Modern Atomic Understanding: From Bohr to Quantum Mechanics
In 1913, Niels Bohr solved Rutherford's stability problem with a clever idea: electrons can only orbit at specific energy levels, like rungs on a ladder. Electrons can jump between levels by absorbing or emitting light, which explained why elements produce specific colours when heated.
Bohr's model worked perfectly for hydrogen but struggled with more complex atoms. The final breakthrough came in the 1920s with the quantum mechanical model.
This modern model describes electrons using wave functions - mathematical equations that tell us the probability of finding an electron in any location around the nucleus. Rather than fixed orbits, we now talk about electron clouds or orbitals where electrons are likely to be found.
Reality Check: The quantum model requires complex maths, but don't worry - understanding the concept of probability clouds is what matters for your exams!
While the quantum model is mathematically challenging, it perfectly explains atomic behaviour and is still used by scientists today.