Question #008eb

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Question #008eb

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Answer 1 · 2017-02-01T18:14:34

Choices a, b, and d are not written properly
and,
there is nothing wrong with choice c

Explanation:

Choice a, b, and d are all not correct valence electron configurations when writing the valence electron shorthand.

Choice a is incorrect because for $n = 2, l = 0$ $n=2, l=0$ there are only two orbital about the ( $s$ $s$ ) subshell.

Choice b is incorrect because two " $2 s^{2}$ $2s^2$ " orbital are written and the next two electron would instead fill the $n = 2, l = 1$ $n=2,l=1$ ( $p$ $p$ ) shell and its 3 orbital.

Choice d is incorrect because for $n = 1$ $n=1$ , $l$ $l$ can only $= 0$ $=0$ . Remember that $l$ $l$ can have value between $0 \to n - 1$ $0 -> n-1$ .

In other words, there is no such thing as a " $1 p$ $1p$ " orbital.

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