(a)
Interpretation:
The color of the spectral line when electron shows the transition from energy level
Concept introduction:
In the spectrum of hydrogen, the individual light bands that result from the absorption or emission of light are known as spectral lines. When the transition of an electron occurs from a higher level of energy to a lower level, a single photon is emitted for each dropping electron.
(b)
Interpretation:
The color of the spectral line when electron shows transition from energy level
Concept introduction:
In the spectrum of hydrogen, the individual light bands that result from the absorption or emission of light are known as spectral lines. When the transition of an electron occurs from a higher level of energy to a lower level, a single photon is emitted for each dropping electron.
(c)
Interpretation:
The color of the spectral line when electron shows the transition from energy level
Concept introduction:
In the spectrum of hydrogen, the individual light bands that result from the absorption or emission of light are known as spectral lines. When the transition of an electron occurs from a higher level of energy to a lower level, a single photon is emitted for each dropping electron.
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INTRO CHEM + MASTERING W/ETEXT
- Describe the properties of an electron associated with each of the following four quantum numbers: n,l,ml, and ms.arrow_forwardIndicate whether each of the following statements is true or false. If false, correct the statement. (a) An electron transition from n=3 to n=1 gives off energy. (b) Light emitted by an n=4 to n=2 transition will have a longer wavelength than that from an n=5 to n=2 transition. (c) A sublevel of l=3 has a capacity of ten electrons. (d) An atom of Group 13 has three unpaired electrons.arrow_forward6.11 Define the term photon.arrow_forward
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