Limitations of Rutherford's Atomic Model

Step 1: Identify electron motion as circular motion around nucleus. Step 2: State that circular motion involves acceleration. Step 3: Apply classical radiation idea. Step 4: Explain predicted collapse. Step 5: Add the separate spectral-line failure.

A simple sketch may show an electron spiralling into the nucleus if it continuously loses energy. Label nucleus, electron path, and energy loss. This is a limitation sketch, not Rutherford's accepted final structure.

A common wrong answer is: Rutherford's model failed because it had no nucleus. This is wrong; its success was the nuclear model, while its failure was explaining stable electron motion and spectra.

The limitations of Rutherford's model are the failures that arise when classical electromagnetic theory is applied to orbiting electrons: it cannot explain atomic stability or the discrete line spectra of atoms.

The limitations of Rutherford's model are the failures that arise when classical electromagnetic theory is applied to orbiting electrons: it cannot explain atomic stability or the discrete line spectra of atoms. Qualitative rule used: an accelerating charge radiates energy according to classical electromagnetism. Condition of failure: Rutherford's orbiting electron is treated classically. Missing feature: quantised stationary states. Hydrogen emits definite spectral lines in the Balmer series in the visible region. Rutherford's model has no quantised energy levels, so it cannot predict these fixed wavelengths.

In Rutherford's model, electrons revolve around the nucleus like planets. An electron in circular motion is accelerating, and classical theory says an accelerating charge should radiate energy continuously. If that happened, the electron would lose energy, spiral into the nucleus, and the atom would be unstable. Rutherford's model also gives no rule for fixed electron energies, so it cannot explain why hydrogen gives sharp spectral lines instead of a continuous spectrum. Qualitative rule used: an accelerating charge radiates energy according to classical electromagnetism. Condition of failure: Rutherford's orbiting electron is treated classically. Missing feature: quantised stationary states. Question: Give two limitations of Rutherford's model. Answer structure: First, orbiting electrons are accelerated charges, so classical theory predicts continuous radiation and collapse into the nucleus. Second, the model does not provide discrete allowed energies, so it cannot explain the line spectrum of hydrogen. Often asked as a short-answer question after Rutherford's model, or as a comparison with Bohr's postulates. It may also appear in assertion-reason form about accelerating electrons and atomic stability. A common wrong answer is: Rutherford's model failed because it had no nucleus. This is wrong; its success was the nuclear model, while its failure was explaining stable electron motion and spectra.