Question

1. which is the correct ending for nitrogens orbital diagram? * 4 point electron configurations electron configuration examples atomic number h 1 1s¹ he 2 1s² li 3 1s²2s¹ be 4 1s²2s² b 5 1s²2s²2p¹ c 6 1s²2s²2p² n 7 1s²2s²2p³ o 8 1s²2s²2p⁴ arrows represent electrons. energy shell and subshells superscript gives number of electrons. electron pair a. 2p³ (three half - filled orbitals) b. 2p⁶ (completely filled) c. 2p² (two half - filled orbitals) d. 3p³ (three half - filled orbitals)

Explanation:

Step1: Recall nitrogen's atomic number

Nitrogen has an atomic number of 7, so it has 7 electrons.

Step2: Write electron - configuration steps

First, fill the 1s orbital with 2 electrons ($1s^{2}$), then the 2s orbital with 2 electrons ($2s^{2}$). The remaining 3 electrons go into the 2p orbitals. According to Hund's rule, electrons fill degenerate orbitals singly first before pairing up. So the 2p sub - shell has 3 half - filled orbitals for nitrogen, written as $2p^{3}$.

Answer:

A. 2p³ (three half - filled orbitals)