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211. From the following sets of quantum numbers, state which are possible. Explain why others are not permitted.
(i) n = 0, l =0, m = 0, s= + 1/2
(ii) n = 1, l =0, m =0, s = +1/2
(iii) n =1, l =1, m = -0, s= +1/2

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212. How many sub-shells are associated with n = 4?

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213. How many electrons will be present in the sub-shells having m_s value of - ¹/₂for n =4 ?

The number of orbitals in 4th shell = n² - 4² = 16 Since each orbital can accommodate a maximum of two electrons with opposite spin, therefore each orbital has one electron with ms = - ¹/₂ .
Hence there will be 16 electrons with ms = - ¹/₂ .

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214. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 0, l = 0, m_l = 0, m_s = +1/2

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215. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 1, l = 0, m_l = 0, m_s = -1/2

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216. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 1, l = 1, m_l = 0, m_s = +1/2

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217. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 2, l = 1, m_l = 0, m_s = -1/2

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218. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 3, l = 3, m_l = -3, m_s = +1/2

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219. Explain, giving reasons, which of the following sets of quantum numbers are not possible:
n = 3, l = 1, m_l = 0, m_s = +1/2

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220.

From the following sets of quantum numbers, state which are possible. Explain why others are not permitted.
(i) n = 1, l = 0, m = +1, s = +1/2

(ii) n = 2, l = 1, m =-1, s = -1/2

(iii) n = 2, l =2, m = 0, s = -1/2

(iv) n =2, l =1, m = 0, s =+1/2

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