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.
For C ~ F, you need draw the proper Lewis structure first, then draw the resonances
![### Discussion Questions:
#### E. NO₃Θ
_Given Answer Space:_
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#### F. H₂N-CΘH-CH=CH-NH₂
_Given Answer Space:_
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![### Drawing Lewis Structures and Resonance for Compounds
#### Instructions
For parts C to F, you need to draw the proper Lewis structure first, then draw the resonances. You **MAY** need to add lone pairs, but the overall charge should agree with the given one.
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**C. H₃C-NO**
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[Draw Lewis Structure Here]
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**D. O₌O⊖O≡O**
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[Draw Lewis Structure Here]
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#### Explanation of Graphs or Diagrams
If there are any, fill the boxes with respective Lewis structures and resonance forms of each compound. The overall charge of the compounds should be in agreement with the given formula.
For part **C**, draw the Lewis structure of H₃C-N═O and any possible resonance forms.
For part **D**, draw the Lewis structure of ozone (O₃) considering the charges and resonance structures that involve alternating double bonds and formal charges.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa7f9c6ce-7c61-4a7b-90a0-6a641d198bf8%2F6cd0f995-0f86-4faa-83ce-5c5d64c54c24%2Fkwodbwu_processed.png&w=3840&q=75)
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