Which orbital notation correctly represents the outermost principle energy level of a nitrogen atom

Which orbital notation correctly represents the outermost principal energy level of a nitrogen atom in the ground state?

A- s(<>) p(< )(< )(< )
B- s(<>) p(<>)(< )( )
C- s(<>) p(<>)(< )(< )
D- s(<>) p(<>)(<>)( )

And can you explain how you would know this??

It's A. When you go from right to left on the periodic table to nitrogen, the first two fill the s orbital. Next the p orbital begins filling, on electron goes into each orbital before they start adding a second to the orbital. So after the s is filled the p counts up to three and that's when you reach nitrogen

C. Nitrogen is the 7th element...B and D are incorrectly written, so by elimination it has to be A or C...nitrogen needs seven arrows...obviously it is C

A- s(<>) p(< )(< )(< )
Since N has 5 valence electrons and electrons half fill and orbital before pairing, 2 of the 5 are in the 2s orbital leaving 3 electrons for the 2p sublevel, all unpaired.