It's interesting how electrons, when they get energized, jump between different levels within their atom, releasing light in the process.

It's like each atom has its own tiny fireworks 🎆 show, creating colorful spectral lines that serve as unique fingerprints for different elements

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The Balmer series is named after Johann Balmer, who in 1885 figured out how to accurately predict the spectral lines emitted by a hydrogen atom using an empirical formula, now known as the Balmer formula.

However, at that time, it was still unclear why these spectral lines were produced.

Balmer Series

In 1913, Niels Bohr explained that when electrons in a hydrogen atom get excited, they move up energy levels based on absorbed energy. As this energy dissipates, they return to lower levels, emitting light and creating a unique, colorful spectrum.

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Related Math!

The equation below shows how to calculate the maximum kinetic energy of an ejected electron.

KEmax = Kinetic energy of the ejected electron

h = Planck's constant

v = Frequency of the incident light

𝜙 = Work function of the material (Minimum energy required to eject an electron)

So knowing now what Planck's Law is, we can dive into what 'Planck's Constant' means.

Simply put, 'Planck's Constant' tells us the exact amount of energy in a 'Quanta'. This value becomes key in Quantum Physics when Einstein used it to explain the photoelectric effect and discover the Photon!

First stop in our study plan, the birth of Quantum Theory.

The Ultraviolet Catastrophe AKA Rayleigh-Jeans Law

This theory proposed that a 'Black Body' could emit continuous radiation and glow infinitely bright as frequency increased. This turned out to be wrong...

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