Students will be able to
- recall that the energy level an electron is in is denoted by the principal quantum number, ,
- recall that the lowest possible value for is 1 and that this represents the most strongly bound electrons,
- recall that the state is called the ground state,
- recall that increases for higher energy levels and that the greater the value of , the less strongly bound an electron is,
- recall that the term electron energy level transition refers to an electron moving between two energy levels,
- calculate the energy difference between two energy levels given the binding energy of each energy level,
- calculate the frequency or wavelength of the emitted or absorbed photon based on the energy levels that an electron transitions between (using ),
- recall that certain groups of transitions have certain names (e.g., Lyman series, Balmer series, Paschen series).
Students should already be familiar with
- the idea that electrons in atoms occupy discrete energy levels,
- the idea that when an electron moves from a higher energy level to a lower energy level, a photon is emitted,
- the idea that an electron can move from a lower energy level to a higher energy level by absorbing a photon,
- the electron volt (eV) as a unit of energy,
- how to convert between joules (J) and electron volts (eV).
Students will not cover
- the other quantum numbers (, , ),
- the energy level configuration for any element other than hydrogen,
- mean excited state lifetimes,
- the difference between stimulated and spontaneous emissions of photons,
- the quantum mechanical origins of discrete energy levels.