OCN- Lewis structure

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OCN^– (cyanate) has one oxygen atom, one carbon atom, and one nitrogen atom.

In the OCN^– Lewis structure, there is a single bond between carbon and oxygen atom, and a triple bond between carbon and nitrogen atom. The oxygen atom has three lone pairs, and the nitrogen atom has one lone pair.

Also, there is a negative (-1) charge on the oxygen atom.

Steps

Use these steps to correctly draw the OCN^– 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
#4 Convert lone pairs of the atoms, and minimize formal charges
#5 Repeat step 4 if needed, until all charges are minimized, to get a stable Lewis structure

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, oxygen lies in group 16, carbon lies in group 14, and nitrogen lies in group 15.

Hence, oxygen has six valence electrons, carbon has four valence electrons, and nitrogen has five valence electrons.

Since OCN^– has one oxygen atom, one carbon atom, and one nitrogen atom, so…

Valence electrons of one oxygen atom = 6 × 1 = 6
Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of one nitrogen atom = 5 × 1 = 5

Now the OCN^– has a negative (-1) charge, so we have to add one more electron.

So the total valence electrons = 6 + 4 + 5 + 1 = 16

Learn how to find: Oxygen valence electrons, Carbon valence electrons, and Nitrogen valence electrons

• Second, find the total electron pairs

We have a total of 16 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 = 16 ÷ 2 = 8

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since carbon is less electronegative than oxygen and nitrogen, assume that the central atom is carbon.

Therefore, place carbon in the center and oxygen and nitrogen on either side.

• And finally, draw the rough sketch

#2 Mark lone pairs on the atoms

Here, we have a total of 8 electron pairs. And two bonds are already marked. So we have to only mark the remaining six electron pairs as lone pairs on the sketch.

Also remember that all three (oxygen, carbon, and nitrogen) are the period 2 elements, so they can not keep more than 8 electrons in their last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are oxygen and nitrogen.

So for oxygen and nitrogen, there are three lone pairs, and for carbon, there is zero lone pair because all six electron pairs are over.

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 oxygen atom, formal charge = 6 – 6 – ½ (2) = -1

For carbon atom, formal charge = 4 – 0 – ½ (4) = +2

For nitrogen atom, formal charge = 5 – 6 – ½ (2) = -2

Here, all three atoms have charges, so mark them on the sketch as follows:

The above structure is not a stable Lewis structure because all three atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.

#4 Convert lone pairs of the atoms, and minimize formal charges

Here we have to convert a lone pair of the nitrogen atom (instead of the oxygen atom). Because nitrogen is less electronegative than oxygen. And so, it can give more valence electrons to share them.

Or remember this way, in OCN^– and similar type structures, we have to make sure that the negative charge comes on the most electronegative element. In this case, the most electronegative element is oxygen.

Therefore, convert a lone pair of the nitrogen atom to make a new C — N bond with the carbon atom as follows:

#5 Repeating step 4 to get a stable Lewis structure

Since there are charges on the atoms, again convert a lone pair of the nitrogen atom to make a new C — N bond with the carbon atom as follows:

In the above structure, you can see that the central atom (carbon) forms an octet. And the outside atoms (oxygen and nitrogen) also form an octet. Hence, the octet rule is satisfied.

Now there is still a negative (-1) charge on the oxygen atom.

This is okay, because the structure with a negative charge on the most electronegative atom is the best Lewis structure. And in this case, the most electronegative element is oxygen.

Also, the above structure is more stable than the previous structures. Therefore, this structure is the most stable Lewis structure of OCN^–.

And since the OCN^– has a negative (-1) charge, mention that charge on the Lewis structure by drawing brackets as follows:

Next: ICl₄^– Lewis structure

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External links

• https://lambdageeks.com/ocn-lewis-structure/
• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/OCN–lewis-structure.html
• https://socratic.org/questions/what-is-the-lewis-structure-for-ocn
• https://topblogtenz.com/ocn-lewis-structure-molecular-geometry-hybridization-polar-or-nonpolar/
• https://techiescientist.com/nco-lewis-structure/