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Toleisnon
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Why are only certain colors of the emission spectrum in Hydrogen visible?
I don't think that is correct. It IS the hydrogen atom's fault ... it doesn't emit a full spectrum, which is what the OP would have found if he had done any research.hilbert2 said:The human retina can detect only a certain range of wavelengths of light, corresponding to electronic transition energies of the pigment molecules in the rod and cone cells. Some other animals may have a vision that can detect wavelengths outside that range. The main point: it's not the hydrogen atom's fault that we don't see its whole emission spectrum, you have to blame evolution for that.
Toleisnon said:Why are only certain colors of the emission spectrum in Hydrogen visible?
Sounds like you want the answer to both questions that Peter pointed out. I have answered one of them in post #4 and Hilbert answered the other in post #2. What about these answers is not clear to you?Toleisnon said:*Why hydrogen only emits certain frequencies when viewing it under a high school spectroscope instead of all of the frequencies (spectral lines)*
The visible light spectrum is a small portion of the entire electromagnetic spectrum, which includes various types of radiation such as radio waves, microwaves, infrared, ultraviolet, and X-rays. The human eye is only able to detect electromagnetic radiation with wavelengths between approximately 400-700 nanometers, which corresponds to the colors red, orange, yellow, green, blue, indigo, and violet. This is due to the specific structure and sensitivity of the photoreceptor cells in our eyes.
When an element is heated or excited in some way, the electrons in its atoms absorb energy and jump to higher energy levels. As the electrons return to their original energy levels, they emit energy in the form of light. The specific energy levels and transitions of each element are unique, resulting in different colors being emitted. This is known as atomic emission spectra and is used to identify elements in spectroscopy.
Yes, the visible colors in an emission spectrum can be altered or controlled by changing the energy input to the element. This can be done by varying the temperature or applying an electric current. Additionally, the type of element and its chemical composition can also affect the colors emitted.
The intensity of a color in the emission spectrum is determined by the number of photons (light particles) emitted at that specific wavelength. This is dependent on the energy levels and transitions of the electrons in the element, as well as the temperature and other factors that may affect the emission process.
The visible emission spectrum appears as a continuous rainbow of colors, but upon closer examination, there are actually gaps or missing colors. This is because the human eye is not able to detect all the wavelengths of light, and therefore, some colors may not be visible to us. Additionally, some colors may be absorbed or reflected by the medium through which the light is passing, further contributing to the gaps in the spectrum.