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The lines on Absorption Atomic Spectra correspond to energies needed for electrons to be excited from a lower energy level to a higher energy level. Assume that the energy needed for an electron in 2p orbital in an O atom to jump to 3s orbital is 3.6*10^-19 J, what is its wavelength of the line atomic spectra in nanometer (nm)?
Note: please use whole numbers and 3 sig figs, or no decimal place.

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dsdrajlin

Answer:

553 nm

Explanation:

When an electron from O absorbs radiation with an energy (E) of 3.6 × 10⁻¹⁹ J, it is excited from orbital 2p to orbital 3s. The wavelength (λ) associated with that radiation can be calculated using the Planck-Einstein equation.

E = h. ν = h . c . λ⁻¹

where,

h is the Planck's constant

c is the speed of light

ν is the frequency

[tex]\lambda = \frac{h.c}{E} =\frac{6.63 \times 10^{-34}J.s \times 3.00 \times 10^{8} m/s}{3.6 \times 10^{-19}J } .\frac{10^{9}nm }{1m} =553nm[/tex]

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