed (incomplete orbital), determines reactivity of an element

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