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.
A benzene ring bonded to a three-carbon chain with a carbonyl group (C=O) at the end of the chain. The oxygen atom in the carbonyl group has two lone pairs of electrons.
**b)** 
A molecule with a long conjugated π-system. It begins with a single bond to an isopropyl group, followed by a sequence of alternating single and double carbon-carbon bonds.
**c)** 
A benzene ring bonded to a two-carbon chain with a positive charge on the second carbon and a double bond following that carbon. The double bond is between the second and third carbon.
**d)** 
A six-membered carbon ring (cyclohexane) bonded to a two-carbon chain with a positive charge on the second carbon and a double bond following that carbon. The double bond is between the second and third carbon.
**Detailed Explanation of Diagrams:**
- **Diagram a):** The molecule features a benzene ring, making it an aromatic compound. An extended chain with a carbonyl group introduces π-π conjugation possibilities. The resonance structures will be possible by delocalizing the electrons on the oxygen in the carbonyl group.
- **Diagram b):** This molecule has a conjugated diene system with isopropyl substitution. This type of conjugation can stabilize the molecule through delocalization of π-electrons.
- **Diagram c):** This structure presents an aromatic benzene ring connected to a positively charged carbon next to a double-bonded carbon. The positive charge can induce shifts in the π-system, creating resonance forms.
- **Diagram d):** The cyclohexane ring conjugated with a positively charged carbon. The presence of the double bond and positive charge suggests resonance stabilization through electron movement in the π-system.
These examples illustrate key principles in drawing and understanding resonance structures in organic compounds, which is central to grasping the behavior of complex molecules in different chemical environments.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F44572439-aee9-40a4-8ec4-b1e043de89f6%2Fbaaa1e35-1d14-4e70-843d-a781ebf75487%2Fx8psbyf_processed.jpeg&w=3840&q=75)
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