What 3 types of emission contribute to an overall emission spectrum?
Answer:
Most light sources can be classified into three main types: continuous, absorption, and emission. A hot, opaque object, like the filament in an incandescent light bulb, emits a continuous spectrum, having light of all wavelengths. A hot, dense gas is another example of an object that emits a continuous spectrum.
There are three types of spectra which an object can emit: continuous, emission and absorption spectra. The examples of these types of spectra shown below are for visible light as it is spread out from purple to red, but the concept is the same for any region of the electromagnetic spectrum.
Continuous spectra
Continuous spectra (also called a thermal or blackbody spectra) are emitted by any object that radiates heat (has a temperature). The light is spread out into a continuous band with every wavelength having some amount of radiation. For example, when sunlight is passed through a prism, it's light is spread out into it's colors.
Absorption spectra
If you look more closely at the Sun's spectrum, you will notice the presence of dark lines. These lines are caused by the Sun's atmosphere absorbing light at certain wavelengths, causing the intensity of the light at this wavelength to drop and appear dark. The atoms and molecules in a gas will absorb only certain wavelengths of light. The pattern of these lines is unique to each element and tells us what elements make up the atmosphere of the Sun. We usually see absorption spectra from regions in space where a cooler gas lies between us and a hotter source. We usually see absorption spectra from stars, planets with atmospheres, and galaxies.
Emission spectra
An emission spectra occurs when the atoms and molecules in a hot gas emit extra light at certain wavelengths, causing bright lines to appear in a spectra. As with absorption spectra, the pattern of these lines are unique for each element. We can see emission spectra from comets, nebula and certain types of stars.
What 3 types of emission contribute to an overall emission spectrum?
What is the wavelength, in nanometers of the bright line of the hydrogen emission spectrum corresponding to the following transition? 1st attempt IN See Periodic Table O See Hint n-5 to n-3 nm
What is the wavelength, in nanometers, of the bright line of the hydrogen emission spectrum corresponding to the following transition? 2nd attempt Feedback See Periodic Table D See Hint n=5 to n=3 ® -717.47 nm
1.explain why there are more lines in the hydrogen emission spectrum than in the absorption spectrum? 2. indicate asborption, from a lower energy level to a higher energy level. Then indicate emission for the same transition as through various pathways, which would then result in many more emission peaks than there was in the original absorption (transition).
A. Describe the spectrum you would observe for the emission spectrum of elemental hydrogen gas. B. Describe the spectrum you would observe for the absorption spectrum of elemental hydrogen gas.
6. The emission spectrum of Na(NaNNa [Ne]3s) is a doublet. [8 points) (a) What are the term symbols for excited states?
would an emission spectrum of an unknown sample be a good way to qualitatively identify which elements are present? What information would you look for in an emission spectrum to allow you to determine quantitative information? In other words, how could you tell how much of a certain element was present?
How would the absorption spectrum of an atom differ from its emission spectrum? How could one measure an absorption spectrum?
Which of these compounds: fluorescein or pyrene would produce an emission spectrum that would overlap (partially or fully) with that of quinine emission spectrum?
1. in the mercury emission spectrum, three intense emission bands can be observed. in the Bohr model of the atom, each of these bands corresponds to a transition from a particular quantum orbital (energy level)n= 1,2,3 ..... for mercury, what color band corresponds to the largest energy difference between levels and which is the smallest? why is that? 2. is it possible for an atom to absorb a photon of red light and remit a photon of violet light? why?
1.(3) The line of longest wavelength in visible light for the emission spectrum of hydrogen, 650nm (Balmer series), would correspond to what electronic transition? 2.(7) Explain the wave-particle duality of matter and light. Why don't we notice this effect in everyday activities? What do electrons behave most like in an atom?