IDNLearn.com: Where your questions meet expert advice and community support. Join our interactive Q&A community and get reliable, detailed answers from experienced professionals across a variety of topics.
Sagot :
To determine the correct Lewis structure for nitrogen gas ([tex]\(N_2\)[/tex]), we need to follow these steps:
1. Count the total number of valence electrons:
- Nitrogen ([tex]\(N\)[/tex]) is in Group 15 (also known as Group V) of the periodic table and has 5 valence electrons.
- Therefore, two nitrogen atoms will have a total of [tex]\(2 \times 5 = 10\)[/tex] valence electrons.
2. Determine the bonding pattern:
- Nitrogen atoms tend to form a triple bond to satisfy the octet rule because each nitrogen atom needs three more electrons to complete its octet.
- A triple bond consists of 6 electrons (3 pairs) being shared between the two nitrogen atoms.
3. Distribute the electrons:
- Start by placing three bonds (which count as 6 electrons) between the two nitrogen atoms:
[tex]\[ N \equiv N \][/tex]
- Each nitrogen atom will now have 2 electrons left (since we started with 10 electrons and used 6 for the triple bond).
4. Add lone pairs:
- Each nitrogen atom will have one lone pair (2 additional electrons).
Putting this all together, the Lewis structure for nitrogen gas ([tex]\(N_2\)[/tex]) is:
```
: N ≡ N :
```
Breaking it down, each nitrogen atom has:
- Three bonding pairs (6 electrons) in the triple bond.
- One lone pair (2 electrons).
This completes the octet for both nitrogen atoms (8 electrons each).
Thus, the correct Lewis structure for nitrogen gas ([tex]\(N_2\)[/tex]) is:
[tex]$ : N \equiv N : $[/tex]
1. Count the total number of valence electrons:
- Nitrogen ([tex]\(N\)[/tex]) is in Group 15 (also known as Group V) of the periodic table and has 5 valence electrons.
- Therefore, two nitrogen atoms will have a total of [tex]\(2 \times 5 = 10\)[/tex] valence electrons.
2. Determine the bonding pattern:
- Nitrogen atoms tend to form a triple bond to satisfy the octet rule because each nitrogen atom needs three more electrons to complete its octet.
- A triple bond consists of 6 electrons (3 pairs) being shared between the two nitrogen atoms.
3. Distribute the electrons:
- Start by placing three bonds (which count as 6 electrons) between the two nitrogen atoms:
[tex]\[ N \equiv N \][/tex]
- Each nitrogen atom will now have 2 electrons left (since we started with 10 electrons and used 6 for the triple bond).
4. Add lone pairs:
- Each nitrogen atom will have one lone pair (2 additional electrons).
Putting this all together, the Lewis structure for nitrogen gas ([tex]\(N_2\)[/tex]) is:
```
: N ≡ N :
```
Breaking it down, each nitrogen atom has:
- Three bonding pairs (6 electrons) in the triple bond.
- One lone pair (2 electrons).
This completes the octet for both nitrogen atoms (8 electrons each).
Thus, the correct Lewis structure for nitrogen gas ([tex]\(N_2\)[/tex]) is:
[tex]$ : N \equiv N : $[/tex]
Thank you for contributing to our discussion. Don't forget to check back for new answers. Keep asking, answering, and sharing useful information. Your search for answers ends at IDNLearn.com. Thanks for visiting, and we look forward to helping you again soon.