for the transition of an electron in a hydrogen atom between the principal quantum number levels 4 and 3, calculate

a) the energy released

b) the wavelength of the line in the spectra.

E = 2.180E-19 x (1/9 - 1/16)

Then E = hc/wavelength

can you explain it a little more cuz i really didn't understand anything!!!!

thank you!

Energy in joules = 2.180E-19(1/n1^2 - 1/n2^2)

n1 = 3 and 1/n^2 is 1/9
n2 = 4 and 1/n^2 is 1/16
The rest of it is algebra.

After you have the energy, then set that in the following equation.
E = hc/wavelength.
h is Planck's constant in J.s
c is speed of light in m/s
wavelength is in meters. Plug and chug.

To calculate the energy released and the wavelength of the line in the spectrum for the transition of an electron between the principal quantum number levels 4 and 3 in a hydrogen atom, we can use the following equations:

a) The energy released (ΔE) can be calculated using the formula:

ΔE = E_final - E_initial

where E_final is the energy of the final state (n=3) and E_initial is the energy of the initial state (n=4).

The energy of an electron in a hydrogen atom at a particular energy level is given by the equation:

E = -13.6 eV / n^2

where n is the principal quantum number.

Plugging in the values for the final and initial states, we get:

E_final = -13.6 eV / 3^2 = -13.6 eV / 9
E_initial = -13.6 eV / 4^2 = -13.6 eV / 16

Substituting these values into the equation for ΔE:

ΔE = (-13.6 eV / 9) - (-13.6 eV / 16)

Now simplify this expression to find the energy released.

b) The wavelength (λ) of the line in the spectrum can be calculated using the equation:

λ = c / ν

where c is the speed of light (approximately 3.00 x 10^8 m/s) and ν is the frequency. The frequency can be calculated using the equation:

ν = ΔE / h

where h is Planck's constant (approximately 6.63 x 10^-34 J·s).

Plugging in the value of ΔE from part a, we get:

ν = ΔE / h

Now substitute the frequency into the equation for wavelength to find the value for the wavelength λ.

By using these steps, you can calculate the energy released and the wavelength of the line in the spectrum for the transition of an electron between the principal quantum number levels 4 and 3 in a hydrogen atom.