5. Three possible resonance structures for dinitrogen monoxide (N20) are drawn below. •. :N=N=0: :NEN-0: :N-N=0: a. How many total valence electrons are available in N2O? b. What is the formal charge on the oxygen atom in the structure farthest to the left? Resonance structures that are considered unimportant when describing the average bonding are those that either have individual atoms bearing a formal charge greater than or equal to two for any individual atom and/or a high total absolute value formal charge for the entire molecule, calculated by adding the absolute values of each of the atoms. Which of these three structures not as important as the other two in determining the accurate structure of N20? Support your conclusion using formal charges. C.
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![**Resonance Structures of Dinitrogen Monoxide (N₂O)**
Three possible resonance structures for dinitrogen monoxide (N₂O) are illustrated below:
1. Structure 1:
\[ \cdot\cdot \text{N}= \text{N}= \text{O} \cdot\cdot \]
2. Structure 2:
\[ \cdot\cdot \text{N}- \text{N}- \text{O} \cdot\cdot \]
3. Structure 3:
\[ \cdot\cdot \text{N}- \text{N} \equiv \text{O} \]
**Questions:**
a. How many total valence electrons are available in N₂O? _______
b. What is the formal charge on the oxygen atom in the structure farthest to the left? _______
c. Resonance structures that are considered unimportant when describing the average bonding are those that either have individual atoms bearing a formal charge greater than or equal to two for any individual atom and/or a high total absolute value formal charge for the entire molecule, calculated by adding the absolute values of each of the atoms. Which of these three structures are not as important as the other two in determining the accurate structure of N₂O? Support your conclusion using formal charges.
**Note:**
The Lewis structures provided are designed to illustrate the different possible arrangements of electrons between nitrogen and oxygen atoms in N₂O. The structures include lone pairs and bonds (single, double, and triple) to show the covalent bonding and electron distribution. Understanding which structure contributes most to the actual description of N₂O involves analyzing the stability indicated by formal charges.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F107b68ef-5916-46d8-b604-d8abbf265ef5%2F7bb1dff8-ff95-4327-8d96-3eb3d5d2513f%2Fg0wbyi_processed.jpeg&w=3840&q=75)
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