Final answer:
Schrödinger's quantum mechanical model treats electrons as wavefunctions, leading to the natural occurrence of quantized energy levels, and contrasts with the Bohr model's fixed electron orbits by introducing a probability distribution for electron locations.
Step-by-step explanation:
The quantum mechanical model of the atom, developed by Erwin Schrödinger, is based on the wave-particle duality of electrons and describes their behavior in terms of wavefunctions. Contrary to earlier atomic models, such as the Bohr model which postulated quantized orbits without a mathematical foundation, the quantization of energy levels in Schrödinger's model arises naturally from the mathematical solutions to the Schrödinger equation. This equation treats electrons as three-dimensional stationary waves around the nucleus and can predict the likelihood of an electron's presence at a given point in space.
One key contrast with earlier models is that in the Bohr model, electrons were presumed to orbit the nucleus in fixed paths or quantized orbits, whereas the Schrödinger model replaced these orbits with a probability distribution of where electrons might be. This reflected a shift from viewing the electron as following a precise path to treating its location as a probability.
Furthermore, the quantum mechanical atomic model allowed for a more precise explanation of atomic spectra and laid the groundwork for modern quantum theory, earning Schrödinger, along with other pioneers like Bohr and Heisenberg, a central place in the development of atomic physics.