What is the total number of p electrons in a single phosphorus atom in its ground state?

3

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5

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9

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15

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Solution

The correct option is C $9$
The electronic configuration of Phosphorous is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$ .
Hence the total number of $p$ electrons is $6 + 3 = 9$ .
Therefore, option C is the right answer.

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What is the total number of p electrons in a single phosphorus atom in its ground state?

The correct option is C 9The electronic configuration of Phosphorous is 1s22s22p63s23p3.Hence the total number of p electrons is 6+3=9.Therefore, option C is the right answer.

The correct option is C $9$
The electronic configuration of Phosphorous is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}$ .
Hence the total number of $p$ electrons is $6 + 3 = 9$ .
Therefore, option C is the right answer.