Which of the following shows the correct quantum numbers (n; ℓ; mℓ) and electron configuration for the highest energy electron (s) in the given atoms? 1. Rb: [Kr]5s 1; n = 5; ℓ = 0; mℓ = 0, 1 2. N: [He]2s 2 2p 3; n = 2; ℓ = 2; mℓ = - 2, - 1, 0, 1, 2 3. Fe: [Ar]4s 2 3d 6; n = 4; ℓ = 0; mℓ = 0 4. Ca: [Ar]4s 2; n = 4; ℓ = 1; mℓ = - 1, 0+1 5. Co: [Ar]4s 2 3d7; n = 3; ℓ = 2; mℓ = - 2, - 1, 0, 1, 2

Co: [Ar]4s 2 3d7; n = 3; ℓ = 2; mℓ = - 2, - 1, 0, 1, 2

Explanation:

Hello,

Quantum numbers for the highest energy level of cobalt are correct, because n matches with the considered sub-orbital 3, l matches with the d region that has a value of 2 based on the rule: if region=s, l=0; if region=p, l=1; if region=d, l=2 and if region=f, l=3 and the ml goes from - 2 to 2 including zero by taking into account the l quantum number. The rest of the options are wrong since the quantum numbers don't match with the corresponding orbitals.

Best regards.