Question
Which of the following representation of excited states of atoms is impossible?(a) $1 s^{1} 2 s^{1}$(b) $[\mathrm{Ne}] 3 s^{2} 3 p^{3} 4 s^{1}$(c) $[\mathrm{Ne}] 3 s^{2} 3 p^{6} 4 s^{1} 3 d^{6}(\mathrm{~d}) 1 s^{2} 2 s^{2} 2 p^{7} 3 s^{2}$
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The s shell can accommodate 2 electrons, the p shell can accommodate 6 electrons, the d shell can accommodate 10 electrons, and the f shell can accommodate 14 electrons. Show more…
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Among the following representations of excited states of atoms which is impossible? (a) $1 s^{1} 2 s^{1}$ (b) $[\mathrm{Ne}] 3 s^{2} 3 p^{3} 4 s^{1}$ (c) $1 s^{2} 2 s^{2} 2 p^{4} 3 s^{2}$ (d) $[\mathrm{Ne}] 3 s^{2} 3 p^{6} 4 s^{3} 3 d^{2}$
Which of these electron configurations are for atoms in the ground state? In excited states? Which are impossible? (a) $1 s^{2} 2 s^{2}$ (b) $1 s^{2} 2 s^{2} 3 s^{1}$ (c) [Ne] $3 s^{2} 3 p^{8} 4 s^{1}$ (d) $[\mathrm{He}] 2 s^{2} 2 p^{6} 2 d^{2}$ (e) $[\mathrm{Ar}] 4 s^{2} 3 d^{3}$ (f) [Ne] $3 s^{2} 2 p^{5} 4 s^{1}$
Which of these electron configurations are for atoms in the ground state? In excited states? Which are impossible? (a) $1 s^{2} 2 s^{1}$ (b) $1 s^{2} 2 s^{2} 2 p^{3}$ (c) $[\mathrm{Ne}] 3 s^{2} 3 p^{3} 4 s^{1}$ (d) [Ne] $3 s^{2} 3 p^{6} 4 s^{3} 3 d^{2}$ (e) $[\mathrm{Ne}] 3 s^{2} 3 p^{6} 4 f^{-i}$ (f) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$
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