an electron in n=5 emits 4052 nm to what energy level does the electron move
1/wavelength = R(1/n^2 - 1/25)
Remember to convert wavelength to m
In the above n^2 is n1 squared and 1/25 is 1/n2 with n2 squared.
R = Rydberg constant = 1.0973E7 m^-1
i got 6.667. what does this mean?
It means you did something wrong.
Post your work and I'll find the error BUT first, did you change 4052 nm to m?
To determine the energy level to which the electron moves when it emits light, we can use the formula for calculating the energy of a photon.
The energy of a photon (E) is given by the equation:
E = hc / λ
Where:
- E represents the energy of the photon
- h is Planck's constant (approximately equal to 6.626 x 10^-34 J·s)
- c is the speed of light in a vacuum (approximately equal to 2.998 x 10^8 m/s)
- λ represents the wavelength of the emitted light in meters
First, let's convert the given wavelength of 4052 nm to meters:
4052 nm = 4052 x 10^-9 meters (since 1 nm = 10^-9 meters)
= 4.052 x 10^-6 meters
Now, we can substitute this value into the energy formula to calculate the energy of the photon emitted by the electron:
E = (6.626 x 10^-34 J·s * 2.998 x 10^8 m/s) / (4.052 x 10^-6 meters)
E ≈ 4.915 x 10^-19 J (rounded to 3 significant figures)
The energy of the photon emitted by the electron is approximately 4.915 x 10^-19 Joules.
Since the electron initially started in the n=5 energy level, it must have moved to a lower energy level after emitting the photon. In the case of an electron transitioning from a higher energy level to a lower one, it typically moves to the energy level that is closer to the nucleus.
In this specific case, the electron could move to any of the energy levels with a principal quantum number (n) smaller than 5. We would need more information or context to determine the exact energy level to which the electron moved.