1. The Bohr Model: Atoms with Orbits pg. 291-294 LO: I can explain what line spectra represent.

2. Neon Signs What gives neon signs their color? Each tube is filled with gas of a specific atom. Electricity excites the gas by exciting electrons which then emit a unique color (wavelength).

3. Light Emission from Elements Mercury Hydrogen

4. Spectra Hydrogen

5. Spectra Continuous Spectra: Uninterrupted range of visible light colors, “rainbow,” which can be seen when using a prism when looking at a white hot lamp (Incandescent).

6. Spectra Line Spectra: Light bands of specific wavelengths with areas of black space (non- continuous) which can be seen looking through a prism at gas filled fluorescent lamps or metal atoms in flame.

7. Spectra  electrons exist only on specific pathways Hydrogen

8. Why do elements have emission spectra? Orbitals: Electrons only travel at specific orbits (energy levels) around the nucleus. The orbits are quantized. The energy of each orbit is specified by a quantum number. The higher the number, the more energy the electron has.

9. Why do elements have “specific” emission spectra? Hydrogen Light emitted = quantum of light energy

10. Why do elements have emission spectra? Poster Drawings How are they connected in your drawing? Energy of electron Wavelength Spectra color Pg. 292-293

11. As n (electron orbitals) increases energy of the electron increases As n (electron orbitals) increases move closer together The energy of light (wavelength) corresponds to the difference in the energy transition Pg. 294