Answer :
The electronic transition in Na from 3p¹ to 3s¹ gives rise to a bright yellow-orange emission at 589.2 nm. The energy of this transition is 0.0017 × [tex]10^{-26}[/tex].
Atoms and molecules undergo electronic transitions as a result of electromagnetic radiation being absorbed or emitted (typically UV or visible). Planck's equation, E = h, relates the energy change connected to a transition to the frequency of the electromagnetic wave.
Three different types of electronic transitions can be taken into consideration: p, s, and n electron-based transitions. transitions involving electrons that transfer charges. D and F electron-based transitions (not covered in this Unit) Emission or absorption of electromagnetic radiation in the form of quantized particles known as photons results from electron transitions.
E= hC/ λ
where,
h = 6.626 × [tex]10^{-34}[/tex]
c = 2.99 × [tex]10^{8}[/tex] m/s
λ = 589.2 nm
E= 6.626 × [tex]10^{-34}[/tex] × 2.99 × [tex]10^{8}[/tex] / 589.2
E= 19.81174 × [tex]10^{-26}[/tex]/ 589.2
E = 0.0017 × [tex]10^{-26}[/tex]
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