Energy Transitions & Bohr Model of Hydrogen Atom Flashcards
When will an electron transition from one energy level to another?
When a photon of a specific energy is either absorbed or emitted by the electron
What is the energy of a photon equal to?
The difference between the two energy levels that the electron transitioned between
ΔEelectron = Ephoton
What must happen for an electron to be able to move from a lower to higher energy level?
An electron must absorb a photon of that particular energy
How to calculate change in energy of electron with example
Lyman, Balmer, etc. series
- Transitions are grouped according to the energy level that they land on
- E.g. all the ones that land on n=1 are called the Lyman series
- Note that the energy level gaps decrease as n increases
The Lyman series of H atom electron transitions produces light in the ___ range
UV
The Balmer series produces light in the ___ range
Visible light
The Brackett & Pfund series produce light inn the ___ range
Far infrared
What equation do you use to calculate the energy of an electron in a given energy level (n)?
Bohr Equation
How to calculate ionization energy
IE = -En = (Zeff^2 RH)/n^2
IE is equation for En but without negative sign
Efinal-Einitial
E.g.:
E∞ - En
E∞ = 0
En calculated using equation (either with Z or Zeff)
When do you use Zeff instead of Z?
When the electron being removed is not the only electron in the atom
