What is the hybridization of the nitrogen atom in the ammonium ion ${\mathrm{NH}}_4{+}^{\mathrm{}}$?

• A. The nitrogen is unhybridized
• B. ${\mathrm{sp}}^3$
• C. ${\mathrm{sp}}^2$
• D. $\mathrm{sp}$

Answer: (B)

Verified step by step guidance

1. Identify the central atom and its bonding environment: In the ammonium ion (NH\_4\^+), nitrogen is the central atom bonded to four hydrogen atoms.
2. Determine the number of regions of electron density around the nitrogen: Since nitrogen forms four single bonds with hydrogen atoms and has no lone pairs in NH\_4\^+, there are four regions of electron density.
3. Recall the hybridization corresponding to the number of electron density regions: Four regions of electron density correspond to sp\^3 hybridization.
4. Confirm that the positive charge indicates nitrogen has donated its lone pair to form a bond, so no lone pairs remain on nitrogen, supporting the sp\^3 hybridization model.
5. Conclude that the nitrogen atom in NH\_4\^+ is sp\^3 hybridized because it forms four sigma bonds arranged tetrahedrally.