Particle in a box and electron excitation

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SUMMARY

The discussion focuses on the excitation of an electron in a calcium atom (Ca, atomic number 20) when light is applied. The possible quantum numbers for the excited electron were analyzed, with options including (4, 0, 0), (4, 1, -1), (4, 1, 0), (4, 1, 1), (5, 2, +1), and (5, 2, -1). The consensus is that the (4, 0, 0) state is not viable due to the presence of valence electrons in the 4s state. Additionally, the promotion to the n=5 state is questioned, particularly regarding the introduction of d orbitals and the spin rule affecting the (5, 2, ±1) states.

PREREQUISITES
  • Understanding of quantum numbers (n, l, m) in atomic physics
  • Knowledge of electron configurations in atoms
  • Familiarity with the concept of electron excitation
  • Basic principles of light-matter interaction
NEXT STEPS
  • Study the quantum mechanical model of the atom, focusing on electron configurations
  • Learn about the rules governing electron excitation and energy levels
  • Research the significance of d orbitals in electron transitions
  • Explore the Pauli exclusion principle and its implications for electron spin
USEFUL FOR

Students studying quantum mechanics, physicists interested in atomic structure, and educators teaching atomic theory and electron behavior.

fredrogers3
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Homework Statement


Hello everyone, I have a question from a practice exam I can't seem to figure out.

1. A Ca atom (atomic number = 20) is in the ground state. Light is shined on the atom, exciting the most energetic electron. Which of the following are possible quantum numbers (n,l,m) of this excited electron? Don't worry about spin.
(a) (4, 0, 0)
(b) (4, 1, -1), (4, 1, 0) and (4, 1, 1)
(c) (5, 2, +1) and (5, 2, -1)
(d) all of the above
(e) none of the above

Homework Equations


See below

The Attempt at a Solution



1. I eliminated a) because the (4,0,0) state would be the 4s state, which is where the valence electrons are already located. Now, I am confused about why this electron cannot be promoted to the n=5 state. If enough energy is added, could it not go this state? Does have to do with the fact that we add a d orbital when we have (5,2,1)?

Thanks
 
Physics news on Phys.org
There is a rule about spin that makes (5,2,+-1) very unlikely.
 

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