Which of the following represent noble gas configuration?

1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10}, | 5 s^{2} 5 p^{6}

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1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10} 4 f^{14}, | 5 s^{2} 5 p^{6} 5 d^{1}, 6 s^{2} |

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1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10}, | 5 s^{2} 5 p^{6} 5 d^{1}, | 6 s^{2} |

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1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10}, |

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Solution

The correct option is A $1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10}, | 5 s^{2} 5 p^{6}$
Except helium $(1 s^{2})$ , All noble gases have the general electronic configuration $n s^{2} n p^{6}$ .
Only option 'a' has configuration $n s^{2} n p^{6}$ . i.e. $1 s^{2}, | 2 s^{2} 2 p^{6}, | 3 s^{2} 3 p^{6} 3 d^{10}, | 4 s^{2} 4 p^{6} 4 d^{10}, | 5 s^{2} 5 p^{6}$ . Hence option (a) is correct.

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