Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:I'll solve this problem step by step:
Step 2:: Understand Nitrogen's Electron Configuration
- Electron configuration is $$1s^{2} 2s^{2} 2p^{3}
- Nitrogen is in Group 15 (VA) of the periodic table - Its atomic number is 7
Step 3:: Determine Valence Electrons
- Nitrogen has 5 valence electrons in its outer shell - To achieve a stable electron configuration like noble gases, it needs to gain 3 electrons
Step 4:: Predict Ion Formation
- The electron configuration becomes $$1s^{2} 2s^{2} 2p^{6}$$, which is identical to neon's configuration
- This allows it to have a complete octet (8 electrons) in its outer shell
Final Answer
Nitrogen forms a N^{3^{-}} (nitride) ion when it becomes an ion.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students