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Niels Bohr's groundbreaking work laid the foundation for understanding how energy is quantized in atoms. He introduced the idea that electrons inhabit specific energy levels, a concept that defied the classical understanding of energy as a continuum. This quantization means that electrons can only possess certain discrete amounts of energy and not an arbitrary value.

When an electron transitions between these discrete energy levels, it must either absorb or emit a quantum of energy – a precise packet, which corresponds to the difference in energy between those levels. This concept is a cornerstone of quantum mechanics, illustrating how energy on the microscopic scale behaves in a stepwise, rather than continuous, fashion.

Bohr's model offers a simplified view of atomic structure, portraying the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits. Bohr suggested that the arrangement and energy of these orbits define the atom's characteristics. Each orbit corresponds to a specific energy level.

The model supports the idea that the stability of an atom is achieved through these allowed orbits. While Bohr's model has been superseded by more complex quantum models, it was instrumental in developing atomic theory by incorporating quantum concepts into the classical atomic structure.

Quantum theory is the theoretical basis of modern physics that provides a framework for understanding the physical properties of atoms and subatomic particles. Bohr's contributions were pivotal in shaping quantum theory, particularly the principle that atomic events can only occur in discrete steps called quanta.

Quantum theory has led to numerous technological advancements and deepened our understanding of the universe from the smallest to cosmic scales. It challenges many of the notions of classical physics, offering a new perspective where probability plays a key role in predicting atomic behavior.

The concept of electron orbits in Bohr's model refers to the distinct paths that electrons are postulated to follow around the nucleus. The innovation of Bohr was stipulating that these orbits are quantized – that is, electrons can only circle the nucleus in certain allowed orbits, and each orbit corresponds to a specific energy level.

In an atom, electrons move from one orbit to another through the absorption or emission of energy, a process termed a 'quantum leap'. This explains the spectral lines observed for each element, as these lines represent the energy released or absorbed as electrons jump between orbits. Although a simplification of the true complexity of electron behavior, Bohr's electron orbits brought a new understanding of atomic emission and absorption spectra.