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Assign formal charges to each atom in the resonance forms of n2o. which resonace form is likely to contribute most to the correct

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transitionstate
Formal Charge is Calculated usinf following Formula,

Formal Charge  =  [# of Valence e⁻] - [# of Lone Pair e⁻ + 1/2 # of Bonding e⁻]

Lets calculate formal charge of Nitrogen in structure 3,

                              Formal Charge  =  [5] - [6 + 2/2]

                              Formal Charge  =  [5] - [6 + 1]

                              Formal Charge  =  [5] - [7]

                              Formal Charge  =  -2

You can calculate Formal charge for each atom in each resonating structure.
Also, the structure B dominates because the oxygen atom has a negative charge and being more electronegative in nature it is plausible. 
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The formal charge is the charge assigned to an atom in a molecule. Second resonance form is most likely to contribute to the structure.

Formal Charge:

It is the charge assigned to an atom in the molecule. It can be calculated by subtracting the Valence electrons in the atom with the total non-bonding electron and bonds.  

Formal charge formula,

FC = VE - ( NBE + B)

Where,

VE - valence electron

NBE - Non- bonded Electrons

B - number of bonds

Calculate the formal charge of Nitrogen for 1st resonance structure of [tex]\rm \bold { N_2O}[/tex],

FC = 5 - ( 4 + 2 )

FC = 5 - 6

FC = -1

So, we can calculate the formal charge for other atoms in the molecules using this formula.

To know more about formal charges refer to the link:

https://brainly.com/question/15315809

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