Question

What do spectral lines tell us about the structure of the atom?

Use words: Bohr model, energy transition, calculation of energy using energy=hf, hydrogen atom, spectral line, colors of visible light, wavelength frequency.

Answer 1

Bohr devised a model of the atom in that each of the electrons have a specific energy - no in betweens. These are called energy levels. The energy level that an electron usually occupies, is called its ground state. When you excite these electrons by giving them energy, they gain energy so that they move further away from the nucleus of the atom to a higher energy level shell (further away = higher energy level). This is it's excited state. The distance travelled is going to be proportional to the energy it receives.

When the electron is done being in its 'excited' state, the electron releases that same amount of energy in the form of a photon and the wavelength of this photon coincides with the wavelength and frequency of visible light. Different colours depend on how much energy was released, for example a very excited electron which gained a lot of energy would release a high frequency, short wavelength wave, that would be shifted to the violet end of the EM spectrum, producing spectral lines at this end, in order to go back to its ground state. Energy=hf gives the energy produced by this, and allows chemists to calculate the energy level of the electron, where h is (Planck's constant) 6.693*10^-4J*s, and f is frequency (Hz) of the incident radiation.

Answer 2

Thank you so much!! You saved my life!!