A hydrogen atom in a certain excited state has its electron in a 5f subshell. Th
ID: 792884 • Letter: A
Question
A hydrogen atom in a certain excited state has its electron in a 5f subshell. The electron drops
down to the 3d subshell, releasing a photon in the process.
a) For each of these subshells, give the n and l quantum numbers, and give the range of possible ml
quantum numbers.
b) How many radial nodes and how many angular nodes does each of the orbitals in part (a) have?
c) Determine the wavelength of light that would be emitted by this process.
d) The hydrogen atom now has a single electron in the 3d subshell. Calculate the energy (in
kJ/mol) required to ionize this (excited state) hydrogen atom. This is the energy required to
remove the electron completely from the atom.
Explanation / Answer
c)
energy in n=5 =-13.6 *z^2/n^2 ev {put n=5)
similarly find energy in n=3 and subtract both to get delta(e)
?E = 1.55x10^-19 J
The wavelength of the emitted photoncan be calculated from the equation;
?E = h ( c / ?) or
? = hc / ?E
where ?E represents the change in energy of the atom, which equals the energy of the emitted photon, h is Planck's costant which is 6.626 10-34 J
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.