2. Consider the resonance structures below Tag ang A C. B C D a. On each structure (A-D) show all lone pair electrons. b. Provide arrows that show electron movement from A to B, B to C, and C to D. Which is the "most contributing" resonance form (A, B, C, or D)? Explain your choice. -00 d. Draw the resonance hybrid for this molecule (use "delta" 8+ or - to show partial charges).
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.
![**2. Consider the resonance structures below**
![Resonance Structures Diagram]
**a.** On each structure (A-D) show *all* lone pair electrons.
**b.** Provide arrows that show electron movement from A to B, B to C, and C to D.
**c.** Which is the "most contributing" resonance form (A, B, C, or D)? Explain your choice.
**d.** Draw the resonance hybrid for this molecule (*use “delta” δ+ or − to show partial charges*).
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### Diagram Explanation
The diagram displays four resonance structures labeled A, B, C, and D. Each structure consists of a series of connected atoms with alternating double and single bonds, and a negatively charged oxygen at the end.
- **Structure A**: Features a negatively charged oxygen at one end of the molecule.
- **Structure B**: Illustrates the movement of the negative charge along the molecule.
- **Structure C**: Shows further delocalization of the negative charge.
- **Structure D**: Continues the delocalization pattern, with the negative charge now on a different oxygen.
The structures are interconnected with double-headed arrows, indicating resonance between them.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe243852a-5427-4fc7-bd56-ad30d22cf89a%2Fadd27644-437a-4ced-828d-c2a52595c2a5%2F69pkerw_processed.png&w=3840&q=75)
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