An electron ps from the 6th to te 3rd energy level in the hydrogen atom:
a) calculate the wavelength
b) calculate the frequency
c) calculate te enrgy
d) into which spectral series would the photon be grouped?
(i really just need to formulas, then i could solve myself...)
1/wavelength = R(1/3^2 - 1/6^2)
R = Rydberg constant.
b) c = wavelength*frequency
c) E = h*frequency
d) You can answer this after you know the wavelength.
To calculate the wavelength, frequency, and energy of the photon emitted during the electron transition from the 6th to the 3rd energy level in the hydrogen atom, we can use the following formulas:
a) Wavelength (λ) can be calculated using the formula:
λ = c / ν
where c is the speed of light in a vacuum (approximately 3.00 × 10^8 m/s) and ν is the frequency of the photon.
b) Frequency (ν) can be calculated using the formula:
ν = c / λ
c) Energy (E) can be calculated using the formula:
E = h * ν
where h is the Planck's constant (approximately 6.626 × 10^-34 J*s).
d) To determine the spectral series to which the emitted photon belongs, we need to use the Rydberg formula:
1/λ = R * (1/n1^2 - 1/n2^2)
where R is the Rydberg constant (approximately 1.097 × 10^7 m^-1) and n1 and n2 are the principal quantum numbers of the initial and final energy levels, respectively.
For this specific transition from the 6th (n1 = 6) to the 3rd (n2 = 3) energy level in the hydrogen atom, you can now substitute the values into the formulas mentioned above to solve for the required quantities.