The emitted wavelengths of an element can be related to the frequency and energy of emission. The emissions from the hydrogen atom were modeled using the Rydberg equation, which Niels Bohr used to develop the Bohr model of the atom. For this exercise, you will need to see the actual spectra of the elements. Click on the "Emission" icon to change the display to emission spectra. Select the element boron (B). Give the wavelength, in Ångströms, the frequency, and the energy of the teal or blue-green emission. Place the cursor on the emission line and hold down the mouse button to display the wavelength of that line in Ångströms (1 Å = 0.1 nm = 1. 10-10 m).