# Nno structure

## How to Calculate the Formal Charges for N2O (Nitrogen dioxide)

20 525 views | 3 Jan. 2019

In order to calculate the

In order to calculate the formal charges for N2O we'll use the equation:

Formal charge = [# of valence electrons] - [nonbonding val electrons] - [bonding electrons / 2]

The number of valence electrons for the atom of interest is found on the Periodic Table.

We find the number of bonding and nonbonding electrons from the Lewis Structure for N2O.

How to draw the N2O Lewis Structure: https://youtu.be/ZlHIQhJlWNs

Nonbonding valence electrons are those around the atom of interest that are not involved in chemical bonds (they aren't being shared with another atom).

Bonding valence electrons are the ones shared between atoms. We'll divide this number by two.

For more help with chemical bonding and formal charge visit http://www.Breslyn.org

Some things to note about N2O Formal Charges:

- Formal charge is different from the oxidation number!

- If you can exceed the octet rule for the central atom it's a good idea to check the formal charges.

- If we have isomers or resonance -- formal charges will help us determine most stable structure.

- The closer the formal charges are to zero the more likely we have the most favorable Lewis structure for the molecule.

- We write the formal charges in (). E.g. (-1)

• Formal Charges: https://youtu.be/vOFAPlq4y_k

• Finding Valence Electrons (element): https://youtu.be/x1gdfkvkPTk

• Exceptions to the Octet Rule: https://youtu.be/Dkj-SMBLQzM

• How to Draw Lewis Structures: https://youtu.be/1ZlnzyHahvo

Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).

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Erin Quintero

Thank you for teaching! This was very helpful

Utkarsh Kumar

*Nitrogen oxide

SOFIQUL ISLAM

To the point. Loved it

# Nno structure

## 59. Homework Assignment #9 - N2O Resonance Structures

35 views | 26 Jul. 2020

Draw three major resonance

Draw three major resonance contributors for the molecule N2O, (linkage pattern:

[N-N-O], being sure to rank the resonance structures in decreasing contribution to the resonance hybrid. Be sure to justify your answer fully!

00:00 N2O Resonance

00:45 Total # of Valence Electrons

01:25 Lewis Structure #1

03:52 Formal Charge

06:05 Resonance Structure #2

06:58 Formal Charge for Structure #2

08:40 Resonance Structure #3

09:58 Formal Charge for Structure #3

12:05 Resonance Ranking Explanation

19:52 Final Ranking

# Nno structure

## Formal Charges: Calculating Formal Charge

619 370 views | 17 May. 2013

A step-by-step description

A step-by-step description on how to calculate formal charges. Formal charges are important because they allow us to predict which Lewis structure is the most likely to exist in the real world.

Get more chemistry help at www.Breslyn.org.

Often you are given a compound with more than one possible Lewis structure. Often this is the case with elements like Sulfur or Phosphorus which can have more than eight valence electrons. In these cases it is important to calculate formal charges to determine which structure is the best. The structure with formal charges closest to zero will be the best.

Mahendra Kumar

Nice trick.
But it is so lenthy can you have another trick to calculate Formal Charge...

Hani baloch

thankyouuu so much

Parul Aggarwal

I guess d formal charge for each atom in covalent compounds is 0.....BTW THANX???????????

Holly Fletcher

For the last example, isn't it positive 1 plus negative 1 plus zero, making the charge 0 on the SO2 with only one double-bonded O? Which would you then choose as most likely to occur because they are equally as electronegative?

K A

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Thank you so much prof.

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Grant MD

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Pimpo Jamir

Thank you so much

Kush Agarwal

One second. Didn't both the SO2 structures have a formal charge of 0?? So why are we only saying that the second one where both oxygens are double bonded is correct??

Sowmya Gudapati

Thank you! I just had a quick question, when both resonance structures have the same overall formal charge what do you do?

Kaushik Sanyal

https://youtu.be/KAVS0kMoofc
Formal charge calculation

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The One

Oxygen has 6 valence electrons, howcome 6 nonbonding electrons and 2 bonding electrons???

Ehung Loh

Sir can u explain why sulphur in so2 with formal charge of 0 is able to have more than 8 valence electrons?

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Edit:
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Abod Alashkar

How did you get 10 electrons on sulfur

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LightcapMath

Another excellent explanation. Question: other than S an P what other element can have more the an octet? David L

Z3FRAN

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Bula Sinha

Sulphur's valency is 6. At 2:47 how can you count two electrons of the right oxygen as bonding electrons of sulphur?? Isn't this incorrect?

Anand Malu

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Robert Henkel

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Thank you??

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Me too from India

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aks1

So sulfer has more than 8 electrons? (in the second structure)

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Bindu Barmecha

How come 2 lone pair electrons are left in sulphur when it is forming double bond with both oxygen(s)

leggomyegggo

Why is the bonding for Hydrogen 2 and not 4?

러버덕덕

non bounding ones are counted as a whole and bounding ones are shared by two
but what’s up with the formal charge having to be close to zero?

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Azizul Hassan

Plzzz tell how to calculate formal charge on tetrahybridoborate??

ok ok

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Mesmerizing Eyes

Could you explain Lewis structure of no

Sarah DeMonia

Why do you divide the bonding electrons by 2?

Natasha Roberts

How would you find the formula charge for Cl3

mahou shoujo

But the Sulfur will then have 10 electrons...

Sheeza Eman

Thankyou??

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DEBASISH SARKAR

Sir the best structure of so2 has more than 8 electrons how is it possible

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angel

instead of diving he bonding electrons into two (2), you can just first transform those bonding electrons into a line then count them as one, less confusion

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Lourdes

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