NI3 (nitrogen triiodide) has one nitrogen atom and three iodine atoms.
In the NI3 Lewis structure, there are three single bonds around the nitrogen atom, with three iodine atoms attached to it. Each iodine atom has three lone pairs, and the nitrogen atom has one lone pair.
Steps
Use these steps to correctly draw the NI3 Lewis structure:
#1 First draw a rough sketch
#2 Mark lone pairs on the atoms
#3 Calculate and mark formal charges on the atoms, if required
Let’s discuss each step in more detail.
#1 First draw a rough sketch
- First, determine the total number of valence electrons
In the periodic table, nitrogen lies in group 15, and iodine lies in group 17.
Hence, nitrogen has five valence electrons and iodine has seven valence electrons.
Since NI3 has one nitrogen atom and three iodine atoms, so…
Valence electrons of one nitrogen atom = 5 × 1 = 5
Valence electrons of three iodine atoms = 7 × 3 = 21
And the total valence electrons = 5 + 21 = 26
Learn how to find: Nitrogen valence electrons
- Second, find the total electron pairs
We have a total of 26 valence electrons. And when we divide this value by two, we get the value of total electron pairs.
Total electron pairs = total valence electrons ÷ 2
So the total electron pairs = 26 ÷ 2 = 13
- Third, determine the central atom
We have to place the least electronegative atom at the center.
Since iodine is less electronegative than nitrogen, the central atom should be iodine, right?
But if we place iodine in the center and nitrogen outside, and calculate the formal charge, then we do not get the formal charges on atoms closer to zero.
And the structure with the formal charges on atoms closer to zero is the best Lewis structure.
Hence, here we have to assume that the central atom is nitrogen.
Therefore, place nitrogen in the center and iodines on either side.
- And finally, draw the rough sketch
#2 Mark lone pairs on the atoms
Here, we have a total of 13 electron pairs. And three N — I bonds are already marked. So we have to only mark the remaining ten electron pairs as lone pairs on the sketch.
Also remember that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell. And iodine is a period 5 element, so it can keep more than 8 electrons in its last shell.
Always start to mark the lone pairs from outside atoms. Here, the outside atoms are iodines.
So for each iodine, there are three lone pairs, and for nitrogen, there is one lone pair.
Mark the lone pairs on the sketch as follows:
#3 Calculate and mark formal charges on the atoms, if required
Use the following formula to calculate the formal charges on atoms:
Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons
For nitrogen atom, formal charge = 5 – 2 – ½ (6) = 0
For each iodine atom, formal charge = 7 – 6 – ½ (2) = 0
Here, both nitrogen and iodine atoms do not have charges, so no need to mark the charges.
In the above structure, you can see that the central atom (nitrogen) forms an octet. And the outside atoms (iodines) also form an octet. Hence, the octet rule is satisfied.
Therefore, this structure is the stable Lewis structure of NI3.
Next: CH2F2 Lewis structure
External links
- https://topblogtenz.com/nitrogen-triiodide-ni3-lewis-structure-molecular-geometry-hybridization-polar-or-nonpolar/
- https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/NI3-lewis-structure.html
- https://lambdageeks.com/ni3-lewis-structure/
- https://oneclass.com/homework-help/chemistry/6910460-lewis-structure-for-ni3.en.html
Deep
Learnool.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.