Question 7.3.1: Apply the Pauli exclusion principle. a. Identify the orbital......
Apply the Pauli exclusion principle.
a. Identify the orbitals in the following list that fill before the 4d orbitals: 3d, 4s, 5s, 6p.
b. What is the maximum number of electrons in the 4f subshell?
c. An electron in an orbital has the following quantum numbers: n = 3, ℓ = 1, m_{ℓ} = +1, and m_{s} = +½. Identify the orbital and the direction of electron spin (up or down).
You are asked to answer questions about orbital filling and to apply the Pauli exclusion principle.
You are given information about specific orbitals or electrons.
a. 3d, 4s, and 5s. In general, orbitals fill in order of increasing (n + ℓ). When two or more
subshells have the same (n + ℓ) value, electrons fill the orbital with the lower n value.
The order of filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ….
b. 14. There are 7 orbitals in the f subshell, and each orbital can hold two electrons.
c. 3p, up. The set of three quantum numbers n = 3, ℓ = 1, m_{ℓ} = +1 together specifies a 3p orbital. The electrons in the 3p orbital are oriented “spin up” (m_{s} = +½) or “spin down” (m_{s} = –½), resulting in two unique sets of four quantum numbers for the two electrons in this orbital.