Question

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

Answer 1

Answer:

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.

Answer 2

The correct quantum numbers and  electron configuration for the highest energy electron will be:

5. $Co: [Ar]4s^2 3d^7$ ; n = 3; l = 2; ml = −2, −1, 0, 1, 2

Quantum numbers:

The set of numbers used to describe the position and energy of the electron in an atom are called quantum numbers.

There are four quantum numbers:

• principal
• azimuthal
• magnetic
• spin quantum numbers

For cobalt (Co):

"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.

Thus, correct option is 5.

Find more information about Quantum number here:

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