According to Bohr's model, what is the significance of an electron transition from a higher energy orbit to a lower energy orbit?
Show answer & explanation
Correct answer: D
Explanation
Answer: A photon of energy equal to the energy difference between the orbits is emitted.
Explanation
In Bohr's Atomic Model, electrons revolve around the nucleus in specific, fixed circular paths called stationary orbits or energy levels.
The Transition: When an electron moves from an orbit with higher energy (E_2) to an orbit with lower energy (E_1), it cannot keep the "extra" energy.
Energy Emission: To maintain stability in the lower orbit, the electron must lose energy. This lost energy is released (emitted) in the form of a single packet of light energy called a photon.
Key Facts for Exams
Absorption vs. Emission: * Lower to Higher orbit = Energy Absorbed (Excitation).
Higher to Lower orbit = Energy Emitted (De-excitation).
Quantization: Bohr proposed that electrons can only exist in certain orbits, meaning their energy is "quantized."
Spectral Lines: Each transition produces a specific color or wavelength of light. This explains why different elements have unique atomic spectra (like a fingerprint).
Exam-Related Practice Questions
Q1: What happens to an electron when it absorbs a photon?
Answer: It jumps from a lower energy orbit to a higher energy orbit (reaches an excited state).
Q: What is the primary reason for the different colors seen in a hydrogen discharge tube?
Answer: Different energy transitions of electrons emitting photons of varying wavelengths/frequencies.