Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Step 1
The 4 quantum numbers are
1) Principal quantum number (n) = shell number or orbit number
2) Azimuthal quantum number (ℓ) = sub-shell number
ℓ = 0 for s orbital, ℓ = 1 for p orbital, ℓ = 2 for d orbital, and ℓ = 3 for f orbital,
3) Magnetic quantum number (mℓ)
The possible values of mℓ are all integers in the range [-ℓ , +ℓ]
4) Spin quantum number (ms ) = either +1/2 or -1/2
The allowable values of ℓ for any particular n are the integers present in the range [0, n) where 0 is included but n is not.
And the allowable values of mℓ for any ℓ are all the integral values in the range [-ℓ, ℓ] where both ends are inculded.
Hence the value of 0 ≤ ℓ < n and the value of -ℓ ≤ mℓ ≤ ℓ
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