1. Hands-on spectrum lines – Introducing microscopic quantum explanations of the emitted photons to non-physics major’s students Vassilis Dimopoulos, George Kalkanis Science, Technology and Environment Laboratory, Pedagogical Department P.E., University of Athens, Greece

2. The Contents mechanic waves duality of light/electron spectrum early models of atom quantum model for the atom of hydrogen

3. Continuous spectrum Emission line spectrum The line spectra serves as a key to the structure of the atom, since any atomic theory must be able to explain why atoms emit light of discrete wavelengths and should be able to predict what these wavelengths are. A spectroscope is used in order to observe the continuous and linear spectra of various lights.

4. ψ(r, θ, φ) = R(r) Θ(θ) Φ(φ) Some of the wave functions for the atom of Hydrogen: Back

5. The wavefunction cannot been pictured Back The ψ 2 is a real number and gives the probability per unit volume that the particle will be found at any given point. The ψ 2 is called the probability density (Serway, 1986) In a dot’s representation the value of ψ 2 is higher when the density of the dots is high The probability density is also called electronic density or electronic cloud

6. We can use the radial probability distribution in order to calculate the probability of finding the electron within the area x < r < y (Serway, 1986). Back Having calculated the probability we converse this number to the frequency of finding the electron in different areas for each state. each state

7. The probability of finding a sphere / unit of surface increases If we move on a circle the higher probability of finding a sphere is on a circle of a specific radius

8. Back The representation of ψ 2 is different to the representation of P(r)

9. Back The representation of ψ 2 is different to the representation of P(r)

10. Back The representation of ψ 2 is different to the representation of P(r)

11. Emphasis is on the microscopic explanation of the spectrum of hydrogen

12. An energy diagram is used in order to confront that a spectral line can be created only by transitions between two discrete energy levels