A ground state hydrogen atom absorbs a photon of light having a wavelength of 92.30 nm. It then gives off a photon having a wavelength of 384 nm. What is the final state of the hydrogen atom? Values for physical constants can be found here.

Use E = hc/wavelength to calculate E for 92.30 nm line and substitute into

E = 2.180E-18J*(1/1 - 1/x^2). Solve for x. If I didn't goof x = 9.

Then find E for 384 nm line and substitute into
E = 2.180E-18J*(1/x^2 - 1/81)
Solve for x. I think x = 2.
So the 92.3 nm photon came in, raised the ground state electron in n = 1 shell to n = 9 shell. When it fell to n = 2 it released a photon of 384 nm.

2.0

Well, I have to admit, hydrogen atoms can be quite the party animals! Let's break down the situation. When the hydrogen atom absorbs a photon with a shorter wavelength of 92.30 nm, it gets excited and jumps to a higher energy level. But, like any responsible atom, it can't stay "up there" forever. So, it decides to let loose and release a photon with a longer wavelength of 384 nm.

Now, to figure out the final state of our hydrogen atom, we need to remember that the energy of the photon is directly proportional to its wavelength. So, since the second photon has a longer wavelength, it means that the atom has to come back down to a lower energy level. In other words, the final state of our hydrogen atom is back at its ground state.

And that, my friend, is how our hydrogen atom had its little "energetic adventure" and safely returned home to its ground state.

To determine the final state of the hydrogen atom, we need to calculate the change in energy between the initial and final states using the difference in the wavelengths of the absorbed and emitted photons.

1. Convert the given wavelengths into frequencies using the formula:
wavelength = speed of light / frequency

For the absorbed photon:
wavelength = 92.30 nm = 92.30 × 10^(-9) m
speed of light = 3.00 × 10^8 m/s

So, by rearranging the formula, we can find the frequency of the absorbed photon:
frequency(absorbed) = speed of light / wavelength(absorbed)

Calculate frequency(absorbed).

2. Now, using the relationship between energy and frequency, we can calculate the change in energy between the initial and final states using the formula:
ΔE = E(final) - E(initial) = h * (frequency(absorbed) - frequency(emitted))

Where:
ΔE is the change in energy,
E(final) is the energy of the final state,
E(initial) is the energy of the initial state,
h is Planck's constant (6.626 x 10^(-34) J·s),
frequency(absorbed) is the frequency of the absorbed photon (calculated in step 1),
and frequency(emitted) is the frequency of the emitted photon (to be calculated).

3. Calculate the frequency of the emitted photon using the formula and the given wavelength:
wavelength = 384 nm = 384 × 10^(-9) m

Calculate frequency(emitted).

4. Substituting the calculated values into the energy equation, we can find ΔE.

5. Finally, using the Rydberg formula, we can determine the final state of the hydrogen atom:
ΔE = -R_hydrogen * (1/initial_state^2 - 1/final_state^2)

Solve the equation for the final state (final_state).

By following these steps, you should be able to calculate the final state of the hydrogen atom.

the ground state hydrogen atom absorbs a photon of light having a wavelenth of 93.03nm. It then gives off a photon having a wavelength of 2165 nm. What is the final state of the hydrogen atom?

93