I’m super excited to teach you the lewis structure of NH2OH in just 6 simple steps.
Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of NH2OH molecule.
So, if you are ready to go with these 6 simple steps, then let’s dive right into it!
Lewis structure of NH2OH contains a single bond between the Nitrogen-Oxygen atoms, Nitrogen-Hydrogen atoms and Oxygen-Hydrogen atoms. The Nitrogen atom (N) is at the center and it is surrounded by two Hydrogen atoms (H) and one OH group. The Nitrogen atom has 1 lone pair 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 NH2OH).
6 Steps to Draw the Lewis Structure of NH2OH
Step #1: Calculate the total number of valence electrons
Here, the given molecule is NH2OH. In order to draw the lewis structure of NH2OH, first of all you have to find the total number of valence electrons present in the NH2OH 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 NH2OH
- 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 Hydrogen:
Hydrogen is a group 1 element on the periodic table.
Hence, the valence electron present in hydrogen is 1 (see below image).
- For Oxygen:
Oxygen is a group 16 element on the periodic table.
Hence, the valence electron present in oxygen is 6 (see below image).
Hence in a NH2OH molecule,
Valence electrons given by each Nitrogen (N) atom = 5
Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by Oxygen (O) atom = 6
So, total number of Valence electrons in NH2OH molecule = 5 + 1(2) + 6 + 1 = 14
Step #2: Select the center atom (H is always outside)
While selecting the center atom, always put the least electronegative atom at the center.
(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table).
Here in the NH2OH molecule, if we compare the nitrogen atom (N), oxygen atom (O) and hydrogen atom (H), then hydrogen is less electronegative than nitrogen and oxygen. But as per the rule, we have to keep hydrogen outside.
So, nitrogen (which is less electronegative than oxygen) should be placed in the center and the remaining hydrogen atoms as well as OH group will surround it.
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of NH2OH molecule, put the two electrons (i.e electron pair) between the atoms to represent a chemical bond between them.
These pairs of electrons present between the atoms form a chemical bond, which bonds these atoms with each other in a NH2OH molecule.
Step #4: Complete the octet (or duplet) on outside atoms. 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 NH2OH, the outer atoms are hydrogen atoms as well as oxygen atom.
Hydrogen already has a duplet (see below image).
So now, you have to complete the octet on oxygen atom (because oxygen requires 8 electrons to have a complete outer shell).
Now, you can see in the above image that the oxygen atom forms an octet.
Also, only 12 valence electrons of NH2OH molecule are used in the above structure.
But there are total 14 valence electrons in NH2OH molecule (as calculated in step #1).
So the number of electrons left to be kept on the central nitrogen atom = 14 – 12 = 2.
So let’s keep these two electrons (i.e 1 electron pair) on the central nitrogen atom.
Now, let’s move to the next step.
Step #5: Check whether the central atom has octet or not
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 is having 8 electrons or not.
As you can see from the above image, the central atom (i.e nitrogen), is having 8 electrons. So it fulfills the octet rule and the nitrogen atom is stable.
Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom
Now, you have come to the final step and here you have to check the formal charge on nitrogen atom (N), oxygen atom (O) as well as each hydrogen atom (H).
For that, you need to remember the formula of formal charge;
Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2
- For Nitrogen:
Valence electrons = 5 (as it is in group 15)
Nonbonding electrons = 2
Bonding electrons = 6
- For Oxygen:
Valence electron = 6 (as it is in group 16)
Nonbonding electrons = 4
Bonding electrons = 4
- For Hydrogen:
Valence electron = 1 (as it is in group 1)
Nonbonding electrons = 0
Bonding electrons = 2
|Formal charge||=||Valence electrons||–||Nonbonding electrons||–||(Bonding electrons)/2|
So you can see above that the formal charges on nitrogen, oxygen as well as hydrogen are “zero”.
Hence, there will not be any change in the above structure and the above lewis structure of NH2OH is the final stable structure only.
Each electron pair (:) in the lewis dot structure of NH2OH represents the single bond ( | ). So the above lewis dot structure of NH2OH can also be represented as shown below.