I'm reviewing for my Chem final and need stuff explained. Please give very in-depth explanations and answers so I can understand how to do it.
The first line of the Balmer series occurs at a wavelength of 656.3 nm. What is the energy difference between the two energy levels involved in the emission that results in this spectral line?
Calculate the frequency (Hz) and wavelength (nm) of the emitted photon when an electron drops from the n=4 to the n=2 level in a hydrogen atom.
An electron in the hydrogen atom makes a transition from an energy state of principal quantum numbers ni to the n=2 state. If the photon emitted has a wavelength of 434 nm, what is the value of ni?
Give the values of the four quantum numbers of an electron in the following orbitals:
The ground-state electron configurations listed here are incorrect. Explain what mistakes have been made in each and write the correct electron configurations.
Al: 1s^2 2s^2 2p^4 3s^2 3p^3
B: 1s^2 2s^2 2p^5
F: 1s^2 2s^2 2p^6.
Please refer to the attached file.
I also converted the docx file into pdf ...
This solution assists with and solves the chemistry review problems.