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 Formate
Consider the resonance structures of formate depicted in the diagram. The two structures represent different possible arrangements of electrons within the formate ion.
### Diagram Explanation
- The left structure shows a formate ion where the carbon is double-bonded to one oxygen atom and single-bonded to another.
- The right structure depicts a different resonance form, with the positions of the double and single bonds switched between the oxygen atoms.
- The double-headed arrow between the structures indicates resonance, showing that the actual formate ion is a hybrid of these two structures.
### Statements to Evaluate
Select the true statements about the resonance structures:
- [ ] Each oxygen atom has a double bond 50% of the time.
- [ ] The actual structure of formate is an average of the two resonance forms.
- [ ] Each carbon–oxygen bond is somewhere between a single and double bond.
- [ ] The actual structure of formate switches back and forth between the two resonance forms.
Resonance structures reflect the delocalization of electrons, and the true form of the molecule is represented by a resonance hybrid.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F76d7f8b2-08eb-4715-bdb9-c3273b88bbdd%2F3a171ec0-bb4d-45e4-be9b-12bef01e3576%2F1edlma_processed.png&w=3840&q=75)
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