What is the change in energy, ΔE, in kilojoules per mole of hydrogen atoms for an electron transition from n = 7 to n = 2?
The Rydberg equation expresses the wavelength, λ, of emitted light based on the initial and final energy states (ni and nf) of an electron in a hydrogen atom:
where RH = 1.097 × 107 m− 1 = 1.097 × 10−2 nm−1.
You may also see this equation written as
the two formulas are equivalent and sometimes used interchangeably. It can help to remember that when light is emitted, E is negative. When light is absorbed, E is positive.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Bohr and Balmer Equations concept. If you need more Bohr and Balmer Equations practice, you can also practice Bohr and Balmer Equations practice problems.