We"re asked to answer 3 components of the problem. Part A asks the only feasible values that ml because that an electron in an s orbital, part B asks the possible worths of mℓfor one electron in a d orbital, and part C asks to check all using setsof quantum numbersthat use for one electron in one atom.
You are watching: What is the only possible value of mℓ for an electron in an s orbital
Recall that thequantum numbersthat define an electron are:
•Principal Quantum Number(n): faces thesize and also energy that the atomic orbital. Thepossible worths for nare1 to ∞.
•Angular inert Quantum Number(l): encounters theshape that the atom orbital. Thepossible values for lare0 come n – 1.
•Magnetic Quantum Number(ml): deals with theorientation of the atom orbitalin 3D space. Thepossible values for mlare the selection of–l to +l.
•Spin Quantum Number(ms): deals with thespin the the electron. Thepossible worths for msare either–1/2 (spin down) or +1/2 (spin up).
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Part A.What is the only feasible value of mℓ because that an electron in one s orbital? Express your answer numerically.
Part B.What room the possible values the mℓ for an electron in a d orbital? Express your answer numerically through sequential values separated by commas.
Part C.Which of the following set of quantum numbers (ordered n, ℓ, mℓ, ms) are possible for an electron in one atom? check all that apply.
a. 3, 2, 0, -1/2b. -4, 3, 1, 1/2c. 3, 2, 2, -1/2d. 5, 3, -3, 1/2e. 3, 1, -2, -1/2f. 3, 3, 1, -1/2g. 2, 1, 0, -1h. 4, 2, 3, -1/2
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