A hydrogen atom in its ground state absorbs a photon of energy 12.1 eV. To what energy level is

step 1 for this exercise, we have, ah, hydrogen atom in its ground state. So in in equals one and this

A hydrogen atom in its ground state absorbs a photon of...

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Quantized Energy Levels

In quantum mechanics, the energy of electrons in atoms is not continuous but instead exists in discrete levels or states. This quantization means that electrons can only exist in specific energy states, and transitions between these states involve precise energy differences.

Photon Absorption and Electronic Transitions

When an electron in an atom absorbs a photon, it gains energy equal to the photon's energy. This absorption causes the electron to jump from a lower energy level to a higher one, but only if the photon's energy exactly matches the energy difference between the two states.

Bohr Model of the Hydrogen Atom

The Bohr model provides a framework for understanding the discrete energy levels of the hydrogen atom. It establishes that the energy associated with each orbit is given by E_n = -13.6 eV/n^2, where n is the principal quantum number. This model explains the emission or absorption of light during transitions between energy states.

Energy Level Calculations

Using the energy formula from the Bohr model, one can calculate the difference in energy between various levels. This calculation is essential for determining which electron transition corresponds to a specific photon energy, as the absorbed energy must match the difference between the initial and final energy levels.

Transcript

Please give Ace some feedback