Emission spectra and the electromagnetic spectrum

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A tiny **packet of light energy**; its energy is given by E = hf (higher frequency → more energy).

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A **fixed, allowed energy** an electron can have in an atom; energy levels are **discrete (quantised)**.

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Continuous = an **unbroken rainbow** (all wavelengths). Line = a few **discrete bright lines** on black, from an excited element.

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An excited electron **falls** from a higher to a lower energy level, emitting a photon of fixed energy (one line per allowed jump).

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That the electron's energy levels are **discrete (quantised)** — fixed lines mean only fixed energy gaps are allowed.

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The spectral lines get **closer together** toward **high frequency/energy**, because the energy levels bunch up at higher n.

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The **biggest energy gap** — an electron falling **to n = 1** (the ground state).

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$c = \lambda f$ — speed of light = wavelength × frequency, so **high f means short λ**.

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$E = hf$ — photon energy = Planck's constant × frequency (higher f → higher E).

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**Radio < red < violet** in frequency, so radio is lowest energy and violet is highest.

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The lines merge; the electron gains just enough energy to **leave the atom** — this gives the **ionisation energy**.