Ready to learn how to draw the lewis structure of NO?
Here, I have explained 5 simple steps to draw the lewis dot structure of NO (along with images).
So, if you are ready to go with these 5 simple steps, then let’s dive right into it!
Lewis structure of NO (or Nitric Oxide) contains one double bond between the Nitrogen (N) atom and Oxygen (O) atom. The Nitrogen atom has 1 lone pair as well as 1 unpaired electron, and the Oxygen atom has 2 lone pairs.
Let’s draw and understand this lewis dot structure step by step.
(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of NO).
5 Steps to Draw the Lewis Structure of NO
Step #1: Calculate the total number of valence electrons
Here, the given molecule is NO (nitrogen monoxide). In order to draw the lewis structure of NO, first of all you have to find the total number of valence electrons present in the NO molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).
So, let’s calculate this first.
Calculation of valence electrons in NO
- For Nitrogen:
Nitrogen is a group 15 element on the periodic table.
Hence, the valence electrons present in nitrogen is 5 (see below image).
- For Oxygen:
Oxygen is a group 16 element on the periodic table.
Hence, the valence electron present in oxygen is also 6 (see below image).
Hence in a NO molecule,
Valence electrons given by Nitrogen (N) atom = 4
Valence electrons given by Oxygen (O) atom = 6
So, total number of Valence electrons in NO molecule = 5 + 6 = 11
Step #2: Select the center atom
While selecting the atom, you have to put the least electronegative atom at the center.
But here in the NO molecule, there are only two atoms. So you can consider any of the atoms as a center atom.
So, let’s assume that the nitrogen atom is a central atom. (You should assume the less electronegative atom as a central atom.)
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of NO molecule, put the two electrons (i.e electron pair) between the nitrogen atom and oxygen atoms to represent a chemical bond between them.
This pair of electrons present between the Nitrogen (N) atom and Oxygen (O) atom forms a chemical bond, which bonds both the nitrogen atom and oxygen atom with each other in a NO molecule.
Step #4: Complete the octet (or duplet) on outside atom. If the valence electrons are left, then put the valence electrons pair on the central atom
Don’t worry, I’ll explain!
In the Lewis structure of NO, we have just assumed the nitrogen atom as a central atom and so the oxygen atom is an outer atom.
So now, we have to complete the octet on this oxygen atom.
Now, you can see in the above image that the oxygen atom forms an octet.
Also, only 8 valence electrons of NO molecule are used in the above structure.
But there are total 11 valence electrons in NO molecule (as calculated in step #1).
So the number of electrons left to be kept on the central atom = 11 – 8 = 3.
So let’s keep these three electrons (i.e 1 electron pair and 1 unpaired electron) on the central atom (i.e nitrogen atom).
Now, let’s move to the next step.
Step #5: Check whether the central atom has octet or not. If it does not have an octet, then move the electron pair from the outer atom to form a double bond or triple bond
In this step, we have to check whether the central atom (i.e nitrogen) has an octet or not.
In simple words, we have to check whether the central Nitrogen (N) atom has 8 electrons or not.
As you can see from the above image, the central atom (i.e nitrogen) has only 5 electrons. So it does not fulfill the octet rule.
Now, in order to fulfill the octet of nitrogen atom, we have to move the electron pair from the outer atom (i.e oxygen atom) to form a double bond.
Now you can see from the above image that the central atom (i.e nitrogen), is having 7 electrons.
If we try to add one more electron pair on the nitrogen atom, then there will be 7+2=9 electrons in its outermost orbit. And nitrogen atom does not have the capacity to hold 9 electrons in its outermost orbit.
Because of this reason, the above lewis dot structure of NO (having 7 electrons on nitrogen atom) is a stable structure.
Each electron pair (:) in the lewis dot structure of NO represents the single bond ( | ). So the above lewis dot structure of NO can also be represented as shown below.