Light and Electrons

The higher the frequency the shorter the wavelength and the lower the frequency  the longer the wavelength. The longer the wavelength the lesser the energy . Wavelength and energy of light are indirect. Wavelength is also indirect with frequency. So frequency and energy of light are directly related.  light emission demonstrates electron transition by spectral lines. To produce these spectral lines you need to have an electron. Each electron produces one spectral line. For example a single atom of hydrogen cannot produce all for hydrogen spectral lines simultaneously. This is because hydrogen only contains one electron. Hydrogen gas can emit more than one spectral lines simultaneously because this is due to the multiple atoms used in your hydrogen gas example because there are more electrons there can be different spectral lines. The significance about the different colors of light observed in spectral lines are the wavelength. Each wavelength has its own unique color range. Red wavelength range range is from 625 to 740 nanometers, oranges range is from 592 to  625 nanometers, yellows range from 565 to 590 centimeters Greens range from 522 to 565 nanometers, blues range from 440 to 520 nanometers, and violets range from 382 to 440. There are different types of hues or shades of each color and they all each emitt different wavelengths. Every color has different energy; violets have the highest energy and the Reds have the lowest energy. So do to violet highest energy they have the shortest wavelength and red  has the longest wavelength because they have the lowest energy. During electron transition energy can either be released or absorbed. When energy is released they are returning to their lower energy levels as they get closer to the nucleus its "ground state." when energy is absorbed it goes to higher energy levels to do this it has to absorb enough energy to break the attraction between the nucleus and the electron. The spectral lines for atoms are unique, different wavelengths are emitted to different atoms. If an electron moves from energy level 5 to energy levels to this electron transition releases energy. The electron moves from a higher energy state to a lower energy state. In this electron transition light is released because the energy is absorbed. The longer the wavelength the lower the frequency the shorter the wavelength the higher the frequency wavelength and frequency are indirect. Light can be used to measure energy transitions of electrons by looking at the wavelength ranges. An example is hydrogen electron transition that involves light with a wavelength in the ultraviolet range which is it 10 to four hundred nanometers can be measured n= 6 to 1. A hydrogen electron transition that involves light with a wavelength in the infrared range which is a thousand 2106 nanometers can be directed as n equals 6 to n  equals 5.