The energy difference between states A and B is twice the energy difference between states B and C (C > B > A). In a transition (quantum jump) from C to B, an electron emits a photon of wavelength 600 nm.
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To find the energy difference between the states A and B, we'll first have to determine the energy difference between B and C.
The relationship between energy and wavelength is given by the equation:
E = hc/λ
Where E is the energy, h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength.
Given that the wavelength of the emitted photon is 600 nm (or 600 x 10^-9 m), we can use the equation to find the energy:
E(BC) = hc/λ
E(BC) = (6.626 x 10^-34 J·s)(3.00 x 10^8 m/s)/(600 x 10^-9 m)
E(BC) ≈ 3.31 x 10^-19 J
Now, we know that the energy difference between A and B is twice the energy difference between B and C. Therefore:
E(AB) = 2 * E(BC)
E(AB) = 2 * 3.31 x 10^-19 J
E(AB) ≈ 6.62 x 10^-19 J
So, the energy difference between states A and B is approximately 6.62 x 10^-19 J.