Often times the lower excited states of an atom is just to re-arrange the electr

Question

Often times the lower excited states of an atom is just to re-arrange the electrons in the last open shell. For example, the last two electrons in the carbon atom remain in the p-shell but occupy different orbitals (different m). a. Use the three Hund's rule to determine the S, L, and J value for the ground state (call them SG, LC, and JG values). b. For the given SG and LG (as determined in part a), Hund's third rule gives J Gr the lowest energy state. What are the possible J values for the excited states? c. The more of Hund's rules are violated, the higher the energy. Determine the highest energy state within the 2p2 multiplicity d. The number of states must be conserved. So for n-electrons in N-states the Pauli exclusion principle gives C_N^n = n!/n!(N-n), and it must equal to sigma(2j + l). Can you figure out the remaining atomic states in the 2p^2 multiple?

Explanation / Answer

The three Hund's Rule are given as follows:

1. The term with maximum multiplicity lies lowest in energy.

2. For a given multiplicity, the term with the largest value of L lies lowest in in energy.

Using these, we can Calculte the values of S, L and J for Carbon, which has two electrons in the 2p shell which have same spin state.

2. For a given multiplicity, the term with the largest value of L lies lowest in in energy.

3. For atoms with less than half-filled shells, the level with the lowest value of J lies lowest in energy.

Related Questions

Navigate

• Browse (All)
• Browse O
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.