The electronic configuration 1s^{2}2s^{2}2p^{ | vedclass

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(D) The given electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{1}$.Counting the total number of electrons: $2 + 2 + 6 + 1 = 11$ electrons.For $Al^{3

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None of these

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(D) The given electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{1}$.Counting the total number of electrons: $2 + 2 + 6 + 1 = 11$ electrons.For $Al^{3+}$ (atomic number $13$),the number of electrons is $13 - 3 = 10$. Configuration: $1s^{2}2s^{2}2p^{6}$.For $Ne$ (atomic number $10$),the ground state configuration is $1s^{2}2s^{2}2p^{6}$. An excited state would involve promotion of an electron to a higher orbital,such as $1s^{2}2s^{2}2p^{5}3s^{1}$.For $Mg^{+}$ (atomic number $12$),the number of electrons is $12 - 1 = 11$. The ground state configuration is $1s^{2}2s^{2}2p^{6}3s^{1}$.Since the configuration $1s^{2}2s^{2}2p^{6}3s^{1}$ represents the ground state of $Mg^{+}$,and none of the options correctly identify this as a ground state species,the correct choice is $D$.

The electronic configuration $1s^{2}2s^{2}2p^{6}3s^{1}$ corresponds to which of the following species?

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