To calculate the change in energy of the atom, we can use the formula:
ΔE = E_final - E_initial
Where ΔE is the change in energy, E_final is the final energy level, and E_initial is the initial energy level.
Given that the electron leaves from n = 4 and enters n = 6, we can substitute these values into the formula:
ΔE = (-2.18 × 10^-18) * ((1/n_final^2) - (1/n_initial^2))
ΔE = (-2.18 × 10^-18) * ((1/6^2) - (1/4^2))
ΔE = (-2.18 × 10^-18) * (1/36 - 1/16)
ΔE = (-2.18 × 10^-18) * (16/576 - 36/576)
ΔE = (-2.18 × 10^-18) * (-20/576)
ΔE = 3.817 × 10^-20 J
To calculate the wavelength of the photon, we can use the formula:
ΔE = hc/λ
Where ΔE is the change in energy, h is Planck's constant (6.62607015 × 10^-34 J*s), c is the speed of light (2.998 × 10^8 m/s) and λ is the wavelength.
Substituting the values:
3.817 × 10^-20 = (6.62607015 × 10^-34) * (2.998 × 10^8) / λ
Solving for λ:
λ = (6.62607015 × 10^-34) * (2.998 × 10^8) / (3.817 × 10^-20)
λ = 5.226 × 10^-7 m
Converting this to nanometers:
λ = 5.226 × 10^-7 * 10^9
λ = 522.6 nm
Therefore, the change in energy of the atom is 3.817 × 10^-20 J and the wavelength of the photon is 522.6 nm.
A hydrogen atom absorb a photon of visible light and it's electron leaves from n=4 and enters n=6 energy calculate the change of energy of the atom and wavelength in (nm) of the photon (R=-2.18×10^-18)
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