Quantum

It specifies the probability of finding an electron in the three-dimensional ​space around the nucleus and is based on solutions of the Schrodinger ​equation. This does not provide a precise path taken by an electron. This ​theory seeks to explain phenomena occurring at an atomic, and even ​smaller, scale. It provides a mathematical framework to study the ​behavior of subatomic particles, explaining phenomena such as ​entanglement and quantum tunneling

Electron Clouds

Instead of defining specific orbits like in Bohr's model, the quantum ​model describes electrons as existing in "clouds" or "orbitals." ​These clouds represent regions where there’s a high probability of ​finding an electron, rather than a fixed path.

Quantum ORbits

Electrons are described by a set of quantum numbers that indicate ​their energy levels, shapes of orbitals, and orientations. These ​quantum numbers help determine the electron’s behavior and the ​arrangement of electrons in an atom.

Uncertainty principle

Introduced by Werner Heisenberg, the uncertainty principle states ​that we cannot simultaneously know both the exact position and ​momentum of an electron. This means that the more accurately we ​know an electron's position, the less accurately we can know its ​momentum, and vice versa.

TRansitions

Electrons can still absorb or emit energy, but rather than jumping ​between fixed orbits, they transition between different energy ​states, represented by various orbitals. The energy changes ​correspond to the differences in energy between these states.

Wave Quality

The quantum model incorporates the idea that particles, like electrons, ​exhibit both wave-like and particle-like properties. This duality is ​fundamental to understanding how atoms behave at a microscopic level.