The Atomic theory model which explains that electrons in an atom revolve round quantized energy levels is attributed to

Explanation

Niels Bohr proposed his atomic model in 1913. His key idea was that electrons orbit the nucleus in specific, fixed energy levels (also called shells or orbits). These energy levels are “quantized,” meaning electrons can only exist at certain energy values and nowhere in between.

In Bohr’s model, an electron can jump from one energy level to another by absorbing or releasing a specific amount of energy (a quantum). When an electron drops to a lower energy level, it gives off light. This explained why elements produce specific colors when heated.

Becquerel is known for discovering radioactivity, not for atomic energy levels. Rutherford proposed the nuclear model where the atom has a dense positive nucleus with electrons around it, but he did not explain quantized energy levels. De Broglie later proposed that electrons behave as both particles and waves (wave-particle duality).

Bohr’s model was a major step forward because it successfully explained the line spectrum of hydrogen. Although it was later replaced by the more accurate quantum mechanical model, his concept of quantized energy levels remains a foundation of modern chemistry.